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CHEMISTRY UNit 4 Bonding PRE/POST Test

Total questions: 29

Worksheet time: 48mins

Name
Class
Date
1.
All of the elements in the same group (column) have EQUAL numbers of _______.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
2.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
3.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
4.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
d)
noble gases
5.
Which type of bond has one pair of electrons shared between atoms?
a)
ionic
b)
single covalent
c)
metallic
d)
double covalent
6.
Which bond is the strongest bond?
a)
single covalent bond
b)
double covalent bond
c)
triple covalent bond
d)
quadruple covalent bond
7.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The number of electrons in the outermost energy level
c)
electrons closest to the nucleus
d)
electrons unbonded to a nucleus
8.
Compared to ionic compounds, molecular or covalent compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
9.

A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?

a)

2

b)

3

c)

4

d)

6

10.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
11.
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
12.
A covalent bond in which electrons are shared unequally is:
a)
polar
b)
a double bond
c)
ionic
d)
polyatomic
13.

In the correct Lewis Structure for methane (CH4), how many lone pairs electrons can be found around Carbon?

a)

0

b)

2

c)

4

d)

8

14.
Each element wants to gain or lose electrons so that it can have the same electron configuration as......
a)
a Noble gas
b)
other elements in its family
c)
other elements in its period
d)
it used to have before reacting
15.

Which of the following describes water (H2O)?

a)
Linear structure, nonpolar
b)
Linear structure, polar
c)
Bent structure, nonpolar
d)
Bent structure, polar
16.

How many lone pairs are on the central atom in ammonia (NH3)?

a)
0
b)
1
c)
2
d)
3
17.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
18.

What kind of bond do you have: F and Cl

Fluorines electronegativity = 4.0

Chlorines electronegativity = 3.0

a)

Non-polar covalent

b)

Polar covalent

c)

ionic

d)

James Bond

19.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
20.

What geometry will this molecule have?

a)

pyramidal

b)

tetrahedral

c)

trigonal planar

d)

bent

21.

Which statement below is correct about the image?

a)

This is an ionic bond where the metal is giving an electron to a nonmetal

b)

This is a covalent bond where the metal is giving an electron to a nonmetal

c)

This is an ionic bond where the nonmetal is giving an electron to a metal

d)

This is a covalent bond where the elements are sharing electrons

22.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
23.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
24.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
25.

What is the correct lewis dot diagram for Boron?

a)
b)
c)
d)
26.

How many covalent bonds can Carbon make?

a)
1
b)
3
c)
4
d)
5
27.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

28.
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.
29.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities

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