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WorksheetsBonding Unit Review
Total questions: 50
Worksheet time: 12hrs 16mins
Name
Class
Date
1.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
2.
What is the molecular geometry of a molecule with this structure ?
a)
tetrahedral
b)
trigonal pyramid
c)
angular or bent
d)
trigonal plane
3.
T or F: Lone pairs around the oxygen atom of a water molecule play no role in determining its molecular geometry?
a)
True
b)
False
4.
The molecular geometry of carbon dioxide is...
a)
tetrahedral
b)
square
c)
planar
d)
linear
5.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Valence electrons
b)
Core electrons
c)
Protons
d)
Neutrons
6.
What is the molecular geometry of PH3?
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
7.
How many bonding domains are in the molecule SO2?
a)
1
b)
2
c)
3
d)
4
8.
How many non-bonding domains are in SiO2 ?
a)
0
b)
1
c)
2
d)
4
9.
Which of the following most likely represents the molecular geometry of water?
a)
A
b)
B
c)
C
d)
D
10.
2 domains, no lone pairs
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Bent
11.
3 domains, no lone pairs
a)
Linear
b)
Trigonal planar
c)
Tetrahedral
d)
Bent
12.
4 domains, 0 non-bonding
a)
Bent
b)
Trigonal planar
c)
Trigonal pyramidal
d)
Tetrahedral
13.
4 domains, three of them are bonding
a)
Trigonal pyramidal
b)
Trigonal Planar
c)
Tetrahedral
d)
Bent
14.
4 domains, two of them lone pairs
a)
Trigonal pyramidal
b)
Bent
c)
Tetrahedral
d)
Trigonal planar
15.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When an atom shares electrons with an another atom
c)
When an atom shares neutrons with an another atom
d)
When one atom takes the other atom's nuetrons
16.
How many electrons would a trigonal planar structure contain?
a)
24
b)
16
c)
26
d)
20
17.
Which substance would not separate when dissolved in water?
a)
CaO
b)
NaCl
c)
PO3
d)
CuI
18.
Which compound would have a high melting point?
a)
CaO
b)
CO2
c)
PI3
d)
SO3
19.
Which substance would be a poor conductor?
a)
NaCl (s)
b)
CO
c)
Both CO and NaCl(s)
d)
NaCl(aq)
(aq = dissolved in water)
(aq = dissolved in water)
20.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core
c)
Valence
d)
Stable
21.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
22.
The theory that is used to predict the arrangement of atoms about a central atom is called?
a)
Valence shell repulsion
b)
Valence shell electron sharing
c)
Valence shell electron pair repulsion
d)
Valence electron shell repulsion pair
23.
Atoms of H only form _________ bonds.
a)
Double
b)
Single
c)
Multiple
d)
Triple
24.
A bond where electrons are NOT shared equally?
a)
polar covalent
b)
nonpolar covalent
c)
ionic
25.
Which of the following is a substance held together by only covalent bonds?
a)
NaCl
b)
HCl
c)
NH4Cl
d)
ZnCl2
26.
Which of the following is substance held together by only ionic bonds?
a)
H3N
b)
CaCl2
c)
NO2
d)
SCl
27.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
28.
Determine the polarity and geometry for HF.
(electronegativities --> H = 2.2; F = 4.0
(electronegativities --> H = 2.2; F = 4.0
a)
no shape, polar
b)
linear, polar
c)
linear, nonpolar
d)
crystal lattice, ionic
29.
Determine the molecular shape for CaCl2.
a)
trigonal planar
b)
trigonal pyramidal
c)
linear
d)
crystal lattice
30.
Determine the number of lone pairs on the central atom of OF2.
a)
none
b)
1
c)
2
d)
it's ionic
31.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
32.
Write the correct formula for Zn2+ and F-.
a)
ZnF2
b)
ZnF
c)
Zn2F
d)
Zn2F4
33.
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
34.
Alkaline Earth elements will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
35.
A charged particle that has gained at least one electron is called a(n) _____.
a)
Anion
b)
Cation
c)
Anonion
d)
chemistry cat
36.
What is the charge on an Aluminium ion?
a)
3+
b)
3
c)
3-
d)
2+
37.
What is the charge of Neon?
a)
0
b)
1+
c)
1-
d)
1
38.
Is the compound Ionic, Covalent, or both?
CO2
CO2
a)
Ionic
b)
Covalent
c)
both
39.
Is the compound Ionic, Covalent, or both?
H2O
H2O
a)
Ionic
b)
Covalent
c)
both
40.
Is the compound Ionic, Covalent, or both? AgCl
a)
Ionic
b)
Covalent
c)
both
41.
Is the compound Ionic, Covalent, or both? CaO
a)
Ionic
b)
Covalent
c)
both
42.
Is the compound Ionic, Covalent, or both? LiOH
a)
Ionic
b)
Covalent
c)
both
43.
The molecule CH2O would have bond angles of _____.
a)
104.5°
b)
107°
c)
109.5°
d)
120°
44.
The molecule PF3 would have bond angles of _____.
a)
104.5°
b)
107°
c)
109.5°
d)
120°
45.
The bond formed between carbon and phosphorus would most likely be...
a)
a nonpolar covalent bond
b)
a polar covalent bond
c)
an ionic bond
46.
The bond formed between magnesium and nitrogen would most likely be...
a)
a nonpolar covalent bond
b)
a polar covalent bond
c)
an ionic bond
47.
The bond formed between oxygen and boron would most likely be...
a)
a nonpolar covalent bond
b)
a polar covalent bond
c)
an ionic bond
48.
Based on the data collected in an experiment the bond type of Unknown Z would most likely be...
a)
held together by covalent bonds.
b)
held together by ionic bonds.
c)
unable to identify due to conflicting results.
49.
What would be the proper chemical formula for combining Al3+ and l- :
a)
Al l3
b)
Al3l
c)
Al l
d)
Al3 l3
50.
What formula results when Ca+2 and Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
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