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Chemical Bonding

Total questions: 110

Worksheet time: 6hrs 30mins

Name
Class
Date
1.

A covalent bond is formed between two non- (a)   that have similar electronegativities.

2.

Bonding which results from the electrical attraction between cations and anions

a)

hydrogen bonding

b)

covalent bonding

c)

metallic bonding

d)

ionic bonding

3.

ability of a substance to be drawn or pulled through a small opening to make a wire

_ _ _ _ _ _ _ _

(a)  

4.

which compound/s has covalent bond

i. NaOH

ii. Na2SO3

iii. O2

iv. CO2

a)

i and ii

b)

ii and iii

c)

iii and iv

d)

i and iv

5.

ability of a substance to be hammered into thin sheets

_ _ _ _ _ _ _ _ _ _ _ _

(a)  

6.

factor to identify the type of bond (ionic and covalent)

i. Octet rule

ii. electronegativity

iii. conductivity

a)

i and ii

b)

i and iii

c)

II and III

d)

i, II and III

7.

The electronic structures of atoms P and Q are shown. P and Q react to form an ionic compound. What is the formula of this compound?

a)

Q2P

b)

P2Q

c)

P2Q6

d)

Q2P6

8.

The electronic configuration of an ion is 2.8.8. What could this ion be?

a)

A

b)

B

c)

C

d)

D

9.

How many electrons are shared between the atoms in a molecule of methane, CH4, and in a molecule of water, H2O?

a)

Methane = 4

Water = 2

b)

Methane = 4

Water = 4

c)

Methane = 8

Water = 2

d)

Methane = 8

Water = 4

10.

The diagram shows the positions of some elements in the Periodic Table. Which elements form ionic bonds with oxygen?

a)

W only

b)

W and X only

c)

Z only

d)

Y and Z only

11.

The diagram shows an outline of part of the Periodic Table. Which two elements could form a covalent compound?

a)

W and X

b)

W and Y

c)

X and Y

d)

X and Z

12.

The proton numbers of four elements are shown. Which element forms a singly charged positive ion in its salts?

a)

A (proton number = 34)

b)

B (proton number = 35)

c)

C (proton number = 36)

d)

D (proton number = 37)

13.

Which compound has ionic bonds?

a)

hydrogen chloride

b)

methane

c)

sodium chloride

d)

water

14.

The following list the electronic structures of four atoms:

W : 2, 1

X : 2, 7

Y : 2, 8, 4

Z : 2, 8, 8


Which two atoms combine to form an ionic compound?

a)

W and X

b)

W and Y

c)

X and Y

d)

X and Z

15.

The following shows the electron structures of four elements.

W = 2, 6

X = 2, 8

Y = 2, 8, 1

Z = 2, 8, 7


Which pair of atoms will form a covalent substance?

a)

two atoms of W

b)

two atoms of X

c)

an atom of W and two atoms of Y

d)

an atom of Y and an atom of Z

16.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
17.
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
18.
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
19.
The bonds in Na2O are best described as 
a)
a.  covalent, because valence electrons are shared.
b)
covalent, because valence electrons are transferred
c)
ionic, because valance electrons are shared.
d)
ionic, because valance electrons are transferred. 
20.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
21.
a)

A

b)

B

c)

C

d)

D

22.
a)

A

b)

B

c)

C

d)

D

23.
a)

A

b)

B

c)

C

d)

D

24.
a)

A

b)

B

c)

C

d)

D

25.
a)

A

b)

B

c)

C

d)

D

26.
a)

A

b)

B

c)

C

d)

D

27.
a)

A

b)

B

c)

C

d)

D

28.
a)

A

b)

B

c)

C

d)

D

29.
a)

A

b)

B

c)

C

d)

D

30.
a)

A

b)

B

c)

C

d)

D

31.
a)

A

b)

B

c)

C

d)

D

32.
a)

A

b)

B

c)

C

d)

D

33.
a)

A

b)

B

c)

C

d)

D

34.
a)

A

b)

B

c)

C

d)

D

35.

Among the elements below, the most stable element is....

a)

8P

b)

9Q

c)

10R

d)

12S

36.

It is known that the electron configuration of atom X: 2.8.5 the atom will be stable if..

a)

binds 3 electrons 7

b)

lose 5 electrons

c)

bind 5 electrons

d)

uses 4 pairs of electrons

37.

The arrangement of the valence electrons for noble gases is octet, except...

a)

Ar

b)

Ne

c)

Cr

d)

He

38.

Which of the following is not a coordination covalent compound?

a)

H2SO4

b)

NH4Cl

c)

HNO3

d)

H2O

39.

Which of the following has the most stable energy?

a)

N

b)

S

c)

O2

d)

He2

40.

The bond formed by the sharing of a shared pair of electrons from one atom that has a lone pair of electrons is...

a)

single covalent bond

b)

double covalent bond

c)

polar covalent bond

d)

coordintion covalent bond

41.

In bonding, which atoms are allowed to deviate from the octet rule...

a)

S

b)

O

c)

N

d)

C

42.

Pairs of compounds of the following elements: 6K, 8L, 15M, 17Q, 9R satisfy the octet rule except...

a)

KL2 dan KQ4

b)

KQ4 dan Q₂L

c)

MQ5 dan KL

d)

MQ3 dan KR4

43.

The following compounds do not comply with the octet or duplet rule.

a)

NH3

b)

BF3

c)

BCl3

d)

SF6

44.

The following are elements which, when bound, will follow the duplet rule, except….

a)

9J

b)

3L

c)

4G

d)

1K

45.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
46.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
47.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
48.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
49.
Predict the bond that will form between Se and Cl
a)
Ionic
b)
Covalent
50.
Using electronegativities, what type of bond is formed by S and Br.
a)
ionic
b)
polar covalent
c)
non-polar covalent
51.
Using electronegativities, what type of bond is formed by Co and F.
a)
ionic
b)
polar covalent
c)
non-polar covalent
52.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
53.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
54.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
55.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
56.
Soluble in Water
a)
Ionic
b)
Covalent
57.
High Melting & Boiling Points
a)
Ionic
b)
Covalent
58.
Relatively soft
a)
Ionic
b)
Covalent
59.

It involves the transfer of electron from metals to nonmetals.

a)

Ionic bonding

b)

Covalent bonding

c)

Metallic bonding

d)

Intermolecular Forces of Attraction

60.

Which of the following pair of atoms has a complete valence electrons?

a)

sodium

b)

silicon

c)

sulfur

d)

argon

61.

What is the chemical formula when sodium ions combines with a sulfide ion?

a)

NaS

b)

NaS2

c)

Na2S

d)

Na2S2

62.

The electronegativity difference between fluorine and oxygen is 0.5. The type of bond present is _____.

a)

ionic

b)

polar covalent

c)

nonpolar covalent

d)

metallic

63.

Which of the following compounds will have the highest melting point?

a)

pure iron

b)

sodium chloride

c)

water

d)

carbon dioxide

64.

Covalent bonding involves the sharing of electrons between _____.

a)

metals and nonmetals

b)

nonmetals

c)

metals

d)

metals and metalloids

65.

What is the chemical name of Na2O

a)

sodium oxide

b)

sodium (II) oxide

c)

disodium oxide

d)

disodium monoxide

66.

What is the chemical formula of aluminum carbonate

a)

Al2CO3

b)

AlCO3

c)

Al2(CO3)3

d)

Al3(CO3)2

67.

What is the chemical name of SF6

a)

sulfur fluoride

b)

sulfur hexafluoride

c)

monosulfur hexafluoride

d)

sulfur (VI) fluoride

68.

Which of the following compounds contains covalent bonding?

a)

LiF

b)

H2S

c)

NaOH

d)

Mg

69.
________ molecules are found in nature as single atom elements
a)
polyatomic
b)
monatomic
c)
elemental
d)
diatomic
70.

______ molecules are found in nature as pairs of two atoms of the same type covalently bonded together.

a)

Diatomic

b)

Monatomic

c)

Polyatomic

d)

Network

71.

Which of the following types of elements can exist in monatomic form?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases

72.

Which of the following types of elements can exist in nature as diatomic molecules?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases.

73.
Why do bonds form?
a)
To fill the valence shell of electrons for the elements involved
b)
to release energy stored in the bonds
c)
because whenever you mix two chemicals, there will be a reaction
d)
because of attraction
74.
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
75.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
76.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
77.

A mixture of two or elements at least one of which is a metal is called

a)

an ion

b)

an alloy

c)

steel

d)

a crystal

78.

Bonds formed by transferring electrons from one atom to another are

a)

ionic

b)

metallic

c)

non polar covalent

d)

covalent

79.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

80.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

81.

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

a)

ionic

b)

metallic

c)

covalent

82.

Ionic compounds are held together by

a)

intermolecular forces

b)

electrostatic forces

c)

magnetic forces

d)

nuclear forces

83.

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

a)

ionic

b)

metallic

c)

covalent

84.

Which compound is held together by electrostatic forces?

a)

NO2

b)

CaSO4

c)

Aluminum

d)

P4O10

85.

Which compound would have a very low melting point?

a)

sodium chloride

b)

copper (II) sulfate

c)

sulfur dioxide

d)

aluminum

86.

Which solid would be a good conductor?

a)

sodium chloride

b)

copper (II) sulfate

c)

glucose

d)

aluminum

87.

Which compound would be a good conductor when in solution?

a)

aluminum

b)

sulfur dioxide

c)

ammonia

d)

sodium nitrate

88.

Which of the following can exist in monatomic form?

a)

Oxygen

b)

Copepr

c)

Sodium

d)

Argon

89.

Predict the bond that is formed between Phosophorus and Chlorine?

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

90.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

91.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

92.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of a strong ionic bond.

a)

TRUE

b)

FALSE

93.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
94.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
95.
The ability of a material to be shaped in all directions without cracking or breaking.
a)
hardness
b)
ductility
c)
malleability
d)
conductivity
96.

Examine the image: How many bonds are formed looking at the model of the compound? And also indetify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

97.

Which of the following is true for ionic bonding & ionic compounds?

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.

98.

How many single bonds will carbon look to make when it bonds covalently?

a)

2

b)

3

c)

4

d)

5

99.

Which of the following elements does NOT form an ion with a charge of 2+?

a)

Beryllium

b)

Strontium

c)

Magnesium

d)

fluorine

100.

When Alkali metals (Group 1) form ions, they ____.

a)

lose 1 proton

b)

gain 1 proton

c)

lose 1 electron

d)

gain 1 electron

101.

How does fluorine (F) obey the octet rule when reacting to form compounds?

a)

It doesn’t change its number of electrons

b)

Fluorine does not obey the octet rule.

c)

It gains electrons.

d)

It gives up electrons.

102.

Which of the following pairs of elements is most likely to form an ionic compound?

a)

magnesium and fluorine

b)

manganese and iron

c)

oxygen and chlorine

d)

sodium and aluminum

103.

Which of the following shows correctly an ion pair and the ionic compound the two ions form?

a)

Sn4+ and N3- form Sn4N3

b)

Cu2+ and O2- form Cu2O2

c)

Cr3+ and I- form CrI

d)

Cr2+ and I- form CrI2

104.

How many valence electrons are transferred from the sodium atom to fluoride in the formation of the compound sodium fluoride?

a)

0

b)

1

c)

2

d)

3

105.

What is the chemical formula of sodium nitride?

a)

NaN

b)

Na2N

c)

Na3N

d)

NaN3

106.

Select the correct formula for boron trichloride.

a)

B2Cl

b)

B3Cl

c)

BCl3

d)

BCl2

107.

From the following compounds, which group is ionic compound?

a)

SO2, NO2, and CO2

b)

KOH, CN and H2S

c)

NaCl, MgBr2, and K2O

d)

NH3, H2O, and SO3

e)

HCl, NaI, and CH4

108.

The atomic number of atom

A = 3, B = 4, C = 17, D = 21, E = 23 and F = 30.

The elements that can form ionic compounds are

a)

A with F

b)

A with E

c)

A with D

d)

B with E

e)

A with C

109.

The pair of compounds below which both ionic compounds are ...

a)

NaCl and KBr

b)

CH4 and NH3

c)

SO2 and HCl

d)

H2O and KBr

e)

KCl and HCl

110.

Atom with atomic number 19 can form ionic compound with atom with atomic number ... .

a)

16

b)

17

c)

18

d)

20

e)

21

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