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Year 10 Chemistry Quiz

Total questions: 103

Worksheet time: 1hrs 10mins

Name
Class
Date
1.

In an exothermic reaction...

a)

energy is taken in and the surroundings get colder.

b)

energy is taken in and the surroundings get warmer.

c)

energy is given out and the surroundings get warmer.

d)

energy is given out and the surroundings get colder.

2.

To break a chemical bond...

a)

energy must be supplied.

b)

energy must be released.

3.

Calorimetry can be used to measure the energy given off when a substance burns.

a)

True

b)

False

4.

Which of these can be used to measure the energy change when a chemical reaction takes place?

a)

Change in colour.

b)

Change in mass.

c)

Change in temperature.

5.

In an exothermic reaction, the products are at...

a)

a lower energy than the reactants.

b)

a higher energy than the reactants.

6.

In an endothermic reaction, the energy released when bonds are formed is...

a)

less than the energy used in breaking old bonds.

b)

greater than the energy used in breaking old bonds.

7.

The same reaction is carried out with and without a catalyst. Which line on the graph shows the reaction with a catalyst?

a)

Line 1

b)

Line 2

8.

If a reaction mixture increases in temperature during a reaction...

a)

the reaction is endothermic.

b)

the reaction is exothermic.

c)

no new chemical bonds have formed.

9.

Energy is needed in a chemical reaction to...

a)

break bonds.

b)

form new bonds.

10.

In an endothermic reaction, the products are at...

a)

a lower energy than the reactants.

b)

a higher energy than the reactants.

11.

When a chemical bond forms...

a)

energy must be supplied.

b)

energy is released.

12.

What effect does adding a catalyst have on the overall energy change of a reaction?

a)

It increases it.

b)

It decreases it.

c)

It has no effect.

13.

In an exothermic reaction the energy required to break old bonds is...

a)

less than the energy released when new bonds form.

b)

greater than the energy released when new bonds form.

14.

Which of these is an endothermic reaction?

a)

Hand warmer

b)

Self-heating can

c)

Photosynthesis

d)

Combustion

15.

Two solutions are added together and the temperature changes from 19°C to 27°C. Is the reaction exothermic or endothermic?

a)

Exothermic

b)

Endothermic

16.

This symbol indicates that a reaction is _____

a)

reversible

b)

irreversible

c)

Unsure which direction it should go

17.

Around what time does the reaction reach equilibrium?

a)

25 min

b)

70 min

c)

45 min

d)

80 min

18.

Changes in pressure will only affect substances that are in the ______ state.

a)

solid

b)

gas

c)

liquid

19.

What are the two factors that help determine that equilibrium is reached?

a)

Forward reaction rate is faster than the reverse and the concentrations are equal

b)

Forward and reverse reaction rates are equal and concentrations are equal

c)

Forward and reverse reaction rates are equal and concentrations are constant

20.

When the rate of the forward reaction is equal to the rate of the backward reaction, the system is said to be in _____

a)

Chemical Balance

b)

Chemical Constant

c)

Chemical Reaction

d)

Chemical Equilibrium

21.

Which of the two graphs reaches equilibrium?

a)

Neither

b)

The left

c)

Both

d)

The right

22.

For the reaction...

SO2 + O2 ⇌ SO3

If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left or right

23.

Which of the following is NOT true at equilibrium?

a)

The concentrations of reactants and products do not change.

b)

The forward and reverse reactions proceed at the same rate.

c)

The concentration of the reactants is equal to the concentration of the products.

d)

The forward and reverse reactions continue to occur.

24.

For the reaction...

SO2 + O2 <−> SO3

If the equilibrium shifts to the right, the concentration of O2 will ___________.

a)

increase

b)

decrease

c)

double

d)

stay the same

25.

The following factors affect the position of equilibrium EXCEPT

a)

Concentration

b)

State of Matter

c)

Temperature

d)

Pressure

26.

Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,

a)

the system will adjust to increase the stress

b)

the system will adjust to reduce the stress

c)

the system will not adjust

27.

What happens to the equilibrium if the concentration of reactants is increased?

a)

The equilibrium shifts to the left

b)

The equilibrium shifts to the right

c)

The equilibrium remains unchanged

28.

How does a decrease in temperature affect the position of equilibrium in a chemical reaction?

a)

Increasing temperature always shifts the equilibrium to the left

b)

Increasing temperature always shifts the equilibrium to the right

c)

Shifts in exothermic direction

d)

Shifts in endothermic direction

29.

All 3 substances in this reaction are gases. Which stresses would not cause a shift to the right? Select all that apply

a)

Decreasing the temperature

b)

Increasing the temperature

c)

Increasing the pressure

d)

Adding a catalyst

e)

Increasing the concentration of ammonia

30.

When pink crystals of cobalt(II) chloride are heated, steam is given off and the colour of the solid changes to blue.

CoCl2.6H2O <=> CoCl2 + 6H2O

What happens when water is added to the blue solid?

a)

Changes to pink, heat is absorbed

b)

Changes to pink, heat is released

c)

Remains blue, heat is absorbed

d)

Remains blue, heat is released

31.

This ion produces a crimson red flame

a)

Na+

b)

Li+

c)

Ca2+

d)

K+

32.

This ion produces a lilac flame

a)

Na+

b)

Ca2+

c)

K+

d)

Ba2+

33.

This ion produces a blue-green flame

(a)  

34.

This ion produces a yellow flame

(a)  

35.

This ion produces a red flame

a)

Ca2+

b)

Na+

c)

Ba2+

d)

Cu2+

36.

This ion produces an apple-green flame

a)

Cu2+

b)

K+

c)

Ca2+

d)

Ba2+

37.

This gas turns limewater (calcium hydroxide) cloudy/milky

a)

Sulphur dioxide

b)

Hydrogen

c)

Carbon dioxide

d)

Oxygen

38.

This halide produces a white precipitate when silver nitrate is added

a)

chloride

b)

bromide

c)

iodide

39.

This halide produces a cream precipitate when silver nitrate is added

a)

chloride

b)

bromide

c)

iodide

40.

This halide produces a yellow precipitate when silver nitrate is added

a)

chloride

b)

bromide

c)

iodide

41.

After acidifying with nitric acid a few drops of barium nitrate solution is added...

a)

A white precipitate is produced - barium sulfite

b)

A white precipitate is produced - barium sulfate

c)

A white precipitate is produced - barium carbonate

d)

A white precipitate is produced - barium hydroxide

42.

When dilute acid is added to a sulfite solution, and the mixture is warmed gently, a gas is produced which

a)

Turns potassium manganate (VI) solution from colorless to purple

b)

Turns potassium manganate (VI) solution from purple to colorless

c)

Turns potassium manganate (VII) solution from colorless to purple

d)

Turns potassium manganate (VII) solution from purple to colorless

43.

To test for this anion sodium hydroxide and aluminium foil is added. The solution is warmed over a bunsen flame. This test is for the _____ ion, _____ gas is produced, which turns ___ litmus paper ___.

a)

Nitrate, ammonia, blue, red

b)

Nitrate, ammonium, blue, red

c)

Nitrate, ammonia, red, blue

d)

Nitrate, ammonium, red, blue

44.

This gas bleaches damp blue litmus paper

a)

carbon dioxide

b)

sulphur dioxide

c)

chlorine

d)

hydrogen

45.

Which positive test result is shown?

a)

Squeaky pop - oxygen gas

b)

Squeaky pop - hydrogen gas

c)

Squeaky pop - chlorine gas

46.

The positive test results for oxygen gas is...

(a)  

47.

This cation can be identified by warming a solution containing the ions with sodium hydroxide solution.

a)

Ammonia

b)

Sodium

c)

Potassium

d)

Ammonium

48.

These cations form a white precipitate when a few drops of sodium hydroxide or ammonia solution is added

a)

Aluminium

b)

Calcium

c)

Zinc

d)

Chromium

49.

When excess sodium hydroxide solution is this white precipitate it dissolves

a)

Calcium hydroxide

b)

Aluminium hydroxide

c)

Zinc hydroxide

d)

Chromium hydroxide

50.

This cation forms a blue precipitate that dissolves in excess ammonia

a)

Ca2+

b)

Fe2+

c)

Fe3+

d)

Cu2+

51.

This cation forms a green precipitate which dissolves in excess sodium hydroxide

(a)  

52.

This ion forms a brown precipitate that does not dissolve in excess sodium hydroxide or ammonia

(a)  

53.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
54.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
55.

Conducts electricity (electrolyte) when molten state or when dissolved in water.

a)

ionic compound

b)

covalent compound

56.

Does NOT conduct electricity when molten state or when dissolved in water. Not an electrolyte.

a)

ionic compound

b)

covalent compound

57.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
58.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
59.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
60.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
61.
usually soft
a)
ionic compounds
b)
covalent compounds
62.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
63.
electrolytes
a)
ionic compounds
b)
covalent compounds
64.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

65.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
66.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

67.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

68.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

69.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

70.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

71.
What type of bond forms between two or more atoms that are charged (+/-)?
a)
Covalent bond
b)
Incomplete bond
c)
Ionic bond
d)
Metallic bond
72.

Form a very organized crystal lattice as a solid

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

73.

Satisfy the octet rule (8 electrons in outer shell) to be stable.

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

74.

Weak interparticle forces

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

75.

When formed have properties that are completely different than the properties of the individual atoms that make them up.

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

76.

Typically flammable

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

77.

Formed by the attraction of opposite charges

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

78.

Very stable

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

79.

Usually soluble in water

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

80.

Polar compounds with poles or dipoles

a)

Ionic

b)

Covalant

c)

Both

d)

Neither

81.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
82.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
83.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
84.
Ionic bonds exist between a metal with a non-metal.
a)
True
b)
False
85.
Magnesium (Mg) and Oxygen (O) form an ________ bond.
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nothing
86.

Valence electrons are transferred

a)

Ionic bonds

b)

Covalent bonds

87.

Valence electrons are shared

a)

Ionic bonds

b)

Covalent bonds

88.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

89.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
90.
What type of bond is this?
a)
ionic
b)
covalent
91.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
92.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
93.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
94.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
95.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
96.

What type of bond involves the sharing of electrons between atoms?

a)

covalent bond

b)

ionic bond

c)

metallic bond

d)

transfer bond

97.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

98.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

99.

How many valence electrons should Lithium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

100.

How many valence electrons should Oxygen have in its Lewis dot model?

a)

5

b)

6

c)

7

d)

8

101.

How many valence electrons should Magnesium have in its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

102.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
103.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)

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