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Honors Chemistry Unit 4 - Test Review

Total questions: 65

Worksheet time: 2hrs 35mins

Name
Class
Date
1.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
2.
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
3.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)

Linear

b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
4.

How many unshared pairs of electrons will a trigonal pyramidal molecule have? 

a)
1
b)
2
c)
3
d)
4
5.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
6.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
7.

By replacing the element symbol, this could be a diagram of which element?

a)

Li

b)

Al

c)

C

d)

Be

8.

How many valence electrons should boron (B) have around its lewis dot structure?

a)

5

b)

6

c)

4

d)

3

9.

Select the correct Lewis structure for Li2O:

a)

b)

c)

d)

10.

What is the correct ABX formula for this molecule?

a)

AB4

b)

AX4

c)

AB3

d)

AB2X2

11.

How many of these are correct?

a)

1

b)

2

c)

3

d)

4-All

12.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
13.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
14.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
15.

How many pairs of electrons are shared between oxygen atoms in a molecule of O2?

a)

1

b)

2

c)

3

d)

4

16.

How many total electrons shared between nitrogen atoms in a molecule of N2?

a)

2

b)

3

c)

6

d)

9

17.

Which electron-dot diagram best represents a compound that contains both ionic and covalent bonds?

a)

A

b)

B

c)

C

d)

D

18.
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.
19.
There are more metals than non metals in the periodic table.
a)
True
b)
False
20.

What is electronegativity and how does it influence bonding between elements?

a)

Electronegativity is the measure of an atom's size and has no influence on bonding

b)

Electronegativity is the measure of an atom's ability to attract and hold electrons. It determines whether the bond will be ionic, polar covalent, or nonpolar covalent.

c)

Electronegativity is the measure of an atom's color and affects the strength of covalent bonds

d)

Electronegativity is the measure of an atom's mass and determines metallic bonding

21.

How does electronegativity predict the type of bonding between elements?

a)

Similar electronegativities form ionic bonds

b)

Electronegativity doesn't affect bonding type

c)

Similar electronegativities form covalent bonds, large differences form ionic bonds.

d)

Large differences in electronegativity form covalent bonds

22.

What are the properties of covalent substances?

a)

Gases, liquids, or soft solids; low melting and boiling points; do not conduct electricity

b)

Liquids; low melting and boiling points; conduct electricity

c)

Solids; high melting and boiling points; conduct electricity

d)

Gases; high melting and boiling points; conduct electricity

23.

What is the difference between intramolecular and intermolecular forces?

a)

Intramolecular forces are within a molecule, intermolecular forces are between molecules.

b)

Intramolecular forces are only in solids, intermolecular forces are only in gases.

c)

Intramolecular forces don't affect substance properties, intermolecular forces determine all properties.

d)

Intramolecular forces are between molecules, intermolecular forces are within a molecule.

24.

What is the role of valence electrons in covalent bonds?

a)

Valence electrons do not play a role in covalent bonds.

b)

Valence electrons are shared to form covalent bonds.

c)

Valence electrons are lost or gained in covalent bonds.

d)

Valence electrons determine the color of the compound.

25.

How does the difference in electronegativity between two atoms affect the bond's polarity?

a)

A large electronegativity difference results in a nonpolar bond.

b)

A small electronegativity difference results in a polar bond.

c)

A large electronegativity difference results in a polar bond.

d)

The electronegativity difference doesn't affect the bond's polarity.

26.

Which type of intermolecular force is the strongest: dipole-dipole, Van der Waals, or hydrogen bonding?

a)

Dipole-dipole

b)

Van der Waals

c)

Hydrogen bonding

d)

All are equally strong

27.

Why does hydrogen bonding occur only with nitrogen, oxygen, and fluorine?

a)

Because these elements have the highest electronegativities.

b)

Because these elements are the smallest in size.

c)

Because these elements have the highest ionization energies.

d)

Because these elements have the most valence electrons.

28.
The molecule shown in the diagram can best be classified as a
a)
polar covalent molecule
b)
nonpolar covalent molecule
c)
ionic compound
d)
nonpolar ionic compound
29.

In the polar covalent molecule of hydrogen chloride (HCl) - the chlorine atom has

a)

a lesser pull on electrons and therefore a positive charge.

b)

has a greater pull and therefore a negative charge.

c)

has no effect on charge because it is neutral.

d)

a lesser effect on valence electrons.

30.
How would you describe this structure?
a)
nonpolar and London forces
b)
polar and dipole-dipole forces
c)
polar and hydrogen bonding forces
d)
nonpolar and hydrogen bonding forces
31.

Is this molecule likely to dissolve in water? CCl4

a)

Yes

b)

No

32.

Classify the following molecule.

a)

polar

b)

nonpolar

33.

Which bond would be considered most Polar

a)

C-O

b)

O-H

c)

C-C

d)

C-Cl

34.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

35.

When you have C-H, what is the polarity?

a)

nonpolar

b)

polar

c)

ionic

36.
A diatomic molecule like O2 is always_______ because electrons are shared ________.
a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
37.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
38.

______ 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

39.

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.

40.
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
41.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
42.
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
43.

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

44.

A compound is made of two nonmetals. It is

a)

ionic

b)

metallic

c)

covalent

45.

Bonds formed by sharing electrons between atoms are

a)

ionic

b)

metallic

c)

covalent

d)

dipole-dipole

46.

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

a)

ionic

b)

metallic

c)

covalent

47.

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

a)

ionic

b)

metallic

c)

covalent

48.

Which compound is held together by opposite charges?

a)

NO2

b)

CaSO4

c)

Aluminum

d)

P4O10

49.

Which compound would have a very low melting point?

a)

sodium chloride

b)

copper (II) sulfate

c)

sulfur dioxide

d)

aluminum

50.

Which solid would be a good conductor?

a)

sodium chloride

b)

copper (II) sulfate

c)

glucose

d)

aluminum

51.

Which compound would be a good conductor when in solution?

a)

aluminum

b)

sulfur dioxide

c)

ammonia

d)

sodium nitrate

52.

What is electronegativity and how does it influence bonding between elements?

a)

Electronegativity is the measure of an atom's size and has no influence on bonding

b)

Electronegativity is the measure of an atom's ability to attract and hold electrons. It determines whether the bond will be ionic, polar covalent, or nonpolar covalent.

c)

Electronegativity is the measure of an atom's color and affects the strength of covalent bonds

d)

Electronegativity is the measure of an atom's mass and determines metallic bonding

53.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

54.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.4

b)

greater than 1.7

c)

between 0.4 and 1.7

d)

exactly 0

55.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
56.

What is the difference in electronegativity for 

SO2SO_2  ?

a)

0.5

b)

1.0

c)

2.0

d)

3.5

57.

H2OH_2O  has a difference in electronegativity of 1.4. Based on the table, what kind of bond is 

H2OH_2O ? 

a)

Nonpolar covalent

b)

Polar covalent

c)

Ionic

58.

NH3NH_3   is a polar covalent compound. Which atom, N or H, will electrons spend MORE time with?

a)

N

b)

H

59.

What is the difference in electronegativity for HBr?

a)

0.7

b)

1.9

c)

2.0

d)

2.8

60.

The electrons in a POLAR covalent bond are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

61.
Why do metals conduct
a)
They are shiny
b)
The electrons are held tightly within the lattice
c)
The electrons are delocalised and able to move
d)
The electrons are shared between two metal ions
62.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

63.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

64.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
65.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.

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