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Chemistry (JW) > Off by heart list > Flashcards

Off by heart list Flashcards

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1
Q

ion

A

electrically charged particle formed by the loss or gain of one or more electrons from an atom or group of atoms

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2
Q

isotopes

A

atoms of the same element with the same number of protons and different numbers of neutrons, therefore with different masses

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3
Q

relative isotopic mass

A

the mass of an isotope relative to 1/12th of the mass of an atom of carbon-12

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4
Q

relative atomic mass

A

weighted mean mass compared with 1/12th of the mass of carbon-12

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5
Q

electronegativity

A

the tendency of an atom in a covalent bond to attract (the bonded pair of electrons) electron density

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6
Q

covalent bond

A

strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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7
Q

dative covalent bond

A

covalent bond in which both electrons come from the same atom

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8
Q

ionic bond

A

electrostatic attraction between positive and negative ions

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9
Q

Avogadro’s constant (definition and formula using it)

A

The number of atoms in one mole of atoms of any element.

no. moles = no.particles/6.02 x 10^23

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10
Q

The ideal gas equation (including units)

A 
pV = nRT
p= Pa
V= m^3
n= mol
R= 8.314 Jmol-1K-1
T= K
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11
Q

Acid

A

a proton donor

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12
Q

Base

A

a proton acceptor/ substance which readily accepts H+ ions from an acid

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13
Q

A Salt is formed when…

A

an acid has one or more hydrogen ions replaced by either a metal ion or an ammonium ion

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14
Q

Weak acid

A

partially dissociates

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15
Q

Strong acid

A

fully dissociates

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16
Q

Alkali

A

a soluble base that releases OH- in aqueous solution

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17
Q

ionisation energy

A

energy required to remove electrons one by one from an atom / energy required to become an ion

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18
Q

reducing agent

A

chemical that is oxidised

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19
Q

oxidising agent

A

chemical that is reduced

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20
Q

disproportionation

A

oxidation and reduction of the same element in a redox reaction

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21
Q

gas volumes equation

A

no. moles = volume (dm3) / 24

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22
Q

solution concentration equation

A

moles (mol) = concentration(moldm-3) x volume (dm3)

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23
Q

homologous series

A

a series of organic compounds having the same functional group and similar chemical properties but with each successive member differing by CH2

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24
Q

structural isomers

A

molecules with the same molecular formula but with different structural formula

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25
Reasons for varying boiling points of organic compounds (2)
- increasing chain length increases surface contact and London forces - more branches, less surface contact, less London forces between molecules
26
Oxidation number : elements in natural state
0
27
Oxidation number : the sum of the atoms of any molecule
0
28
Oxidation number : the sum of the components of any ion
The charge on that ion
29
Oxidation numbers - rules for order of assigning oxidation numbers to specific elements
- Groups 1,2,3 always equal to charge (+1,+2,+3) - Fluorine always -1 - Hydrogen usually +1 - Oxygen usually -2 - Chlorine usually -1
30
Products of complete combustion
CO2 and H20
31
Products of incomplete combustion
CO, C and H20
32
Valency
Number of electrons an atom loses or gains (ionic) or the number of bonds it can form (covalent)
33
Difference between relative molecular mass and relative formula mass
Molecular- for simple molecules | Formula- for giant structures
34
What does a binary compound contain and how do you name them?
Contains two elements only. | Use name of first element but change the end of the second to -ide (in ionic, metal ion always comes first)
35
Molar mass
Mass per mole of a substance (gmol-1)
36
Empirical formula
Simplest whole number ratio of atoms of each element present in a compound
37
Molecular formula
The actual number and type of atoms of each element in a molecule
38
Hydrated Salt
Water molecules are part of the compounds crystalline structure (water of crystallisation)
39
First ionisation energy
The energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms (to form 1 mole of gaseous 1+ ions)
40
Free radical
A radical is a species with an unpaired electron
41
Stereoisomers
Have the same structural formula but different arrangements in space
42
Electrophiles
Species with a whole of partial positive charge. They are electron loving. ELECTRON PAIR ACCEPTORS
43
Explaining why Markovnikoffs (ov's) Rule is followed
The secondary (or tertiary) carbocation formed in the reaction is more energetically stable than the primary (or secondary) one which would be formed if the addition was the other way round, and so less activation energy is needed.
44
Homolytic fission
Covalent bond breaks with each bonded atom taking an electron from the shared pair of electrons from the bond.
45
Periodicity
Regular repeating pattern of variations of properties with Ar and Position on the periodic table
46
Bond enthalpy
Energy needed to break one mole of bonds in the substance in the gaseous state.
47
Reflux
Continuous process of evaporation followed by condensation
48
What are the standard conditions ?
298K and 100kPa
49
Standard enthalpy of formation
Energy required to make one mole of compound from its constituent elements in their standard states
50
First electron affinity
Energy change when one mole if singly negative ions is made from one mole of gaseous atoms
51
Mean bond enthalpy
Average energy change when one mole of a particular bond is broken in one mole of gaseous molecules
52
What does Hess’ Law state?
That the energy change of a reaction is independent of the route, providing the conditions are constant
53
Activation energy
Minimum amount of energy needed for a reaction to take place
54
Standard enthalpy change,
The heat energy change at constant pressure under standard conditions (pressure 100 kPa ; temperature 298 K ).
55
Standard molar enthalpy change of formation,
The enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions, with all reactants and products in their standard states.
56
Standard molar enthalpy change of combustion
The enthalpy change when one mole of a compound is completely burned in excess oxygen under standard conditions, all reactants and products in their standard states.
57
Mean bond energy
The enthalpy change when 1 mole of a particular type of bond is broken or made (all species in the gas phase) averaged over many different molecules
58
Lattice enthalpy
Energy released when one mole of a crystal is formed from its constituent ions in their gaseous state , standard conditions
59
Standard conditions?
298K , 100/101 kPa
60
Enthalpy of atomisation
Enthalpy change when one mole of gaseous atoms is formed from the element in its standard state
61
Electron affinity
Enthalpy change accompanying the gain of 1 mole of electrons by 1 mole of atoms in the gaseous phase
62
Enthalpy of formation
Enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard states
63
Transition Metal
Element which forms one or more stable ions which have incompletely filled d orbitals
64
Complex ion
Metal ion surrounded by coordinately bonded ligands
65
What do all ligands have in common?
Active lone pairs of electrons in the outer energy level. They are used to form coordinate bonds with the metal ion
66
Coordination number
Number of coordinate bonds that are formed with the central metal or ion
67
Standard electrode potential
Potential difference/ voltage of half call compared with standard hydrogen electrode Standard conditions: 298K, 1moldm-3, 1atm
68
Half life
Time for concentration to reduce by half
69
Charge on anode/cathode in cells
anode= negative | cathode=positive
70
More positive electrode potential=
better oxidising agent (gives up electrons more readily)
71
calculate overall cell potential
more positive - more negative
72
rate =
concentration/time
73
zero order
concentration has no effect on rate
74
first order
change in concentration gives same change to the rate
75
second order
any change in concentration changes the rate by the square of the concentration change
76
What is rate constant specific to?
Temperature
77
Bigger value of k =
faster reaction
78
half life equation=
ln 2 / k
79
gradient of a rate-concentration graph =
k
80
rate determining step
the slowest step of the reaction mechanism | reactants in this step are in the rate equation
81
fuel cells
produce electrical power using the energy from the chemical reaction of a fuel with oxygen
82
pH
-log10[H+]

Chemistry (JW) (3 decks)

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