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.2 Optional Test 6 Review

Total questions: 145

Worksheet time: 4hrs 14mins

Name
Class
Date
1.
What is the correct term for "bond that forms when electrons are shared equally"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
2.
What is the correct term for "bond that forms between a metal and a nonmetal"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
3.
What is the correct term for "bond that forms when electrons are shared unequally"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
4.
Using the diagram of carbon dioxide, determine how many valence electrons each oxygen has after bonding with the carbon atom.
a)
8
b)
6
c)
4
d)
2
5.
Which compound contains covalent bonds?
a)
NaI
b)
K2O
c)
N2O3
d)
BeO
6.
Which two elements would form an ionic bond?
a)
carbon and hydrogen
b)
oxygen and silicon
c)
cesium and iodine
d)
potassium and calcium
7.
Which is not a property of ionic compounds?
a)
They are formed when nonmetals bond to nonmetals.
b)
They form crystals.
c)
They dissolve in water.
d)
They have high melting points.
8.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
9.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
10.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
11.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
12.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
13.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
14.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
15.
The correct name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
16.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
17.
Is hydrogen considered a metal or a non-metal?
a)
metal
b)
nonmetal
c)
metalloid
d)
nothing at all!
18.
What is the correct formula for dichlorine monoxide?
a)
Co₃O
b)
ClO₂
c)
Cl₂O
d)
(Cl₂)₂O
19.

What is the name of AlPO4?

a)

Aluminum phosphoxie

b)

Monoaluminum tetraphosphate

c)

Aluminum (III) phosphate

d)

Aluminum phosphate

20.
What is the name of NH4Cl?
a)
nitrogen tetrahydrogen chloride
b)
ammonium chlorine
c)
ammonium chloride
d)
ammonium chlorate
21.

What is the correct IUPAC name for Cu2O ?

a)

Copper oxide

b)

Copper oxalate

c)

Copper (II) oxide

d)

Copper (I) oxide

22.

What is the correct chemical formula for magnesium iodide?

a)

MgI2

b)

Mg2I

c)

MgI

d)

Mg2I2

23.

What is the proper IUPAC name of the compound P3O5?

a)

Triphosphorus pentoxide

b)

Phosphorus pentoxide

c)

Triphosphorus oxide

d)

Phosphorus oxide

24.

What is the correct IUPAC formula for aluminum sulfide?

a)

Al3S2

b)

Al2S

c)

AlS2

d)

Al2S3

25.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
26.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
27.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
28.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
29.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
30.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
31.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
32.
The name of the compound NH4F is
a)
Nitrogen hydrogen fluorine
b)
Ammonium Fluoride
c)
Ammonia Fluoride
d)
Nitrogen tetrahydride fluoride
33.
The name of Al₂(SO₄)₃ is
a)
aluminum sulfur oxide
b)
aluminum sulfate
c)
aluminum trisulfate
d)
aluminum (III) sulfate
34.
The name of Ca₃(PO₄)₂ is
a)
calcium phosphide oxide
b)
calcium phosphate
c)
tricalcium diphosphate
d)
carbon phosphate
35.
The name of Fe(OH)₂ is
a)
iron oxide
b)
iron hydroxide
c)
iron (II) hydroxide
d)
iron dihydroxide
36.
The chemical formula of sodium sulfate is
a)
S₂SO₄
b)
NaSO₂
c)
NaSO₄
d)
Na₂SO₄
37.
What is the NAME of....
Na2S
a)
sodium (II) sulfide
b)
sodium sulfide
c)
disodium sulfide
d)
sodium sulfur
38.
The correct name of Mg₃N₂ is
a)
manganese nitride
b)
magnesium nitride
c)
magnesium (III) nitride
d)
trimagnesium dinitride
39.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
40.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
41.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
42.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
43.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
44.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
45.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
46.

Is this the correct structure for CH2O?

a)

Yes

b)

No

47.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
48.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
49.
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
50.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
51.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

52.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

53.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

54.

In HCN (Carbon is usually the central atom) what kind of bond is between the C and N

a)

Single

b)

Double

c)

Triple

55.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
56.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
57.
In a Lewis structure, what do you do  with the total number of valence if your ion is + charged?
a)
Divide the valence number by 1
b)
Multiply the valence number by 1
c)
Add 1 to the valence number
d)
Subtract 1 from the valence number
58.
In a Lewis structure, what do you do  with the total number of valence if your ion is 2- charged?
a)
Add 2 to the valence number
b)
Subtract 2 from the valence number
c)
Multiply the valence number by 2
d)
Divide the valence number by 2
59.
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
60.
Choose the structure that forms a double bond.
a)
Carbon monoxide (CO)
b)
Carbon dioxide (CO2)
c)
Water (H2O)
d)
Cyanic Acid (HCN)
61.
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
62.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
63.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
64.
For carbonate ions, how many resonance structures can be drawn ?
a)
2
b)
3
c)
4
d)
5
65.
For carbonate ions, what is the bond strength between C and O
a)
C-O (single bond)
b)
C=O (double bond)
c)
C≡O (triple bond)
d)
C-O(between single and double bond)
66.
How many resonance structures for NO3- ion?
a)
1
b)
2
c)
3
d)
4
67.
What is the bond strength between N and O?
a)
N-O (Single bond)
b)
N=O (double bond)
c)
N Ξ O (Triple bond)
d)
N-O (between single and double bond)
68.
How many resonance structure for SO2 ?
a)
1
b)
2
c)
3
d)
4
69.
What is the bond strength between S and O?
a)
1
b)
1.5
c)
2
d)
3
70.

What is the name for when more than one valid Lewis structure can be drawn for a molecule?

a)

coordinate covalent bond

b)

resonance

c)

endothermic

d)

structural formula

71.
Partial charges like the ones shown here are called:
a)
dipoles
b)
deltas
c)
ions
d)
magnetic poles
72.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
73.
 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
74.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
75.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
76.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
77.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
78.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
79.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

80.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
81.
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .
a)
eg = tetrahedral, mg = tetrahedral
b)
eg = linear, mg = linear
c)
eg = octahedral, mg = square planar
d)
eg = trigonal bipyramidal, mg = tetrahedral
82.

Is this molecule polar?

a)

Yes

b)

No

83.

Is this molecule polar?

a)

No

b)

Yes

84.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
85.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
86.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
87.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
88.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
89.
What is the bond angle for this molecule?
a)
109.5
b)
120
c)
107
d)
90
90.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
91.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
92.
What is the molecular shape of a silicon dioxide molecule?
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
93.
Determine the molecular shape of carbon tetrafluoride.
a)
linear
b)
trigonal planar
c)
bent
d)
tetrahedral
94.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
95.
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
96.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
97.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
98.
What is the molecular geometry of OF2?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Planar
99.
What is the geometric configuration of CO2? 
a)
Bent 
b)
Trigonal planar
c)
Trigonal pyramidal
d)
Linear 
100.

What molecular geometry is shown?

a)

linear

b)

bent

c)

trigonal planar

d)

pyramidal

101.

What molecular geometry is shown?

a)

linear

b)

bent

c)

trigonal planar

d)

pyramidal

102.

What is the molecular geometry if the central atom has:


3 bonding and 1 nonbonding domains

a)

trigonal pyramidal

b)

trigonal planar

c)

tetrahedral

d)

bent

103.

What is the molecular geometry if the central atom has:


2 bonding and 2 nonbonding domains

a)

trigonal pyramidal

b)

trigonal planar

c)

tetrahedral

d)

bent

104.

What is the molecular geometry if the central atom has:


5 bonding and 0 nonbonding domains

a)

trigonal pyramidal

b)

trigonal planar

c)

tetrahedral

d)

trigonal bipyramidal

105.

What is the molecular geometry if the central atom has:


4 bonding and 1 nonbonding domains

a)

seesaw

b)

trigonal planar

c)

tetrahedral

d)

trigonal bipyramidal

106.

What is the molecular geometry if the central atom has:


6 bonding and 0 nonbonding domains

a)

square pyramidal

b)

trigonal planar

c)

tetrahedral

d)

octahedral

107.

What is the molecular geometry if the central atom has:


4 bonding and 2 nonbonding domains

a)

square planar

b)

trigonal planar

c)

tetrahedral

d)

bent

108.

What is the molecular geometry if the central atom has:


2 bonding and 0 nonbonding domains

a)

linear

b)

bent

c)

tetrahedral

d)

seesaw

109.

What is the molecular geometry if the central atom has:


3 bonding and 0 nonbonding domains

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

seesaw

110.

What is the molecular geometry if the central atom has:


4 bonding and 0 nonbonding domains

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

bent

111.

What is the molecular geometry if the central atom has:


2 bonding and 1 nonbonding domains

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

bent

112.

What is the molecular geometry if the central atom has:


3 bonding and 1 nonbonding domains

a)

trigonal pyramidal

b)

trigonal planar

c)

tetrahedral

d)

bent

113.

Which of the following is octahedral?

a)

SCl6

b)

XeI4

c)

NBr5

d)

CH4

114.
To determine the SHAPE of a molecular compound you assess the number of bonding groups and unshared electron pairs...
a)
on the central atom only
b)
on all elements in the compound
c)
on the cations only
d)
on the anions only
115.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

116.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

117.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar
118.

Why is the molecule polar?

a)

There is a non bonding pair electrons on the central atom.

b)

There are different types of elements bonded to the central atom.

c)

There are no non bonding pairs on the central atom and all of the atoms bonded to the central atom are the same.

119.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

120.
a)
non-polar
b)
polar
--->
c)
polar
<---
d)
polar
polar, pointing straight up
121.
a)
non-polar
b)
polar
--->
c)
polar
<---
d)
polar
polar, pointing straight down
122.
a)
non-polar
b)
polar
--->
c)
polar
<---
d)
polar
polar, pointing straight up
123.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

124.

A weak IMF will result in a

a)

high melting point

b)

high viscosity

c)

high surface tension

d)

low surface tension

125.

A strong IMF increases

a)

boiling point

b)

solubility

c)

flammability

d)

malleability

126.

List the strongest to weakest IMFs.

a)

Hydrogen Bond, London Dispersion, Dipole-dipole

b)

London Dispersion, Dipole-dipole,

Hydrogen Bond

c)

Hydrogen Bond, Dipole-dipole, London Dispersion

d)

Dipole-dipole, Hydrogen Bond, London Dispersion

127.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

128.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

129.
Which of the following factors plays an important role in the identification of specific intermolecular forces in a molecule?
a)
bond type
b)
density
c)
solubility
d)
molecular polarity
130.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

131.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

132.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

133.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

134.

Intramolecular forces are the forces

a)

within molecules

b)

between molecules

135.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
136.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

137.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

138.

A substance with weak intermolecular attractions are most likely (a)   at room temperature

139.

Attractions between molecules are

a)

covalent bonds

b)

intramolecular attractions

c)

intermolecular attractions

d)

ionic bonds

140.

Which is NOT true about hydrogen bonding?

a)

occurs between two molecules

b)

occurs as a special covalent bond

c)

occurs when one of the molecules has a hydrogen directly bonded to a N, F or O

d)

Is stronger than a dipole-dipole attraction

141.

Match the following molecules to the type of intermolecular attractions

a)

Weak force, low boiling point

1.

Dipole-Dipole attraction

b)

Stronger because it is a "real" bond. Conducts electricity as a liquid or solution

2.

Ionic bonds

c)

Weakest force, lowest boiling points

3.

Dispersion Forces

d)

Conducts electricity always, malleable, ductile

4.

Metallic bonding

e)

Strongest force for covalent bonded molecules, soluble in water. Has H with F, O, or N

5.

Hydrogen bond

142.

Which type of intermolecular attraction is shown (#1 in the diagram)?

a)

Hydrogen bond

b)

Dipole-dipole

c)

Ionic bond

d)

Metallic bond

143.

Which type of bonding does this molecule have (careful - not the intermolecular attractions)

a)

Hydrogen bond

b)

Covalent bond

c)

Ionic bond

d)

Metallic bond

144.

Which of these will NOT conduct electricity?

a)

Ag (silver)

b)

Brass (an alloy)

c)

NaCl dissolved in water

d)

Solid NaCl

145.

Which of these will NOT conduct electricity?

a)

Mg (Magnesium)

b)

Steel (an alloy)

c)

Liquid (melted) CaCl2

d)

Solid CaCl2

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AQA Paper 2 Practise Questions

141 questions

AQA Paper 2 Practise Questions

quiz

Worksheet

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9th - 12th Grade

Optional EOC Review

146 questions

Optional EOC Review

quiz

Worksheet

•

9th Grade

Quiz Bowl Review (General Science)

140 questions

Quiz Bowl Review (General Science)

quiz

Worksheet

•

7th - 12th Grade

Science - Chapter 8(2, 3)

141 questions

Science - Chapter 8(2, 3)

quiz

Worksheet

•

10th Grade

Finals Prep-Year Recap (2022)

141 questions

Finals Prep-Year Recap (2022)

quiz

Worksheet

•

12th Grade

ES 1 First Semester Review

140 questions

ES 1 First Semester Review

quiz

Worksheet

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10th Grade