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Interim Chem Assessment

Total questions: 116

Worksheet time: 2hrs 56mins

Name
Class
Date
1.

What sub-atomic particle is labelled A?

a)

Neutron

b)

Electron

c)

Ion

d)

Atom

2.

What sub-atomic particle is labelled B?

a)

Neutron

b)

Electron

c)

Ion

d)

Atom

3.

Which atom has 4 electrons?

a)

Atom A

b)

Atom B

c)

Atom C

d)

Atom D

4.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

5.

An oxygen atom has reacted to get a full outer shell. What is the correct charge for the ion?

a)

+

b)

-

c)

2+

d)

2-

6.

Count the electrons in this atom's outer shell. What will happen when this atom reacts?

a)

It will gain 2 electrons and become a 2- ion.

b)

It will gain 3 electrons and become a 3- ion.

c)

It will lose 5 electrons and become a 5- ion.

d)

It will gain 3 electrons and become a 3+ ion.

7.

This ion was formed when a magnesium atom...

a)

lost two outer electrons

b)

gained two outer electrons

c)

lost one outer electron

d)

gained 6 electrons

8.

This is a lithium atom. To form a lithium ion it must...

a)

Gain one electron

b)

Lose one electron

c)

Gain two electrons

d)

Lose two electrons

9.

Sodium is a metal. It loses one electron when it reacts. The correct chemical symbol for a sodium ion would be..?

a)

Na+

b)

Na-

c)

Na2+

d)

Na+

10.

Predict the formula of the ionic compound that forms from Potassium and Chlorine

a)

KCl2KCl_2  

b)

KClKCl  

c)

P2ClP_2Cl  

d)

PClPCl  

11.
What will be the chemical formula for 
K+1 and Cl-1
a)
KCl
b)
K2Cl
c)
KCl2
d)
KCl3
12.

What is the correct formula for when K and F bond?

a)

KF

b)

K2F

c)

KF2

d)

K2F3

13.

How does an ionic bond form?

a)

The metal transfers electrons to the non metal

b)

The two metals share electrons

c)

The non metal transfers electrons to the metal

d)

The two non metals share electrons

14.

Which properties are all characteristics of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

15.

Select all the true statements:

a)

Each outer shell electron in Cl is represented by a cross.

b)

In Na, the total charge is -2.

c)

Na+ and Cl- are held together by electrostatic attraction.

d)

Na+ has a full outer shell of electrons.

16.

This is an image of the giant ionic lattice representing Sodium Chloride, what is represented by the +?

a)

Cl ion

b)

Cl atom

c)

Na atom

d)

Na ion

17.

This is an example of particles in a _________.

a)

solid

b)

liquid

c)

gas

18.

This is an example of particles in a ______.

a)

solid

b)

liquid

c)

gas

19.

Label the diagram.

a)Melting
b)vaporizing
c)condensing
d)solidifying
1
2
3
4
1)
2)
3)
4)
20.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
21.
Who stated that all atoms of the same element are excacty alike?
a)
Democritus
b)
Dalton
c)
Thomson
d)
Borh
22.

Which scientist is given credit for discovering the electron?

a)

Bohr

b)

Dalton

c)

Thomson

d)

Rutherford

23.

Who discovered that electrons travel in specific orbits around the nucleus?

a)

Bohr

b)

Schrodinger

c)

Democritus

d)

Rutherford

24.

Whose gold foil experiment led to his conclusion that the nucleus of an atom contained protons?

a)

Rutherford

b)

Bohr

c)

Thomson

d)

Dalton

25.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

26.

Which model was created after the discovery of the nucleus?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

27.

Which one of these is Dalton's Model?

a)
b)
c)
d)
28.

What is a particle with one negative charge called?

a)

electron

b)

proton

c)

quark

d)

neutron

29.

Who discovered electrons?

a)

Rutherford

b)

Bohr

c)

J.J. Thompson

d)

Democritus

30.

Which model was created after the discovery of electrons?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical Model

d)

Plum Pudding

31.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Neils Bohr, Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Neils Bohr, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford, and Neils Bohr

d)

John Dalton, Neils Bohr, JJ Thomson, Democritus, & Ernest Rutherford

32.
Ernest Rutherford discovered that the atom was mostly _________________ and has a _______________ charged nucleus.
a)
empty space, positively
b)
empty space, negatively
c)
full of protons, positively
d)
full of neutrons, negatively
33.

Within Dalton's Atomic Theory, he had proposed...

a)

Atoms were the smallest particles that existed and could be divisible

b)

Atoms were the smallest particles that existed and were round

c)

Atoms were the smallest particles that existed and could not be divisible

34.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
35.

Worked with Rutherford to discover particles with no charge -- called neutrons.

a)

James Chadwick

b)

Niels Bohr

c)

Democritus

d)

Thomson

36.

What is this process?

a)

melting

b)

vaporization

c)

condensation

d)

evaporation

37.

What does exothermic mean?

a)

Energy is transferred from reaction to surroundings, in the form of heat

b)

Energy is transferred from surroundings to reaction, in the form of heat

c)

Energy is transferred from reaction to surroundings, in the form of kinetic energy

d)

Energy is transferred from surroundings to reaction, in the form of kinetic energy

38.

What is the best equipment for measuring temperature changes?

a)

Measuring cylinder

b)

pH probe

c)

Thermometer

d)

Polystyrene cup

39.

What is the best equipment for measuring temperature changes?

a)

Measuring cylinder

b)

pH probe

c)

Thermometer

d)

Polystyrene cup

40.

What must you do before you add the acid and alkali together?

a)

Estimate the final volume of the solution

b)

Measure the starting temperature of the acid

c)

Put a lid on it

d)

Add water to the acid

41.
Find the mean:
28, 18, 19, 18, 17
a)
20
b)
18
c)
11
d)
19
42.

Find the mean of the numbers below:


1, 8, 7, 5, 6, 4, 7, 6

a)

40

b)

5.5

c)

44

d)

5

e)

6.5

43.
Find the mean:
28, 18, 19, 18, 17
a)
20
b)
18
c)
11
d)
19
44.

This atom, neon is a member of the group called the noble gases. Why are the noble gases unreactive?

a)

Because they already have full outer shells

b)

Because they have an even number of electrons

c)

Because they only need to gain one electron

45.

Covalent bonds are usually formed between...

a)

A metal and a non-metal

b)

Two non-metals

c)

Two metals

46.

What is a polymer?

a)

Long chain of ionic bonds

b)

Long chain Hydrocarbon

c)

Long chain of covalent bonds

47.

What is a monomer?

a)

The small repeating unit of a polymer

b)

A disease

c)

A molecule consisting of 1 type of atom.

d)

A covalent lattice.

48.

As polymers increase in lenght, they also increase in _______ (2 answers)

a)

melting points

b)

thermostability

c)

intermolecular forces

d)

difference in monomers

49.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
50.

The diagram shows an electrolysis experiment.

During the electrolysis, sodium was formed at electrode P and chlorine at electrode Q.

Which choice correctly identifies P, Q and X?

a)

P = anode; Q = cathode; X = concentrated solution of sodium chloride in water

b)

P = anode; Q = cathode; X = molten sodium chloride

c)

P = cathode; Q = anode; X = concentrated solution of sodium chloride in water

d)

P = cathode; Q = anode; X = molten sodium chloride

51.

Copper and hydrogen can each be formed by electrolysis.

At which electrodes are these elements formed?

a)

A

b)

B

c)

C

d)

D

52.

The electrolyte is Sodium Chloride solution: NaCl (aq)

The ions inside are: Na+ Cl- and H+ OH-

What will be made at the anode?

a)

H2 - hydrogen gas

b)

Na - sodium metal

c)

O2 - oxygen gas

d)

Cl2 - chlorine gas

53.

The electrolyte is Sodium Chloride solution: NaCl (aq)

The ions inside are: Na+ Cl- and H+ OH-

What will be made at the anode?

a)

H2 - hydrogen gas

b)

Na - sodium metal

c)

O2 - oxygen gas

d)

Cl2 - chlorine gas

54.

The electrolyte is Potassium Chloride solution: KCl (aq)

The ions inside are: K+ Cl- and H+ OH-

What will be made at the cathode?

a)

H2 - hydrogen gas

b)

K - potassium metal

c)

O2 - oxygen gas

d)

Cl2 - chlorine gas

55.

The electrolyte is Potassium Sulfate solution: K2SO4 (aq)

The ions inside are: K+ SO4- and H+ OH-

What will be made at the anode?

a)

O2 - oxygen gas

b)

K - potassium metal

c)

S - Sulphur

d)

Cl2 - chlorine gas

56.

Sodium Chloride solution contains:

Na+ Cl- and H+ OH-

Which ion will be changed at the cathode?

a)

OH-

b)

Cl -

c)

Na+

d)

H+

57.

Sodium Chloride solution contains:

Na+ Cl- and H+ OH-

Which ion will be changed at the anode?

a)

OH-

b)

Cl -

c)

Na+

d)

H+

58.

Potassium Chloride solution contains:

K+ Cl- and H+ OH-

Which ion will be changed at the anode?

a)

OH-

b)

Cl -

c)

K+

d)

H+

59.

Silver Bromide solution contains:

Ag+ Br - and H+ OH-

Which ion will be changed at the Cathode?

a)

OH-

b)

Br -

c)

Ag+

d)

H+

60.

Silver Bromide solution contains:

Ag+ Br - and H+ OH-

Which ion will be changed at the anode?

a)

OH-

b)

Br -

c)

Ag+

d)

H+

61.

Copper iodide solution contains:

Cu2+ I - and H+ OH-

Which ion will be changed at the anode?

a)

OH-

b)

I -

c)

Cu2+

d)

H+

62.

Copper Fluoride solution contains:

Cu2+ F - and H+ OH-

Which ion will be changed at the Cathode?

a)

OH-

b)

F -

c)

Cu2+

d)

H+

63.

Silver Chloride solution contains:

Ag+ Cl - and H+ OH-

Which two ions will be changed at the electrodes?

a)

OH-

b)

Cl -

c)

Ag+

d)

H+

64.

The electrolyte is Potassium Chloride solution: KCl (aq)

The ions inside are: K+ Cl- and H+ OH-

What will be made at the anode?

a)

H2 - hydrogen gas

b)

K - potassium metal

c)

O2 - oxygen gas

d)

Cl2 - chlorine gas

65.

In aluminum extraction the electrodes are made of

a)

carbon (graphite)

b)

aluminum and oxygen

c)

platinum

d)

steel

66.

The anode has to be replaced frequently because

a)

The oxygen reacts with the carbon anode to form carbon dioxide

b)

Aluminum reacts with the carbon to form aluminum carbide

c)

The anode gets impurities that impact the extraction

d)

The anode is too hot and it will reduce their electrical conductivity

67.

What do you add to aluminium ore to reduce its melting temperature?

a)

Dendrite

b)

Malachite

c)

Bauxite

d)

Cryolite

68.

Why is Aluminium expensive? (2 answers)

a)

The process takes a lot of electricity

b)

Aluminium is rare

c)

The electrodes need to be replaced often

d)

The mines are deep

69.

During electrolysis, what will the Aluminium Oxide split into?

a)

Al3+ and O2-

b)

Al and O

c)

Al+ and O-

d)

Aluminium and Oxide

70.

Which ion will be attracted to the positive electrode (anode)?

a)

Al3+

b)

O2-

c)

H+

d)

All of them

71.

When the Oxygen ion arrives at the graphite (Carbon) anode, what gas will it form?

a)

CO2

b)

H2O

c)

H2

d)

O2

72.

When the Oxygen ion arrives at the graphite (Carbon) anode, what gas will it form?

a)

CO2

b)

H2O

c)

H2

d)

O2

73.
Which of the following is a noble gas that is heavier than air?
a)
Hydrogen
b)
Helium
c)
Argon
d)
Sodium
74.
Which of these is not a noble gas?
a)
Helium
b)
Argon
c)
Nitrogen
d)
Krypton
75.
True or false: Noble gases react with water
a)
True
b)
False
76.
Which of the following describes the law of conservation of mass?
a)
In a reaction, atoms are created or destroyed.
b)
In a reaction, atoms are not lost or made.
c)
In a reaction, the mass of the product may be more or less than the reactants.
d)
In a reaction, mass never stays the same.
77.

P4O10 had a mass of ​12g , and H3PO4 has a mass of 90g, accroding t the law of conservation of mass what is H2O mass? ​ ​ (a)  

Choose from the below words
78g
102
102g
90g
12g
78.

127 g Cu + 32 g O2 = (a)   g CuO

79.

11.5 g Na + (a)   ._ g Cl2 = 29.9 g NaCl

80.

11.5 g Na + (a)   ._ g Cl2 = 29.9 g NaCl

81.

If it looks like mass was lost, then a ​ (a)   must have been produced in the chemical reaction.

Choose from the below words
gas
solid
liquid
82.

If it seems like mass was gained in a chemical reaction, a ​ (a)   must have been a reactant.

Choose from the below words
gas
solid
liquid
83.

When substances are mixed and it produces a ​ (a)   , this is evidence of a chemical reaction. ​ Often ​ (b)   occur when a gas is produced.

Choose from the below words
gas
bubbles
proton
electron
84.

(a)   is the gain of oxygen atoms.

85.

(a)   is the loss of oxygen atoms.

86.

Is this an oxidation or reduction reaction?

water → hydrogen + oxygen

a)

Oxidation

b)

Reduction

87.

Is this an oxidation or reduction reaction?

carbon + oxygen → carbon dioxide

a)

Oxidation

b)

Reduction

88.

Is it acid or alkali when the pH is 4 pH

a)

Acid

b)

Alkali

c)

Neutral

89.
A solution with a pH of 3.6 would be...
a)
Acid
b)
Base
c)
Neutral
d)
Acid and Base
90.

Acid + Alkali --> Salt + Water

a)

neutralization reaction

b)

synthesis

c)

decomposition

d)

single displacement

91.

Acids are source of

a)

hydrogen ions

b)

hydroxide ions

92.

The image shows a PH scale. Which option indicates strong acid?

a)

a

b)

b

c)

c

d)

d

93.

As an acid becomes stronger…

(Higher Tier Question)

a)

More H+ ions disassociate

b)

More OH- ions disassociate

c)

The acid doubles

d)

The H+ and OH- balance

94.

An example of a strong acid is…

(Higher Tier Question)

a)

hydrochloric acid

b)

ethanoic acid

c)

carbonic acid

d)

benzoic acid

95.

What colour would universal indicator be when mixed with a strong acid?

a)

Blue

b)

Red

c)

Green

d)

Purple

96.

Universal indicator, when mixed with a strong acid, turns (a)   in colour.

97.

When carbonates react with acids, which gas is produced?

a)

Hydrogen

b)

Carbon dioxide

c)

Oxygen

d)

Nitrogen

98.
A neutralisation reaction is a reaction between 
a)
Acid and a Base 
b)
Acid and water 
c)
Base and water 
d)
None of the above 
99.

Which of the following is a neutralization reaction?

a)

2Na + Cl2 → 2NaCl

b)

CH4 + 2O2 → CO2 + 2H2O

c)

HCl + KOH → KCl + H2O

d)

CaCO3 → CO2 + CaO

100.

Metal carbonates react with acid to form....

a)

Salt, carboxylic acid and water

b)

Salt, carbon dioxide and water

c)

Salt and carbonated water

d)

Salt and hydrogen

101.

Metal carbonates react with acid to form....

a)

Salt, carboxylic acid and water

b)

Salt, carbon dioxide and water

c)

Salt and carbonated water

d)

Salt and hydrogen

102.

Calcium carbonate + hydrochloric acid -->

a)

Calcium chloride + hydrogen

b)

Calcium choride + water

c)

Calcium chloride + carbon dioxide + water

d)

Calcium sulfate + carbon dioxide + water

103.

According to pH scale, indicator will turn red if a solution is...

a)

Acidic

b)

Alkali

c)

Neutral

d)

Precipitate

104.

which gas is formed when calcium carbonate reacts with hydrochloric acid?

a)

calcium chloride

b)

hydrogen

c)

oxygen

d)

carbon dioxide

105.

which in the following is the right equation for reaction between metal carbonates and acid?

a)

Metal carbonate + hydrochloric acid → metal chloride + water + hydrogen

b)

Metal carbonate + hydrochloric acid → metal chloride + carbon dioxide

c)

Metal carbonate + hydrochloric acid → metal chloride + water + carbon dioxide

106.

Put these steps in order to Investigate the volume of carbon dioxide produced when different masses of calcium carbonate was used.​ (a)   ​ ​ (b)   ​ (c)   ​ (d)   ​ (e)  

Choose from the below words
Support a gas syringe with a stand, boss and clamp
Using a measuring cylinder, add 50 cm3 of dilute h
Add 0.4 g of calcium carbonate to the flask. Immed
Every 10 seconds, record the volume of gas produce
Repeat with different masses of calcium carbonate
107.

Calculate the relative formula mass of

copper (ii) chloride, CuCl2


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

a)

90

b)

135

c)

137

d)

99.5

108.

Calculate the relative formula mass of

sulphuric acid H2SO4


[Relative atomic mass:

H = 1, S = 32, O = 16]

a)

96

b)

98

c)

100

d)

92

109.

Calculate the relative formula mass of

copper (ii) chloride, CuCl2


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

110.

Calculate the relative formula mass of

aluminium sulphate, Al2(SO4)3


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

111.
% of Ca in Ca(CN)2
a)
60.6% Ca
b)
43.5% Ca
c)
50.0% Ca
d)
75.5% Ca
112.
Find the percent composition of each element in N2S2 
a)
69.6% N, 30.4%S
b)
15.2% N, 84.8% S
c)
30.4% N, 69.6% S
d)
65.2% N, 34.8% S
113.
What is the mass percentage of carbon in carbon dioxide?
a)
27.3%
b)
42.9%
c)
57.1%
d)
72.7%
114.

50g of sodium hydroxide is dissolved in water to make up 200cm3 . What is the concentration in dm3.

a)

0.25 g/dm3

b)

2.5 g/dm3

c)

25 g/dm3

d)

250 g/dm3

115.

Give the equation for calculating concentration from the mass of substance and volume of solution.

a)

Concentration = mass x volume

b)

Concentration = mass ÷ volume

116.

Choose a correct unit for concentration.

a)

g

b)

gdm

c)

g/dm3

d)

mol

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