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Alevel chemistry year2 > Chemistry mock weak points > Flashcards

Chemistry mock weak points Flashcards

(80 cards)

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1
Q

What ions are most likely to be aqueous

A

soluable compounds like NaCl, KNO3 and strong acids/bases

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2
Q

What ions are likely to not be aqeuous

A

insoluable ionic compounds eq CaCo3 and covalent compounds

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3
Q

What is an acid

A

Hydrogen donator/ protons

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4
Q

What is a base

A

Contains hydroxide ions and reacts neutralises Acids

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5
Q

What is an alkali

A

a base dissolved in a solution

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6
Q

What is first ionisation energy

A

energy require to remove one mole of an electron from 1 mole of gaseous atoms

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7
Q

What are the 3 factors that affect ionisation energy

A

Nuclear charge- increased pull from the nucleus makes it harder to remove an electron
atomic radius- the number of shells affects how far the valence electrons are from the nucleus attraction
shielding- the presence of shells of an atom weaken the affect of the nucleus attraction

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8
Q

What is the trend of first ionisation energy down a group

A

there are more shells despite increase nuclear attraction the valence electrons are further away therefore it decreases down the groupW

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9
Q

What is the trend of first ionisation energy across a period

A

The number of shells stays the same but nuclear charge increases so its harder to remove an electron therefore first ionisation energy increases

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10
Q

What are the two exceptions to first ionisation energy increase across the period

A

groups 2,3/ 5,6
2,3 this is due to the furtherest electron being in a P orbital compared to its prior being in an S, p orbitals have higher energy levels and therefore are easier to remove
5,6 the repulsion from both electrons being in the same orbital makes it easier for the electron to be removed

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11
Q

What is an induced DP DP interaction

A

random movement of electrons can cause a momentary DP of charge in atoms when then cause a other atoms to gain charges and be attracted to one another

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12
Q

What increases the strength of induced DP DP interactions

A

Larger molecules with more electrons have larger electron clouds as well as molecules with large surface area as they have large exposed electron clouds

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13
Q

What is a permanent DP interaction

A

The weak interaction between two polar molecules

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14
Q

What is a hydrogen bond

A

Hydrogen bonded to O,F,N have high cause for the molecule to become polar which can then bond to other similar molecules

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15
Q

Allotropes meaning

A

different forms of the same element

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16
Q

graphite

A

Hexagonal sheets with weak intermolecular bonds between the sheets, carbons each bonded to 3 others with a delocaised electron

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17
Q

Diamond

A

4 carbon bonds tetrahedral shape with a very high boiling point

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18
Q

Silicon

A

same structure as diamond 4 Si bonds which make up a lattice structure

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19
Q

Metallic bonding

A

Where metal atoms give up electrons to become delocalised positive atoms held together by delocalised electrons

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20
Q

How does melting/boiling point vary in metallic bonding

A

The amount of electrons per positive atom affects how strong the bonding is

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21
Q

What are the other properties of metallic bonding

A

Maliable- ions can slide over each other
Conductivity- delocalised electrons can carry charge
solubility- insoluble unless in liquids

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22
Q

Melting and boiling points in metals across a period

A

increases across a period as there are more delocalised electrons which make metallic bonding stronger

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23
Q

Melting and boiling points in giant covalent structures

A

very high due to the strong covalent bonds holding them together B,C and Si

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24
Q

Melting and boiling points in simple molecular structures

A

much lower due to being held together by only induced dp dp interactions. Larger molecules have higher electron clouds so have higher Bp S8 P4 Cl2

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25
Reactivity down the group
As the energy require to remove an electron decreases down the group reactivty increases down the group
26
Group 2 Metal + Water
Metal hydroxide + hydrogen metal hydroxide can dissolve in water to produce hydroxide ions which make strong alkaline solutions
27
Group 2 metals + Oxygen
Metal oxides
28
Group 2 metals + acids
Salt + hydrogen
29
Uses of group 2 metals
used in agriculture to neutralise acid soils can also be used as antacids for acids in the stomach
30
What is the trend in reactivity down the group Halogens
Atomic radius increases as well as shielding this makes it harder to pull in an electron to from an ion so down the group halogens get less reactive
31
Displacement of halogens
More reactive halogens when displace a less reactive halogen from its solution
32
How to distinctly see halogens
Add mixture to organic solvent like hexane and shake a solvent layer containing the halogen will form on top
33
What colours do the halogens show
violet pink - iodine orange red- bromine yellow/green- chlorine
34
test for halides
Add Dilute acids eg HNO3 to test for other ions and then add silver nitrate Chlorine white bromine cream iodine yellow
35
Halide solubility in NH3
Cl- dissolves in dilute Br- dissolves in conc I - doesn't dissolve at all
36
Making bleach
2NaOH + Cl2 -> NAClO + NaCl + H20
37
Formation for Chlorate(I) ions
Cl2 + H20 reverisble HCl + HClO HClO + H2O reversible CLO- + H3O CLO is chlorate ion
38
Test for Carbonate
Add a dilute ass if it bubbles it is present
39
Test for sulfates
Add Ba+ ions eg Barium nitrate will form a white ppt
40
Test for amonia
Heat mixture under damp red litmus paper should turn blue
41
Standard enthalpy change of reaction
Enthalpy change when a reaction takes place in molar quantites of the equation in standard states under standard condtions
42
Standard enthalpy change of formation
enthalpy change 1 mole of a compound is formed from its elements under standard conditions in its standard states
43
enthalpy change of combustion
enthalpy change when 1 mole of a substance in burnt completely in oxygen in its standard states under standard conditions
44
standard enthalpy of neutralisation
Enthalpy change when acids and alkali react together to make 1 mole of water in standard states under standard conditions
45
What is hess' law
The total change of a reaction is the same no matter the route taken
46
when calculating enthalpies
follow the arrow correct way and rearrange using the unkown value as X and making the 2 values equal to each other
47
What kind of reactions do alkenes undergo
electrophillic addition
48
How do alkenes produce alkanes
hydrogen with a nickel catalyst at 150 degrees
49
How to produce dihaloalkanes from alkenes
room temp and pressure no catalyst
50
test for unsaturation in alkenes
add bromine water should go from brown to colourless
51
how to make alcohol from alkene
Steam phosphoric catalyst 300degrees at 60/70 atm
52
subsitution alcohol their OH group with a halide
Conc H2SO4 at room temp
53
elimination of alcohol where a H and OH are removed to make an alkene
acid catalyst 170 degrees
54
Oxidation of primary alcohol to aldehyde
gently heat alcohol with potassium dichromate(VI) and sulfuric acid and distil oxidising agent also used reflux with oxidising agent
55
Oxidation of secondary alcohol to make ketone
reflux the alcohol with acidified dichromate(VI) to make a ketone
56
How do haloalkanes react
nucleophilic substitution
57
Hydrolysis of haloalkanes
done with warm aqeous alkali or water
58
SHC equation
Q= mcΔT
59
Percentage uncertainty
uncertainty * number of times measure/ measure value *100
60
Pv = nrt units
P= Pa V= M3 dm3/100 N= moles R= 8.314 T= temperature(K degress +273)a
61
what are standard conditions
298K 100Kpa
62
What is average bond enthalpy
average enthalpy change when 1 mole of covalent bonds are broken in gaseous conditions
63
creation of ozone
O2-> 2o. in uv light O2+O -> O3
64
chlorine radical fomation and attack ozone
CF2Cl2 -> CF2Cl2 + Cl. Cl. + o3-> ClO + O2 ClO+O -> Cl. + o2
65
Other atoms attack ozone
R. + O3 -> RO. + O2 RO. + O. -> R. + 02
66
Which group takes priory in benzene ring
phenyl groups
67
What kind of reactions does benzene undergo
electrophillic substitution nucleophiles attracted to high electron density
68
Why is benzene stable and how does it react
Very stable ring so takes a very strong nucleophile to break the ring
69
What is the carrier for alkylation and acylation of phenols and regeneration
AlCl3 Alcl3 + H+ -> AlCl4
70
reaction bebtween Ch3Cl + AlCl3
Ch3Cl + AlCl3 -> AlCl4 + Ch3+
71
What is the halogen carrier for nitration of benzene
Concentrated Sulfuric acid
72
Reaction for nitration explain
Conc H2so4 Conc HNO3 H2SO4 + HNO3 -> HSO4- H2NO3 H2NO3 -> H2 + NO3 sulfuric acid is a stronger acid than HNO3 and gives a hydrogen to nitric acid froms an unstable compound which decomposes to form a nitronium ion
73
Aromatic, aliphatic and alicylic
Aromatic- contains benzene ring Aliphatic- anything containing straight or cyclic carbon molecules thats not benzene Alicylic- contain cyclic molecules eg cyclohexane but does not contain benzene
74
What are phenols
Benzene with an OH group which adds to the electron density so it makes it more reactive weak acid partially dissociates in solution
75
What is the test for phenols
FeCl3 positive test is purple colour
76
Phenol + Base
Salt + water
77
Phenol + metal
Salt + hydrogen
78
Phenol + BR
tribromo phenol which decolourises br water
79
Electron donating phenol
OH and NH2 add electron density to the benzene ring which makes it easier to react, increases densities at 2,4 and 6
80
Electron withdrawing phenol
NO2 dont have p orbitals to add to the ring so removes electron density from 2,4 and 6 and directs to 5 and 3

Alevel chemistry year2 (4 decks)

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