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Bonding Test Review

Total questions: 50

Worksheet time: 55mins

Name
Class
Date
1.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

2.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
3.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
4.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
5.

How many electrons should Carbon have around its Lewis dot model?

a)

1

b)

3

c)

4

d)

5

6.

In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?

a)

1

b)

4

c)

3

d)

2

7.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
8.

Which of the following elements will NOT be surrounded by an octet of electrons in a correctly drawn Lewis structure?

a)

carbon

b)

oxygen

c)

chlorine

d)

hydrogen

9.

Which of the following is an ionic bond?

a)

H3N

b)

CaCl2

c)

NO2

d)

SCl

10.

How many valence electrons do elements in Group 2A have?

a)

12

b)

4

c)

1

d)

2

11.

Choose the structure that forms a double bond.

a)

Carbon monoxide (CO)

b)

Carbon dioxide (CO2)

c)

Water (H2O)

d)

Cyanic Acid (HCN)

12.

Choose the structure that forms a triple bond.

a)

Hydrogen

b)

Fluorine

c)

Oxygen

d)

Nitrogen

13.

How many valence electrons are in Phosphorus?

a)

15

b)

4

c)

5

d)

31

14.

How many electrons does each line indicate are shared?

a)

1

b)

2

c)

3

d)

4

15.
What is the first thing you need to do when drawing Lewis Structures?
a)
Draw your bonds
b)
Count the number of valence electrons
c)
Subtract to make the valence number even
d)
Add to make the valence number even
16.

After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?

a)

Place dots until everything has eight

b)

Place dots only around the terminal atoms

c)

Add a multiple bond

d)

Have eight only around the central atom

17.

How many covalent bonds does carbon need to form in order to have a full octet?

a)

2

b)

3

c)

4

d)

5

18.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

6

c)

8

d)

2

19.

The chemical formula for an ionic compound of potassium and oxygen is

a)

KO.

b)

K2O.

c)

K2O2.

d)

KO2.

20.

Which is most likely to form a negative ion?

a)

an element from group 7

b)

a metal

c)

an element from group 1

d)

an element with atoms that have eight valence electrons

21.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

22.

The name of CaI₂ is

a)

calcium iodine

b)

carbon iodide

c)

calcium (II) iodide

d)

calcium iodide

23.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithium (I) bromide

24.

What is the formula for magnesium phosphide?

a)

Mg3P2

b)

Mg2P3

c)

MgP

d)

Mg3(PO3)2

25.

Negative ions form when atoms _________ valence electrons.

a)

lose

b)

gain

c)

share

26.

Which of the following would produce an cation?

a)

O

b)

N

c)

K

d)

F

27.

Ions are:

a)

atoms with a positive or negative charge

b)

atoms with no charge

c)

atoms with ONLY a positive charge

d)

atoms with ONLY a negative charge

28.

Cations are

a)

positive

b)

negative

c)

on the right side of the periodic table.

d)

nonmetals

29.

This causes the mass of the nucleus to increase.

a)

adding an electron

b)

adding a neutron

c)

more orbitals

d)

adding negatively charged particles

30.

This particle determines what element you have - the elements identity.

a)

electron

b)

proton

c)

neutron

d)

valence shell

31.

Which particles make up the nucleus of an atom?

a)

protons and neutrons

b)

electrons and protons

c)

electrons, protons, and neutrons

d)

electrons and neutrons

32.

An atom has 10 protons, 12 neutrons and 10 electrons what is its mass number.

a)

12

b)

10

c)

20

d)

22

33.

Most of the mass of an atom is contained here.

a)

electron orbitals

b)

nucleus

c)

shells

d)

atomic #

34.

Which of the following molecules is the most polar?

a)

H − Cl

b)

H − Br

c)

H − I

d)

H − F

35.

Does the following reference Polar, Nonpolar, or both:

"slight positive and slight negative charge"?

a)

Polar

b)

Nonpolar

c)

Both

36.

water is a .............................. molecule.

a)

nonpolar

b)

polar

37.

Does the following reference Polar, Nonpolar, or both:

"electronegativity values are the same"?

a)

Polar

b)

Nonpolar

c)

Both

38.

Does the following reference Polar, Nonpolar, or both:

"unequal sharing of electrons"?

a)

Polar

b)

Nonpolar

c)

Both

39.

What is the correct formula for aluminium fluoride?

a)

Al3F3

b)

AlF

c)

Al3F

d)

AlF3

40.

Would an NO bond, be polar or nonpolar, or ionic?

The Electronegativity of N is 3.0

The Electronegativity of O is 3.5

a)

polar

b)

nonpolar

c)

ionic

41.
When naming an anion what suffix is added to the name?
a)
-ion
b)
-ate
c)
-ide
d)
-ite
42.
What is the correct name for FeBr2
a)
Iron Bromide
b)
Iron (II) Bromine
c)
Iron (II) Bromide
d)
Iron Bromide (II)
43.
Name the ionic compound SnSe2
a)
Tin diselenide
b)
Tin (IV) selenide
c)
Tin selenide
d)
Tin (II) selenide
44.
iron(II) oxide
a)
FeO
b)
FeO2
c)
Fe2O
d)
Fe2O2
45.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
46.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

London dispersion forces

c)

Hydrogen Bonds

47.
A molecule containing polar covalent bonds is always polar.
a)
True
b)
False
48.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
49.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
50.

What explains the very high melting and boiling point of water?

a)

Dipole-dipole forces between water molecules

b)

Hydrogen bonds between water molecules

c)

Van Der Waals forces between water molecules

d)

Molecule-ion attractions between water molecules

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