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Bonding and Nomenclature Practice

Total questions: 36

Worksheet time: 26mins

Name
Class
Date
1.

Why do all bonds form?

a)

to fill the outermost energy level

b)

so an atom can be unstable

c)

so the number of protons and electrons can equal.

d)

so they can gain neutrons.

2.

Valence electrons are found

a)

outermost energy level

b)

innermost energy level

c)

some where in the electron cloud

3.

An atom with 1 valence electron 'needs' a full shell, so it can either gain 7 electrons or lose 1. Which is more likely to occur?

a)

nothing

b)

gain 7

c)

lose 1

4.

How do covalent bonds form?

a)

by sharing electrons between atoms

b)

by donating or receiving electrons

5.

What two types of atoms make a covalent bond?

a)

2 nonmetals

b)

2 metals

c)

1 metal and 1 nonmetal`

6.

How many valence electrons does Boron have?

a)

1

b)

2

c)

3

d)

4

7.

Ionic bonds are between

a)

metals and nonmetals

b)

2 metals

c)

2 nonmetals

8.

Atoms are most stable when their outer shell is full or complete.

a)

true

b)

false

9.

How are ionic bonds formed?

a)

transfer of electrons

b)

sharing of electrons

10.

Group numbers on the periodic table help us determine

a)

number of valence electrons

b)

state of the element (solid, liquid, gas)

11.

Electrons are involved in chemical reactions, not protons or neutrons.

a)

true

b)

false

12.

Water is an example of what?

a)

covalent compound

b)

ionic compound

13.

Salt (NaCl) is an example of what?

a)

ionic compound

b)

covalent compound

14.

Atoms involved in a covalent bond are not charged, while atoms involved in an ionic bond are charged (negative or positive)

a)

true

b)

false

15.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
16.
How many valence electrons does hydrogen have?
a)
1
b)
2
c)
3
d)
4
17.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
18.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
19.
This is a correct dot diagram for neon (Ne)
a)
true
b)
false
20.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
21.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
22.
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
23.
How many valence electrons do most atoms need to be stable?
a)
1
b)
2
c)
6
d)
8
24.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
25.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
26.
What is oxidation number of H in H2O?
a)
0
b)
-2
c)
-1
d)
+1
27.
What is oxidation number of Fe in FeO ?
a)
+2
b)
-2
c)
0
d)
+1
28.

What is the correct formula for a compound formed from Na + and S -2

a)

Na2S

b)

NaS2

c)

Na2S2

d)

NaS

29.

What is the correct formula for a compound formed from the ions K + and N-3

a)

KN

b)

KN3

c)

K3N3

d)

K3N

30.

What is the oxidation number of magnesium in magnesium chloride (MgCl2)?

a)

+2

b)

-2

c)

12

d)

0

31.

Zinc fluoride

a)

ZnF2

b)

Zn2F

c)

ZnF

d)

Zn2F4

32.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

33.

When naming ionic compounds, the metal is always named first and the nonmetal is always named second.

a)

True

b)

False

34.

Write the correct formula for Sodium Chloride.

a)

SC

b)

SCl

c)

NaCl

d)

NaCl2

35.

What is the proper name for CH4?

a)

Monocarbon hydride

b)

Carbon tetrahydride

c)

Monocarbon tetrahydride

36.

What is the proper name for S2O2?

a)

Sulfur oxide

b)

Sulfur dioxide

c)

Sulfur (II) oxide

d)

Disulfur dioxide

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