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Chemistry A level > AS preperation final notes > Flashcards

AS preperation final notes Flashcards

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1
Q

When asked for definition involving mass?

A

Weighted mean mass of…

In comparison to 1/12th of the mass of an atom of C 12

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2
Q

First IE=

A

Energy required to remove
1 electron from each atom
In 1 mole of gaseous atoms
To form 1 mole of +1 ions

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3
Q

Orbital=

A

Region of space which can hold up to 2 electrons with opposite spin

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4
Q

Order of subshells

A

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6

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5
Q

Acid=

A

Releases H+ ions in solution

Proton donor

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6
Q

Base=

A

Compound which neutralises an acid, to form a salt

Proton acceptor

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7
Q

Alkali=

A

A soluble base, which releases OH- ions in solution

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8
Q

Silver ion

A

AG+

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9
Q

Ammonium ion

A

NH4+

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10
Q

Zinc ion:

A

Zn 2+

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11
Q

Carbonate ion

A

CO3 2-

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12
Q

Sulfate ion

A

SO4 2-

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13
Q

Nitrate ion

A

NO3 -

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14
Q

Phosphate ion

A

PO4 3-

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15
Q

Silver chloride =

A

White precipitate

Soluble in dilute and conc ammonia

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16
Q

Silver Bromide =

A

Cream precipitate

Soluble in conc ammonia, not dilute

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17
Q

Silver Iodide =

A

Yellow precipitate

Not soluble in ammonia

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18
Q

Writing an ionic equation:

A

Balanced equation with states
Split all aqueos solutions into ions
Cancel out anything which is aqueous on both sides
Rewrite

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19
Q

Sulphate ions test

A

Add Barium chloride

If present white precipitate forms

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20
Q

Carbonate ions test:

A

Add dilute Nitric acid, and bubble gas through limewater

If present goes cloudy

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21
Q

Ammonium ions test

A

Heat

Damp litmus paper goes blue

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22
Q

Ionic bonding=

A

Electrostatic attraction between positive and negative ions

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23
Q

Covalent bond=

A

Strong electrostatic attraction between
Shared pair of electrons
And nuclei of bonded atoms

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24
Q

Average bond enthalpy=

A

Average enthalpy change that occurs when:
Breaking by homolytic fission of 1 mole of a given type of bond
In molecules of a gaseous species

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25
Q

2 BP around central atom:

A

Linear

180

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26
Q

3BP around central atom:

A

Trigonal planar

120

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27
Q

4 BP around central atom

A

Tetrahedral
109.5
2 normal bonds and 2 different types of wedges

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28
Q

3 BP and 1 LP around central atom:

A

Pyramidal:
107
1 normal bond, 2 different types of wedges

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29
Q

2 BP and 2 LP around central atom

A

V shaped
104.5
2 normal bonds

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30
Q

6 BP around central atom:

A

Octahedral
90
2 normal, 2 of one type of wedge, 2 of other type of wedge

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31
Q

Electronegativity=

A

Ability of an atom to attract the bonding electrons in a covalent bond

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32
Q

Number of particles=

A

6.02x10^23 x moles

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33
Q

Formula involving mass molar mass and moles

A

Moles = mass / molar mass

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34
Q

Finding ratio in water of crystallisation

A

Find moles of solid
Find moles of water
Find ratio

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35
Q

Percentage error=

A

(Total uncertainty/ value measured) x 100

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36
Q

Formula for moles with conc and volume

A

Moles = concentration x volume

37
Q

How to find volume of gas at rtp

A

Volume = 24dm^3 x volume

38
Q

Ideal gas equation:

A

Pressure (Pa) x Volume (M^3) = moles x 8.314 x temp (kelvin)

39
Q

Atmostpheres to pascals =

A

multiply by 100,000

40
Q

Chlorine features:

A

Gas, green

41
Q

Bromine features:

A

Liquid, brown

42
Q

Halogens colour in water:

A 
Cl = colourless/pale green
Br = orange
I= Orange
43
Q

Halogens colour in hexane:

A 
Cl = Green
Br = Orange
I = purple
44
Q

Disproportionation reaction =

A

Oxidation and reduction of the same element

45
Q

Homologous series =

A

A series of organic compounds having the same functional group
But each successive member differing by CH2

46
Q

Functional group=

A

A group of atoms responsible for characteristic reactions of a compound

47
Q

3 steps in radical substitution?

A

Initiation:
Br2 = 2Br@
Homolytic splitting via UV light

Propagation:
Br@ + CH4 = HBr + CH3@
CH3@ + Br2= CH3Br + Br@

Termination:
CH3@ + Br@ = CH3Br
Br@ + Br@ = Br2
CH3@ + CH3@ = CH3CH3

48
Q

Describe Carbon single bond

A

End on overlap of atomic orbitals, producing a sigma bond

49
Q

Describe a Carbon double bond

A

Second bond produced by sideways overlap of P orbitals to form a pi bond
Electrons above and bellow plane of atom

50
Q

Stereoisomer=

A

molecules that have same structural formulae but different arrangements of atoms in space

51
Q

When can E/Z isomerism occur?

A

Restricted rotation around double bond

Each C of double bonds has different groups attached

52
Q

How to name E/Z isomerism

A

Functional groups on opposite sides=E
On same side= Z
Put these in front of name
Functional group= one with highest mass, includes everything bonded directly to nearest atom

53
Q

How to name cis/trans bonding?

A

When 1 of the groups attached to each side of the double bond is the name
Same side= cis
Different sides= trans

54
Q

Ethene + Hydrogen reaction

A

= Ethane

Requires 150 degrees and Ni catalyst

55
Q

Ethene + Bromine=

A

Di-Bromoethane

56
Q

Ethene + Hydrogen Bromide=

A

Bromoethane

57
Q

Ethene + H2O=

A

Ethanol
Water is steam
Phosphoric acid catalyst

58
Q

Electrophile=

A

An atom (or group of atoms), attracted to an electron rich centre, where it accepts electrons to form a new covalent bond

59
Q

Drawing electrophilic addition

A

Draw Alkene with Hydrogen bromide bellow, with hydrogen being closer
Hydrogen is delta positive, bromide is delta negative
Draw curly arrow from double bond to hydrogen
Draw curly arrow from covalent bond in Hydrogen bromide, to the Bromide

Draw alkane, but one carbon is missing a hydrogen and C has a positive charge
Draw Bromide ion with lone pair, and a negative charge
Draw curly arrow from lone pair to positive Carbon

Draw molecule

60
Q

Markownikoffs rule

A

Most likely product of electrophilic substitution is where Hydrogen bonds to C which is attached to the least amount of Carbons

61
Q

Primary alcohol=

A

Carbon OH is attached to bonded to 1 Carbon

62
Q

Secondary alcohol=

A

Carbon OH is attached to bonded to 2 Carbons

63
Q

Tertiary alcohol=

A

Carbon OH is attached to bonded to 3 Carbons

64
Q

Reflux=

A

Continues boiling and condensing of a mixture, to prevent loss of volatile components

65
Q

Nucleophile=

A

An electron pair donor

66
Q

How to draw nucleophilic substiution

A

Draw Halkoalkane, with C being delta + and Halogen being delta -
Draw an OH group with a lone pair and a negative charge
Draw curly arrow from lone pair to delta positive C
Draw curly arrow from Bond between Halogen and C to the halogen
Halogen replaced by OH producing a halide ion

67
Q

Measuring reactivity of haloalkanes

A

Reagant= silver Nitrate solution
Conditions= Hot water bath and Ethanol as co solvent
Observe time for silver halide precipitate to form
Ionic equations for both steps
Trend iodoethane fastest, chloroethane slowest
Factor strength of C-Halogen bond
Explain why C-Cl is strongest

68
Q

Dehydration of alcohols=

A

Heat under reflux
Catalyst of conc sulphuric or phosphoric acid used
Double bond formed, water produced

69
Q

Colour change if an oxidation reaction successful?

A

Red to green

70
Q

How to produce an aldehyde?

A

Add oxidising agent to primary alcohol

Gentle heating with distillation

71
Q

What’s an aldehyde?

A

C double bonded to O, and bonded to a H

Ending = al

72
Q

How to produce a carboxylic acid

A

Make aldehyde, add more oxidising agent and heat under reflux

73
Q

Carboxylic acid=

A

C double bonded to an O
And C bonded to an OH
Ends in “oic acid”

74
Q

How to produce a Ketone?

A

Add oxidising agent to a secondary alcohol

Heat under reflux

75
Q

Ketone=

A

Carbon double bonded to O

76
Q

Can tertiary alcohols be oxidised?

A

No, stays red

77
Q

Esterfication=

A

Carboxylic acid + alcohol = Ester + water

Heat under reflux and sulphuric acid catalyst

78
Q

Naming an ester:

A

First words ends in “yl”
Second word ends in “oate”
Longest alcohol C chain determines what’s in front of yl
Longest C chain in carboxylic acid goes in front of oate

79
Q

How to find heat change, and enthalpy change?

A

Heat change (joules) = mass of solution x change in temp x 4.18

To find enthalpy change divide heat change by 1000
and then divide by the amount of fuel used
Units= kJ mol^-1

80
Q

Standard enthalpy change of combustion:

A

1 mole of substance completely reacts with oxygen

Under standard conditions-

81
Q

Standard enthalpy change of formation:

A

1 mole of compound is formed from it’s elements

Under standard conditions-

82
Q

Standard enthalpy change of neutralisation:

A

:

Reaction of acid and alkali to produce 1 mole of H2O, under standard conditions-

83
Q

Lattice enthalpy

A

Formation of 1 mole of an ionic compound, from it’s gaseous ions
Standard conditions

84
Q

Atominsation enthalpy:

A

Formation of 1 mole of gaseous atoms from elements in standard states
Standard conditions

85
Q

Electron affinity

A

One electron added to each atom of an element to form 1 mole of gaseous 1- atoms
Uses up an electron

86
Q

Born haber cycle:

A

Start with elements in natural states
Go upwards atomise metal
atomise gas
all ionisation energies
all electron affinitys (worst one goes down)
Reach gaseous ions
Gaseous ions to ionic compound= lattice enthalpy
Elements in natural state to ionic compound = formation

87
Q

Entropy

A

Measure of organisation

Entropy change (joules) = (Add up all S values of products) - (Add up all values of S values of reactants)

88
Q

Gibbs free energy (negative it can happen)

A

Enthalpy change - (kelvin x entropy change)

CONVERT DEGREES TO KELVIN BY ADDING 273
CONVERT ENTROPY TO KJ BY DIVING BY 1000

89
Q

Atom economy formula?

A

Atom economy = mass of atoms of desired products/ mass of atoms in reactants

Chemistry A level (16 decks)

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