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NCEA L2 Chemistry Externals 2.4, 2.5 & 2.6 Revision

Total questions: 134

Worksheet time: 2hrs 46mins

Name
Class
Date
1.

Type of Reaction for Alkene → Alcohol

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reaction

2.

Type of Reaction for Alkene → Diol

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reaction

3.

Type of Reaction for Alkane → Haloalkane

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reaction

4.

Type of Reaction for Alcohol → Alkene

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reaction

5.

Type of Reaction for Haloalkane → Alkene

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

6.

Type of Reaction for Carboxylic Acid + Universal Indicator →

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

7.

Type of Reaction for Carboxylic Acid + Litmus →

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

8.

Type of Reaction for Carboxylic Acid + Metal Carbonate →

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

9.

Type of Reaction for Carboxylic Acid + Metal Hydrogen Carbonate →

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

10.

Type of Reaction for alkene + alkene + alkene ... →

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

11.

Type of Reaction for Alcohol → Alkene

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

12.

Type of Reaction for Alkene → Alkane

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

13.

Type of Reaction for Haloalkane → Amine

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

14.

Type of Reaction for Haloalkane → Alkene

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

15.

Type of Reaction for Haloalkane → Alcohol

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

16.

Type of Reaction for Alcohol → Haloalkane

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

17.

Type of Reaction for Alcohol → Carboxylic Acid

a)

Substitution

b)

Elimination

c)

Addition

d)

Oxidation

e)

Acid - Base Reactions

18.

Will rapidly decolourise Br2 water

a)

alkane

b)

alkene

c)

alcohol

d)

amine

19.

Will slowly decolourise Br2 water - needs uv and/or heat

a)

alkane

b)

alkene

c)

carboxylic acid

d)

amine

20.

Will turn GREEN Universal Indicator BLUE

a)

amine

b)

alcohol

c)

carboxylic acid

d)

haloalkane

21.

Will turn RED litmus BLUE

a)

amine

b)

alcohol

c)

carboxylic acid

d)

haloalkane

22.

Will turn BLUE litmus RED

a)

amine

b)

alcohol

c)

carboxylic acid

d)

haloalkane

23.

Would produced bubbles of colourless gas with NaHCO3

a)

amine

b)

alcohol

c)

carboxylic acid

d)

haloalkane

24.

Would turn MnO4- from purple to brown

a)

alkane

b)

alcohol

c)

amine

d)

alkene

25.

Would turn H+/MnO4- from purple to colourless (no heat needed)

a)

alkane

b)

alcohol

c)

amine

d)

alkene

26.

Would turn H+/Cr2O72- from orange to green (heat needed)

a)

alkane

b)

alcohol

c)

amine

d)

alkene

27.

2-chlorobutane is_______ in water

a)

soluble

b)

insoluble

28.

propanoic acid is_______ in water

a)

soluble

b)

insoluble

29.

butan-2-amine is_______ in water

a)

soluble

b)

insoluble

30.

heptane is_______ in water

a)

soluble

b)

insoluble

31.

hexanoic acid is_______ in water

a)

soluble

b)

insoluble

32.

Colour change when H+/MnO4- is warmed with a primary alcohol

a)

purple to brown

b)

purple to colourless

c)

orange to green

d)

orange to colourless

33.

Colour change when ethene is shaken with Br2 water

a)

purple to brown

b)

purple to colourless

c)

orange to green

d)

orange to colourless

34.

Type of reaction (unbalanced).

CH3CH2Cl → CH3CH2OH

a)

addition

b)

substitution

c)

elimination

d)

oxidation

35.

Type of reaction (unbalanced).

CH2=CH2 → CH3CH2OH

a)

addition

b)

substitution

c)

elimination

d)

oxidation

36.

Type of reaction (unbalanced).

CH3CH2Cl → CH2=CH2

a)

addition

b)

substitution

c)

elimination

d)

oxidation

37.

Type of reaction (unbalanced).

CH2=CH2 → CH2Br-CH2Br

a)

addition

b)

substitution

c)

elimination

d)

oxidation

38.

Type of reaction (unbalanced).

CH2=CH2 → CH2OH-CH2OH

a)

addition

b)

substitution

c)

elimination

d)

oxidation

39.

Type of reaction (unbalanced).

CH3CH2OH → CH2=CH2

a)

addition

b)

substitution

c)

elimination

d)

oxidation

40.

Type of reaction (unbalanced).

CH3CH2OH → CH3COOH

a)

addition

b)

substitution

c)

elimination

d)

oxidation

41.

Type of reaction.

CH3COOH + NaOH → CH3COO-Na+ + H2O

a)

acid-base

b)

substitution

c)

elimination

d)

oxidation

42.

Type of reaction.

CH3COOH + NaHCO3 →

CH3COO-Na+ + H2O + CO2

a)

acid-base

b)

substitution

c)

elimination

d)

oxidation

43.

What reagent is needed to change an alkene to an alcohol?

a)

KOH (aq)

b)

concentrated H2SO4

c)

H2O/ dilute H2SO4

d)

Cr2O72-/H+

44.

Which reagent is needed to change a haloalkane to an alcohol?

a)

KOH (aq)

b)

KOH(alc)

c)

H2O/ dilute H2SO4

d)

Cr2O72-/H+

45.

Which reagent is needed to change a haloalkane to an amine?

a)

KOH (aq)

b)

NH3(alc)

c)

H2O/ dilute H2SO4

d)

Cr2O72-/H+

46.

Which reagent is needed to change CH3CH2OH to CH3COOH

a)

KOH (aq)

b)

NH3(alc)

c)

H2O/ dilute H2SO4

d)

Cr2O72-/H+

47.

Which reagent is needed to change an alcohol to an alkene?

a)

KOH (alc)

b)

water/dilute H2SO4

c)

concentrated H2SO4

d)

Cr2O72-/H+

48.

Which reagent is needed to change CH3CH=CH2 to CH3CHClCH3

a)

Cl2 (aq)

b)

SOCl2

c)

PCl3

d)

HCl

49.

What is the product of the reaction: CH3CH2NH2 + HCl

a)

CH3CH2Cl + NH3

b)

CH3CH2NH2Cl

c)

CH3CH2NH3Cl

d)

CH3CH2NH2HCl

50.

alkene ------> alcohol - reaction type?

a)

addition

b)

substitution

c)

elimination

d)

oxidation

51.

haloalkane ------> alcohol - reaction type?

a)

addition

b)

substitution

c)

elimination

d)

oxidation

52.

alcohol ------> carboxylic acid - reaction type?

a)

addition

b)

substitution

c)

elimination

d)

oxidation

53.

Hardness is a property associated with

a)

metallic solids

b)

ionic solids

c)

covalent network solids

d)

all of these

54.

haloalkane ------> alkene - reaction type?

a)

addition

b)

substitution

c)

elimination

d)

oxidation

55.

A high melting point and boiling point indicates

a)

strong attraction between atoms or ions

b)

weak strong attraction between atoms or ions

c)

metallic bonding only

d)

covalent molecular solid

56.

The type of solid that is brittle is

a)

metallic

b)

ionic

c)

covalent network

d)

covalent molecular

57.

The type of solid that has a low melting and boiling point is

a)

metallic

b)

ionic

c)

covalent network

d)

covalent molecular

58.

The type of solid that conducts electricity as a solid and liquid is

a)

metallic

b)

ionic

c)

covalent network

d)

covalent molecular

59.

The type of solid that is malleable and ductile is

a)

metallic

b)

ionic

c)

covalent network

d)

covalent molecular

60.

The covalent network solid that conducts electricity due to delocalised electrons is

a)

diamond

b)

graphite

c)

silicon dioxide

d)

all of these

61.

To conduct electricity a solid needs "mobile charge carriers"; these are

a)

delocalised electrons

b)

bonded electrons

c)

delocalised electrons and ions in molten or aqueous ionic substances

d)

ions in molten or aqueous ionic substances

62.

non polar solids e.g iodine and wax, tend to dissolve in

a)

polar solvents e.g. water

b)

non polar solvents e.g. hexane

c)

both water and hexane

d)

nothing at all

63.

ionic solids e.g. NaCl, tend to dissolve in

a)

polar solvents e.g. water

b)

non polar solvents e.g. hexane

c)

both water and hexane

d)

nothing at all

64.

Correct order for DECREASING electronegativity

a)

F O N/Cl S/C P/H

b)

F O N/Cl P/H S/C

c)

P/H S/C N/Cl O F

d)

F O Cl/S N/C P/H

65.

electronegativity increases

a)

from left to right and going up the periodic table

b)

from left to right and going down the periodic table

c)

from right to left across the periodic table

d)

there is no pattern at all

66.

Sodium chloride: Type of solid, type of particles, type of bonding

a)

ionic, ions, ionic

b)

metal, atoms, metallic

c)

covalent molecular, molecule, weak intermolecular

d)

covalent network, atoms, covalent

67.

Silicon dioxide: Type of solid, type of particles, type of bonding

a)

ionic, ions, ionic

b)

metal, atoms, metallic

c)

covalent molecular, molecule, weak intermolecular

d)

covalent network, atoms, covalent

68.

Silver: Type of solid, type of particles, type of bonding

a)

ionic, ions, ionic

b)

metal, atoms, metallic

c)

covalent molecular, molecule, weak intermolecular

d)

covalent network, atoms, covalent

69.

Iodine: Type of solid, type of particles, type of bonding

a)

ionic, ions, ionic

b)

metal, atoms, metallic

c)

covalent molecular, molecule, weak intermolecular

d)

covalent network, atoms, covalent

70.

Bond type: attraction between loosely held valence electrons & positively charged nuclei of neighbouring atoms

a)

ionic

b)

covalent

c)

metallic

71.

Bond type: electrostatic attraction between oppositely charged ions

a)

ionic

b)

covalent

c)

metallic

72.

Bond type: one in which one or more pairs of electrons are shared by two atoms

a)

ionic

b)

covalent

c)

metallic

73.

Bond occurring between covalent molecules - READ CAREFULLY!

a)

weak intermolecular

b)

weak intramolecular

c)

strong intermolecular

d)

strong intramolecular

74.

Bond occurring between atoms in a covalent molecule - READ CAREFULLY!

a)

weak intermolecular

b)

weak intramolecular

c)

strong intermolecular

d)

strong intramolecular

75.

Two elements that are electron deficient in their covalent molecules

a)

B and Be

b)

B and Br

c)

Be and Br

d)

B and N

76.

Number of valence electrons of an element in group 16

a)

6

b)

16

c)

4

d)

no way to tell

77.

Three covalent network solids

a)

diamond, graphite, silicon dioxide

b)

diamond, graphite, sulfur dioxide

c)

sodium chloride, graphite, silicon dioxide

d)

silver, glucose, silicon dioxide

78.

The covalent network solid that conducts electricity

a)

diamond

b)

graphite,

c)

silicon dioxide

d)

all of these

79.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is conctant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
80.

Identify the incorrect statement about achieving equilibrium.

a)

achieved when product and reactant concentrations are equal

b)

achieved when forward and reverse reaction rates are same

c)

achieved when concentration of reactants is stable/constant

d)

achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

81.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
82.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
83.
It is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
a)
reversible reaction
b)
irreversible reaction
c)
decomposition reaction
d)
synthesis
84.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
85.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
86.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
87.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
88.
During equilibrium, the rates of the forward and the reverse reaction are ________
a)
the same 
b)
unequal
c)
unequal for exothermic reactions
d)
unequal for endothermic reactions
89.
If a reaction is reversible and has reached equilibrium, what can be said about the amounts of reactants and products?
a)
some reactant, some product
b)
no reactant, all product
c)
all reactant, no product
90.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
91.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
92.
What is the activation energy?
a)
the quantity of heat absorbed in a reaction
b)
the minimum energy needed to begin a reaction
c)
the energy given off after reactants collide.
d)
both the energy and frequeny of collisions in increased
the energy difference between reactants and products
93.

A base is a substance

a)

That releases OH- ions when dissolved in water

b)

That releases H+ ions when dissolved in water

c)

Does not release any ions when dissolved in water

d)

None of the above

94.

In a test of pH levels, a baking soda has a pH of 9 and bleach has a pH of 12. What is true about there relationship?

a)

Both of the solution are Bases

b)

Both of the solution are Acids

c)

The Baking soda is an acid and the Bleach is a base

d)

The baking soda is a base and the Bleach is an Acid.

95.

A pH of 3 is how many times more acidic than a pH of 5?

a)

2

b)

20

c)

10

d)

100

96.
If you have a substance with a pH of 7.1 it is a(n).....
a)
Acid
b)
base
97.

The picture below shows the relative concentrations of H+ and OH- in a solution. Is the solution an acid or a base?

a)

acid

b)

base

98.

An acid

a)

is a substance that releases H+ ions when dissolved in water

b)

is a substance that does not release any ions when dissolved in water

c)

is a substance that releases OH- when dissolved in water

d)

releases an equal amount of OH- and H+ ions when dissolved in water

99.

Water has a neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

100.
According to the pH range which substance is more acidic than lemon juice
a)
Hydrochloric acid
b)
cabbage
c)
milk
101.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
102.
The substance that dissolves a solute to form a solution; the most plentiful substance in the solution
a)
solute
b)
solvent
c)
product
d)
reactant
103.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
104.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
105.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
106.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
107.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
108.
All chemical bonds involve two atoms sharing electrons.
a)
True
b)
False
109.
Chemical bonds form when atoms
a)
combined nuclei
b)
give up neutrons
c)
gain protons
d)
share or transfer electrons
110.
If an atom loses two electrons what charge will it have?
a)
+ 2
b)
 - 2
c)
+1
d)
-1
111.
Bonds that form between two metals are called ______________ bonds.
a)
ionic 
b)
covalent
c)
metallic
d)
pervasive
112.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
113.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
114.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
115.
When electrons are shared unequally a/an ___________ bond is formed 
a)
ionic 
b)
hydrogen
c)
polar covalent 
116.
A bond that forms when electrons are transferred is called a/an
a)
ionic bond
b)
covalent bond
c)
hydrogen bond
117.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
118.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
119.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
120.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
121.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

122.
Which statement is true regarding endothermic reactions?
a)
a) Temperature change is positive and enthalpy change is positive
b)
b) Temperature change is positive and enthalpy change is negative
c)
c) Temperature change is negative and enthalpy change is positive
d)
d) Temperature change is negative and enthalpy change is negative
123.
Endothermic reactions feel
a)
warm
b)
cold
124.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
125.

A reaction that gives out energy to the surroundings causes the surroundings ....

a)

temperature to drop

b)

temperature to rise

c)

temperature to remain constant

d)

temperature to vary

126.
Temperature is a measure of average [blank] energy of individual atoms.
a)
heat
b)
potential
c)
mechanical
d)
kinetic
127.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
128.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
129.
True/False: The rate of a chemical reaction is unrelated to the spontaneity of the reaction.
a)
True
b)
False
130.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
131.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
132.
N2 +  3H2 −->  2NH3 
How many moles of ammonium are produced when 3 moles of nitrogen react with hydrogen?
a)
6 moles Ammonium
b)
1.5 moles ammonium
c)
9 moles ammonium
d)
9 moles hydrogen
133.
_?_  is the amount of energy (joules) required to raise the temperature of 1 mole of a substance by 1 K.  Units are J/mol-K.
a)
Thermal energy
b)
Molar heat capacity
c)
A calorie
d)
Specific heat
134.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic

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