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Review G9

Total questions: 118

Worksheet time: 1hrs 19mins

Name
Class
Date
1.

LiBr

a)

Ionic

b)

Covalent

c)

Both

2.

PBr5

a)

Ionic

b)

Covalent

c)

Both

3.

A material with a high melting point

a)

Ionic

b)

Covalent

c)

Both

4.

Nonconductive in the solid form.

a)

Ionic

b)

Covalent

c)

Both

5.

A material that has a low boiling point

a)

Ionic

b)

Covalent

c)

Both

6.

Cl2

a)

Ionic

b)

Covalent

c)

Both

7.

Cu(NO3)2

a)

Ionic

b)

Covalent

c)

Both

8.

A material that forms a solid crystal lattice at room temperature.

a)

Ionic

b)

Covalent

c)

Both

9.

Ag2O

a)

Ionic

b)

Covalent

c)

Both

10.

Strength of the bond is directly related to the molar mass of the substance.

a)

Ionic

b)

Covalent

c)

Both

11.

The valence electrons are shared when the outermost orbitals overlap.

a)

Ionic

b)

Covalent

c)

Both

12.

A material that is held together by electrostatic attractions caused by electron transfer.

a)

Ionic

b)

Covalent

c)

Both

13.

A single particle can be classified as a "molecule".

a)

Ionic

b)

Covalent

c)

Both

14.

A single particle can be classified as a "formula unit".

a)

Ionic

b)

Covalent

c)

Both

15.

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

16.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
17.

Which of the following is true for BOTH ionic and covalent compounds?

a)

They bond to attain a noble gas configuration

b)

During bonding, atoms will increase in mass.

c)

They either transfer or share protons to get the atomic number of a noble gas.

d)

They always act like the noble gas that comes before them.

18.

Typically soluble in water.

a)

Ionic

b)

Covalent

c)

Both

19.

Does not form electrolyte solutions.

a)

Ionic

b)

Covalent

c)

Both

20.

The number of charges helps identify the strength of the bond.

a)

Ionic

b)

Covalent

c)

Both

21.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
22.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds
23.

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

a)

ionic compound

b)

covalent compound

24.

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

a)

ionic compound

b)

covalent compound

25.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
26.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
27.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
28.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
29.
usually soft
a)
ionic compounds
b)
covalent compounds
30.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
31.
electrolytes
a)
ionic compounds
b)
covalent compounds
32.

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

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

33.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
34.

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

35.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

36.

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

37.

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.

38.

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

39.
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
40.

Form a very organized crystal lattice as a solid

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

41.

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

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

42.

Weak interparticle forces

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

43.

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

44.

Typically flammable

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

45.

Formed by the attraction of opposite charges

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

46.

Very stable

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

47.

Usually soluble in water

a)

Ionic

b)

Covalent

c)

Both

d)

Neither

48.

Polar compounds with poles or dipoles

a)

Ionic

b)

Covalant

c)

Both

d)

Neither

49.

What are ions?

a)

Particles that bond together through ionic bonds

b)

Atoms that lose or gain electrons

c)

Atoms with full outer shells

d)

Particles with opposite charges

50.

How can ions be represented using equations?

a)

By showing the movement of electrons with arrows

b)

By placing big square brackets around them

c)

By writing the atom's charge in the top right corner

d)

By drawing dots and crosses to represent electrons

51.

What is the force that holds ions together in an ionic compound?

a)

Covalent bond

b)

Ionic bond

c)

Electrostatic force

d)

Metallic bond

52.

What type of bond is an ionic bond?

a)

Weak

b)

Moderate

c)

Strong

d)

Unstable

53.

How are electrons represented in a dot and cross diagram?

a)

As dots

b)

As crosses

c)

As arrows

d)

As shells

54.

What is the general rule for the movement of electrons in an ionic bond?

a)

Electrons move from the non-metal to the metal

b)

Electrons move from the metal to the non-metal

c)

Electrons move from the outermost shell to the inner shells

d)

Electrons move randomly between atoms

55.

In the formation of magnesium chloride (MgCl2), how many outer electrons does magnesium have?

a)

1

b)

2

c)

6

d)

7

56.

In the formation of magnesium chloride (MgCl2), how many outer electrons does each chlorine atom need?

a)

0

b)

1

c)

6

d)

7

57.

What are ions formed from?

a)

Atoms losing or gaining nuclei

b)

Atoms losing or gaining electrons

c)

Atoms losing or gaining neutrons

d)

Atoms losing or gaining protons

58.

What does a sodium atom become when it loses one electron?

a)

Sodium 2+ ion

b)

Sodium 1+ ion

c)

Sodium 1- ion

d)

Sodium 2- ion

59.

Why does a sodium atom need to lose one electron?

a)

To become unstable

b)

To become lighter

c)

To become stable with a full outer shell

d)

To become heavier

60.

What does a chlorine atom become when it gains one electron?

a)

Chlorine 2- ion

b)

Chlorine 2+ ion

c)

Chlorine 1- ion

d)

Chlorine 1+ ion

61.

What is the force called that attracts two ions with opposite charges?

a)

Nuclear force

b)

Electrostatic force

c)

Gravitational force

d)

Magnetic force

62.

What is an ionic bond?

a)

A weak force between ions with opposite charges

b)

A strong force between atoms

c)

A weak force between atoms

d)

A strong force between ions with opposite charges

63.

What is the diagram called that shows the formation of ionic compounds?

a)

Dot and cross diagram

b)

Molecular model

c)

Lewis structure

d)

Bohr model

64.

In a dot and cross diagram, how are the electrons of different atoms represented?

a)

One atom's electrons as dots and the other's as crosses

b)

All as crosses

c)

One atom's electrons as circles and the other's as squares

d)

All as dots

65.

What should you use to show the movement of electrons in a dot and cross diagram?

a)

A circle

b)

A square

c)

A line

d)

An arrow

66.

When drawing dot and cross diagrams, what is sometimes omitted to make the drawing quicker?

a)

The innermost shells

b)

The nucleus

c)

The protons

d)

The outermost shell

67.

In the formation of magnesium chloride (MgCl2), how many electrons does magnesium lose?

a)

Two

b)

Three

c)

One

d)

Four

68.

How many chloride ions are formed when magnesium reacts with chlorine to form MgCl2?

a)

Three

b)

One

c)

Two

d)

Four

69.

What charge does a magnesium ion have after losing electrons in the formation of MgCl2?

a)

1+

b)

2+

c)

2-

d)

1-

70.

What charge does each chloride ion have in the formation of MgCl2?

a)

2-

b)

2+

c)

1+

d)

1-

71.

How are the ions arranged in a dot and cross diagram involving more than two ions?

a)

Randomly

b)

In a straight line

c)

As they would be in a real compound

d)

In a circular pattern

72.

What does covalent bonding involve?

a)

Transfer of electrons from a metal to a non-metal atom

b)

Transfer of electrons from a non-metal to a metal atom

c)

Sharing of electrons between two metal atoms

d)

Sharing of electrons between two non-metal atoms

73.

What is the chemical formula of the following covalent substance?

a)

CO2

b)

CH4

c)

CO

d)

CH3

74.

In covalent bonding, atoms share electrons because...

a)

they are sociable

b)

They are generous

c)

They end up with a full outer shell and are more stable

d)

They became less stable

75.

In a covalent substance, which electrons are shared between atoms?

a)

Outer-shell electrons

b)

Inner-shell electrons

c)

All the electrons

d)

None of them

76.

What kind of bond is formed when three pairs of electrons are shared between two atoms?

a)

Single

b)

Double

c)

Triple

d)

Quadruple

77.

Which substance is being shown in the dot-and-cross diagram?

a)

Water

b)

Methane

c)

Nitrogen

d)

Ammonia

78.

Correct diagram for HF

a)
b)
c)
d)
79.

What is the main purpose of a dot and cross diagram?

a)

To illustrate the transfer of electrons

b)

To represent the atomic mass

c)

To show the movement of protons

d)

To display the atomic nucleus

80.

What happens to a sodium atom when it forms an ion?

a)

It gains two electrons

b)

It loses one electron

c)

It gains one proton

d)

It loses two protons

81.

Why do atoms form ions?

a)

To change their element type

b)

To achieve a full outer electron shell

c)

To decrease their atomic mass

d)

To increase their atomic number

82.

What charge does a chloride ion have?

a)

1 plus

b)

2 minus

c)

2 plus

d)

1 minus

83.

What type of force holds ionic compounds together?

a)

Nuclear force

b)

Electrostatic force

c)

Gravitational force

d)

Magnetic force

84.

In a dot and cross diagram, how are electrons from different atoms represented?

a)

As triangles and circles

b)

As dots and crosses

c)

As lines and dots

d)

As circles and squares

85.

What is the charge of a magnesium ion in MgCl2?

a)

1 plus

b)

2 plus

c)

1 minus

d)

2 minus

86.

How many chloride ions are needed to balance one magnesium ion in MgCl2?

a)

One

b)

Two

c)

Three

d)

Four

87.

What is the general rule for electron movement in ionic bonding?

a)

Electrons move from gases to liquids

b)

Electrons move from solids to gases

c)

Electrons move from metals to nonmetals

d)

Electrons move from nonmetals to metals

88.

Why might you only draw the outermost shell in a dot and cross diagram?

a)

To make the diagram more colorful

b)

To simplify the diagram

c)

To highlight the nucleus

d)

To show the atomic mass

89.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

90.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

91.

What do electrons do in a metallic bond?

a)

They stay on the metal atom.

b)

They are transferred from atom to atom.

c)

They form a covalent bond with another atom.

d)

They float around freely.

92.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

93.

Why are metals good conductors of electricity?

a)

The electric current can easily travel along the surface of the metal because it is smooth.

b)

A negative charge can easily push the sea of electrons in one direction, making a current.

c)

Metals attract electricity.

d)

Metals are malleable.

94.

Why are metals malleable? (They can bend without breaking.)

a)

Metals are very smooth.

b)

Metals have a sea of electrons.

c)

The sea of electrons form a strong metallic bond.

d)

Even though the metal ions repel each other, the electron sea holds all the atoms in place.

95.

What do we call electrons that move freely in a metallic bond?

a)

sea of electrons

b)

lone electrons

c)

unpaired electrons

d)

covalent electrons

96.

What property of metals is the image describing?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

97.

What property of metals is being shown in figure 1(b) in the image?

a)

malleable (bend without breaking)

b)

ductile (stretched into a wire)

c)

conductive (can conduct electricity)

d)

shiny

98.

What is the one thing responsible for a metal being malleable, ductile, and conductive?

a)

metal atoms

b)

its covalent bonds

c)

its valence electrons

d)

its sea of free-floating electrons

99.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
100.
A cation is a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
101.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
102.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

103.

Beryllium, Be, will ____ valence electrons when forming an ionic bond.

a)

lose 4

b)

gain 4

c)

lose 2

d)

gain 2

104.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
105.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
106.

What will be the charge of a bromine ion?

a)

+7

b)

-7

c)

-1

d)

+1

107.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
108.
Ionic bonds consist of the ____ of valence electrons.
a)
sharing
b)
transfer
109.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
110.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
111.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
112.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
113.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

114.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
115.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
116.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
117.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
118.
Which of the following is NOT true of ionic compounds?
a)
Metal ions have a + charge
b)
Non-metal ions have a - charge
c)
They conduct electricity when they are solid
d)
They are arranged in a giant lattice

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