Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Alevel chemistry year2 > Chemistry mock weak points > Flashcards

Chemistry mock weak points Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What ions are most likely to be aqueous

A

soluable compounds like NaCl, KNO3 and strong acids/bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What ions are likely to not be aqeuous

A

insoluable ionic compounds eq CaCo3 and covalent compounds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is an acid

A

Hydrogen donator/ protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a base

A

Contains hydroxide ions and reacts neutralises Acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is an alkali

A

a base dissolved in a solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is first ionisation energy

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is a permanent DP interaction

A

The weak interaction between two polar molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Allotropes meaning

A

different forms of the same element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

graphite

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Diamond

A

4 carbon bonds tetrahedral shape with a very high boiling point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Silicon

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Metallic bonding

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Reactivity down the group

A

As the energy require to remove an electron decreases down the group reactivty increases down the group

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Group 2 Metal + Water

A

Metal hydroxide + hydrogen
metal hydroxide can dissolve in water to produce hydroxide ions which make strong alkaline solutions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Group 2 metals + Oxygen

A

Metal oxides

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Group 2 metals + acids

A

Salt + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Uses of group 2 metals

A

used in agriculture to neutralise acid soils
can also be used as antacids for acids in the stomach

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is the trend in reactivity down the group Halogens

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Displacement of halogens

A

More reactive halogens when displace a less reactive halogen from its solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

How to distinctly see halogens

A

Add mixture to organic solvent like hexane and shake a solvent layer containing the halogen will form on top

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What colours do the halogens show

A

violet pink - iodine
orange red- bromine
yellow/green- chlorine

34
Q

test for halides

A

Add Dilute acids eg HNO3 to test for other ions and then add silver nitrate
Chlorine white
bromine cream
iodine yellow

35
Q

Halide solubility in NH3

A

Cl- dissolves in dilute
Br- dissolves in conc
I - doesn’t dissolve at all

36
Q

Making bleach

A

2NaOH + Cl2 -> NAClO + NaCl + H20

37
Q

Formation for Chlorate(I) ions

A

Cl2 + H20 reverisble HCl + HClO
HClO + H2O reversible CLO- + H3O
CLO is chlorate ion

38
Q

Test for Carbonate

A

Add a dilute ass if it bubbles it is present

39
Q

Test for sulfates

A

Add Ba+ ions eg Barium nitrate will form a white ppt

40
Q

Test for amonia

A

Heat mixture under damp red litmus paper should turn blue

41
Q

Standard enthalpy change of reaction

A

Enthalpy change when a reaction takes place in molar quantites of the equation in standard states under standard condtions

42
Q

Standard enthalpy change of formation

A

enthalpy change 1 mole of a compound is formed from its elements under standard conditions in its standard states

43
Q

enthalpy change of combustion

A

enthalpy change when 1 mole of a substance in burnt completely in oxygen in its standard states under standard conditions

44
Q

standard enthalpy of neutralisation

A

Enthalpy change when acids and alkali react together to make 1 mole of water in standard states under standard conditions

45
Q

What is hess’ law

A

The total change of a reaction is the same no matter the route taken

46
Q

when calculating enthalpies

A

follow the arrow correct way and rearrange using the unkown value as X and making the 2 values equal to each other

47
Q

What kind of reactions do alkenes undergo

A

electrophillic addition

48
Q

How do alkenes produce alkanes

A

hydrogen with a nickel catalyst at 150 degrees

49
Q

How to produce dihaloalkanes from alkenes

A

room temp and pressure no catalyst

50
Q

test for unsaturation in alkenes

A

add bromine water should go from brown to colourless

51
Q

how to make alcohol from alkene

A

Steam phosphoric catalyst 300degrees at 60/70 atm

52
Q

subsitution alcohol their OH group with a halide

A

Conc H2SO4 at room temp

53
Q

elimination of alcohol where a H and OH are removed to make an alkene

A

acid catalyst 170 degrees

54
Q

Oxidation of primary alcohol to aldehyde

A

gently heat alcohol with potassium dichromate(VI) and sulfuric acid and distil oxidising agent also used
reflux with oxidising agent

55
Q

Oxidation of secondary alcohol to make ketone

A

reflux the alcohol with acidified dichromate(VI) to make a ketone

56
Q

How do haloalkanes react

A

nucleophilic substitution

57
Q

Hydrolysis of haloalkanes

A

done with warm aqeous alkali or water

58
Q

SHC equation

A

Q= mcΔT

59
Q

Percentage uncertainty

A

uncertainty * number of times measure/ measure value *100

60
Q

Pv = nrt units

A

P= Pa
V= M3 dm3/100
N= moles
R= 8.314
T= temperature(K degress +273)a

61
Q

what are standard conditions

A

298K 100Kpa

62
Q

What is average bond enthalpy

A

average enthalpy change when 1 mole of covalent bonds are broken in gaseous conditions

63
Q

creation of ozone

A

O2-> 2o. in uv light
O2+O -> O3

64
Q

chlorine radical fomation and attack ozone

A

CF2Cl2 -> CF2Cl2 + Cl.
Cl. + o3-> ClO + O2
ClO+O -> Cl. + o2

65
Q

Other atoms attack ozone

A

R. + O3 -> RO. + O2
RO. + O. -> R. + 02

66
Q

Which group takes priory in benzene ring

A

phenyl groups

67
Q

What kind of reactions does benzene undergo

A

electrophillic substitution nucleophiles attracted to high electron density

68
Q

Why is benzene stable and how does it react

A

Very stable ring so takes a very strong nucleophile to break the ring

69
Q

What is the carrier for alkylation and acylation of phenols and regeneration

A

AlCl3
Alcl3 + H+ -> AlCl4

70
Q

reaction bebtween Ch3Cl + AlCl3

A

Ch3Cl + AlCl3 -> AlCl4 + Ch3+

71
Q

What is the halogen carrier for nitration of benzene

A

Concentrated Sulfuric acid

72
Q

Reaction for nitration explain

A

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
Q

Aromatic, aliphatic and alicylic

A

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
Q

What are phenols

A

Benzene with an OH group which adds to the electron density so it makes it more reactive
weak acid partially dissociates in solution

75
Q

What is the test for phenols

A

FeCl3 positive test is purple colour

76
Q

Phenol + Base

A

Salt + water

77
Q

Phenol + metal

A

Salt + hydrogen

78
Q

Phenol + BR

A

tribromo phenol which decolourises br water

79
Q

Electron donating phenol

A

OH and NH2 add electron density to the benzene ring which makes it easier to react, increases densities at 2,4 and 6

80
Q

Electron withdrawing phenol

A

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 (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions