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Unit 3 Quiz

Total questions: 70

Worksheet time: 3hrs 46mins

Name
Class
Date
1.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
2.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
3.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
4.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
5.
What do you call a bond that forms when electrons are transferred from one atom to another?
a)
a compound bond
b)
an ionic bond
c)
a crystal bond
d)
an atomic bond
6.
Definition:  a regular, ordered arrangement of atoms, ions, or molecules
a)
crystal lattice
b)
atomic lattice
c)
ionic lattice 
d)
molecular lattice
7.
Which group of the periodic table is most stable (already has 8 valence electrons)?
a)
Alkali metals
b)
Transition metals
c)
Halogens
d)
Noble gases
8.
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.
9.
What does malleable mean?
a)
able to be shaped
b)
will break easily
c)
can be used for wire
d)
is shiny
10.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
11.
Metals like to ________ electrons.
a)
Gain
b)
Lose
c)
Anhilate
d)
Juggle
12.
According to VSEPR, molecules adjust their geometry 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
13.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
14.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
15.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
16.

What is the shape of an ammonia (NH3) molecule?

a)

Tetrahedral

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Octahedral

17.
SiCl4 has what shape?
a)
square planar
b)
square pyramidal
c)
tetrahedral
d)
octahedral
18.
How many lone pairs are in this molecule's structure?
a)
6
b)
2
c)
0
d)
4
19.
Will this molecule be polar or nonpolar? CCl4
a)
polar
b)
nonpolar
20.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
21.
What shape will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
22.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
23.
What geometry will this molecular structure have?: CS2
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
24.
The ammonia molecule (NH3) is a dipole because it contains _____.
a)
nonpolar bonds and is symmetrical
b)
nonpolar and is asymmetrical
c)
polar bonds and is asymmetrical
d)
polar bonds and is symmetrical
25.
Which IMFA is the predominant IMFA for non-polar molecules?
a)
London Dispersion Forces
b)
Dipole Dipole
c)
Hydrogen Bonding
d)
Both Dipole Dipole and Hydrogen Bonding
26.
Which bond has electrons that are shared equally?
a)
Non-polar ionic
b)
Non-polar covalent
c)
Polar covalent
d)
Ionic
27.
Is the molecule H2O polar or non-polar?
a)
polar
b)
non-polar
28.
Intermolecular force present in Cl2?
a)
permanent dipole-dipole
b)
H-bond
c)
london dispersion
d)
metallic
29.
The polarity of a bond between two elements can be best determined by
a)
The difference in electronegativity between the elements
b)
The difference in first ionization energy between the elements
c)
The number of electrons shared in the bond
d)
The difference in atomic radius between the elements
30.
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
31.
Which bond is most polar?
a)
H-F
b)
H-Cl
c)
H-Br
d)
H-I
32.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
33.

Hydrogen bonding is between hydrogen and another element. Which of these is NOT one of the elements?

a)

Fluorine

b)

Nitrogen

c)

Oxygen

d)

Carbon

34.

Intermolecular forces are between...

a)

different atoms

b)

different molecules

35.

Intarmolecular forces are between...

a)

different atoms

b)

different molecules

36.
What kind of bond forms between a cation and an anion?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
37.
What kind of bond forms between two nonmetals?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
38.
This type of model shows only the valence electrons of an element? 
a)
Bohr diagram 
b)
Childers model
c)
Lewis-dot diagram 
d)
What is a valence electron again?
39.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
40.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
41.
Which of these forces applies to all molecules
a)
London Dispersion
b)
Dipole dipole
c)
Hydrogen Bonding
d)
Covalent bonding
42.

In the Lewis structure for sulfur, how many dots should be around the symbol “S”?

a)

2

b)

3

c)

4

d)

6

e)

8

43.

Which of the following contains a double bond?

a)

C2H4

b)

H2

c)

OF2

d)

CF4

e)

OH-

44.

This is a correct dot diagram for neon (Ne)

a)

True

b)

False

45.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
46.

What is the ONLY part of the atom that makes a chemical bond

a)

Nucleus

b)

Electrons

c)

Valence Electrons

d)

Protons

47.

Which is the correct Lewis Dot Structure for NH3?

a)
b)
c)
48.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
49.

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

a)

4

b)

6

c)

8

d)

2

50.
Which of the following is the correct LD Diagram for Hydrogen Cyanide? HCN?
a)
A
b)
B
c)
C
d)
D
51.
Does H2O have hydrogen bonding?
a)
yes
b)
no
52.

Brass is an example of a/an ________________ alloy because zinc atoms replace copper atoms.

a)

substitutional

b)

interstitial

c)

eutetic

d)

vacancy

53.

Steel is an example of a/an _______________ alloy because carbon atoms move between the iron atoms’ crystal structure.

a)

eutetic

b)

interstitial

c)

substitutional

d)

vacancy

54.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
55.
Metallic bonding is...
a)
a type of covalent bond.
b)
a type of ionic bond.
c)
an attraction between positive ions and electrons.
56.
Which of these is NOT an alloy?
a)
bronze
b)
copper
c)
brass
d)
stainless steel
57.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
58.
What is the ability of a substance to allow heat, sound, or electricity to flow through it?
a)
Malleability
b)
Ductility
c)
Solubility
d)
Conductivity
59.

What intermolecular forces would exist between molecules of HF?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

Hydrogen Bonding

d)

All of the above

60.

What IMF would exist between molecules of BrF5?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

LDF and Dipole-Dipole Forces

d)

None

61.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
62.

For which of the following would hydrogen bonding occur between molecules?

a)
b)
c)
d)
63.
Which type of bond has one pair of electrons shared between atoms?
a)
ionic
b)
single covalent
c)
metallic
d)
double covalent
64.

Is this molecule polar or nonpolar?

a)

polar

b)

nonpolar

65.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
66.
Which two substances are covalent compounds?
a)
C6H12O6 (s) and KI (s)
b)
KI (s) and NaCl (s)
c)
C6H12O6 (s) and HCl (g)
d)
NaCl (s) and HCl (g)
67.
Which molecule contains a triple covalent bond between its atoms?
a)
N2
b)
O2
c)
F2
d)
H2
68.
Which compound contains only covalent bonds?
a)
NaOH
b)
Ba(OH)2
c)
Ca(OH)2
d)
CH3OH
69.
Which of the following most likely represents the molecular geometry of water?
a)
A
b)
B
c)
C
d)
D
70.
What kind of bond occurs between the carbons in C2H2?
a)
single
b)
double
c)
triple
d)
quadruple

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