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Practice g11

Total questions: 137

Worksheet time: 4hrs 21mins

Name
Class
Date
1.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
2.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
3.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
4.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
5.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
6.

A substance that dissolves in a liquid is called the...

a)

Solvent

b)

Solute

c)

Solution

d)

Salient

7.

Which of these statements about the halogens is incorrect?

a)

They are reactive because they easily gain one electron

b)

They form ions with a charge of +1

c)

They include fluorine, chlorine, bromine and iodine

d)

They get less reactive as their atomic number increases

8.

What is the correct formula of silver nitrate?

a)

AgNO3

b)

AgNO2

c)

Ag(NO3)2

d)

Ag2NO3

9.

What is the correct formula of magnesium sulphate?

a)

Mg(SO4)3

b)

MgSO4

c)

MnSO4

d)

Mg(SO4)2

10.

What is the correct formula of calcium hydroxide?

a)

Ca(OH)3

b)

Ca(OH)2

c)

CaOH

d)

Ca2OH

11.

Which of these equations is correctly balanced?

a)

Mg + O2 → 2MgO

b)

2Mg + O2 → MgO

c)

2Mg + O2 → 2MgO

d)

Mg + O2 → MgO

12.

Which of the following terms describes the structure of common salt, quicklime, and copper sulphate?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

13.

Which of the following terms describes the structure of iodine, oxygen, and carbon dioxide?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

14.

Name this molecule.

a)

Methane

b)

Ethane

c)

Propane

d)

Butane

15.

Damp red litmus paper turning blue is a positive test for which gas?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

d)

ammonia

e)

chlorine

16.

Damp red litmus paper turning blue, then bleaching white, is a positive test for which gas?

a)

hydrogen

b)

oxygen

c)

carbon dioxide

d)

ammonia

e)

chlorine

17.
The picture below is an example of _________________.
a)
osmosis
b)
isotonic
c)
diffusion
d)
active transport
18.
Reactions that release energy are called-
a)
activation
b)
endothermic
c)
mesothermic
d)
exothermic
19.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
20.

Which of the "Halogens" is found in liquid state at room temperature?

a)

Flourine

b)

Astatine

c)

Iodine

d)

Bromine

21.

Crude oil is a a mixture of hydrocarbons

a)

True

b)

False

22.
How many electrons does chlorine need to gain in order to have a full outer shell? 
a)
7
b)
0
c)
1
d)
8
23.

A measuring cylinder is used to measure the volume of a liquid. What is the volume of the liquid?

a)

43 cm3

b)

46 cm3

c)

48 cm3

d)

54 cm3

24.
Molecules are closest together in a 
a)
Solid
b)
Liquid
c)
Gas
25.

What is diffusion?

a)

when molecules move

b)

when molecules move from a high concentration to a low concentration

c)

no movement

d)

molecules move everywhere

26.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
27.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
28.
Most of the mass in an atom is concentrated in the...
a)
electrons
b)
nucleus
c)
protons
d)
empty space
29.
What does the nucleus consist of?
a)
Protons + Electrons
b)
Neutrons + Electrons
c)
Atoms
d)
Protons + Neutrons
30.

Isotopes are the atoms of the same element with the same number of.............. but different number of............

a)

electrons/neutrons

b)

neutrons/protons

c)

protons/neutrons

d)

electrons/protons

31.

Elements contain only one type of atoms.

a)

True

b)

False

32.
What is a pure substance made of two or more elements that are chemically combined called?
a)
A. element
b)
B. compound     
c)
C. mixture
d)
D. solution
33.
silver spoon
a)
A. MIXTURE
b)
B. COMPOUND
c)
C. ELEMENT
34.
A pure substance...
a)
is an element or a compound
b)
is an element or a mixture
c)
is a compound or a mixture
d)
is a mixture
35.
NaHCO3 is an example of —
a)
an abbreviation
b)
a compound
c)
a mixture
d)
an element
36.

How can you get salt from salty water?

a)

evaporate the water; then crystallisation

b)

condense the water; then crystallisation

c)

Filtration

37.

What separation method could you use to separate water from ink?

a)

filtration

b)

distillation

c)

electrolysis

38.

Mixtures can be separated using chromatography.

a)

True

b)

False

39.

Ink can be separated by a method of -----------------------------------------------

a)

distillation

b)

filtration

c)

chromatography

d)

sedimentation

40.
Which element has an electron configuration of 2.5?
a)
Oxygen
b)
Nitrogen
c)
Phosphorus
d)
Carbon
41.
Which element has the electron configuration of 2.7?
a)
Krypton
b)
Iodine
c)
Flourine
d)
Barium
42.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
43.

Nitrogen will ____ electrons to become stable.

a)

gain 1

b)

lose 1

c)

gain 3

d)

lose 3

44.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
45.
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
46.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
47.

What is the mass number of magnesium?

a)

2

b)

4

c)

12

d)

24

48.
What is the relative formula mass of NaOH?
a)
20
b)
39
c)
40
d)
45
49.

Which alkali metal is most reactive out of the following?

a)

rubidium

b)

potassium

c)

sodium

d)

lithium

50.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

51.

Which gas is released when the alkali metals react with water?

a)

hydrogen

b)

oxygen

c)

hydroxide

d)

carbon dioxide

52.

Which of the "Halogens" has yellowish green color?

a)

Chlorine

b)

Bromine

c)

Flourine

d)

Iodine

53.
Which gas in our atmosphere is most abundant?
a)
Argon
b)
Oxygen
c)
Nitrogen
d)
Carbon Dioxide
54.
What percentage of our atmosphere is made up of other gases such as argon, water vapor, and carbon dioxide?
a)
1%
b)
21%
c)
78%
d)
90%
55.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-14
d)
1-20
56.

The laboratory test for oxygen is that

a)

it relights a glowing splint

b)

it relights a burning splint

c)

it changes lime water to milky

d)

it makes a glowing splint go out

57.

Turns limewater milky

a)

Hydrogen

b)

Oxygen

c)

Ammonia

d)

Carbon dioxide

58.

Makes a squeaky pop sound when lit

a)

Hydrogen

b)

Oxygen

c)

Chlorine

d)

Ammonia

59.

This causes the mass of the nucleus to increase.

a)

adding an electron

b)

adding a neutron

c)

more orbitals

d)

adding negatively charged particles

60.

Has a mass of 1/2000th the mass of a proton.

a)

electron

b)

neutron

c)

nucleus

d)

electron cloud

61.

What are valence electrons?

a)

electrons on the first orbital always

b)

nucleus

c)

the outermost shell

d)

electrons on the outermost orbital

62.
The particles of the atom you can find by knowing the atomic number.
a)
neutrons
b)
protons and electrons
c)
protons and neutrons
d)
atomic mass
63.
The subatomic particle that determines the identity of an element.
a)
neutron
b)
proton
c)
electron
d)
outer shell
64.
What charge does the nucleus have and why?
a)
positive - the neutrons do not have a charge
b)
positive - the neutrons and protons are positively charged particles
c)
neutral - the neutral charge dominates the positive charge
d)
neutral - electrons cancel out the positive charge of the atom
65.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

66.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

67.

How many electrons does it have?

a)

197

b)

79

c)

118

d)

none of the above

68.

What do these isotopes of carbon all have in common?

a)

neutrons & mass number

b)

atomic number and neutrons

c)

atomic number

d)

protons, atomic number, and mass number

69.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
70.

The following is a:

a)

Compound

b)

Element

c)

Mixture of elements

d)

Mixture of compounds

71.
This picture represents which of the following?
a)
Element
b)
Compound
c)
Mixture
72.

Milk contains water, fat, salt and protein.


Milk is an example of ....

a)

an element

b)

a mixture

c)

a compound

73.

What happens to the mass of a liquid into which a soluble solute is added?

a)

The mass decreases

b)

The mass stays the same

c)

The mass increases

d)

It is impossible to tell

74.

Which of these phrases describes the particles in a solid?

a)

The particles are not in a regular arrangement and can move past each other.

b)

The particles are in a regular arrangement and can move past each other.

c)

The particles are far apart and can move randomly.

d)

The particles are in a regular arrangement and can only vibrate around fixed positions.

75.

If you were using filtration, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

76.

If you were using simple evaporation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

77.

If you were using distillation, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

78.

If you were using chromatography, what would you be trying to separate?

a)

A soluble solid from a liquid

b)

A mixture of two solids

c)

An insoluble solid from a liquid

d)

A mixture of two or more liquids

79.

Which of these statements is true?

a)

A neutron has a mass 1/1840 of a proton

b)

An electron has the same charge as a proton

c)

In any atom, the number of electrons is equal to the number of neutrons

d)

All atoms of a particular element have the same number of protons

80.

What is the electron configuration of the ion that this atom would form?

a)

2,8,2

b)

2,8,1

c)

2,8

d)

2,8,8

81.

75% of naturally occurring chlorine is Cl-35. The remaining chlorine is Cl-37. Which of the below equations shows how to calculate the relative atomic mass of chlorine?

a)

(75x37) + (25x35) / 100 = 35.5

b)

(75x35) + (25x37) / 100 = 35.5

c)

(75x37) + (25x35) / 100 = 35

d)

(75x35) + (25x37) / 100 = 37

82.

Which of these statements about Group 1 metals is incorrect?

a)

They are very reactive because they lose their inner shell electrons

b)

They form ions with a charge of +1

c)

They are very reactive because they lose their outer shell electron

d)

They react with water to form an alkaline solution

83.

Why are the noble gases so unreactive?

a)

They made a group decision not to react

b)

They have a large number of electrons

c)

They don't like to give up electrons

d)

They have a full outer shell of electrons

84.

Which of these statements about the halogens is incorrect?

a)

They are reactive because they easily gain one electron

b)

They form ions with a charge of +1

c)

They include fluorine, chlorine, bromine and iodine

d)

They get less reactive as their atomic number increases

85.

Which of the following substances conduct electricity when solid? (Could be more than one)

a)

diamond

b)

potassium chloride

c)

copper

d)

carbon disulfide

86.

Which of the following substances conduct electricity when liquid? (Could be more than one)

a)

diamond

b)

potassium chloride

c)

copper

d)

carbon disulfide

87.

Which of the following terms describes the structure of sand, graphite and diamond?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

88.

Which of the following terms describes the structure of sodium, steel, and iron?

a)

simple covalent

b)

giant covalent

c)

giant ionic

d)

metallic

89.

Simple molecular substances have low melting and boiling points because... (tick all statements that help explain it)

a)

they have weak intermolecular forces

b)

it takes more energy to separate the molecules

c)

the covalent bonds are very strong

d)

it takes less energy to separate the molecules

90.

Simple molecular substances do not conduct electricity because... (tick all statements that help explain it)

a)

they have delocalised electrons

b)

they do not have delocalised electrons

c)

they do not contains ions

d)

the covalent bonds are very strong

91.

Diamond is very hard because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the intermolecular forces require a lot of energy to be broken

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

92.

Diamond has a very high melting point because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the intermolecular forces require a lot of energy to be broken

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

93.

Diamond does not conduct electricity because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

it does not have any delocalised electrons or ions

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that cannot slide over each other

94.

Graphite is soft because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the forces between the layers are weak

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

95.

Graphite has a high melting point because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the forces between the layers are weak

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

96.

Graphite can conduct electricity because... (tick all statements that help explain it)

a)

the carbon atoms are linked by very strong covalent bonds

b)

the electrons can move along the layers from one atom to the next

c)

the covalent bonds require a lot of energy to be broken

d)

the atoms are arranged in layers that can slide over each other

97.

Which of these are properties of metals? (Tick all that apply)

a)

High densities

b)

High melting and boiling points

c)

Good conductors of heat and electricity

d)

Malleable

98.

In an endothermic reaction, heat is ,,,

a)

given out

b)

taken in

99.
acid + metal ----->
a)
salt + hydrogen
b)
salt + water + carbon dioxide
c)
salt + water
d)
salt + carbon dioxide
100.

Acid + Carbonate ----->

a)

salt + hydrogen

b)

salt + water + carbon dioxide

c)

salt + water

d)

salt + carbon dioxide

101.
Magnesium + sulphuric acid --> ?
a)
magnesium sulfate + water
b)
magnesium sulfate + hydrogen
c)
magnesium chloride + hydrogen
d)
magnesium chloride + water
102.
Zinc + nitric acid --> ?
a)
zinc sulfate + water
b)
zinc sulfate + hydrogen
c)
zinc nitrate + hydrogen
d)
zinc chloride + water
103.
Which metal is the least reactive out of: copper, magnesium, zinc and iron?
a)
copper
b)
magnesium
c)
zinc
d)
iron
104.
Which equation correctly shows the displacement of copper by zinc?
a)
copper + zinc sulphate --> copper sulfate + zinc
b)
zinc sulphate + copper --> copper sulfate + zinc
c)
copper sulfate + zinc --> zinc sulfate + copper
105.
Salts produced by the reactions of hydrochloric acid are known as... 
a)
chlorines
b)
nitrates
c)
chlorides
d)
bromides
106.
How do you know when a reaction between a metal and an acid is complete?
a)
All the metal is dissolved
b)
There is a color change in the acid
c)
Bubbles don't form when more metal is added
d)
All the acid evaporates
107.
Why is burning a salt one way to determine the metal used in preparing it?
a)
Each metal burns a different color.
b)
Some metals burn and some don't.
c)
Each metal has a different colored smoke.
d)
Burning salts is not will not help determine the metal.
108.
In a reaction between an acid and a carbonate gas bubbles will appear. What is that gas?
a)
helium
b)
hydrogen
c)
oxygen
d)
carbon dioxide
109.
Interpret the following equation in terms of moles:
Li3N + 3NH4NO3 --> 3LiNO3 + (NH4)3N
a)
lithium nitride reacts with ammonium nitrate
b)
3 moles of lithium nitrate and 3 moles of ammonium nitrate are produced
c)
3 moles of ammonium nitrate produces 1 mole ammonium nitride
d)
1 mole lithium nitride produces 3 moles ammonium nitrate
110.
Which of the following represent a mole ratio between silver nitrate and copper(II) nitrate in the following reaction:
2AgNO3 + Cu --> Cu(NO3)2 + 2Ag
a)
2 mol AgNO3 / 2 mol Ag
b)
2 mol Ag / 2 mol AgNO3 
c)
2 mol AgNO3 / 2 mol Cu(NO3)2
d)
2 mol AgNO3 / 1 mol Cu(NO3)2
111.
For the following reaction, how many moles of copper is need to produce 8 moles of silver?
2AgNO3 + Cu --> Cu(NO3)2 + 2Ag
a)
1 moles
b)
2 moles
c)
4 moles 
d)
8 moles
112.
How many hydrogen atoms are in one molecule of Amonium Sulfite (NH4)2SO3?
a)
6.02 x 1023
b)
2
c)
4
d)
8
113.
How many moles are in 6 x 1023 molecules of H2O?
a)
1
b)
2
c)
6
d)
600
114.
Which of the following would have more mass?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
115.
How many moles are in 8.30 X 1023 molecules of H2O?
a)
1.38 X 1023 moles H2O
b)
1.38 moles H2O
c)
2 moles H2O
d)
138 moles H2O
116.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25
d)
1.91 x 1022
117.

The number 6.022 x 1023 is called what?

a)

Avocado's Number

b)

Avogadro's Number

c)

Alejandro's Number

d)

Bohr's Number

118.

Which has more molecules?

a)

1 mole H2O

b)

1 mole NaCl

c)

1 mole Al(OH)3

d)

These are all the same

119.

What are the units for molar mass?

a)

g

b)

g/mole

c)

amu

d)

atoms

120.

The best definition for a mole provided below is

a)

The unit for the mass of something

b)

The unit for the amount of a substance

c)

The unit for the volume of something

d)

The unit for the area of a substance

121.
How are the mole and atomic masses of elements related?  
a)
The atomic mass of any substance is always equal to 1 mole of that substance 
b)
The atomic mass added up with itself by 6.02 x 1023 equals the amount of atoms
c)
The atomic mass is the amount of protons plus number of atoms
d)
Atoms combined make up molecules, which are the measurement of atomic masses 
122.

Why is the mole used to measure the atom?

a)

Atoms are extremely tiny particles, and their size varies from element to element

b)

Atoms are all the same size for every element

c)

Some atoms cannot be counted using the mole

123.
Which compound has the smallest molar mass?
a)
CO
b)
CO2
c)
H2O
d)
H2O2
124.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
125.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
126.
How many moles of carbon atoms are there in 5g of carbon?
a)
60 mol
b)
17 mol
c)
0.42 mol
d)
7 mol
127.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
128.
Hydrochloric acid can react with sodium thiosulfate solution to form a sulfur precipitate. The equation is:
Na2S2O3(aq) + 2HCl(aq) → 2S(s) + SO2(g) + 2NaCl(aq) + H2O(l)
Which list below contains only changes that will decrease the rate of this reaction?
a)
Increase the temperature, increase the hydrochloric acid concentration and add a catalyst
b)
Decrease the temperature and add a catalyst
c)
Decrease in temperature, decrease in concentration of the hydrochloric acid, addition of water to the sodium thiosulfate
d)
Decrease the concentration of the sodium thiosulfate solution and increase the temperature
129.
Under certain conditions, cyclohexane can react to form benzene and hydrogen according to the equation:
C6H12(g) → C6H6(g) + 3H2(g); ΔH=+206 kJ mol-1
Which two changes could be used to increase the rate of reaction?
a)
Add a catalyst and reduce the temperature
b)
Add a catalyst and decrease the pressure
c)
Increase the temperature and the external pressure
d)
Add a catalyst and decrease the concentration of cyclohexane
130.
The reaction between zinc and hydrochloric acid may be represented by the equation: 
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g); ΔH = -154 kJ mol-1
In an investigation of this reaction using excess Zn and 2 M HCl(aq) in an open flask, the graph shown was plotted from the data collected.
Which of the following would be a suitable quantity for the vertical axis of the graph?
a)
Number of collisions per second.
b)
Rate of reaction.
c)
Temperature.
d)
Number of ion.
131.
Catalysts are thought to increase the rate of a chemical reaction by
a)
supplying the energy needed to overcome the activation energy
b)
increasing the temperature of the reaction
c)
providing less surface area for the reaction
d)
providing an alternative reaction pathway with a lower activation energy
132.
The equation and energy profile for combustion of methane is shown. 
According to the information provided on this profile, the activation energy for the reaction:
0.5CO2(g) + H2O(g) → 0.5CH4(g) + O2(g)
would be
a)
1635 kJ
b)
2135 kJ
c)
2490 kJ
d)
4270 kJ
133.
The main reason for the use of catalysts in most industrial processes is to
a)
reduce greenhouse gas emissions
b)
reduce the energy requirement for a reaction
c)
reduce waste production
d)
increase the yield of product
134.
Increasing the temperature of a chemical reaction
a)
lowers the activation energy of the reaction
b)
increases the energy of the reactant particles only
c)
increases the value of ΔH for the reaction
d)
increases the energy of the reactant and product particles
135.
Which of the following changes that can be made to a chemical reaction will result in a greater proportion of successful collisions between reactant particles?
I. addition of a catalyst
II. grinding reactant lumps into a powder
III. increasing the concentration of reactants
a)
I only
b)
II and III only
c)
I and II only
d)
I, II and III
136.
Which of the following would increase the INITIAL reaction rate between 5.0 g aluminium and 20.0 mL of 1.00 M hydrochloric acid?
a)
Conducting the experiment in a 50 mL beaker rather than a 100 mL beaker. 
b)
Using a larger volume of acid.
c)
Cleaning the surface of the metal with sandpaper.
d)
Increasing the pressure under which the experiment was conducted.
137.
Not all collisions between reactant particles result in the formation of products. This could be due to
i. the molecules not colliding with sufficient energy
ii. the concentration of reactants being low
iii. the reaction reaching equilibrium
iv. the reactants not colliding in the correct orientation
a)
all of the above
b)
i only
c)
iii only
d)
i and iv

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