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Chemistry Exam Prep 10K1 Weds June 12th

Total questions: 153

Worksheet time: 2hrs 9mins

Name
Class
Date
1.
Which particle has a positive charge?
a)
electron
b)
orbital
c)
proton
d)
neutron
2.
Choose the particle that has no charge.
a)
nucleus
b)
neutron
c)
proton
d)
electron
3.
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
4.
Has a mass of 1/200th the mass of a proton.
a)
electron
b)
neutron
c)
nucleus
d)
electron cloud
5.
An electron has a _____ charge.
a)
negative
b)
positive
c)
neutral
6.
Which particles make up the nucleus of an atom?
a)
protons and neutrons
b)
electrons and protons
c)
electrons, protons, and neutrons
d)
electrons and neutrons
7.
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
8.
The subatomic particle that determines the identity of an element.
a)
neutron
b)
proton
c)
electron
d)
outer shell
9.
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
10.
What is the mass number and name of an element with 8 protons and 8 neutrons?
a)
16 - Carbon
b)
16 - Oxygen
c)
24 - Oxygen
d)
8 - Neon
11.
An element with a mass number of 10 and an atomic number of 6 has how many protons?
a)
5
b)
8
c)
6
d)
10
12.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
13.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
5
d)
25
14.
Matter that cannot be broken down into a simpler substance – building blocks of life.
a)
neutron
b)
atom
c)
electron
d)
quarks
15.
Elements on the periodic table increase by...
a)
atomic mass
b)
size
c)
mass number
d)
atomic #
16.
An atom has 13 protons, 15 neutrons and ___ electrons what is its mass number?
a)
13
b)
26
c)
28
d)
15
17.
Most of the mass of an atom is contained here.
a)
electron orbitals 
b)
nucleus
c)
shells
d)
atomic #
18.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
19.
Protons and Electrons balance the charge of an atom.
a)
True
b)
False
20.
Which letter represents a proton?
a)
A
b)
B
c)
C
d)
D
21.
Which letter represents an electron?
a)
A
b)
B
c)
C
d)
D
22.
Which letter represents the nucleus?
a)
A
b)
B
c)
D
d)
E
23.
Which scientist discovered the electron, which helped him develop a model of the atom?
a)
Niels Bohr
b)
John Dalton
c)
Ernst Rutherford
d)
J.J Thompson
24.
What contribution did John Dalton make to the atomic theory?
a)
He discovered that every atom was positively charged
b)
He discovered that every element consisted of one type of atom
c)
He discovered that atoms had nuclei
d)
He discovered that atoms could be divided into smaller parts
25.
Who discovered the nucleus of an atom?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
26.
He proposed the "muffin" or "plum pudding model of the atom.
a)
John Dalton
b)
Niels Bohr
c)
Ernest Rutherford
d)
JJ Thomson
27.
He discovered the neutron in the nucleus and completed the current atomic model.
a)
J.J. Thomson
b)
Ernest Rutherford
c)
Niels Bohr
d)
James CHadwick
28.
How many ELECTRONS fit on the 3rd Electron Shell?
a)
2
b)
4
c)
8
d)
18
29.
What element is displayed in the atom model?
a)
Helium
b)
Hydrogen
c)
Calcium
d)
Lithium
30.

Isotopes are atoms of the same element with a

a)

different number of protons.

b)

different number of electrons

c)

similar number of gluons.

d)

different number of neutrons.

31.

Which scientist discovered the electrons?

a)

Dalton

b)

Thomson

c)

Atristotle

d)

Bohr

32.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

33.

The smallest particle of an element that still represents that element.

a)

Nucleus

b)

electron

c)

proton

d)

atom

34.

What is the neutral particle found in the nucleus called?

a)

proton

b)

neutron

c)

electron

d)

quark

35.

All matter is made of

a)

energy

b)

atoms

c)

electrons

d)

compounds

36.

Matter always has mass.

a)

true

b)

false

37.

In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.

a)

Atoms

b)

Parts

c)

Molecules

d)

Hydrogen

38.

Who was the Greek philosopher who called the smallest particle of matter an "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

39.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

40.

Who is the scientist who proposed the "solar system" model of an atom where the electrons orbit around the nucleus?

a)

Democritus

b)

Niels Bohr

c)

Ernest Rutherford

d)

Chadwick

41.

The majority of an atom's mass exists where?

a)

In the nucleus

b)

In the electron cloud

c)

In the space between the nucleus and the electrons

d)

In the neutrons

42.

What did James Chadwick discover?

a)

neutrons

b)

electrons

c)

the atomic theory

d)

protons

43.

J.J. Thomson provided evidence that an atom...

a)

is the smallest particle of matter

b)

contains negatively charged particles

c)

has an overall negative charge

d)

has an overall positive charge

44.

Match the following

a)

From his Gold Foil Experiment, he concluded that the atom is mostly empty space with a tiny, positively charged, dense center he called the nucleus.

1.

Ernest Rutherford

b)

Concluded the atom had negatively charged particles that he named electrons. Proposed the Plum-Pudding Model of the atom.

2.

J. J. Thomson

c)

Proposed a model of the atom in which electrons travel around the nucleus in orbits.

3.

Niels Bohr

45.

Match the following

a)

Proposed that all matter is made up of tiny indivisible particles called atoms.

1.

Democritus

b)

In 1803, proposed the atomic theory of matter.

2.

John Dalton

c)

Describes mathematically the wave properties of electrons.

3.

Quantum Theory

46.

Which of the following points was included in Dalton's atomic theory, but later found to be not true?

a)

All matter is composed of atoms.

b)

Atoms of a given element are identical.

c)

Atoms of different elements combine to form compounds.

d)

In chemical reactions, atoms are separated, rearranged, or combined.

47.

How does the current Quantum Model differ from the Bohr Model?

a)

The Quantum Model show a dense, solid atom, and Bohr's model shows an empty space atom.

b)

In Bohr's model, the electrons are in the nucleus, and in the Quantum Model electrons are outside the nucleus.

c)

The Quantum Model agrees with Bohr's model, except that the orbits are further apart.

d)

The Quantum Model has an electron cloud, and Bohr's model shows electrons in orbits around the nucleus.

48.

Match the following images to the correct atomic model name.

a)

1.

Billiard Ball Model

b)

2.

Quantum Mechanical Model

c)

3.

Bohr Model

d)

4.

Plum Pudding Model

e)

5.

Rutherford Model

49.

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

50.

Whose model of the atom is represented in the image?

a)

Thomson

b)

Bohr

c)

Dalton

d)

Rutherford

51.

Who developed the Periodic Table of Elements?

a)

Dmitri Mendeleev

b)

Dmitri Mendeleev and Scientists

c)

Dmitri Mendeleev and Julius Lothar Meyer

d)

Dmitri Mendeleev, Julius Lothar Meyer and other Scientists

52.

3 elements that were discovered in 1871

a)

Gallium

b)

Galiium and Germanium

c)

Gallium, Germanium and Scandium

d)

Gallium, Germanium, Scandium and Hydrogen

53.

Elements discovered in 1890

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Noble Gases

54.

2 rows beneath the main periodic table

a)

Lanthanide

b)

Lanthanide and Actinide

c)

Lanthanide and Hydrogen

d)

Actinide and Hydrogen

55.

What is the periodic law?

a)

Elements have numbers

b)

Elements have specific names

c)

Elements are organized based on families

d)

Elements are organized based on atomic masses

56.

Book Mendeleev wrote in 1867

a)

Principals in Chemistry

b)

Principles in Chemistry

c)

Principles of Chemistry

d)

Organic Chemistry

57.

Why was Mendeleev's students struggling in his Science Class?

a)

It was boring

b)

It was too much info

c)

There's no fun activities

d)

There's no system to organize elements

58.

Number of known elements in the 1800's

a)

10

b)

20

c)

30

d)

63

59.

As of 2012, how many elements are there?

a)

100

b)

110

c)

115

d)

118

60.

98% of the Universe is made of

a)

H and N

b)

H and C

c)

H and O

d)

H and He

61.

What would be the product at the negative electrode in the electrolysis of Sodium Chloride solution

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

62.

What would be the product at the positive electrode in the electrolysis of Sodium Chloride solution

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

63.

What would be the product at the negative electrode in the electrolysis of molten Sodium Chloride

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

64.

What would be the product at the positive electrode in the electrolysis of molten Sodium Chloride

a)

Sodium

b)

Chlorine

c)

Hydrogen

d)

Oxygen

65.

What would be the product at the negative electrode in the electrolysis of Silver Nitrate solution

a)

Silver

b)

Nitrogen

c)

Hydrogen

d)

Oxygen

66.

What would be the product at the positive electrode in the electrolysis of Silver Nitrate solution

a)

Silver

b)

Nitrogen

c)

Hydrogen

d)

Oxygen

67.

What is the name given to the negative electrode

(a)  

68.

What name is given to the positive electrode

(a)  

69.

What is the third product produced in the electrolysis of Silver Nitrate solution

a)

Silver Nitrate

b)

Water

c)

Nitric Acid

d)

Silver Hydroxide

70.

What is the product at the negative electrode in the electrolysis of Copper Iodide solution

a)

Copper

b)

Iodine

c)

Hydrogen

d)

Oxygen

71.

What is the product at the positive electrode in the electrolysis of Copper Iodide solution

a)

Copper

b)

Iodine

c)

Hydrogen

d)

Oxygen

72.

What is the third product produced in the electrolysis of Copper Iodide solution

a)

Copper Iodide

b)

Copper Hydroxide

c)

Water

d)

Hydrogen Iodide

73.

What particles carry the electrical charge through the electrodes

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

74.

What particles carry the electrical charge through the electrolyte

a)

Electrons

b)

Ions

c)

Atoms

d)

Molecules

75.

What would you observe at the negative electrode in the electrolysis of Sodium Chloride solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

76.

What would you observe at the positive electrode in the electrolysis of Sodium Chloride solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

77.

What would you observe at the positive electrode in the electrolysis of Copper Sulphate solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

78.

What would you observe at the negative electrode in the electrolysis of Copper Sulphate solution

a)

Bubbles of gas that burn with a squeaky pop

b)

Bubbles of gas that relight a glowing splint

c)

Bubbles of gas that bleach damp litmus paper

d)

Solid deposits in the electrode

79.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
80.

During electrolysis, the negatively charged ions (anions) are attracted to the ________.

a)

anode

b)

cathode

81.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile in the molten state.

d)

There are no ions in solid lead(II) bromide

82.

Anions get discharged by ________ electrons at the ___________

a)

gaining, cathode

b)

losing, anode

c)

gaining, anode

d)

losing, cathode

83.

Positive ions (cations) move towards the cathode (-) where they will discharge by....

a)

Breaking apart

b)

Losing electrons

c)

Clumping together.

d)

Gaining electrons

84.

What ions are present in molten aluminium oxide?

a)

Al3+, O2-, H+, OH-

b)

Al3+, O2-

c)

Al3+, OH-

85.

___________ electrode is an inert electrode.

a)

Copper

b)

Iron

c)

Carbon

d)

Zinc

86.
What particle carries the charge in the wire?
a)
electron
b)
proton
c)
ion
d)
atom
87.
What particle carries the charge in the electrolyte?
a)
electron
b)
proton
c)
ion
d)
atom
88.

If the fork is to be electroplated with silver metal, what electrolyte should be used?

a)

Molten silver chloride

b)

Aqueous silver nitrate

c)

Sodium chloride solution

d)

Copper(II) sulphate solution

89.

What is the half-equation for the discharge of hydroxide ions?

a)

2O2- --> O2 + 4e-

b)

OH- --> OH + e

c)

4OH- --> 2H2O + O2 + 4e-

d)

2H2O + O2 + 4e- --> 4OH-

90.

In electrolytic cell that uses aqueous copper(II) sulfate as electrolyte and copper plates as electrodes, what is the product at the anode?

a)

Oxygen gas and water

b)

Copper metal

c)

Copper(II) ions

d)

Hydrogen gas

91.

What is the equation to show what happens to Cl- ions at the anode.

a)
Cl- --> Cl + e-   
b)
2Cl- --> Cl2 + 2e-   
c)
Cl2 + 2e-   2Cl- 
d)

Cl2 + 2e-  -->  2Cl- 

92.

Electroplating is an industrial process where objects are coated by a thin layer of a nonreactive metal by electrolysis. What should be used as the cathode in this process?

a)

Graphite electrode

b)

The electroplating metal

c)

The object to be electroplated

d)

Magnesium ribbon

93.

The picture shows electrolysis of copper(II) sulfate solution using graphite electrodes. Besides formation of a brown solid on the cathode, what other observations can be made?

a)

The mass of graphite anode decreases.

b)

The blue colour solution becomes paler.

c)

Bubbles of gas form at the anode.

d)

The blue colour solution becomes darker.

94.

The diagram shows the electrolysis of concentrated hydrochloric acid and concentrated aqueous sodium chloride using carbon electrodes.

At which electrode(s) is hydrogen produced?

a)

electrode 1 only

b)

electrodes 1 and 3

c)

electrode 2 only

d)

electrodes 2 and 4

95.

Electricity is passed separately through concentrated hydrochloric acid, concentrated aqueous sodium chloride and dilute sulfuric acid.

In which rows are the electrolysis products correctly named?

a)

1, 2 and 3

b)

1 and 2 only

c)

1 and 3 only

d)

2 and 3 only

96.

This question is about a simple cell made up of zinc and copper electrodes and sulfuric acid. The following is true.

a)

Copper ionises and becomes smaller.

b)

Zinc is the positive terminal.

c)

Effervescence will be seen at both electrodes.

97.

What are the electrode products when molten silver iodide is electrolysed between inert electrodes?

a)

A

b)

B

c)

C

d)

D

98.
Which of the following pairs of metals will produce the greatest voltage in a simple cell?
a)
Iron and copper
b)
Zinc and copper
c)
Calcium and magnesium
d)
Lead and copper
99.

In an electrolysis experiment, the same amount of charge deposited 6g of titanium and 16g of copper. The charge on teh copper ion was 2+. What was the charge on the titanium ion?

(a)  

100.

Match the following products to their respective electrolytes and electrodes.

a)

dilute NaCl

(+ electrode)

1.

colourless gas (oxygen)

b)

dilute NaCl

(- electrode)

2.

colourless gas (hydrogen)

c)

Conc.NaCl

(+ electrode)

3.

yellowish green gas

(chlorine)

d)

Conc.NaCl

(- electrode)

4.

colourless gas (hydrogen)

101.

What happens to the concentration of sodium chloride during electrolysis using dilute NaCl as electrolyte and inert electrodes?

(a)  

102.

Three different compounds are electrolysed.

Which one gives a yellow green gas at the anode?

a)

1

b)

2

c)

3

103.

In the electrolysis of molten sodium chloride, the products are molten sodium and chlorine gas. What is the volume of chlorine gas obtained at room temperature and pressure if the mass of molten sodium obtained is 230g?

a)

60dm3

b)

120dm3

c)

240dm3

d)

480dm3

104.

Covalent bonds are formed between...

a)

two or more metal atoms

b)

two or more non-metal atoms

c)

a metal and a non-metal atom

105.

Covalent bonds are formed when electrons are transferred between atoms.

a)

True

b)

False

106.

Atoms can only share electrons in the (a)   shell.

107.

Fluorine is a diatomic molecule. Fluorine is in Group 7. How many electrons are shared in this covalent bond?

(a)  

108.

Oxygen is a diatomic molecule. Oxygen is in Group 6. How many electrons are shared in this covalent bond?

(a)  

109.

The structure of ammonia is shown in the diagram. What is the formula for ammonia?

a)

NH3

b)

HN3

c)

N3H

d)

HN3

110.

What are the disadvantages of using displayed formulae, like the one shown?

a)

The 3D structure of the molecule is not shown.

b)

They can show how atoms are bonded in large molecules.

c)

They do not show which atom each electron comes from.

d)

They can be used to find the structural formula of the molecule.

111.

Select the properties of simple covalent substances.

a)

Low melting and boiling points.

b)

High melting and boiling points.

c)

Do not conduct electricity.

d)

Good conductors of electricity.

112.

Why do simple covalent substances not conduct electricity?

a)

They have low melting points.

b)

They have low boiling points.

c)

There are no delocalised electrons or free ions to carry the charge.

d)

The molecules are too large.

113.

Covalent structures have low melting and boiling points because it does not take much energy to break the _____ intermolecular forces.

a)

weak

b)

strong

114.

Which of these statements about nanoparticles is correct?

a)

They have large volume to surface area ratios

b)

They have large surface area to volume ratios

c)

They have small surface area to volume ratios

115.

To calculate the surface area of a cube, which formula is used?

a)

Length x width x height

b)

Length x width x 6

116.

The surface area of this cube would be calculated as:

3 x 3 x 6 = (a)   Inches2.

117.

Calculate the surface area of this cube (sides: 5cm).

Answer = (a)   cm2.

118.

To calculate the volume of a cube, which formula is used?

a)

Length x width x height

b)

Length x width x 6

119.

The volume of this cube would be calculated as:

3 x 3 x 3 = (a)   Inches3.

120.

Calculate the volume of this cube (sides: 5cm).

Answer = (a)   cm3.

121.

The surface area to volume ratio of this cube is therefore 54:27. What is the simplest version of this ratio?

a)

54:27

b)

2:1

c)

5:2

d)

3:1

122.

Select all the uses of nanoparticles below.

a)

Catalysts

b)

Suncreams

c)

Cosmetics

d)

Sock deodorizers

123.

Which is a concern over the use of nanoparticles in suncreams?

a)

Zinc Oxide nanoparticles block UV light from reaching the skin.

b)

Zinc Oxide nanoparticles are invisible.

c)

They could pass through the skin into the body and have harmful effects.

124.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

125.

The following equation shows the formation of magnesium oxide from magnesium metal. Which statement is correct for this reaction?

2Mg(s) + O2(g) → 2MgO(s) ΔH = -1204 kJ

a)

1204 kJ of energy are released for every mole of magnesium reacted

b)

602 kJ of energy are absorbed for every mole of magnesium oxide formed

c)

602 kJ of energy are released for every mole of oxygen reacted

d)

1204 kJ of energy are released for every two moles of magnesium oxide formed

126.

For the reaction 2H2(g) + O2(g) → 2H2O(g) the bond enthalpies (in kJ/mol) are

H-H = x, O=O = y, O-H = z

Which calculation will give the value, in kJ/mol, of ΔH for the reaction?

a)

2x + y - 2z

b)

4z - 2x - y

c)

2x + y - 4z

d)

2z - 2x - y

127.
Which is an example of an endothermic physical reaction? 
a)
a) Ice melting 
b)
b) Combustion 
c)
c) Steam condensing 
d)
d) Photosynthesis
128.

Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....

a)

+ 160 kJ

b)

-63 kJ

c)

- 160 kJ

d)

-217 kJ

129.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

130.

What kind of energy change happens in the photosynthesis reaction in plant leaves?

a)

Endothermic

b)

Exothermic

c)

No change

131.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

132.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

133.

How can we figure out if an overall reaction is endo- or exo-thermic? It is the difference between _______ and __________.

a)

hot and cold temperatures

b)

energy to break and energy to form bonds.

c)

time to form a bond versus time to break a bond

134.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

135.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

136.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

137.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

138.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
139.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

140.

Which of the following is true for ionic bonding & ionic compounds? (3 correct statements)

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

141.

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

142.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting point and it conducts electricity when molten or dissolved

c)

A high boiling point and it conducts electricity when solid

143.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

144.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

145.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds which require a large amount of heat energy to overcome these strong bonds.

d)

They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

146.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

147.

Be and F can combine to form BeF2, an ionic compound. Select ALL the true statements.

a)

Each Be atom loses two electrons from the outer shell.

b)

Each F atom gains two electrons from Be.

c)

The force holding the ionic compound together is electrostatic attraction.

d)

Each F ion has a charge of -1

148.

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.

149.

A single crystal of table salt (Sodium Chloride) is one giant ionic lattice, the Na+ and Cl- ions are held together in a (a)   lattice.

150.

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When melted ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

151.

Sodium Oxide is Na2O. Meaning there are 2 Na present for every O in the ionic compound. As the Oxygen ion has a charge of -2, what charge does each Sodium ion have?

a)

-1

b)

-2

c)

+2

d)

+1

152.

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

153.

What is the correct formula for aluminium oxide? Aluminium is in group 3 and oxygen is in group 6.

a)

Al₂O₃

b)

AlO

c)

AlO₄

d)

Al₂O

e)

Al₃O₂

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