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WJEC GCE AS LEVEL UNIT 2 CHEMISTRY

Total questions: 86

Worksheet time: 51mins

Name
Class
Date
1.

ACTIVATION ENERGY

a)

The minimum energy required to start a reaction by breaking bonds

b)

The maximum energy required to start a reaction by breaking bonds

c)

The minimum energy required to end a reaction by breaking bonds

d)

The maximum energy required to end a reaction by breaking bonds

2.

Standard enthalpy change

a)

the enthalpy change when reactants in their standard states are converted to products in their standard states under standard conditions

b)

The energy required to break one mole of the stated bond in a gaseous state under standard conditions

c)

The enthalpy change when one mole of a substance in its standard shape is burnt completely in excess oxygen under standard conditions

d)

The enthalpy change when one mole of a substance in its standard state is formed from its constituent elements

3.

Average bond enthalpy

a)

the enthalpy change when reactants in their standard states are converted to products in their standard states under standard conditions

b)

The energy required to break one mole of the stated bond in a gaseous state under standard conditions

c)

The enthalpy change when one mole of a substance in its standard shape is burnt completely in excess oxygen under standard conditions

d)

The enthalpy change when one mole of a substance in its standard state is formed from its constituent elements

4.

Standard enthalpy change of combustion

a)

the enthalpy change when reactants in their standard states are converted to products in their standard states under standard conditions

b)

The energy required to break one mole of the stated bond in a gaseous state under standard conditions

c)

The enthalpy change when one mole of a substance in its standard shape is burnt completely in excess oxygen under standard conditions

d)

The enthalpy change when one mole of a substance in its standard state is formed from its constituent elements

5.

Standard enthalpy change of formation

a)

the enthalpy change when reactants in their standard states are converted to products in their standard states under standard conditions

b)

The energy required to break one mole of the stated bond in a gaseous state under standard conditions

c)

The enthalpy change when one mole of a substance in its standard shape is burnt completely in excess oxygen under standard conditions

d)

The enthalpy change when one mole of a substance in its standard state is formed from its constituent elements

6.

In exothermic reactions, products more stable than reactants

a)

True

b)

False

7.

In exothermic reactions, products less stable than reactants

a)

True

b)

False

8.

In endothermic reactions, products less stable than reactants

a)

True

b)

False

9.

In endothermic reactions, products more stable than reactants

a)

True

b)

False

10.

Bond making…

a)

required energy

b)

Releases energy

11.

Bond breaking…

a)

required energy

b)

Releases energy

12.

Finding enthalpy change from bond enthalpies

a)

Products - reactants

b)

Reactants - products

13.

Heat (energy) change

a)

-mct

b)

-mct/n

14.

Molar enthalpy change

a)

-mct

b)

-mct/n

15.

Hess law

a)

the enthalpy change of a reaction is independent of the route taken

b)

the enthalpy change of a reaction is dependent of the route taken

c)

the enthalpy change of a reaction = the route taken

16.

Specefic heat capacity

a)

the energy required to raise 1g of a substance by 1k without a change of state.

b)

the energy required to raise 1kg of a substance by 1k without a change of state.

c)

the energy required to raise 1g of a substance by 1C without a change of state.

d)

the energy required to raise 1g of a substance by 1k with a change of state.

17.

Process of a reaction

a)

Fastest at start bc reactant has greatest concentration

b)

Rate of reaction slows down as concentration of reactant decreases

c)

Rate of reaction becomes zero as reactant is used up

d)

Slowest at start bc reactant was smallest concentration

18.

If concentration double and rate is unchanged

a)

K[A]^0

Zero order

No correlation

b)

K[A]^1

First order

c)

K[A]^2

Second order

19.

If concentration double and rate doubles

a)

K[A]^0

Zero order

No correlation

b)

K[A]^1

First order

c)

K[A]^2

Second order

20.

If concentration double and rate quadrouples

a)

K[A]^0

Zero order

No correlation

b)

K[A]^1

First order

c)

K[A]^2

Second order

21.

Rate of reaction

a)

Change in concentration of a reactant or product over time

b)

How long a given reaction takes to completion

c)

The difference in concentration

d)

how much product is made in a reaction

22.

Rate of reaction units

a)

moldm3s-1

b)

Moldm-3s1

c)

Mol-1dm3s

d)

Moldms

23.

Catalyst

a)

a substrate that increases the rate of a chemical reaction without being used up in the process

b)

a substrate that decreases the rate of a chemical reaction without being used up in the process

c)

a substrate that increases the rate of a chemical reaction being used up in the process

d)

a substrate that decreaases the rate of a chemical reaction being used up in the process

24.

Homogenous catalyst

a)

The catalyst is in the same phase as the reactants

b)

the catalyst is not in the phase as the reactants

c)

Work by absorbing reactants to break bonds

d)

Work by combining with reactants to form an intermediate which break down to form product

25.

heterogenous catalyst

a)

The catalyst is in the same phase as the reactants

b)

the catalyst is not in the phase as the reactants

c)

Work by absorbing reactants to break bonds

d)

Work by combining with reactants to form an intermediate which break down to form product

26.

Factors affecting rate of reaction

a)

light

b)

Particle size 1/x

c)

Catalysts

d)

Temperature

e)

Concentraton

27.

Cons of fossil fuels

a)

non renewable

b)

Combustion produces co2

c)

Acid rain

d)

carbon monoxide from incomplete combustion

e)

Hole in ozone layer

28.

Pros of fossile fuels

a)

Reliable (available at all times

b)

Have many different forms for different uses

c)

Land use

d)

Water + fertiliser needed

29.

Cons of biofuel

a)

land use

b)

resources needed (water + fertiliser)

c)

Co2 released in other parts - factory building and transport

d)

Unreliable

30.

Carbon neutral

a)

A chemical process does not lead to an overall increase in CO2 levels

b)

a chemical process releases no CO2

c)

A chemical process releases CO

d)

A chemical process is good for the environment

31.

Pros of biofuels

a)

renewable

b)

Carbon neutral

c)

Economic security

d)

free

32.

Biofuel

a)

fuels produced from organic matter

b)

Fuels formed from the organic matter of plants and microorganisms that lived millions of years ago

33.

fossil fuel

a)

fuels produced from organic matter

b)

Fuels formed from the organic matter of plants and microorganisms that lived millions of years ago

34.

Whats true about solar power?

a)

renewable

b)

Not sutable for the uk

c)

Release a large ammount of energy

d)

dangerous when accidents happen

35.

Whats true about nuclear power?

a)

renewable

b)

Not sutable for the uk

c)

Release a large ammount of energy

d)

dangerous when accidents happen

36.

Green principles

a)

prevent waste - increase atom economy

b)

Use catalysts - increase energy efficiency

c)

Use renewable raw materials

d)

use high temperatures

37.

Green principles

a)

use safer methods and chemicals

b)

Prevent pollution and accidents

c)

design for biodegradation

d)

Produce more oxygen

38.

Molecular ion

a)

The positive ion formed in a mass spectrometre

b)

the negetive ion formed in a mass spectrometre

c)

The neutral ion formed in a mass spectrometre

39.

Fragmentation

a)

The splitting of a molecule in a mass spectrometre into smaller parts

b)

The joining of molecules in a mass spectrometre into larger parts

c)

Different molecular ions

40.

Mass spec CH3

(a)  

41.

Mass spec COOH

(a)  

42.

What mass spec tells us

a)

mr

b)

abundance

c)

isotopes

d)

functional groups

43.

What does ir tell us

a)

Functional groups

b)

position of functional groups

c)

mr

d)

abundance

44.

What does ir tell us

a)

Functional groups

b)

position of functional groups

c)

mr

d)

abundance

45.

What does nmr tell us

a)

Number of different H/C envrionments

b)

types of environments

c)

ratio of number of protons in each environment

d)

how many atoms in a molecule

46.

Compounds are unreactive if…

a)

the bonds are strong, EAct very high

b)

Bonds within molecule not very polar

c)

bonds are weak, low EAct

d)

Bonds are very polar, providing electrostatic attraction for reacting species

47.

Compounds are reactive if…

a)

the bonds are strong, EAct very high

b)

Bonds within molecule not very polar

c)

bonds are weak, low EAct

d)

Bonds are very polar, providing electrostatic attraction for reacting species

48.

Highly branched molecules…

a)

lower bpt

Weaker intermolecular forces

b)

Molecules cant get close to eachother

c)

Larger number and strength of van der waals forces

d)

more energy required to break IMF

High BPT

49.

As molecule size increases…

a)

lower bpt

Weaker intermolecular forces

b)

Molecules cant get close to eachother

c)

Larger number and strength of van der waals forces

d)

more energy required to break IMF

High BPT

50.

Alkane c1 to c4

a)

Gas

b)

liquid

51.

Alkane c5 to c20

a)

Gas

b)

liquid

52.

Molecular formula

a)

CnHn

Shows atoms and how many of each type there are

b)

CH3CH2CH3

Shows the groups in sufficient detail so compound is unambiguous

c)

H H

| |

H - C - C - H

| |

H H

Shows all the bonds and atoms in the molecule

d)

/\/\/

Shows the carbon/ hydrogen backbone of the molecule with any functional group

53.

shortened formula

a)

CnHn

Shows atoms and how many of each type there are

b)

CH3CH2CH3

Shows the groups in sufficient detail so compound is unambiguous

c)

H H

| |

H - C - C - H

| |

H H

Shows all the bonds and atoms in the molecule

d)

/\/\/

Shows the carbon/ hydrogen backbone of the molecule with any functional group

54.

displayed formula

a)

CnHn

Shows atoms and how many of each type there are

b)

CH3CH2CH3

Shows the groups in sufficient detail so compound is unambiguous

c)

H H

| |

H - C - C - H

| |

H H

Shows all the bonds and atoms in the molecule

d)

/\/\/

Shows the carbon/ hydrogen backbone of the molecule with any functional group

55.

skeletal formula

a)

CnHn

Shows atoms and how many of each type there are

b)

CH3CH2CH3

Shows the groups in sufficient detail so compound is unambiguous

c)

H H

| |

H - C - C - H

| |

H H

Shows all the bonds and atoms in the molecule

d)

/\/\/

Shows the carbon/ hydrogen backbone of the molecule with any functional group

56.

Functional group isomerism

a)

aldehydes

-HC=O

b)

Ketones

-C=OC

c)

Carbon

C=C

d)

Hydroxyl

O-H

57.

Functional group isomerism

a)

Alcohols

-C-OH

b)

Ethers

-C-O-C

c)

Esters

-C-O-C

||

O

d)

Hydroxyl

O-H

58.

Functional group isomerism

a)

Alcohols

-C-OH

b)

Carboxylic acid

-C-O-H

||

O

c)

Esters

-C-O-C

||

O

d)

Hydroxyl

O-H

59.

CnH2nO

C=0

-one

a)

Ketone

b)

Aldehyde

c)

carboxylic acid

d)

Ester

60.

CnH2nO

C=0

|

H

-al

a)

Ketone

b)

Aldehyde

c)

carboxylic acid

d)

Ester

61.

CnH2nO2

C=0

|

OH

-oic acid

a)

Ketone

b)

Aldehyde

c)

carboxylic acid

d)

Ester

62.

Fermentation

a)

An enzyme catalysed reaction that converts sugars to ethanol

b)

Remove OH from one C and H from adjacent to form double bond

c)

Effervesence

- can be tested with lime water

63.

dehydration

a)

An enzyme catalysed reaction that converts sugars to ethanol

b)

Remove OH from one C and H from adjacent to form double bond

c)

Effervesence

- can be tested with lime water

64.

obversation if CO2 produced

a)

An enzyme catalysed reaction that converts sugars to ethanol

b)

Remove OH from one C and H from adjacent to form double bond

c)

Effervesence

- can be tested with lime water

65.

Straight chain alcohols

a)

Aliphatic

b)

Aromatic

66.

Carbon in alcohols linked to eachother in a ring

a)

Aliphatic

b)

Aromatic

67.

Primary alcohol

a)

OH joined to carbon joined to only one other

b)

OH joined to carbon joined to only two others

c)

OH joined to carbon joined to three others

68.

secondary alcohol

a)

OH joined to carbon joined to only one other

b)

OH joined to carbon joined to only two others

c)

OH joined to carbon joined to three others

69.

tertiary alcohol

a)

OH joined to carbon joined to only one other

b)

OH joined to carbon joined to only two others

c)

OH joined to carbon joined to three others

70.

Primary alcohol oxidation

a)

Forms an aldehyde + H2O.

Oxidised again to form carboxylic acid

b)

Forms ketone + H2O

c)

Does not undergo a reaction because theres no hydrogen on adjacent carbon that can be lost

71.

secondary alcohol oxidation

a)

Forms an aldehyde + H2O.

Oxidised again to form carboxylic acid

b)

Forms ketone + H2O

c)

Does not undergo a reaction because theres no hydrogen on adjacent carbon that can be lost

72.

tertiary alcohol oxidation

a)

Forms an aldehyde + H2O.

Oxidised again to form carboxylic acid

b)

Forms ketone + H2O

c)

Does not undergo a reaction because theres no hydrogen on adjacent carbon that can be lost

73.

Esterification of carboxylic acids

a)

Carboxylic acid + alcohol <=> ester + h2o

b)

CH4+Cl2->CH3Cl+HCl

c)

CH2O+O2<=>CO2+H2O

d)

C6H12OG->2C2H5OH+2CO2

74.

FERMENTATION

a)

Carboxylic acid + alcohol <=> ester + h2o

b)

CH4+Cl2->CH3Cl+HCl

c)

CH2O+O2<=>CO2+H2O

d)

C6H12OG->2C2H5OH+2CO2

75.

ESSENTIAL PROCESS OF BIOMASS AND FOSSIL FUEL

a)

Carboxylic acid + alcohol <=> ester + h2o

b)

CH4+Cl2->CH3Cl+HCl

c)

CH2O+O2<=>CO2+H2O

d)

C6H12OG->2C2H5OH+2CO2

76.

PHOTOCHLORINATION OF METHANE

a)

Carboxylic acid + alcohol <=> ester + h2o

b)

CH4+Cl2->CH3Cl+HCl

c)

CH2O+O2<=>CO2+H2O

d)

C6H12OG->2C2H5OH+2CO2

77.

Use of aciifies potassium chromate

a)

an oxidising agent

b)

changes colour from orange to green

c)

Test for primary and secondary alcohols

d)

Test for tertiary alcohols

78.

Electrophillic addition

a)

Pair of electrons in pi bond attract electrophile. Eg hbr joins ethene to for bromoethane

b)

A reaction in which reagents are combined to give one product

c)

A reaction in which one atom/group is replaced by another atom/grouo

79.

addition reacton

a)

Pair of electrons in pi bond attract electrophile. Eg hbr joins ethene to for bromoethane

b)

A reaction in which reagents are combined to give one product

c)

A reaction in which one atom/group is replaced by another atom/grouo

80.

substitution reacton

a)

Pair of electrons in pi bond attract electrophile. Eg hbr joins ethene to for bromoethane

b)

A reaction in which reagents are combined to give one product

c)

A reaction in which one atom/group is replaced by another atom/grouo

81.

Stereoisomer requirements

a)

C=C double bond

b)

Different groups on each C

c)

Halogen group

d)

At least 4 carbons

82.

Uses of electrophillic substitution

a)

hydrogenation - making unsaturated bonds saturated to make things like butter

b)

Test for alkenes

c)

Alcohol oxidation

d)

Esterification

83.

Carbocations

a)

Electrophiles

b)

Accept a pair of electrons

c)

Nucleophiles

d)

Have a lone pair

84.

Carbanions

a)

Electrophiles

b)

Accept a pair of electrons

c)

Nucleophiles

d)

Have a lone pair

85.

Z isomer

a)

Groups on same side of the carbon double bond

b)

Groups on oppisite sides of the double bond

86.

E isomer

a)

Groups on same side of the carbon double bond

b)

Groups on oppisite sides of the double bond

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