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Chemical Bonding Mastery Set

Total questions: 90

Worksheet time: 56mins

Name
Class
Date
1.

Why do atoms form covalent bonds?

a)

To achieve stability and become 'happy'

b)

To increase their mass

c)

To lose electrons rapidly

d)

To become radioactive

2.

Arrange the following types of bonds in order from weakest to strongest: single, double, triple, ionic.

a)

Single, Double, Triple, Ionic

b)

Ionic, Triple, Double, Single

c)

Triple, Double, Single, Ionic

d)

Double, Single, Triple, Ionic

3.

Which of the following is NOT a subtype of covalent bond?

a)

Single bond

b)

Double bond

c)

Triple bond

d)

Quadruple bond

4.

In covalent bond diagrams, what does a single line between two atoms represent?

a)

A pair of electrons shared between the atoms

b)

Two pairs of electrons shared between the atoms

c)

A single electron shared between the atoms

d)

No electrons shared between the atoms

5.

When drawing Lewis structures, how are unbonded electrons and electrons in bonds represented?

a)

Unbonded electrons are shown as dots and electrons in bonds are shown as lines

b)

Unbonded electrons are shown as lines and electrons in bonds are shown as dots

c)

Both unbonded electrons and electrons in bonds are shown as dots

d)

Both unbonded electrons and electrons in bonds are shown as lines

6.

What is true about a covalent double bond?

a)

Two atoms each pool 2 of their electrons and share a total of 4 electrons between themselves.

b)

Two atoms each pool 4 of their electrons and share a total of 8 electrons between themselves.

c)

Two atoms each pool 1 of their electrons and share a total of 2 electrons between themselves.

d)

Two atoms do not share any electrons in a double bond.

7.

In a covalent triple bond, how many electrons do two atoms share between themselves to reach a duet or octet?

a)

6 electrons

b)

3 electrons, but only one atom shares

c)

4 electrons, with two from each atom

d)

8 electrons, with four from each atom

8.

Which of the following molecules contains a triple covalent bond?

a)

N≡N

b)

O=O

c)

H-H

d)

Cl-Cl

9.

Refer to the diagram. What kind of bond is shown?

a)

Single covalent

b)

Ionic

c)

Double covalent

d)

Triple covalent

10.

Which type of covalent bond will an atom like Hydrogen or Fluorine form if it needs 1 more valence electron?

a)

A single bond

b)

A triple bond with extra electrons

c)

A double bond

d)

No bond

11.

An atom like Oxygen needs 2 more valence electrons. What types of bonds can it form to satisfy this need?

a)

One double bond or two single bonds

b)

Two triple bonds

c)

One single bond and one triple bond

d)

Three single bonds

12.

Which of the following bonding arrangements is possible for an atom like nitrogen or phosphorus that needs 3 more valence electrons?

a)

1 triple bond

b)

1 double bond and 1 single bond

c)

3 single bonds

d)

All of the above

13.

Following the Octet rule, what would the chemical formula for the covalent compound formed between fluorine and oxygen be?

a)

OF

b)

OF2

c)

O2F

d)

F2O2

14.

Which prefix is used to indicate that there are four atoms of an element in a covalent compound?

a)

Tetra

b)

Penta

c)

Hexa

d)

Tri

15.

What is the main difference in naming covalent compounds compared to ionic compounds?

a)

Prefixes are used to show the number of atoms of each element in covalent compounds

b)

The first element's name is always changed in covalent compounds

c)

Covalent compounds do not use the -ide ending

d)

Ionic compounds use prefixes to show the number of atoms

16.

What is the standard name for the covalent compound H2O?

a)

Dihydrogen monoxide

b)

Hydrogen oxide with two hydrogens

c)

Monohydrogen oxide

d)

Hydrogen dioxide

17.
A substance which has a high melting point, conducts electricity when dissolved in water, and has a crystalline structure probably has what type of bond?
a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
18.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

19.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

20.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

21.

A compound forms between a metal and a nonmetal. It is

a)

ionic

b)

metallic

c)

covalent

22.

Ionic compounds are held together by

a)

intermolecular forces

b)

electrostatic forces

c)

magnetic forces

d)

nuclear forces

23.

A compound that is a poor conductor and has low melting and boiling points is most likely

a)

ionic

b)

metallic

c)

covalent

24.

Generally, atoms form bonds so that _______________.

a)

Each atom loses its electrons

b)

Each atom has a full outer shell

c)

Each atom has an unstable electron configuration

d)

Each atom gains electrons

25.
A ____________is the force that holds atoms together in a compound.
a)
Chemical Formula
b)
Chemical Reaction
c)
Chemical Bond
d)
Synthesis Reaction
26.

When does an atom become an ion?

a)

When it gains or loses electrons and takes on a charge.

b)

When it is stable because it has a full set of valence electrons.

c)

When it forms a compound with another atom.

27.

How many oxygen are in one unit of the compound Fe2O3Fe_2O_3  ?

(a)  

28.

How many electrons do most elements want to have in their outer shell to be stable?

(a)  

29.

What ionic charge would an atom with this electron dot diagram form?

a)

+2

b)

2

c)

-2

30.

What ionic charge would an element with this electron dot diagram take on?

(a)  

31.

What is the correct name for the compound MgI2MgI_2  

a)

magnesium iodide

b)

magnesium diiodide

c)

monomagnesium diiodide

32.
What are valence electrons?
a)
sum of the protons and neutrons
b)
protons minus electrons
c)
electrons in the inner shells
d)
electrons in the outer shell
33.
If an atom gains two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
34.
How many valence electrons does oxygen have?
a)
2
b)
4
c)
5
d)
6
35.

How many valence electrons does Al have?

a)

3

b)

4

c)

5

d)

6

36.

How many valence electrons does Br have?

a)

5

b)

6

c)

7

d)

8

37.

Lithium has 1 valence electron, to bond with iodine what would it do?

a)

share an electron with iodine.

b)

Give an electron to iodine.

c)

It depends on the temperature: if it is hot it will give its electron to iodine but if it is cold it will take an electron from iodine.

d)

Lithium and iodine will not react and form a bond.

38.

How many valence electrons does Mg have?

a)

1

b)

2

c)

3

d)

4

39.

If H bonds with O, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

40.

If Fe bonds with F, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

41.

If N bonds with S, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

42.

If Cu bonds with O, what kind of bond will form?

a)

covalent

b)

ionic

c)

metallic

d)

none of these

43.

The correct name for MgF2 is ______________.

a)

magnesium fluoride

b)

magnesium difluoride

c)

manganese difluoride

d)

magnesium (II) fluoride

44.

The correct name for N2O is ____________.

a)

dinitrogen monoxide

b)

dinitrogen oxide

c)

nickel oxide

d)

nickel (I) oxide

45.

BeI2

a)

Beryllium (II) iodide

b)

Beryllium iodine

c)

Beryllium iodide

d)

Beryllium (I) iodide

46.

Strontium nitride

a)

SrN

b)

Sr3N2

c)

Sr2N3

d)

N3Sr2

47.

Aluminum fluoride

a)

AlF

b)

AlF2

c)

Al3F

d)

AlF3

48.
What is the name of the compound P2O5
a)
Pentaphosphorus dioxide
b)
Phoshphide dioxide
c)
Diphosphorus pentoxide
49.
What is the correct name for N2O4?
a)
Nitrogen oxide
b)
Dinitrogen Tetraoxide
c)
Nitrogen iodide 
d)
Dinitrogen oxygenide
50.
Which of the following gives the correct chemical formula for the compound Magnesium Phosphide?
a)
Mg2P3
b)
MgP
c)
Mg3P2
d)
MgP2
51.

The name of monatomic negative ions (anions) all end in what suffix?

a)

-ate

b)

-ite

c)

-ium

d)

-ide

52.

What is formula for calcium chloride?

a)

CaCl

b)

CaCl2

c)

ClClO3

d)

CaC2

53.

What is the charge on the sulfide ion?

a)

-1

b)

-2

c)

-3

d)

+2

54.

What is the charge on the nitride ion?

a)

-1

b)

-2

c)

-3

d)

+2

55.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
56.

What is the correct name for the compound, P4S3?

a)

tetrapotassium trisodium

b)

triphosphorus tetrasulfide

c)

phosphorus sulfur

d)

trisulfur tetraphosphide

e)

 tetraphosphorus trisulfide

57.

What is the correct name for the compound, BrF3?

a)

bromine trifluoride

b)

monoboron trifluoride

c)

 tribromine monofluoride

d)

monobromine fluoride

e)

 trifluorine monobromide

58.

What is the correct molecular formula for the compound, sulfur tetrafluoride?

a)

SF

b)

SF4

c)

SiF4

d)

SF5

e)

SF3

59.

What is the correct molecular formula for the compound, sulfur dioxide?

a)

SeO2

b)

SO

c)

SO2

d)

S2O

e)

SO4

60.

What is the correct molecular formula for the compound, disulfur dichloride?

a)

S2Cl2

b)

Si2Cl2

c)

SCl

d)

S2Cl4

e)

S16Cl4

61.

What is the correct name for the compound, PF5?

a)

phosphorus pentafluoride

b)

monophosphorus pentafluoride

c)

potassium fluoride

d)

pentafluorine monophosphide

e)

phosphorus tetrafluoride

62.

What is the correct molecular formula for the compound, selenium tetrafluoride?

a)

Se4F

b)

SF4

c)

SeF8

d)

SeF4

e)

SeF

63.

What is the correct molecular formula for the compound, disulfur decafluoride?

a)

S2F 10

b)

SF5

c)

Na2F10

d)

S8F10

e)

S10F2

64.

What is the correct name for the compound, NF3?

a)

sodium trifluoride

b)

mononitrogen trifluoride

c)

trifluorine mononitride

d)

nitrogen trifluoride

e)

nitrogen fluoride

65.

What is the correct molecular formula for the compound, dinitrogen trioxide?

a)

NO3

b)

Na2O3

c)

N2O3

d)

N4O3

e)

N2O

66.

What is the correct molecular formula for the compound, tetraphosphorus decasulfide?

a)

P4S10

b)

P2S5

c)

PS

d)

P10S4

e)

K4S10

67.

What is the correct name for the compound, IF7?

a)

monoiodine heptafluoride

b)

iodine heptafluoride

c)

heptaiodine monofluoride

d)

iodine fluoride

e)

none of these are correct

68.

What type of ions do metals form?

a)

cations

b)

anions

69.

What types of ions do nonmetals form?

a)

cations

b)

anions

70.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
71.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
72.

How many valence electrons are shown in this Bohr diagram?

a)

2

b)

3

c)

5

d)

8

73.

How many valence electrons?

a)

2

b)

5

c)

8

d)

10

74.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

75.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
76.

Which of these is correct?

a)
b)
c)
77.

The element sulfur

a)

will lose two electrons to become stable

b)

will gain six electrons to become stable

c)

will lose six electrons to become stable

d)

will gain two electrons to become stable

78.

Electron dot diagrams are used to represent ____.

a)

atomic mass

b)

valence electrons

c)

protons

d)

the structure of the nucleus

79.

In a chemical formula, the number of each type of atom in the compound is shown by small numbers called ____.

a)

superscripts

b)

chemical symbols

c)

subscripts

d)

oxidation numbers

80.

The charges for metal ions are _______.

a)

positive

b)

covalent

c)

negative

d)

neutral

81.

Which of the following elements forms a negative ion in its ionic compounds?

a)

Mg, magnesium

b)

Cl, chlorine

c)

Al, aluminum

d)

Li, lithium

82.

The elements that make up a compound and the exact number of atoms of each element in a unit of the compound can be shown in a ____.

a)

chemical formula

b)

subscript

c)

superscript

d)

chemical symbol

83.

The charges for nonmetal ions are _______.

a)

neutral

b)

positive

c)

negative

d)

covalent

84.

Which of the following compounds will NOT have ionic bonds?

a)

CH4

b)

LiF

c)

NaCl

d)

MgF2

85.

Why do the noble gases NOT form compounds readily?

a)

They have empty outer energy levels

b)

They have no electrons

c)

They have seven electrons in the outer energy levels

d)

Their outer energy levels are completely filled with electrons

86.

a charged particle

a)

ion

b)

nucleus

c)

molecule

d)

multiple covalent bond

87.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
88.

What is a Lewis Dot Structure?

a)

It shows all of the particles in the atom.

b)

Contains protons and neutrons

c)

Only shows the element symbol and it's outer most electron shell

d)

Contains protons and electrons

89.

What element is this?

a)

Na

b)

P

c)

N

d)

S

90.

Why are both Hydrogen and Helium considered exceptions to the octet rule?

a)
Because they are noble gases
b)
Because they have more than 8 electrons in their outermost shell
c)
Because they have less than 8 electrons in their outermost shell
d)
Because they only require 2 electrons in their outermost shell to be stable

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