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Chemistry A Level Flashcards

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1
Q

What is enthalpy change of atomization?

A

Enthalpy change of atomization ΔHatθ - enthalpy change when 1 mole of gaseous atoms is formed from its elements under standard conditions

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2
Q

What is lattice energy?

A

Lattice Energy ΔHlatθ -enthalpy change when one mole of an ionic compound is formed from its gaseous ions under standard conditions.

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3
Q

What is lattice dissociation enthalpy?

A

Lattice dissociation enthalpy is the enthalpy change that takes place when one mole of an ionic compound is broken down to form its gaseous ions. If gaseous ions are turned into a solid lattice, ΔH is negative.

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4
Q

What is lattice dissociation enthalpy?

A

Lattice dissociation enthalpy is the enthalpy change that takes place when one mole of an ionic compound is broken down to form its gaseous ions. If gaseous ions are turned into a solid lattice, ΔH is negative.

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5
Q

What are the properties of negative ΔHlatθ?

A

More negative ΔHlatθ → stronger ionic bonding → more stable ionic compound

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6
Q

What does it mean when ΔHlatθ value is similar theoretically and experimentally?

A

If theoretical and experimental ΔHlatθ value similar, bonding is pure ionic, otherwise it is intermediate between ionic and covalent

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7
Q

What are the two factors that affect lattice enthalpy?

A
  • Ionic charge - increasing the ionic charge increases the attraction between the positive and negative ions meaning a larger, more negative lattice formation
    enthalpy.
  • Ionic radius - decreasing the ionic radius means the ions are closer together in the lattice so the attraction between the ions is stronger meaning a larger, more negative lattice formation enthalpy and its more exothermic
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8
Q

What is lattice energy proportional to?

A

ΔHlatθ ∝ Radius of Ion/ Charge on Ion
​

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9
Q

What is the first electron affinity?

A

First electron Affinity ΔHeaθ - enthalpy change when 1 mole of electrons is added to 1 mole of gaseous atoms to form 1 mole of gaseous anions under standard conditions. It is measured in kJ mol-1 and always has a negative sign to show energy is released.

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10
Q

What is the trend of electron affinity?

A
  • Electron affinity decreases down the group because although nuclear charge increases, electron shielding and atomic radius increase so there is less attraction between the nucleus and an incoming electron.
  • This means less energy is released as you go down the group.
  • Fluorine and oxygen are exceptions to this rule as they have lower electron affinities than expected. This is because they are relatively small so are already crowded with electrons which repel an incoming electron.
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11
Q

What is the second electron affinity?

A

Second electron affinity is the energy required to add one electron to each ion in one mole of gaseous 1- ions to form one mole of gaseous 2- ions. This requires energy because the negative ion repels the incoming electron. Electron affinities are endothermic because when electron added to negative ion, increased repulsion present therefore requires input of energy

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12
Q

What enthalpy changes does the Born-Haber cycles use?

A
  • Lattice enthalpy of formation or lattice enthalpy of dissociation.
  • Enthalpy change of atomisation.
  • Enthalpy change of formation.
  • First ionisation energy - the energy required to remove one electron from one mole of gaseous atoms to form one mole of gaseous 1+ ions. In Born-Haber cycles, his is only used for metals.
  • First electron affinity - the energy released when each atom in one mole of gaseous atoms gains an electron forming one mole of gaseous 1- ions. In Born-Haber cycles, this only applies to non-metals
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13
Q

How is lattice enthalpy calculated?

A

Lattice enthalpy is calculated using Born-Haber cycles.

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14
Q

How is the Born-Haber cycle made for the endothermic process?

A
  • ΔHfθ of an element under standard conditions = 0
  • Endothermic Processes:
    Bottom to top:
    ΔHiθ
    ​ΔHatθ
    ​ΔHeaθ 2nd and 3rd

​

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15
Q

How is Born-Haber cycle made with the exothermic process?

A
  • ΔHfθ of an element under standard conditions = 0
  • Exothermic Processes:
    Top to bottom:
    ΔHfθ
    ​ΔHeaθ
    ​ΔHlattθ
    ​ΔHhydθ
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16
Q

What is the enthalpy change of a solution?

A

Enthalpy change of solution ΔHsolθ - enthalpy change when one mole of ionic solid is dissolved in sufficient water to form a very dilute solution under standard conditions (can be positive or negative)

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17
Q

What is the enthalpy change of hydration?

A

Enthalpy change of hydration ΔHhydθ - enthalpy change when one mole of specified gaseous ions dissolves in sufficient water to form a very dilute solution under standard conditions

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18
Q

What are the factors affecting hydration

A
  • Factors affecting ΔHθhyd = factors affecting ΔHθlat
  • Ionic charge - increasing the ionic charge increases the attraction between the positive and negative ions meaning a larger, more negative lattice formation
    enthalpy.
  • Ionic radius - decreasing the ionic radius means the ions are closer together in the lattice so the attraction between the ions is stronger meaning a larger, more negative lattice formation enthalpy.
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19
Q

What dose the solubility of ionic salts depend on?

A

Solubility of ionic salts depend on value of ΔHθsol the more negative = more soluble

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20
Q

What is ion polarization?

A

Ion polarization is distortion of the electron cloud on an anion by a neighbouring cation

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21
Q

What is polarizing power?

A

Polarizing power is the ability of a cation to attract electrons and distort and anion

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22
Q

How is polarization increased?

A
  • Cation has a higher charge density: high positive charge and small size
  • Anion has greater polarizability: high negative charge and large size
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23
Q

What is the trend of thermal stability of group 2 CO3 and (NO3)2?

A
  • Down the group, polarizing power decreases
  • Mg2+ > Ca2+ > Sr2+ > Ba2+
  • The greater the polarization, the more distorted is the anion causing it to weaken the C – O bond
  • Therefore, easier to form CO2 and XO and compound less stable.
  • Order of stability: Ba2+ > Sr2+ > Ca2+ > Mg2+
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24
Q

What are things about Solubility of group 2 Hydroxides & Sulphates?

A
  • Radius of cation increases down group \therefore∴ charge density decreases
  • Attraction of cation to water molecule decreases therefore the value of ΔHhydθ becomes less exothermic
  • ΔHθlat also decreases but decrease is relatively smaller because of large size of anions compared to cations
  • ΔHθsol becomes less exothermic because decrease in ΔHθhyd is greater than decrease in ΔHθlat therefore the solubility of Hydroxide increase and Sulphate decrease down the group
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25
Q

How do you predict spontaneity by looking at the ΔH and ΔS?

A
  • When ΔH is negative and ΔS is positive: Using the equation, ΔH is negative and TΔS is positive so -TΔS is negative. Regardless of temperature, ΔG is always negative so the reaction is spontaneous at all temperatures.
  • When ΔH is positive and ΔS is negative: Using the equation, ΔH is positive and TΔS is negative so -TΔS is positive. Both terms are positive regardless of temperature so ΔG is always positive and the reaction is never spontaneous.
  • When ΔH and ΔS are positive: Using the equation, ΔH is positive and TΔS is positive so -TΔS is negative. Increasing the temperature causes -TΔS to get more
    negative. At high temperatures, -TΔS will outweigh ΔH and ΔG will be less than 0 so the reaction will be spontaneous. The reaction won’t be spontaneous at low temperatures.
  • When ΔH and ΔS are negative: Using the equation, ΔH is negative and TΔS is negative so -TΔS is positive. At high temperatures, -TΔS becomes more positive so
    will outweigh ΔH meaning the reaction won’t be spontaneous. The reaction will be spontaneous at low temperatures.
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26
Q

When is Gibbs free energy spontaneous and when isn’t it ?

A
  • A reaction or process is spontaneous/feasible when ΔG is less than or equal to 0.
  • If ΔG is positive, the reaction is not spontaneous at the temperature used in the calculation.
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27
Q

What is the Gibbs equation?

A

ΔG = ΔH - TΔS
ΔG - Gibbs free energy change (kJ mol-1)
ΔH - enthalpy change (kJ mol-1)
T - temperature (K)
ΔS - entropy change (kJ K-1 mol-1)

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28
Q

How do you find the minimum temperature at which Gibbs reaction is spontaneous?

A
  • To find the minimum temperature at which a reaction is spontaneous when given ΔH and ΔS,
    rewrite the equation as: ΔH - TΔS < 0 and rearrange to find temperature.
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29
Q

What is electrolysis?

A

Electrolysis is the decomposition of a compound into its element by an electric current

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30
Q

What makes an electrolysis cell?

A
  • Electrolyte is a compound that is decomposed (molten/ionic)
  • Electrodes are the rods which allow current to enter electrolyte (inert/reactive)
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31
Q

What happens when an electrolyte is molten?

A

When the electrolyte is molten, cations (positive ions) move to the cathode and gain electrons to form atoms. Anions move towards the anode, lose electrons and become atoms

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32
Q

What is the equation of a molten electrolyte at the anode and cathode?

A
  • At the cathode: positive ions reduced to atoms
    Pb2+(l) + 2e- → Pb(s)
  • At the anode: negative ions oxidized to atoms/molecules
    2NO3-(l) → NO2(g) + O2(g) + 2e-
    SO42-(l) → SO2(g) + O2(g) + 2e-
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33
Q

What is the standard electrode potential?

A

Standard electrode potential (EӨ): the emf (electromotive force) of a half cell compared with a hydrogen half cell under standard conditions.

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34
Q

What is produced in the cathode and anode in aqueous electrolytes when using inert electrodes?

A
  • When using inert electrodes to electrolyse a solution, if the metal ions are below hydrogen in the electrochemical series (more positive EӨ), the metal atoms will be produced at the cathode.
  • If the metal is above hydrogen in the electrochemical series, hydrogen gas will be produced at the cathode.
  • Metals from lead to zinc in the electrochemical series depend on the concentration, with the more concentrated ions becoming atoms.
  • A very dilute solution will form hydrogen and when the metal ion concentrations are similar, both may form atoms.
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35
Q

What is produced in the cathode and anode in aqueous electrolysis when the electrodes are non-inert?

A
  • When electrolysing a solution with non-inert electrodes, the same reaction takes place at
    the cathode.
  • At the anode, atoms in the anode lose electrons to form ions in the electrolyte.
  • The net charge is a transfer of an element from the anode to the cathode.
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36
Q

What happens in aqueous electrolyte at the cathode by Eθ and regarding the concentration?

A

Aqueous Electrolyte:
At the cathode
By Eθ
- Eθ > 0‎ then metal less reactive than H so metal formed
- Eθ < 0‎ then metal more reactive than H so H2(g)
formed
By Concentration
- Following results from above, if solution very dilute, this occurs greater 2H+(aq)+2e- → H2(g)

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37
Q

What happens in aqueous electrolyte at the anode by Eθ and regarding the concentration?

A

By Eθ
- Eθ > 0.4‎ then non-metal less reactive than OH so non-metal formed
- Eθ < 0.4‎ ‎ then non-metal more reactive than OH so H2O(l) formed
By concentration
4OH−(aq) → 2H2O(l) + O2(g) + 2eZ-2

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38
Q

What is the standard conditions of standard electrode potential Eθ?

A

Standard conditions:
- Temperature: 298 K
- Pressure: 1 atm (101 kPa)
- Concentration: 1.00 mol dm-3

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39
Q

What is the standard cell potential?

A

Standard cell potential (EӨcell): the emf (electromotive force,) when two half cells are connected under standard conditions

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40
Q

What is Emf?

A

Emf: electromotive force, the voltage when no current flows

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41
Q

What is Faraday constant?

A

The Faraday constant (F) is equal to the Avogadro constant (L) multiplied by the charge of
an electron in coulombs (e): F = Le
1 faraday = 9.65 x 104 C mol-1 (coulombs per mole)
- A coulomb is a quantity of electricity.
Number of coulomb = current (amps) x time (seconds).
- Avogadro’s constant is the number of particles in one mole of any substance. This is equal to 6.02 x 10^23

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42
Q

How do calculate the number of coulombs?

A

Number of coulomb (Q) = current (amps) (I) x time (seconds) (t)
Q=It
- Mass of a substance liberated is proportional to the quantity of electricity which passes through electrolyte

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43
Q

How do you find the mass of a substance liberated during the electrolysis?

A
  1. Multiplying current (amps) by time (seconds) to find the number of coulombs.
  2. Convert the number of coulombs to faradays using the conversion 1 faraday = 96500 C mol-1
  3. Divide the Faraday constant by the Avogadro constant to find the quantity of charge in coulombs
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44
Q

How do you calculate Avogadro’s constant from experimental results?

A
  1. Multiply the current (amps) by the time (seconds) to find the number of coulombs.
  2. Use the cathode reaction,
    - 1 mol of electrons forms 1 mol of silver
  3. Calculate the number of moles by dividing the mass change by the atomic mass of the atom.
  4. Find the number of coulombs in one mole of electrons by dividing the calculated number of coulombs from step 1 by the number of moles in step 3.
  5. To calculate the Avogadro constant, divide the number of coulombs in one mole of electrons by the charge on an electron
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45
Q

How do you calculate the EӨ cell

A

EӨ cell = EӨ reduction (positive terminal) - EӨ oxidation (negative terminal).

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46
Q

How do you know which electrode is being oxidised?

A

Half cells with more negative electrode potentials are more likely to be oxidised and lose electrons. When two half cells are connected, the more negative half cell will always undergo oxidation

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47
Q

What are the half cells?

A
  • A cell can be made by connecting two half cells with different electrode potentials. One half cell will release electrons while the other will gain them.
  • The half cell with the more positive EӨ (positive terminal) will gain electrons while the half cell with the more negative EӨ (negative terminal) will release electrons
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48
Q

What is the standard hydrogen electrode (S.H.E)?

A
  • It is a reference cell, used to measure Eθ of any other half cell
  • Consists of H2(g) at 298K and 1atm bubbling around a Pt electrode in contact with an aq. solution of H+ ions at 1.00 mol dm-3 conc. (e.g. HCl­(aq) or ½ H2SO4(aq)
  • Pt electrode is inert, allows conduction and is coated with finely divided Pt serving as a catalyst. Being porous, retains large amounts of H2(g)
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49
Q

What is a salt bridge?

A
  • Used to complete the electrical circuit allowing the movement of ions between two half cells so that ionic balance is maintained; electrically neutral
  • A strip of filter paper soaked in KNO3(aq)
  • Salt used should not react with ions forming a ppt. e.g. KCl in a cell containing Ag2+ would form insoluble ppt.
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50
Q

What are the features of electrolysis?

A

Each half cell must contain one element in two oxidation states. To create a closed circuit and allow charge to flow, a salt bridge must be placed between the two solutions and a wire must connect the two electrodes. A voltmeter measures the potential difference of the cell.

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51
Q

How do you know when a reaction is feasible or spontaneous?

A

A reaction is feasible, or spontaneous, if the cell potential is positive

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52
Q

What are the features of electrode potential of halogens?

A
  • As the value of EӨ becomes more positive, the position of the equilibrium lies further to the
    right and the element is more likely to be reduced. - An oxidising agent is a species which oxidises another species while being reduced.
  • Fluorine is the most powerful oxidising agent in the group because it has the most positive EӨ value.
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53
Q

What does a hydrogen fuel cell consist of?

A
  • Two platinum coated porous electrodes that allow gases to pass through
  • Electrolyte; either acidic or alkaline
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54
Q

What happens in an acidic electrolyte?

A
  • Negative Electrode (anode):
    2H2(g) 4H+(aq) + 4e-
  • positive Electrode (cathode):
    O2(g) + 4H+(aq) + 4e- 2H2O(l)
    Overall reaction:
    O2 + 2H2(g) 2H2O(l)
  • H+ ions removed at positive electrode replaced by those produced at negative electrode so concentration of electrolyte remains constant
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55
Q

What happens in an alkaline electrolyte?

A
  • Negative Electrode (anode):
    2H2(g) + 4OH-(aq) 4H2O(l) + 4e-
  • Positive Electrode (cathode):
    O2(g) + 2H2O(l) + 4e- 4OH-(aq)
  • Overall reaction:
    O2 + 2H2(g) 2H2O(l)
  • OH- ions removed at -ve electrode replaced by those produced at +ve electrode so conc. of electrolyte remains constant
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56
Q

What are the advantages of hydrogen fuel cell?

A
  • No pollutants – by product is water
  • More energy per gram of fuel than other fuels
  • Lightweight
  • Operate with high efficiency
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57
Q

How do you write redox reaction?

A

Half equations can be combined to form a redox equation. The number of electrons on both sides of the redox equation must be the same so that the electrons are cancelled out.

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58
Q

What are the steps of redox reaction?

A
  1. Half equations
  2. Decide the positive and negative terminals:
    The more positive standard electrode potential so this is the positive terminal and the forward reduction reaction occurs. It is more negative and so undergoes oxidation.
  3. Balance the electrons
  4. Combine equations
  5. Cancel species that appear on both sides
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59
Q

What is the Nernst equation?

A

The Nernst equation is used to calculate the electrode potential of a half cell when the concentration of aqueous ions changes.

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60
Q

How do calculate Nernst equation?

A

E = Eθ + (0.059/z) log ([oxidised form] / [reduced form])

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61
Q

What happens to Eθ when the concentration of a substrate decreases or increases?

A
  • If concentration less than 1 mol dm-3,log[oxidized form] is negative and E is less than Eθ
  • If conc. more than 1 mol dm-3, log[oxidized form] is positive and E is more than Eθ
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62
Q

What happens when acids and alkalis are added to water?

A

When acids and alkalis are added to water, they dissociate/ionize and a dynamic equilibrium is set up

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63
Q

What are conjuagate acid-base pair?

A

An acid and a base that are only different by one proton are called a conjugate acid-base pair

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64
Q

What are strong acids?

A
  • HA(aq) + H2O(l) ‎→‎ H+(aq) + A-(aq)
  • Equation position to the right
  • Dissociates completely ‎therefore [Acid] = [Ions]
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65
Q

What are weak acids?

A
  • HA(aq) + H2O(l) ‎⇌‎ H+(aq) + A-(aq)
  • Equation position to the left
  • Dissociates partially ‎therefore [Acid] ‎≠‎ [Ions]
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66
Q

How do you calculate pH or H+ concentration?

A

pH = -log10[H+]
[H+] = 10-pH

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67
Q

How do you calculate the acid dissociation constant?

A

Ka = [H+][A−] / [HA]
- For the equation HA ⇋ H+ + A
- Ka is the acid dissociation constant. The lower the Ka value, the further left the equilibrium lies.
- For weak acids, the Ka is very small so Ka values can be converted into pKa values
- As pKa increases, the strength of the acid decreases.

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68
Q

How do you calculate pKa values?

A
  • pKa = -log10(Ka)
  • As pKa increases, the strength of the acid decreases.
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69
Q

What is pH scale?

A
  • Gives strength of acid depending on H+
  • Use –log of values as they are very small giving pH
  • Lower pH value, stronger the acid
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70
Q

How do calculate pH?

A

−log[H+]=pH ⇔ [H+]=10−pH

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71
Q

What are the steps to work out the pH of a strong base?

A
  1. Calculate the concentration of hydroxide ions.
  2. Calculate the concentration of H+ ions using Kw
  3. Convert [H+] into pH, pH = -log10[H+].
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72
Q

What are the steps to work out the pH of weak acid?

A
  1. For the equation HA(aq) ⇋ H+(aq) + A-(aq):
    - Assume that a very small number of hydrogen ions come from the dissociation of water, so [H+] = [A-]
    - Assume that the concentration of acid at equilibrium is the same as the original concentration because it is a weak acid so little dissociation has occurred.
  2. Rewrite Ka, Ka = [H+]^2 / [HA]
  3. Rearrange Ka before entering the values to calculate [H+]
  4. Convert [H+] into pH
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73
Q

How do you calculate the ionic product of water?

A

Kw = [H+][OH-]
- Kw is the ionic product of water. The value of Kw
varies with temperature.
- At room temperature, this is equal to 1.00 x 10-14 mol2 dm-6

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74
Q

How do calculate the ionic product of a concentration of water?

A

Kc = [H+][OH−] / [H2O]
- Water molecules can function as both acids and bases; one molecule (base) accepts H+ from second one (acid)
H2O(l) ⇌ H+(aq) + OH-(aq)

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75
Q

How do you calculate pH of an alkali?

A

−log throughout equation therefore −log1×10−14=14∴
14 = pH + pOH

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76
Q

What is a buffer solution?

A

A solution in which pH doesn’t change significantly when small amounts of acids or alkali added

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77
Q

What are two things a buffer solution van be?

A

A buffer solution can be:
- Acid: Weak acid + its salt
e.g. CH3COH and CH3COONa
- Alkali: Weak alkali + its salt
e.g. NH3 and NH4Cl

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78
Q

What is an acidic buffer?

A

An acidic buffer has a pH less than 7 and contains a large amount of weak acid and its conjugate base (from a salt) and relatively few H+ ions in equilibrium

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79
Q

What must the optimum blood pH?

A

Blood pH must remain between 7.35 and 7.45

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80
Q

What is an alkaline buffer?

A

An alkaline buffer has a pH greater than 7 and contains a weak base and its salt.

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81
Q

What happens in respiration in the blood cells?

A

-Respiration in cells produces carbon dioxide and carbon dioxide combines with water in blood
CO2(aq) + H2O(aq) ⇌ H+(aq) + HCO3-(aq)
- The enzyme carbonic anhydrase is present to supply HCO3- ions and increase its concentration similar to acidic buffers

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82
Q

What happens when the pH in our blood increases?

A

If pH increases (hydrogen ion concentration decreases), the position of equilibrium will shift to the right to increase the concentration of hydrogen ions. If pH falls (hydrogen ion concentration increases), the position of equilibrium will shift to the left to remove the added H+ ions.

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83
Q

What happens when we increase H+ ions in the blood?

A

CO2(aq) + H2O(aq) ⇌ H+(aq) + HCO3-(aq)
- Equation shifts to the left
- Reduces H+
- pH of blood unchanged

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84
Q

What happens when we increase H+ ions in the blood?

A

CO2(aq) + H2O(aq) ⇌ H+(aq) + HCO3-(aq)
- Equation shifts to the right
- Increases H+
pH of blood unchanged

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85
Q

How do you calculate pH of buffer solutions?

A

pH=pKa +log([Salt] / [Acid])

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86
Q

What are the assumptions of weak acids you make when calculating buffer solutions?

A

For weak acids, two assumptions were made:
1) [H+] = [A-] - this is no longer true as the buffer contains a much larger concentration of A- . The concentration of A- is assumed to be the same as the concentration of the salt as the number of A- ions coming from HA is tiny (as it is a weak acid).
2) [HA] at equilibrium = [HA] at the start - this is assumed for the buffer because the added A-
ions from the salt push the equilibrium to the left meaning there is little dissociation of the acid.

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87
Q

Define solubility product (Ksp)?

A

Its a product of concentration of each ion in a saturated solution of sparingly soluble salt at 298K raised to the power of moles in dissociation equation

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88
Q

What are assumptions of solubility product (Ksp)?

A
  • The concentration of ions is independent of amount of solid
  • Ksp values change only with temperature
  • Concentration of ions = solubility of salt
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89
Q

What insures that the solubility for a compound is the same?

A

The solubility product for a compound will always be the same under the same conditions provided that the solution is saturated. If two compounds are mixed together, a precipitate will only form if the ionic concentrations give a value greater than the solubility product (otherwise, the solution won’t be saturated).

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90
Q

What is precipitation?

A

Precipitation is when two aq. solutions of ionic substance are mixed, a ppt. will form provided the Ksp of the insoluble solid is less than ionic product of ions present

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91
Q

What is the common ion effect?

A

The lowering of solubility of an ionic compound by addition of a common ion to the solution

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92
Q

What is titration?

A
  • Titration is the method used to find conc. of a solution by gradually adding to it a second solution of known conc. until neutralization point is reached
  • Progress of neutralization reaction monitored using a pH meter and shown on a graph
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93
Q

What is the equivalence point and end point of titration?

A

Equivalence point: mid-point of near-vertical portion of the graph where no. of mols H+ = no. of mols OH-
End point: volume of alkali/acid added when indicator just changes colour

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94
Q

How do you choose a suitable indicator for titration?

A
  • Sharp colour change at end point
  • End point must be ±2 pH of equivalence point
  • Indicator should give distinct colour change
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95
Q

What happens to the indicators Phenolphthalein and Methyl orange at low pH and high pH ?

A

Indicator - Phenolphthalein Methyl orange
Colour at low pH - Colourless Red
pH Range - 8.2 – 10.0 3.2 – 4.4
Colour at high pH - Pink Orange

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96
Q

What is the general solubility rule of solvents?

A
  • General solubility rule: like dissolves like
  • Covalent substances dissolve/mix in other covalent substances
  • Ionic substances do not dissolve/mix in other covalent substance (exception is water)
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97
Q

What happens the solubility in water?

A
  • Although covalent, highly polar nature makes it excellent solvent for ionic substances
  • Dissolves some covalent substances because they either react or form H-bonds with water molecules
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98
Q

What is the partition law?

A
  • The Partition law is a solutes solubility will be differed in two different liquids that are immiscible. The solute will be more soluble in one of the two.
  • Measured in [conc.]: g cm-3 or mol dm-3
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99
Q

What is partition coefficient (Kpc)

A
  • Partition coefficient (Kpc): equilibrium constant that relates the concentration of solute partition between two immiscible solves at a particular temperature.
  • Kpc = Conc. of Solute in Solvent 1 / Conc. of Solute in Solvent 2
  • Place concentration of the first solvent mentioned on top of the Kpc expression
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100
Q

How do you find the reactions involved in Partition Coefficients, Kpc?

A
  • Two immiscible liquids will form two separate layers in a separating funnel with the less dense layer on top. - If substance X is dissolved in both of these liquids, it may be more soluble in one layer than another.
  • A dynamic equilibrium will be set up at the boundary
    between the two liquids:
    X(in more dense liquid) ⇋ X(in less dense liquid)
    There are no units for the partition coefficient because any units cancel out.
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101
Q

What is a rate equation?

A

Rate equation: for the reaction A + B → C, the rate equation is rate = k[A]m[B]n (m is the order of the reaction with respect to A, n is the order of reaction with respect to B)

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102
Q

What is the rate constant?

A

Rate constant: the constant (k) linking rate of reaction and the concentration of reactants. This value changes with temperature and use of a catalyst but remains the same if only concentrations of reactants are changed.

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103
Q

What does the rate of the constant depend on?

A
  • Larger the rate constant, faster the reaction
  • Depends on temperature
  • Unit depends on overall order of reaction
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104
Q

What is the order of the reaction?

A

Order of reaction: the power to which the concentration of a reactant is raised in the
rate equation (this could be 0, 1 or 2)

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105
Q

What is the half life of a reaction?

A

Half-life: the amount of time taken for the concentration of the reactants to halve

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106
Q

What does it mean if a reaction is 0 ordered?

A
  • If a reaction is 0 order with respect to reactant P, the rate is unaffected by changing the
    concentration of P
  • The overall order of a reaction is equal to the sum of all the orders of the reactants
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107
Q

What does it mean if a reaction is first ordered?

A
  • If a reaction is first order with respect to reactant Q, doubling the concentration of Q with double the rate (rate ∝ [Q] or rate = k[Q])
  • The overall order of a reaction is equal to the sum of all the orders of the reactants
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108
Q

What does it mean if a reaction is second ordered?

A
  • If a reaction is second order with respect to X, doubling the concentration of X will quadruple the rate (rate ∝ [X]2 or rate = k[X]2)
  • The overall order of a reaction is equal to the sum of all the orders of the reactants
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109
Q

How do you calculate the rate constant of the half life (t½)?

A
  • Only used with first order reactions
  • The half life (t½) of a first order reaction is constant. This means the time taken for the
    concentration of reactants to half is always the same.
  • The relationship between the rate constant (k)
    k= 0.693 / t½
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110
Q

What is the relationship between temperature and the rate constant?

A
  • Increasing the temperature, increases the value of k
  • k= R/[A][B]
  • When temperature is increased, the k.e. of reacting molecules increases resulting in more successful collisions
  • Reactants change faster to products therefore conc. of reactants decreases.
  • Using fraction above, numerator increases and denominator gets smaller therefore kk increases
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111
Q

What does the rate of a reaction mechanism describe?

A

A reaction mechanism describes the steps involved in making and breaking bonds during a reaction.

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112
Q

What is a rate-determining step?

A

Rate-determining step: the stage with the slowest rate in a multi-step reaction.

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113
Q

What are things you need to keep in mind in n a multistep reaction?

A
  • The rate of reaction is dependent on the slowest step that needs the highest activation energy.
  • Rate equation includes only reactants that are present in the rate-determining step.
  • The orders with respect to the reactants are the moles of the reactants in the rate determining step
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114
Q

What must be included in the rate-determining step ?

A
  • The slowest step of a reaction ( the rate- determining step) must include reactants which
    have an impact on the rate of reaction when their concentrations are changed.
  • Zero order reactants have no influence on the rate of a reaction so they cannot be included in the
    rate-determining step.
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115
Q

When constructing a reaction mechanism what do the power in the equation indicate?

A
  • When constructing a reaction mechanism, the powers in the rate equation indicate the number of molecules of each substance involved in the slowest step
  • Any intermediates generated in the slowest step must be reactants in another step as they are not present in the balanced overall equation.
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116
Q

What is sampling?

A

Sampling: method that involves taking small sample of a reaction mixture at various times and then carrying out chemical analysis on sample.

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117
Q

How do you measure the rate of colour change in a reaction?

A

Colorimeter measures amount of light absorbed as it passes through solution; recorded as absorbance.

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118
Q

How do you measure the rate of change in volume of gas produced in a reaction?

A
  • Measure change in volume of gas using a gas syringe
  • Take down readings at regular intervals
  • Plot graph and calculate rate of reaction
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119
Q

What is continuous measurement?

A

Continuous is a method that involves monitoring a physical property over a period of time

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120
Q

What are things you need to do before and during an experiment when making a graph?

A
  • Before experiment, create calibration curve by finding absorbance of different concentration and plot a graph of concentration against absorbance
  • During experiment, measure absorbance from meter at regular intervals, and use calibration curve to convert values into concentrations
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121
Q

What is a homogeneous and heterogeneous catalyst?

A

A homogeneous catalyst is in the same phase as the reactants while a heterogeneous catalyst is in a different phase to the reactants

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122
Q

How does a homogeneous catalysts take part in the reaction?

A
  • Forms intermediate with reactant
  • Intermediate breaks down giving product
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123
Q

Define catalyst

A

A catalyst is a substance which speeds up the rate of a reaction without being chemically changed at the end

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124
Q

What is the rate of the reaction of a homogeneous catalyst depend on?

A

Rate of reaction dependant on conc. of catalyst

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125
Q

How does hetrogeneous catalyst take part in a reaction

A
  • Catalyst provides surface on which reaction occurs
  • Reactant particles adsorbed on surface on collision with catalyst
  • Molecular rearrangement occurs - bonds in reactants break and new bonds in product formed
  • Product molecules desorbed from surface
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126
Q

What does the rate of a reaction of a heterogeneous reaction depend on?

A

Rate of reaction dependant on surface area of catalyst

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127
Q

What does absorption in heterogenous catalysts mean?

A

Adsorption: weak bonds formed between reactant molecules & surface of catalyst (diffusion on to surface)

128
Q

What does deporption in hetrogenous catalysts mean?

A

Desorption: releasing of product molecules from surface of catalyst (diffusion away from surface)

129
Q

What are key points of Boltzmann distribution?

A
  • The area under the curve is equal to the total number of particles present.
  • The Boltzmann distribution is for gases
  • No particles have no energy.
  • There is no maximum energy.
  • Only particles with energy above the activation energy have sufficient energy to react when they collide.
130
Q

What are the trends in group 2 metals?

A
  • The reactions of Group 2 metals, metal oxides, metal hydroxides and metal carbonates generally
    indicate that reactivity increases as you go down Group 2.
  • Reactivity increases down the group because ionisation energy decreases due to the increasing atomic radius and the shielding effect of electrons. This means further down the group, the electrons become easier to remove so reactivity increases.
131
Q

What are the expectations of group 2 metals trends?

A

Some exceptions to this trend can be seen when sulfates and hydroxides are produced, however this is due to the insolubility of some sulfates and hydroxides inhibiting reactions.

132
Q

What happens when carbonates and nitrates react down group 2 ?

A

Both carbonates and nitrates become more thermally stable as you go down Group 2.

133
Q

What is the stability of group 2 nitrate and carbonate compounds influenced by?

A

The stability of the compounds is influenced by charge density of the cation and how polarised the
anion becomes.

134
Q

What is the trend of ions formed from elements at the top of group 2 and what does this trend mean?

A
  • Ions formed from elements at the top of group 2 are smaller than those at the bottom.
  • A smaller +2 ion has a greater charge density because the same charge is packed into a small volume.
  • This means smaller group 2 ions have a greater polarising effect on neighbouring negative ions.
135
Q

What is the trend of thermal stability of the nitrates and carbonates of group 2 elements?

A
  • The more polarised the anion is, the less heat is required for thermal decomposition to occur.
  • This means that thermal stability increases down the group because ions further down the group are worse at polarising the anion so more heat energy is required to break bonds for thermal decomposition.
136
Q

What are things about the solubility of group 2 hydroxides and sulfates?

A
  • The trend in the solubility of sulfates is opposite to the trend in the hydroxides
  • Compounds with very low solubilities are often said to be sparingly soluble.
  • Most sulfates are soluble in warm water except barium sulfate which is insoluble.
137
Q

What is the solubility trends of the Group 2 metal hydroxides?

A

Group 2 element - X Hydroxide - X(OH)2
Magnesium Least soluble
Calcium
Beryllium
Barium Most soluble

138
Q

What is the solubility trends of the Group 2 metal sulfate?

A

Group 2 element - X Sulfate - XSO4
Magnesium Most soluble
Calcium
Beryllium
Barium Least soluble

139
Q

What is the lattice enthalpy trend down group 2?

A

As you go down Group 2, the lattice enthalpy required to break up the compound decreases
because the size of the positive ions increases

140
Q

What does the cation trend in group 2 relate to?

A

-As the cations increase in size down the group, the enthalpy change of hydration (the amount of energy released as the ions bond to water molecules) also decreases.

141
Q

What does a larger cation mean in a compound?

A

Larger cations means there is more space between ions in the compound so there are weaker forces of attraction between the ions.

142
Q

What is the solubility in of group 2 metal hydroxides in terms of enthalpy change of hydration and lattice energy?

A

For hydroxide ions (relatively small ions), the lattice enthalpy falls faster than the enthalpy change of hydration of the cations. This means the enthalpy change of solution will become more negative down the group (more exothermic)

143
Q

What is the solubility in of group 2 metal sulfates in terms of enthalpy change of hydration and lattice energy?

A
  • For sulfate ions (relatively large ions), the lattice enthalpy falls slower than the hydration enthalpy of the cations. This means the enthalpy of solution will become more positive down the group (more endothermic).
  • The more exothermic the enthalpy of solution is, the more soluble a compound is. Therefore sulfates become less soluble down the group and hydroxides become more soluble down the group.
144
Q

What are transition elements?

A

Transition elements are found in the d-block of the periodic table. Transition elements form one or more stable ions with incomplete d orbitals.

145
Q

What is the trend of filling electron orbitals and what the exceptions to this trend?

A
  • The 4s orbital is filled before the 3d so the 4s electrons are removed before the 3d electrons.
  • Also remember that the electron configurations of
    copper and chromium are different than expected as the 4s orbital only has one electron.
  • This is so that the 3d subshell is filled for copper and half filled for chromium, as these are more stable electron configurations.
146
Q

Why are scandium and zinc transition metals?

A

Scandium and Zinc are not transition metals because:
- Sc3+ has no e-s in the d-orbital
- Zn2+ contains a full d-orbital

147
Q

How are different d orbitals on the axis?

A
  • dxy, dxz, ​dyz have d-orbitals in between axis
  • dx2−y2 and dz2 have d-orbitals along axis
  • dz2 is formed by the merging of dx2−z2 and dy2−z2
148
Q

What are the melting point trends of transition metals?

A
  • Transition metals have higher melting points that metals found in the s-block, like calcium.
  • This is because the transition metals have the extra 3d electrons so metallic bonding is stronger, requiring more energy to overcome
149
Q

What are the density trends of transition metals?

A
  • As you go across the periodic table, nuclear charge increases.
  • This draws the electrons inwards slightly, decreasing the atomic radius. As a result, transition metals have higher densities than metals in the s-block because the atoms are smaller so atoms fit into a given volume compared with s-block metal atoms.
  • Density is also greater because atomic mass increases across the period.
150
Q

What are the variable oxidation states of transition metals?

A
  • Transition metals can exist in variable oxidation states.
  • Variable oxidation states form because the electrons in the 4s and 3d orbitals have very
    similar energies.
  • This means that a relatively similar amount of energy is required to gain or lose different numbers of electrons.
  • Most common oxidation state +2 when 2e-s from 4s lost
151
Q

What leads to transition elements forming high and low oxidation states?

A
  • Transition elements show highest oxidation states when they combine with O or F (most electro-ve)
  • When transition elements form compounds with high oxidation states above +4, they form large oxyanions and are covalent (acidic oxides)
  • When transition elements in lower oxidation states they form ionic compounds (basic oxides)
152
Q

What is a complex?

A

A complex is an ion or molecule formed by a central metal atom/ion surrounded by one or more ligands

153
Q

What does a complex consist of?

A
  • Central transition metal ion (positive) that can accept e-s
  • Ligand (negative) is a species that contains a lone pair of e-s that forms a dative bond to a central metal atom/ion
154
Q

What is a coordination number?

A

Coordination number is a number of coordinate or dative bonds to the central metal atom/ion

155
Q

Why do transition metals form complexes?

A
  • Ion are small in size so they have a strong electric field around them which attract e–rich ligands
  • They have empty 4s and 4p orbitals that are hybridised and can accept e-
  • Different metal ions show different coordination number with same ligands
156
Q

What is a ligand?

A

Ligand: a species that has a lone pair of electrons that forms a dative covalent bond with a central metal atom or ion

157
Q

What is a monodentate ligands?

A

Monodentate ligands: forms only one coordinate bond with central metal ion (donates one pair of e-s)

158
Q

What is liganded exchanges?

A

When ligands swap places with one another, this is called ligand exchange or ligand substitution. The coordination number and shape of the ion stays the same if the ligands are a similar size and charge.

159
Q

What is a bidentate ligand?

A

Bidentate ligands: forms 2 coordinate bonds with central metal ion (donates 2 pairs of e-s per molecule)

160
Q

How do you name lignads?

A
  • If neutral and -ve ligands present, first name -ve ligand
  • If ligands all neutral -ve or contain more than one of each, name in alphabetical order
161
Q

How do you represent coordination numbers?

A
  • For monodentate ligands, use prefixes mono-, di-, tri-, tetra-, hexa-
  • For bi and polydentate ligands, use prefixes mono-, bis-, tris-, tetrakis-, pentakis-
162
Q

How do you name a central metal ion?

A
  • If complex ion +ve/ neutral – use normal name
  • If complex ion –ve, use name ending –ate; special:
  • Iron = Ferrate
  • Lead = Plumbate
  • Copper = Cuprate
  • Oxidation no. of metal ion in Roman numeral and ‘ion’
163
Q

How do you write a formula for complex number?

A
  • Metal ion written first followed by ligand
  • Place charge on formula in square brackets
  • Total charge on complex = sum of charge on metal ions and charge on ligand
  • If ligands all neutral, charge on complex = charge on metal ion
164
Q

What is the transition metal complex shape?

A

Transition metal complexes can be described as linear, octahedral, tetrahedral or square planar, depending on the ligands and the metal ions in the complex

165
Q

What is the geometry of a linear transition metal?

A

A linear complex is most commonly formed by a
silver metal ion with two coordinate bonds. The
bond angles are 180

166
Q

What is the geometry of a octahedral transition metal?

A

An octahedral complex is formed when a metal ion has 6 coordinate bonds. This happens with water and ammonia because they are small so 6 ligands are able to surround the central metal ion. Two octahedral complexes are shown below, one with a single type of ligand and the second with a mixture of ligands. The bond angles are 90.
.

167
Q

What is the geometry of tetrahedral transition metals?

A

If there are four coordinate bonds in a complex the shape is usually tetrahedral. The bond angles are 109.5.

168
Q

What is the geometry of square planer transitional element?

A

Sometimes a square planar shape when there are four coordinate bonds instead of a tetrahedral shape. The bond angle is 90. The compound shown is cisplatin, an anti cancer drug.

169
Q

What is Cis-trans isomerism?

A

Square planar complexes with two pairs of ligands show cis-trans isomerism. A trans isomer is when the two paired ligands are opposite each other in the complex. A cis isomer is when the pair of ligands are next to each other.

170
Q

What is an optical isomerism?

A

Optical isomerism is where an ion can exist in two forms which are non-superimposable mirror images. This occurs in octahedral complexes with three bidentate ligands.

171
Q

How does cisplatin work?

A
  • DNA contains bases, one of which is guanine. A nitrogen atom in guanine forms a coordinate bond with the platinum ion in cisplatin, replacing a chloride ion ligand.
  • A second nitrogen from a different guanine base bonds to the platinum ion, replacing the other chloride ion ligand.
  • The cisplatin has bonded to the DNA strands, creating a kink in the strands and preventing correct cell replication.
172
Q

What are the issue of cisplatin?

A
  • Cisplatin can also bind to DNA in healthy cells. This is a problem for cells which replicate frequently, like hair cells and blood cells. This is why the drugs can cause hair loss and why it can suppress the immune system.
  • The drug can also cause kidney damage.
  • The issues with the drug are minimised by giving patients small dosages and by targeting the tumour directly.
173
Q

What is cisplatin?

A

Cisplatin is a complex of platinum(II) containing two ammonia ligands and two chloride ion ligands. It has a square planar shape. Cisplatin is used as an anticancer drug.

174
Q

What happens when transition metals react with hydroxide ions?

A

Metal aqua ions react with hydroxide ions to form precipitates. Hydroxide ions are monodentate ligands
Not ligand exchange; hydroxide ions remove hydrogen ions from water ligand

175
Q

What happen when transition metals reacct with ammonia solutions?

A
  • Small amount of ammonia
  • Initially, ammonia acts as a base and hydrogen ions are pulled off the hexa aqua ion as above.
  • Excess ammonia
  • Ammonia replaces water as a ligand
  • Only 4 of the 6 water molecules replaced
176
Q

What happens when transtion metals react with chloride ions?

A

Chloride ions act as monodentate ligands when they react with metal aqua ions. They are charged and larger so only four Cl- ions are able to fit around the metal ion. This means the coordination number decreases from 6 to 4.

177
Q

What is a stability constant?

A

Stability constant, Kstab: the equilibrium constant for the formation of the complex ion in a solvent from its constituent ions or molecules
Water not included in Kstab expression because concentration almost constant

178
Q

What are strength of different ligands?

A
  • Exchange of ligands can be explained in terms of completing equilibria of forward & backward reaction
  • Equilibrium position lies towards more stable complex
  • Adding excess weak ligand can shift equilibrium backward and form weaker complex
179
Q

What makes a stability constant stronger?

A
  • Stability constants are used to compare stability of any two ligands
  • The greater the Kstab value, the more stable the complex
  • Kstab values may be given on log10 scale as values large
  • Stability constants for complexes with bi/polydentate ligands very high
180
Q

What are the conditions for complex to be be coloured?

A
  • At least one d-orbital must be occupied by an e-
  • At least one d-orbital must not be fully occupied
181
Q

Why are some d-block metals colourless?

A

Hence, some compounds of d-block metals colourless:
- All Sc compounds colourless because 3d0
- All Zn compound colourless because 3d10

182
Q

What are the factors that determine transition colour complex?

A

Factors that determine colour of complex (which affects the splitting of d-orbitals):
- Magnitude of ΔE
- Strength of ligands
- Oxidation state of metal ion
- Geometry of complex

183
Q

What does the colour Spectrum mean regarding ΔE?

A

Large ΔE = light absorbed from blue = complex red-ish
Small ΔE = light absorbed from red = complex blue-ish

184
Q

How do you name organic compounds?

A
  1. Identify the longest carbon chain that contains the functional group.
  2. Identify the functional group on the chain. This gives you the suffix or prefix of the compound.
  3. Count along the carbon chain so that the functional group has the lowest number.
  4. If there are any side chains, add these as prefixes (e.g. methyl-) to the beginning of the name. Do the same if there are other (less important) functional groups. Put these at the start of the name in alphabetical order.
  5. If there are two or more identical functional groups or side chains use the prefixes di-, tri- and tetra- before that section of the name.
185
Q

What are functional groups?

A

Functional group - a group of atoms responsible for the characteristic reactions of an organic compound.

186
Q

What is an electrophile reaction?

A

Electrophile - a molecule or substance that acts as an electron pair acceptor.

187
Q

What is an addition reaction?

A

Addition - a reaction where two or more molecules react to form a larger molecule.

188
Q

What is an elimination reaction?

A

Elimination - a reaction in which two substituents are removed from a molecule in a mechanism with one or two steps.

189
Q

What is a chiral centre?

A

A chiral centre is an atom with four different groups bonded to it. This arrangement creates compounds which are non-superimposable mirror images of each other. If a compound has a chiral centre, it will display optical isomerism. It is possible for compounds to have more than one chiral centre.

190
Q

How do you spot chiral centres?

A

Chiral centres can be spotted in organic compounds by identifying a carbon atom which is bonded to four different groups.

191
Q

Why do synthetic drugs often only contain a single isomer?

A
  • A chiral drug extracted from a natural source often contains a single optical isomer
  • More effective
  • Fewer side effects
  • Reduces cost long term as money isn’t wasted producing the optical isomer that is ineffective.
192
Q

Why do optical isomers have different shapes?

A
  • Optical isomers of a molecule have different arrangements of bonds so they have different shapes.
    -This means that only one of the enantiomers may fit into the active site (binding site) of an enzyme. As a result, only one of the enantiomers will cause the desirable effect
193
Q

What is an optical isomerism?

A
  • Optical isomerism is another branch of stereoisomerism. It occurs when there is a chiral
    centre.
  • Optical isomers have the same molecular and structural formula but they are mirror images of one
    another
194
Q

What are enantiomers?

A

The two mirror images are called enantiomers, they have identical physical and chemical properties except one

195
Q

How do you identify optical isomer enantiomers?

A

Optical isomers enantiomers can only be identified by their ability to rotate plane polarised light in equal and opposite directions.

196
Q

How do you make racemic mixtures?

A

If there is an equal mixture of each enantiomer then this is called a racemic mixture. This mix has no effect on plane polarised light as the equal and opposite rotations cancel out to zero

197
Q

What are the properties of benzene?

A
  • Clear, colourless, non-polar liquid at r.t.p
  • It is volatile and has a low b.p.
  • Relatively unreactive due to strong bonding
  • Burns with smoky flame
198
Q

What is the bond of benzene?

A
  • Benzene is a planar molecule with bond angles of 120.
  • All the carbon-to-carbon bonds are identical so it has a regular hexagonal shape.
  • There are C-H and C-C sigma bonds as well as a delocalised pi system above and below the carbon ring.
  • One electron from each carbon is delocalised into the pi (π) system which contains 6 electrons
199
Q

What is electrophile substitution mechanism?

A
  • E+ attacks (pi) π e- ring, accepting a pair of e- from benzene
  • An intermediate +ve specie is formed in which +ve charge is delocalized around the ring (more stable than a normal carbocation)
  • Proton eliminated from +ve intermediate to restore stability and \piπ system of delocalized e-s reformed
200
Q

What is the electrophile substitution mechanism bond?

A
  • An H-atom on the ring can be substituted by other atoms/groups
  • All carbon atoms identical and benzene ring symmetrical hence any H-atom can be substituted
  • An electrophile (E+) can attack the ring of (pi) π e-s but benzene highly stable so E+ must be very strong.
  • A +ve ion can be generated by heterolytic fission of a covalent bond hence catalyst needed to generate E+
201
Q

What is the halogenation electrophilic substitution reaction?

A

C6H6(l) + X2(g/l) →{catalyst}→ C6H5X(l) + HX(g)
- Reagent: dry Cl2 gas / pure Br2 liquid
- Conditions: Temperature/pressure: r.t.p.
- Catalyst: anhydrous AlCl3(s) / FeBr3(s)
- Generating electrophile: catalysts are e- deficient halogen carriers, form dative bond drawing e- from halogen molecule producing X+
- AlCl3 + Cl2 →[AlCl4]- + Cl+
- Regenerating catalyst:
H+ + [AICl4]− → HCl + AlCl3

202
Q

What is nitration electrophilic substitution reaction?

A

C6H6(l) + H2SO4/HNO3 → C6H5NO2(l) + H2SO4(g) + H2O
- Reagent: nitrating mixture; conc. HNO3 / conc. H2SO4
- Condition: Temp.: 45-55C under reflux
- Generating electrophile:
2H2SO4 + HNO3 → 2HSO4- + NO2+ + H3O+
- Regenerating catalyst:
2HSO4- + H3O+ + H+→ 2H2SO4 + H2O

203
Q

What is Alkylation/Acylation electrophilic addition reaction?

A

C6H6(l) + RCl/RCOCl → {AlCl_3} → C6H5R/C6H5RCO + HCl(g)
- Reagent: alkyl halide (RCl) / acyl chloride (RCOCl)
- Condition: Temp.: heat under reflux
- Catalyst: anhydrous AlCl3
- Generating electrophile:
AlCl3 + RCl/RCOCl [AlCl4]- + R+/RCO+
- Regenerating catalyst: H+ + [AlCl4]- HCl + AlCl3

204
Q

What is hydrogenation electrophilic addition reaction?

A

C6H6(l) + 3H2(g) →{Nickel}→ C6H12
- Type of reaction: electrophilic addition
- Conditions: Temp.: 150ºC
- Catalyst: nickel

205
Q

What is Chloromethyl Benzene side chain reactions?

A

C6H5CH3(l) + Cl2(g) → C6H5CH2Cl(l) + HCl
- Type of reaction: free radical substitution
- Reagent: Cl2(g)
- Condition: u.v. light
- With excess Cl2 a mixture of di, tri chloromethyl benzene can be obtained

206
Q

What is benzonic acid side chain reactions?

A

C6H5CH3(l) + 3[O] → C6H5COOH(l) + 2H2O
- Type of reaction: oxidation
- Reagent: KMnO4(aq) or K2Cr2O7(aq)
- Condition: heat under reflux (2 to 3 hours)
- Alkyl gp. always oxidized regardless of chain length
- If more than one alkyl gp., each one oxidized

207
Q

What is the ring activating groups?

A
  • Alkyls, NH2, OH
  • Donates e- to the ring
  • positive inductive effect
  • electro-sub faster
  • Increase e- density at position 2 and 4
208
Q

What is the ring deactivating group?

A
  • Cl, NO2, COOH
  • Withdraws e- from ring
  • negative inductive effect
  • electro-sub slower
  • Sub. occurs at pos. 3 & 5
209
Q

What is friedel-crafts reaction?

A

Friedel-Crafts reactions involve electrophilic substitution of aromatic rings, there are two types - Alkylation and Acylation.
Alkylation involves the substitution of alkyl groups such as CH3, C2H5 and C3H7, acylation involves the substitution of acyl groups such as CH3C=O in both cases a catalyst is needed this is because the attacking species isn’t a strong enough electrophile

210
Q

Why is chlorbenzene less reactive than benzene?

A
  • Chlorine is a ring deactivating group
  • Chlorine is more electronegative than carbon, and draws electrons in the ring towards itself.
  • Hence electron density around ring decreases, less attractive for electrophiles and so reaction is slower
211
Q

Why is haloarenes less reactive than haloalkenes?

A
  • the halogen atom in halogenoarene is much less reactive than that in a halogenoalkane
  • Lone pair of e‑s of Cl overlap slightly with p orbitals of benzene ring giving C–Cl a double bond character
  • Makes C–X bond much stronger therefore nucleophilic substitution difficult
  • High density of e-s on benzene ring tends to repel the approaching –ve charged nucleophile
212
Q

What is the hydrolysis nucleophilic substitution reaction?

A

C6H5Cl(l) + NaOH(aq) → C6H5OH(l) + NaCl(aq)
- Type of reaction: nucleophilic substitution
- Reagent: sodium hydroxide
- Condition: Temp.: 300-330C, Press: 150-300 atm
- Rate of Hydrolysis: (slowest to fastest)
R-CH2F → R-CH2CI → R-CH2Br → R-CH2I

213
Q

What are arenes?

A

Arenes are aromatic hydrocarbons

214
Q

Why do Arenes undergo substitution?

A
  • Aromatic hydrocarbons, are able to undergo electrophilic substitution.
  • Aromatic hydrocarbons delocalise electron systems and makes it a very stable molecule. Aromatic hydrocarbons is highly attractive to electrophiles because of the high electron density in the ring.
  • Electrophiles can be a positive ion or a positive end of a polar molecule. When the reaction takes place, the delocalised electron system remains in the compound and one of the hydrogen atoms swaps places with the electrophile.
215
Q

What is the benzene substitution with chlorine reaction?

A

The reaction of benzene with chlorine requires an aluminium chloride catalyst.
C6H6 + Cl2 → C6H5Cl + HCl
The mechanism for the electrophilic substitution reaction:
Stage 1: The aluminium chloride catalyst generates the electrophile from chlorine.
Cl2 + AlCl3 → AlCl4- + Cl+
Stage 2: The electrophile reacts with the benzene molecule.
Stage 3: The hydrogen ion reacts with the AlCl4-, reforming the AlCl3 catalyst.
AlCl4- + H+ → AlCl3 + HCl

216
Q

What is the benzene substitution nitration reaction?

A

The reaction of benzene to form nitrobenzene requires a mixture of concentrated nitric acid and concentrated sulfuric acid to generate the electrophile.
Stage 1: The electrophile is generated from concentrated nitric acid and concentrated sulfuric acid.
H2SO4+ HNO3 → H2O + NO2+ + HSO4-
Stage 2: The NO2+ electrophile reacts with the benzene molecule in electrophilic substitution.
Stage 3: The hydrogen ion reacts with the HSO4-, reforming the H2SO4 catalyst.
H+ + HSO4- → H2SO4

217
Q

What is the benzene substitution of an acyl group?

A

Acylation of benzene involves the substitution of an acyl group. This reaction takes place when benzene is reacted with ethanoyl chloride in the presence of an aluminium chloride catalyst.
Stage 1: The electrophile is generated from ethanoyl chloride and aluminium chloride.
CH3COCl + AlCl3 → AlCl4- + CH3CO+
Stage 2: The CH3CO+ electrophile reacts with the benzene molecule.
CH3CO+ + C6H6 → C6H5COCH3 + H+
Stage 3: The aluminium chloride catalyst is regenerated.
H+ + AlCl4- → AlCl3 + HCl

218
Q

What is the benzene substitution of an alkyl group?

A

Alkylation of benzene involves the substitution of an alkyl group. The reaction occurs in the same way as the acylation reaction takes place above. It requires a halogenoalkane as a reactant as they contain a polar bond between the carbon and halogen.
Stage 1: CH3Cl + AlCl3 → AlCl4- + CH3+
Stage 2: CH3+ + C6H6 → C6H5CH3 + H+
Stage 3: H+ + AlCl4- → AlCl3 + HCl

219
Q

How does hydrogenation of benzene ring take place?

A
  • Hydrogenation takes place when hydrogen atoms are added all around the benzene ring, removing the delocalised electron system.
  • A cycloalkane is formed as the product.
  • The reaction is carried out with hydrogen, in the presence of a nickel catalyst. A temperature around 150C is required.
220
Q

What happens when halogen reacts with methylbenzene?

A

When a halogen reacts with methylbenzene, two possible reactions can take place depending on the conditions. The halogen can bond to the benzene ring or the methyl group.
- Substitution in the benzene ring: This reaction happens in the presence of aluminium chloride and in the absence of UV light.
- Substitution in the methyl group: This reaction happens in the presence of UV light, without a catalyst. The reaction can continue to undergo substitution so that all the hydrogen atoms in the methyl group are replaced by chlorine atoms, forming C6H5CCl

221
Q

What is the difference in reactivity between chlorobenzene and chloroalkane?

A
  • Chlorobenzene is much less reactive than chloroalkane. This is because the C-Cl bond in
    chlorobenzene is much stronger than in an halogenoalkane.
  • The aromatic C-Cl bond is stronger due to one of the lone pairs on the chlorine atom interacting with the delocalised electron system, strengthening the bond.
  • For reactions, like nucleophilic substitution, the C-Cl bond would require breaking. Since the chlorobenzene bond requires more energy to break, chlorobenzene is less reactive.
222
Q

What is phenol?

A
  • Phenol is an aromatic alcohol; a white crystalline solid that is both corrosive and anaesthetic
  • OH group is ring activating so phenol more reactive than benzene and substituents attached at positions 2,4 and 6
223
Q

What is phenyl benzoate?

A
  • Benzoyl chloride is very unreactive because the
    -COCl group is directly attached to a stable benzene ring. To produce the ester phenyl benzoate, phenol is first converted into an ionic compound by dissolving it in sodium hydroxide.
  • This produces the phenoxide ion:
    The phenoxide ion is more reactive than the phenol so this ion can react with benzoyl chloride to produce phenyl benzoate
224
Q

What is phenyl benzoate?

A
  • Benzoyl chloride is very unreactive because the
    -COCl group is directly attached to a stable benzene ring. To produce the ester phenyl benzoate, phenol is first converted into an ionic compound by dissolving it in sodium hydroxide.
  • This produces the phenoxide ion:
    The phenoxide ion is more reactive than the phenol so this ion can react with benzoyl chloride to produce phenyl benzoate
225
Q

What happens when phenol reacts with a base?

A

C6H5OH(l) + NaOH(aq) →{r.t.p}→ C6H5O-Na+(aq)
H2O
- Type of reaction: Neutralization
- Reagent: sodium hydroxide
- Condition: r.t.p.
Regenerating phenol:
- When strong acid (HCl) added to solution of sodium phenoxide, phenol regenerated
C6H5O-Na+(aq) + HCl(aq)­ → C6H5OH(l) + NaCl
- Initially dense white emulsion formed then slowly oily liquid layer of phenol separates

226
Q

What happens when phenol reacts with sodium?

A

C6H5OH(l) + Na(s) →{r.t.p}→ C6H5O-Na+(aq) + ½H2(g)
- Type of reaction: metal and acid, redox
- Condition: r.t.p.
- Reacts with Na liberating H2 gas
- phenol does not react with metal carbonate to liberate CO2 hence shows its fairly weaker than other carboxylic acids
- Phenol reacts with metals in the same way that most acids. The reaction occurs slower than comparable acid-metal reactions because phenol is a weak acid.

227
Q

What happens when phenol undergoes bromination?

A

-Type of reaction: electrophilic substitution
- Reagent: aq. Bromine
- Condition: r.t.p. (no catalyst)
- Rapid reaction, forms a white ppt.
- No catalyst needed since Br2 molecule easily polarized by increase ­e- density in ring

228
Q

What happens when phenol undergos nitration?

A
  • Type of reaction: electrophilic substitution
  • Reagent: dilute nitric acid
  • Condition: r.t.p.
  • If concentrated nitric acid used, then trinitrophenol produced
229
Q

What leads to a stronger acid?

A
  • Higher the Ka value
  • More easily H+ is donated
  • More stable is the conjugate base
230
Q

What is the structure of phenol?

A
  • phenol is an aromatic alcohol
  • the OH group is attached directly to the benzene ring
  • it is an almost colourless crystalline solid of formula C6H5OH
231
Q

What is the production of plastics used for?

A

production of plastics
- antiseptics
- disinfectants
- resins for paints

232
Q

What is the realtive acidities of ethanol?

A

C2H­5OH + H2O ⇌ C2H5O- + H3O+
- Ka: 10-18 mol dm-3
- Ability to donate H+ ions: C2H5 is an e- donating gp. which increases charge density on O of OH
‎- More attraction between O–H so loss of H+ difficult
Stability of conjugate base:
- In ethoxide ion, C2H5 gp. increases –ve charge
- Makes ethoxide ion more basic than OH-
- Ability to accept H+ increases, moving equi. to left

233
Q

What is the relative acidities of water?

A

H2O + H2O ⇌ OH- + H3O+
- Ka: 10-16 mol dm-3
- No e- donating or withdrawing gp. present hence ability to donate and accept H+ ion is the same

234
Q

What is the relative acidities of phenol?

A

C6H­5OH + H2O ⇌ C6H5O- + H3O+
- Ka: 10-10 mol dm-3
- Ability to donate H+ ions: OH is a ring activating gp. & the lone pair of e-s on O becomes part of delocalized e- system
- Decreases e- density on O of OH and attraction between O and H decreases so H+ lost more easily
Stability of conjugate base:
- In phenoxide ion, -ve charge on O delocalized around ring and reduces tendency to attract H+
- Conjugate base stable

235
Q

What are the tests of phenol?

A

Test 1:
Reagent: Iron(III) Chloride (FeCl3(aq)) – yellowish brown
Observation: violet colour obtained

Test 2:
Reagent: bromine water (Br2(aq)) – orange
Observation: white ppt. obtained

236
Q

Why does the acidity of carboxylic acids decrease as carbon chain length increases?

A
  • Alkyl groups are e- donating groups which have a positive inductive effect increasing strength of O–H bond, and making it more difficult to donate H+
  • Alkyl groups increase negative charge on ion formed when dissociated, making it easier to accept the H+ and reform the molecule
237
Q

Why does the acidity of carboxylic acids increases when H atoms are substituted by electro negative atoms?

A
  • Chlorine atoms show a –ve inductive effect withdrawing –ve charge from the molecule, reducing the strength of the O–H, and hence making H+ be lost more easily
  • Conjugate base is more stabilized due to the extended delocalization of the negative charge on the –COO- and so less likely to bond with a H+ ion
  • If an e- donating gp. present molecule less acidic
  • If an e- withdrawing gp. present molecule more acidic
238
Q

What is the structure of carboxylic acid

A
  • Carboxylic acids are weak acids due to the structure of the carboxylate ion (RCOO-) which forms in solution.
  • In the carboxylate ion, a delocalised pi system
    develops over the -COO- group because the lone pair on the negatively charged oxygen overlaps with the p orbitals of the carbon atom.
  • This delocalised system distributes the negative charge through the -COO- group, making the carboxylate ion more stable.
239
Q

What are carboxylic acids?

A
  • Carboxylic acids are weak acids and dissociate incompletely in aqueous solutions
    R–COOH + H2O ⇌ R–COO- + H3O+
  • The O–H bond in carboxylic acid is weakened by the carbonyl group C==O
  • The carboxylate ion is stabilized by the delocalization of e-s around the –COO- group, spreading and reducing the density of -ve charge making it less likely to bond with H+
240
Q

What was the formation of acyl chlorides?

A
  • Acyl chlorides can be formed from carboxylic acids using sulfur dichloride oxide (SOCl2).
  • In this reaction, sulfur dioxide, hydrogen chloride and an acyl chloride are produced. The products are relatively easy to separate since SO2 and HCl are both gases.
    CH3COOH + SOCl2 → CH3COCl + SO2 + HCl
  • Acyl chloride can also be produced from carboxylic acids by using phosphorus(V) chloride
    or phosphorus(III) chloride
241
Q

What is the oxidation of methanoic acid?

A

HCOOH + [O] → CO2 + H2O
- With Tollens’ Reagent:
- Ag+ gets reduced to silver – silver mirror formed
- With Fehling’s Solution:
- Cu2+ gets reduced to Cu+ – copper(I) oxide (red)
Note: can use stronger [O] agents; Mn or Cr

242
Q

What is oxidation of ethanedioic acid?

A

HOOC–COOH + [O] → CO2 + H2O
- With warm Acidified Manganate(VII) - KMnO4/H+:
Purple/pink to colourless
- can also use Acidified Dichromate(VI)
Changes from orange to green

243
Q

What is acid hydrolysis of esters?

A
  • When esters react with water an acid catalyst is required. This reaction is reversible so excess water must be used to ensure the position of equilibrium is shifted as far towards the products as possible.
  • This reaction can occur when the ester is mixed with dilute acid.
    CH3CH2COOCH3 + H2O ⇌ CH3CH2COOH + CH3OH
244
Q

What is alkali hydrolysis of esters?

A
  • An ester can be hydrolysed by heating it under reflux with a dilute alkali (such as sodium
    hydroxide). These reactions are not reversible so the products are easier to separate.
    CH3CH2COOCH3 + NaOH → CH3CH2COONa + CH3OH
  • To convert the carboxylate salt product into a carboxylic acid, excess strong dilute acid can be added to the salt (after the alcohol has been removed from the products by distillation).
245
Q

What are acyl chlorides?

A
  • Acyl chlorides, also known as acid chlorides are acid
    derivatives. They have a similar structure to carboxylic acids, with the -OH group being replaced by a chlorine atom.
    Acyl chlorides have the suffix -oyl chloride,
    e.g. propanoyl chloride.
246
Q

What is the reaction of alcohols and acyl chlorides?

A
  • Esters are produced when alcohols and acyl chlorides react together.
  • When an alcohol reacts with an acyl chloride, a vigorous reaction takes place and steamy fumes of
    hydrochloric acid are produced.
247
Q

What is the reaction of phenol and acyl chlorides?

A
  • Phenols are aromatic compounds with an alcohol group bonded to the benzene ring.
  • The reaction between phenols and acyl chlorides produces an aromatic ester
248
Q

What is the reaction with primary amines and acyl chloride?

A
  • A primary amine contains an -NH2 group bonded to an alkyl group. Methylamine has the formula CH3NH2.
  • When a primary amine reacts with an acyl chloride, an N-substituted amide is produced. In the reaction below, N-methylpropanamide is formed (‘methyl’ comes from the alkyl group on the primary amine).
  • The hydrogen chloride produced reacts with the excess primary amine so the overall equation for the reaction can be written as:
    CH3CH2COCl + 2CH3NH2 → CH3CH2CONH2
    + CH3NH3Cl
249
Q

What is the relative ease of Hydrolysis with water of Acyl Chlorides, Alkyl Chlorides and Aryl
Chlorides?

A
  • Acyl chlorides react vigorously with cold water to produce a carboxylic acid and hydrogen chloride gas. E.g. CH3COCl + H2O → CH3COOH + HCl.
  • Alkyl chlorides have almost no reaction with water.
  • Aryl chlorides have no reaction with water.
250
Q

What was relative Ease of Hydrolysis with sodium hydroxide of Acyl Chlorides, Alkyl Chlorides and Aryl
Chlorides?

A
  • Acyl chlorides react vigorously with hydroxide ions to produce salts and water:
    CH3COCl + NaOH → CH3CONa + NaCl + H2O
  • Alkyl chlorides react with hydroxide ions to produce an alcohol and a salt:
    CH3Cl + NaOH → CH3OH + NaCl
    ● Aryl chlorides generally have no reaction with hydroxide ions
251
Q

What is the relative ease of Hydrolysis of Acyl Chlorides, Alkyl Chlorides and Aryl
Chlorides?

A
  • Acyl chlorides contain the group -COCl.
  • Alkyl chlorides are chloroalkanes containing C-Cl.
  • Aryl chlorides are aromatic compounds with a chlorine atom bonded to a benzene ring
  • The reactions above show that the relative ease of hydrolysis is acyl chlorides > alkyl chlorides > aryl chlorides. Acyl chlorides are hydrolysed the easiest while aryl chlorides are the least likely to undergo hydrolysis.
252
Q

What is the formation of alkyl amines by subsitution?

A

R–X + NH3 → R–NH2 + HX(g)
- Type of reaction: nucleophilic substitution
- Reagent: hot conc. NH3 in ethanol
- Condition: heat under reflux

253
Q

What is the formation of alkyl amines from halogenoalkanes?

A
  • Heat the halogenoalkane in a sealed tube with concentrated ammonia in an ethanol solvent (reflux cannot be used as ammonia is too volatile). To ensure that a primary amine is formed, rather than an ammonium salt, an excess of ammonia must be used.
254
Q

What is the formation of alkyl amines from reduction?

A

R–C ‎≡‎ N + 4[H] ‎→‎ R–CH2NH2
- Type of reaction: reduction of a nitrile
- Reagent: hydrogen gas
- Reducing Agents (catalyst):
LiAlH4 in dry ether
Nickel
- Conditions: high temp. and pressure

R–CO­–NH2 + 4[H] → R–CH2NH2 + H2O
- Type of reaction: reduction of an amide
- Reducing Agent (catalyst):
LiAlH4 in dry ether
- Conditions: high temp. and pressure Conditions: r.t.p.

255
Q

What is the formation of aryl amines from reduction?

A
  • Type of reaction: reduction of nitrobenzene
  • Reagent: conc. HCl with Tin
  • Condition: heat
256
Q

What is the basicity of amines?

A
  • Bases are proton acceptors (electron donors)
  • N-atoms in amines have a lone pair of e-s
  • N donates lone pair and accepts H+ forming dative bond
257
Q

What is a coupling reactions of diazonium salts?

A
  • Type of reaction: electrophilic substitution
  • Reagent: aromatic amines or phenols
  • Azo compounds are complex compounds involving a minimum of two aromatic rings joined by N=N coupling
  • Benzene diazonium ion carries a +ve charge and readily reacts with cold alkaline solutions of aromatic amines and phenols to give brightly coloured azo-compounds
  • Bright orange dye formed
  • By using alterative aryl compounds to phenol, a range of brightly coloured dye can be formed.
258
Q

What is the bromination reaction of phenyl amine?

A
  • Type of reaction: electrophilic substitution
  • Reagent: aq. Bromine
  • Conditions: r.t.p. (no catalyst)
  • Forms a white ppt
259
Q

What is the diazotization reaction of phenyl amine?

A
  • (–N2+ is called diazonium ion)
  • Type of reaction: diazotization reaction
  • Reagent: nitrous acid (NaNO2 with excess HCl(aq))(HNO2 weak, unstable acid so produced by reaction NaNO2 with excess HCl)
  • Condition: low temp. (5∘C)
  • Diazonium salts of aryl amine stabilized by delocalization of –N2+ ion’s e-s over benzene ring
  • However, diazonium ion highly unstable and can decompose above 10C to
260
Q

What is the neutrality of amides?

A
  • The presence of the electron withdrawing oxygen atom means that the lone pair on the amide’s nitrogen atom is not available to be donated to e.g. H+ ions
  • Hence, amides are neutral
261
Q

What is optical activity of amino acids?

A

Optical activity: all amino acids (except glycine) have a chiral carbon therefore they are optically active

262
Q

What are amides structure?

A
  • Amides contain the -CONH2 group. They are neutral despite the fact that they contain an -NH2 group.
  • This is because the lone pair on the nitrogen is delocalised into the pi bond between oxygen and carbon meaning the nitrogen atom is unable to attract a hydrogen ion, so is a much weaker base than amines.
  • The delocalisation also makes the molecule
    more stable so disrupting the delocalisation to accept a hydrogen ion would require a lot of
    energy.
263
Q

What is the formation of amides reaction with ammonia?

A
  • When acyl chlorides react with ammonia, an amide and hydrogen chloride gas is produced. Amides are organic compounds with the group -CONH2.
  • The suffix for naming an amide is -amide so for the reaction below, the product formed is propanamide.
  • The hydrogen chloride produced reacts with the excess ammonia to produce ammonium chloride so the overall equation for the reaction can be written as:
    CH3CH2COCl + 2NH3 → CH3CH2CONH2 + NH4Cl
264
Q

What is the reaction with primary amines in the formation of amides?

A
  • A primary amine is an organic compound with an -NH2 group bonded to an alkyl group, like methylamine, CH3NH2.
  • The product formed from the reaction between a primary amine and acyl chloride is called an N-substituted amide.
  • The hydrogen chloride produced reacts with the excess primary amine so the overall equation for the reaction can be written as:
    CH3CH2COCl + 2CH3NH2 → CH3CH2CONH2
    + CH3NH3C
265
Q

How do basic amino group and acidic carboxyl group interact?

A
  • Carboxyl group donates a proton to amino group
  • Amino group accepts proton and zwitterion formed
  • Amino acids solids at r.t.p. due to ionic bonds that exist between zwitterions
  • Presence of zwitterions means that amino acids are soluble in water
266
Q

What is a zwitterion?

A

Zwitterion: ion that contains regions of +ve & –ve charge

267
Q

What is a way in which electrophoresis can be used to separated amino acids?

A
  1. A piece of moistened filter paper is placed on a microscope slide.
  2. Crocodile clips are attached to each end of the paper and connected to a battery.
  3. A drop of amino acid solution is added to the middle of the paper.
  4. The apparatus is left for a period of time to enable separation to occur.
  5. Ninhydrin is sprayed onto the paper to make the colourless amino acid solution visible. The paper is dried and warmed gently, causing the amino acids to be seen as coloured spots.
268
Q

What is the peptide hydrolysis bond?

A

Hydrolysis: involves breaking of peptide links by reaction with water catalysed by an acid or alkali catalyst, giving back the amino acids, temp. nearly 90C

269
Q

What is a peptide bond?

A
  • Amide link formed by nucleophilic attack of –NH2 group of one amino acid on –COOH group of another
  • Reaction is a condensation reaction as H2O eliminated
  • Reaction can continue to occur as product still has –NH2 and –COOH group present
  • Dipeptide → Tripeptide → Polypeptide (protein)
  • Proteins are polymers of amino acids; many polypeptide chains held together by intermolecular forces
270
Q

What is electrophoresis?

A

Electrophoresis is used to separate, identify and purify amino acids obtained when protein hydrolysed

271
Q

What is techniques of electrophoresis?

A

Technique based on separating ions placed in an electric field. When sample placed between two electrodes:
- +ve charge ions move towards –ve charged electrode
- –ve charge ions move towards +ve charged electrode
- Sample placed on absorbent filter paper (or gel)
- Buffer solution carries ions along (back or forth)

272
Q

What are the properties of a zwitterion?

A
  • An amino acid contains both an acidic group
    (-COOH) and a basic group (-NH2).
  • The carboxylic acid donates a proton to the amine group to form a zwitterion (an ion containing a positive and negative charge).
  • A zwitterion has no overall electrical charge but it
    contains separate parts that are charged.
  • If an amino acid has a carboxylic acid or amine group in the R group, only one acidic and one basic group will be involved in the formation of the zwitterion.
  • In water, proton transfer will occur to form a charged ion.
273
Q

What is the reactions of phenylamine?

A
  • The -NH2 group in phenylamine activates the benzene ring meaning that it is more reactive.
  • This is because the lone pair on nitrogen is delocalised into the pi system, increasing the electron density meaning electrophiles are more attracted.
  • The -NH2 has a 2,4-directing effect meaning that groups will generally be substituted at the 2-position and the 4-position (with the carbon that is bound to the amine group being 1-position).
274
Q

What is condensation polymerisation?

A

Condensation polymerisation is the joining together of monomers to form a polymer with the
release of a small molecule such as water or HCl.

275
Q

What are the physical properties of polymers?

A
  • Only C and H present = only VDW forces present
  • Presence of Cl or F = dipoles = permanent dipole interaction
  • Longer chains with have fewer side chains have stronger VDW forces
276
Q

What is needed for polyester monomers to link with ester bonds?

A

A polyester contains monomers linked with ester bonds. For this link to form, either of the
following is needed:
- A monomer containing 2 carboxylic acid groups and a monomer containing 2 alcohol groups.
- A monomer containing both an alcohol and a carboxylic acid group

277
Q

How is an ester linkage of polyster formed?

A
  • The ester linkage is formed during a condensation reaction when H is lost from the OH of an alcohol and OH is lost from the COOH of a carboxylic acid.
  • The H+ and OH- combine to form water.
  • A monomer containing two -COCl (acyl chloride) groups may be used instead of the carboxylic acid. The only difference is that HCl forms instead of water
278
Q

What is needed for amide bonds in polyamides to for?

A

A polyamide contains monomers held together by amide bonds. For this link to form, either of the following is needed:
- A monomer containing 2 carboxylic acid groups and a monomer containing 2 amine groups.
- A monomer containing both a carboxylic acid and an amine group.

279
Q

How do you form an polyamides amide linkage

A
  • The amide linkage is formed during a condensation reaction when H is lost from the NH2 of an amine and OH is lost from the COOH of a carboxylic acid.
  • Water forms when the H+ and OH- combine.
  • As with ester bond formation, a monomer containing two -COCl (acyl chloride) groups can
    be used instead of the carboxylic acid, forming HCl instead of water
280
Q

What is a repeat unit?

A

A repeat unit is a structure that occurs in a molecule many times. Sometimes the repeat unit is made up of one monomer, sometimes it contains a pair of monomers.

281
Q

What is a protein?

A
  • Proteins are polymers made from amino acids.
  • Amino acids contain an amine group (-NH2) and a carboxylic acid group (-COOH).
  • The general structure of an alpha amino acid is
    shown below (where R represents any group):
  • A dipeptide contains 2 amino acids joined together with an amide bond. A polypeptide contains many amino acids bonded together in a chain by amide bonds.
282
Q

What is the structure of DNA?

A

DNA are polynucleotides; made by condensation polymerization of nucleotides.

283
Q

What is the function of DNA?

A
  • Can make copies of itself so that genetic information can be pass on from generation to generation
  • Contains sequence of bases that form genetic code used to synthesize proteins
284
Q

What are nucleotides in DNA are made up of?

A
  • A sugar called deoxyribose
  • A phosphate group
  • A nitrogen-containing base
285
Q

What is DNA replication?

A

Process of copying DNA during cell division

286
Q

What is semi-conservative replication?

A
  • H-bonds and VDWs between base pairs in part of a DNA are broken and this part of the double helix unwinds
  • In the nucleus, there are nucleotides to which two extra phosphates have been added (nucleotide triphosphate)
  • The bases of the nucleotide triphosphates pair up with complimentary bases on the old strand and H-bonds & VDW forces form between original and new strands.
  • Enzymes catalyse the polymerization reaction
  • Each new strand contains a sequence of bases that is complimentary to the original strand
287
Q

What is the significance of H-bonding in replication of DNA?

A
  • When a new strand built on template of old strand, the incoming nucleotide is selected for its ability to pair with base in the old strand
  • H-bonding plays an important role in the recognition as different number of H-bonds involved in each pair
288
Q

What is non-solvent based adhesive silyl modified polymers (SMP)?

A
  • A polymer that contains silicon bonded to oxygen
  • They set by reacting with moisture in air; water hydrolyses silicon-oxygen parts, forming cross-linkages
  • Effectively bonds polymer chains to each other with strong covalent bonds of siloxane cross-linkage
289
Q

What is the non-solvent based adhesive epoxy resin?

A
  • Example of thermosets: polymers that form extensive networks of covalent cross-links
  • Very strong and cannot be melted and remoulded
  • Formed by reacting a monomer with expoyethane (triangular molecule CH2CH2O) and a diamine are mixed
290
Q

What is the non-solvent adhesive superglue?

A
  • Uses addition reaction to stick objects together
  • The monomer is CH2­==C(CN)COOCH3, methyl cyanoacrylate, and addition takes place across C==C
  • Polymerisation initiated by presence of moisture
291
Q

What makes polymers conduct electricty?

A

Polymers generally insulators but ethyne can conduct electricity
- Contains alternate single & double carbon-carbon bonds
- Can conduct electricity because p-orbitals on neighbouring carbon atoms overlap resulting in long bands of delocalized \piπ e-s free to move along the chain
- Doping: other substances, such as iodine, added to improve electrical conductivity of polymer

292
Q

What are the advantages of polymer conductors over metal conductors?

A
  • Do not corrode
  • Much less dense
  • Shaped more easily
293
Q

What are the disadvantages of plastics?

A
  • Non-biodegradable
  • On combustion, give out harmful vapours
294
Q

What are biodegradable plastics?

A
  • Can contain small amounts of starch: bacteria and fungi in moist soil can break it down into smaller compounds, increase surface area and easier to decompose
  • Can be made from monomers derived from plants e.g. PLA: soil microorganism can digest it easily
295
Q

How can biodegradables plastics be hydrolysed in acidic conditions?

A
  • Polyamides broken down to carboxylic acids & amines
  • Polyesters broken down to carboxylic acids & alcohols
296
Q

What are photodegradable plastics?

A
  • Carbonyl group (–C==O) can absorb energy from ultraviolet waves
  • Causes bonds in region of carbonyl group to weaken and break
297
Q

What are the disadvantages of photodegradable plastics

A
  • Plastic usually buried under \therefore∴ cannot get sunlight
  • If recycled, products are weaker
298
Q

What are biodegradable polymers?

A
  • Poly(alkenes) are chemically inert (very unreactive) meaning they are difficult to biodegrade.
  • Some polymers, such as LDPE, can be degraded using light. Light (typically UV) causes the polymer chains to break so the material crumbles.
  • Polyesters are biodegradable and can be hydrolysed using dilute acids or alkalis (slower
    hydrolysis with acids)
299
Q

What are examples of polyesters?

A
  • Synthetic polyesters: terylene
  • Natural polyesters: fats
300
Q

What are addition polymers?

A
  • Monomers are alkenes; polymer formed is polyalkene
  • Alkene joins to itself, no molecule lost
  • Molecular mass of polymer is multiple of monomer
301
Q

How do you you predict polymerisation?

A

Addition polymerisation
- Monomers contain C=C double bonds.
- Main chain of the polymer only contains C-C single bonds.
- Main chain contains nitrogen or oxygen atoms as well as carbon atoms.
- The polymer is the only product of the reaction.

Condensation polymerisation
- Monomers contain -OH and -COOH or -COCl for polyesters. Monomers contain -NH2 and -COOH or
-COCl for polyamides.
- Main chain contains nitrogen or oxygen atoms as well as carbon atoms.
- The polymer and a small molecule like water or HCl are formed during the reaction

302
Q

How do complete the acid hydrolysis of proteins reactions?

A

The acid hydrolysis of proteins is very similar to the acid hydrolysis of polyamides. There are two ways to complete this reaction:
- Heat protein at 110°C with 6 mol dm-3 hydrochloric acid for 8 hours (slow method).
- Place protein in a sealed tube containing 6 mol dm-3 hydrochloric acid and an atmosphere of nitrogen. Place in a microwave for 5-30 minutes (depending on the protein), using temperatures up to 200°C. Faster method for small samples of protein during analysis.

303
Q

What is the temperature change and reaction spontaneity for exothermic reactions?

A
  • if temperature is increased
  • TΔS value becomes more +ve
  • ΔG +ve therefore less likely to be spontaneous
304
Q

What is the temperature change and reaction spontaneity for endothermic reaction?

A
  • if temperature is increased
  • TΔS value become more -ve
  • ΔG -ve therefore more likely to be spontaneous
305
Q

What is enthalpy-driven reaction?

A

If ‎∆H > T∆S
Enthalpy-driven reaction: flow of thermal energy provides most of the free energy in the reaction

306
Q

What is entropy-driven reaction?

A

If ‎∆H < T∆S
Entropy-driven reaction: increased disorder provides most of the free energy in the reaction

307
Q

What is gibbs free energy calculation?

A

ΔGθ reaction = ΔG2θ −ΔG1θ
​Form Hess’s cycle and calculate Free Energy as you would enthalpies (using moles etc.)

308
Q

What is entropy in equilibrium reaction?

A
  • At position of equilibrium, the total entropy change of forward reaction equals the total entropy change of backward reaction
  • Under standard reactions, the overall entropy change is zero
309
Q

What is gibbs free energy?

A

ΔG=−TΔStotal
​- Gibbs free energy (G): amount of energy in a system that is available to do useful work
- Standard molar Gibbs free energy of formation
(ΔGfθ ): the free energy change that accompanies the formation of one mole of a compound from its elements in their standard state

310
Q

How do calculate total entropy change?

A

Firstly, calculate the entropy change for a reaction
ΔSθ system =ΔSθ products −ΔSθ reactants

Next, calculate entropy change in the surroundings
TΔSθ surroundings = −ΔHreactionθ / T
​- T in Kelvin; std. temp. = 298K
- If ΔHθ reaction in kJ mol-1, change to J by × 1000
- Negative sign part of equation, always put it

Use values calculated to find total entropy change
ΔSθ total = ΔSθ system −ΔSθ surroundings
If ΔSθ total positive, reaction is feasible

311
Q

What is the entropy change in exothermic reactions?

A
  • Energy released to surroundings
  • Increases ways of arranging the energy of molecules in surrounding
  • Entropy increases
  • Increased probability of chemical change occurring spontaneously
312
Q

What is the entropy change in endothermic reactions?

A
  • Energy absorbed from surroundings
  • Decreases ways of arranging the energy
  • Entropy decreases
  • Increased probability of chemical change occurring spontaneously
313
Q

What causes entropy to change?

A
  • As a substance changes state from (s) → (l) → (g); its entropy increases as molecules become more disordered
  • When an ionic salt is dissolved in water (s) → (aq); the entropy increases as as the crystal breaks up and the ions find their way between the water molecules
  • Increasing the temperature of a substance (without changing state) increases entropy e.g. when heating a gas, the number of different possibilities for arranging the energy over the molecules increases.
  • If a reaction increases the number of gas molecules, the entropy increases as gases have higher entropies than solids or liquids
  • Simpler substances with fewer atoms have lower entropy values than more complex substances
  • For similar substances, harder substances have lower entropy values
314
Q

What is entropy?

A
  • Entropy: measure of the ‘disorder’ of a system
  • A system becomes more stable when its energy is spread out in a more disordered state
315
Q

What is spontaneous change?

A
  • Spontaneous change: a change that tends to happen naturally; once started, the change will carry on
  • Spontaneous changes may not be instantaneous or happen rapidly; most are slow and need an input of energy to start

chemistry a level (2 decks)

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