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Bonds and Electronegativity

Total questions: 77

Worksheet time: 3hrs 35mins

Name
Class
Date
1.

How many atoms are in Zinc acetate?

a)

12

b)

15

c)

20

d)

14

2.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
3.
What is the charge on the hydroxide ion?
a)
0
b)
-1
c)
-2
d)
-3
4.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
5.

How many atoms total are in AlPO4?

a)

4

b)

5

c)

6

d)

7

6.

How many atoms total are in NaOH?

a)

1

b)

2

c)

3

d)

4

7.
What is the formula for sodium nitrate?
a)
Na3NO
b)
NaNO
c)
Na3NO3
d)
NaNO3
8.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
9.
Find the formula zinc sulfate
a)
ZnSO3
b)
ZnSO4
c)
ZnS
d)
Zn(SO4)2
10.
What is the formula for copper (II) hydroxide?
a)
CuOH
b)
Cu(OH)2
c)
Cu2OH
d)
Cu2O
11.
What does this image represent?
a)
Atom
b)
Element
c)
Molecule
d)
Marshmallows
12.
Carbon dioxide (CO2) contains how many atoms of oxygen?
a)
0
b)
1
c)
2
d)
3
13.

Which term represents the attraction one atom has for the electrons in a bond with another atom?

a)

(1) electronegativity

b)

(2) electrical conductivity

c)

(3) first ionization energy

d)

(4) mechanical energy

14.

In a bond between an atom of carbon and an atom of fluorine, the fluorine atom has a

a)

(1) weaker attraction for electrons

b)

(2) stronger attraction for electrons

c)

(3) smaller number of first-shell electrons

d)

(4) larger number of first-shell electrons

15.

Which element has an atom with the greatest tendency to attract electrons in a chemical bond?

a)

carbon

b)

chlorine

c)

silicon

d)

sulfur

16.

Use your knowledge and electronegativity sheet to predict what type of bond would form between phosphorus and flourine

a)

Ionic

b)

Polar Covalent

c)

Non polar Covalent

d)

Metallic

17.

Use your knowledge and electronegativity sheet to predict what type of bond would form between calcium and bromide?

a)

Non polar Covalent

b)

Polar Covalent

c)

Ionic

d)

Metallic

18.

Electronegativity is a measurement of the ability of a nucleus to_____________.

a)

attract bonding electrons

b)

attract other nuclei

c)

attract electrons in the non valence energy

19.

Which of the following formulas represents a polar molecules?

a)

CO2

b)

CCl4

c)

H2

d)

H2O

20.

In covalent bonds, electrons are ___________________

a)

shared

b)

gained

c)

transferred

d)

lost

21.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
22.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
23.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

24.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
25.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
26.
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
27.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

28.

What type of bonding does this picture show?

a)

Ionic

b)

Covalent

29.
Magnesium (Mg) and Oxygen (O) form an ________ bond.
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nothing
30.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

31.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
32.

Which bond type is associated with a large difference in electronegativity?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Hydrogen bond

33.

What is the main characteristic of a covalent bond?

a)

Electron transfer

b)

Electron sharing

c)

Proton transfer

d)

Neutron sharing

34.

Which type of bond involves the sharing of electrons?

a)

Ionic Bonds

b)

Covalent Bonds

c)

Metallic Bonds

d)

Hydrogen Bonds

35.

Covalent compounds usually do not:

a)

Dissolve in water

b)

Conduct electricity

c)

React with acids

d)

Form gases

36.

Which of the following is an example of a covalent compound?

a)

Sodium chloride (NaCl)

b)

Water (H2O)

c)

Magnesium oxide (MgO)

d)

Calcium carbonate (CaCO3)

37.

What is a characteristic of ionic compounds regarding their melting and boiling points?

a)

Low melting and boiling points

b)

High melting and boiling points

c)

No melting and boiling points

d)

Variable melting and boiling points

38.

What is the key characteristic of the ions formed in ionic bonds?

a)

They are neutral

b)

They are oppositely charged

c)

They are positively charged only

d)

They are negatively charged only

39.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

40.

In metallic bonds electrons are:

a)

shared

b)

move around the nuclei randomly

c)

transferred

41.

Malleability and ductility are characteristics of compounds with

a)

covalent bonds

b)

metallic bonds

c)

ionic bonds

d)

alloy bonds

42.

Why are metals good conductors?

a)

they have mobile electrons

b)

they have mobile atoms

c)

they have crystal structures that can rearrange

d)

they have mobile protons

43.

Malleability means

a)

the ability to be drawn into a wire

b)

the electrons of metals are mobile

c)

the ability to be hammered into a shape

d)

the ability to be a conductor of electricity

44.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
45.

Why do metals conduct heat and electricity?

a)

They are shiny

b)

The electrons are held tightly within the lattice

c)

The electrons are delocalised and able to freely move (in the sea)

d)

The electrons are shared between two metal ions

46.
What does malleable mean?
a)

able to be shaped

b)

will break easily

c)

can be used for wire

d)

is shiny

47.

CHECK ALL THAT APPLY:

Electronegative atoms that are often involved in Hydrogen Bonds.

a)

Nitrogen

b)

Carbon

c)

Oxygen

d)

Fluorine

e)

Calcium

48.

Why don't noble gases form bonds?

a)

They all have a full octet

b)

Noble gases do form bonds

c)

They only bond when with eachother

d)

none of these answers are correct

49.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

50.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

51.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
52.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
53.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
54.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
55.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
56.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

57.

Silicon dioxide is the compound in sand. What is its formula?

a)

SO2

b)

NaO2

c)

SiO2

d)

SiO

58.

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

59.

a type of covalent bond that shares two pairs of electron

a)

single bond

b)

double bond

c)

triple bond

60.

Which particle is responsible for bonding?

a)

Electrons

b)

Protons

c)

Nucleus

d)

Neutrons

61.

Which element is most likely to form 2 bonds?

a)

Carbon

b)

Fluorine

c)

Nitrogen

d)

Sulfur

62.

Which of the following is a characteristic property of ionic compounds?

a)

They form crystalline solids and have low melting points.

b)

Form solids and gases at room temperature.

c)

They form hard crystals with high melting points.

d)

They are generally gases with extremely high boiling points.

63.

What kind of bond would form between 2 oxygen atoms

a)

Ionic

b)

Polar Covalent

c)

Metallic

d)

Nonpolar Covalent

64.
Question Image

Match the three types of chemical bonds.

a)

A

1.

Ionic

b)

B

2.

Covalent

c)

C

3.

Metallic

65.

What element is more positive in the models given for water and ammonia?

a)

Oxygen

b)

Nitrogen

c)

Hydrogen

66.

What is shared in covalent bonds?

a)

Electrons

b)

Metals

c)

Nonmetals

d)

Protons

e)

Neutrons

67.
Question Image

Match the following

a)

A

1.

Ionic Bond

b)

B

2.

Polar Covalent Bond

c)

C

3.

Nonpolar Covalent Bond

68.

What bond type do the molecules circled have?

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

d)

Metallic

69.

What bond type do the molecules circled have?

a)

Ionic

b)

Metallic

c)

Polar Covalent

d)

Nonpolar Covalent

70.
Question Image

Match the model with its bond type.

a)

Ionic Bond

1.

c

b)

Nonpolar Covalent Bond

2.

a

c)

Polar Covalent Bond

3.

b

71.

What type of bond does water have? Select TWO.

a)

Nonpolar

b)

Polar

c)

Covalent

d)

Ionic

e)

Metallic

72.

What does this picture illustrate? (Select all that apply)

a)

Sharing valence electrons

b)

Covalent bonding

c)

transferring valence electrons

d)

ionic bonding

e)

two nonmetals

73.

How do covalent bonds form?

a)

Donating & receiving valence electrons between atoms

b)

Oppositely charged ions attract each other & form bonds

c)

Scientists are still not sure how they form

d)

Sharing valence electrons between atoms

74.

How many covalent bonds are created in a single water molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

75.

How many covalent bonds are created in a single ammonia molecule?

a)

0

b)

1

c)

2

d)

3

e)

4

76.

How many pairs of valence electrons are being shared in a single water molecule?

a)

0 pair - 0 valence electrons

b)

1 pair - 2 valence electrons

c)

2 pair - 4 valence electrons

d)

3 pair - 6 valence electrons

77.

Match the covalent bond types.

a)

1.

Single Bond

b)

2.

Double Bond

c)

3.

Triple Bond

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