Chemistry Final Exam
Review and Practice

Chapters Covered
– ESSENTIALLY
CUMMULATIVE
– List of Chapters:

CP:
.
4, 5, 7, 8,
14, 15, 18, 19

H: 5, 6, 7, 8, 12, 14, 18
Topics to Expect:
Periodic Table:
s, p, d, f blocks
Metal, Metalloid,
Non –metal, etc.
Electron Configuration: Electron Configuration:
Orbitals and SubLevels Atomic #, mass, core
notation
Valence Electrons
Periodic Trends:
Bonding:
Covalent and Ionic
Lewis dot diagrams
Bonding:
Electronegativity
Solutions:
solubility curves
Acid and Bases and pH
Chemical and Physical Properties
Atomic Radii, Electronegativity,
Ionic Radii, Ions /Compounds
Family names
Bonding :
molecular shapes,
intermolecular forces
to determine if nonpolar covalent
or polar covalent, both bond and
molecules.
Atomic Sturcture and
Electron Configuration






Location of electrons in s, p, d, f orbitals.
Shape and number of s and p orbitals.
Number of electrons each orbital each sublevel
and each level can hold.
Location of s, p, d, f blocks on periodic table.
Lewis dot diagrams.
Formation of complete octets by transfer of /
sharing of electrons.
Electron Configuration &
Periodic Table





Filling orbital diagrams
Writing electron configurations
Core notation using chemical symbol of preceding
noble gas
Trends for physical and chemical properties
Atomic radii, ionization energy, electronegativity
Bonding




Ionic versus covalent
Valence electrons and dot diagrams
Lewis structures: shared pairs and lone pairs
Stability of “octet” electron arrangement of noble gases
Molecular Shapes and Polarity




Recognize drawings of ball and stick models
Use VSEPR
Recognize dipole as electrons being pulled towards the
higher electronegative element, causing a partial
negative charge on that atom and a partial positive
charge on the lower electronegative atom
Dispersion, dipole-dipole, hydrogen bonding: types of
intermolecular forces in covalent compounds
Solutions
Solubility Curves
 Vocabulary

– Saturated, Unsaturated, Supersaturated
– Solute, Solvent, Solution, etc.

Molarity definition and calculation
Acids, Bases and pH
Acid and base characteristic
 Vocabulary:

– Ka, dissociation, electrolyte,amphoteric
neutralization reaction and products

Self Ionization of Water and pH
– Defintion / math formula
– Calculation from molarity
#1
What is the maximum number of
electrons that can by held in an
“s” sublevel?
A.
 B.
 C.
 D.

1
2
6
8
#2
What is the maximum # of e- that
can by held in a “p” sublevel?
A.
 B.
 C.
 D.

1
2
6
8
#3
What is the total number of
sublevel for n=2?
A.
 B.
 C.
 D.

1
2
6
8
#4
For an element whose electron
configuration is [Ne]3s23p3, how
many dots would the Lewis dot
diagram have?
A.
 B.
 C.
 D.

3
5
8
13
How many dots does the Lewis
dot diagram for chlorine have?
#5
A.
 B.
 C.
 D.

3
5
7
8
#6
A positive lithium ion is formed
when a neutral lithium atom:
A.
 B.
 C.
 D.

gains one proton
gains one electron
loses one proton
loses one electron
#7
When a potassium atom becomes
an ion, it:
A.
 B.
 C.
 D.

gains one proton
gains one electron
loses one proton
loses one electron
When a calcium atom becomes
an ion, it:
#8
A.
 B.
 C.
 D.

gains two protons
gains two electrons
loses two protons
loses two electrons
#9
Use the periodic table to locate
K; what block is it in?
a.
 b.
 c.
 d.

s-block
p-block
d-block
f-block
#10
What does
1
[Ar]4s
represent?
a. the full electron configuration of K
 b. the abbreviated electron configuration
for K
 c. the full mass designation for K
 d. the block designation for K

#11
What does Ar represent in
[Ar]4s1?
a. the block of the periodic table
 b. the highest orbital filled
 c. the chemical symbol of the preceding
noble gas
 d. the chemical symbol of the element

#12
What kind of bond is predicted to
form between B and H if their
electronegativities are 2.0 and 2.2
respectively?
a.
 b.
 c.
 d.

nonpolar covalent
polar covalent
ionic
intermolecular
#13
A bond is nonpolar covalent if
the difference in
electronegativities between
the two atoms is:
A.
 B.
 C.
 D.

2.1 or more
between 0.5 and 2.1
less than 0.4
less than zero
#14
Which of the following bonds
would be considered completely
nonpolar?
A.
 B.
 C.
 D.

H-N
O-O
O-C
F-Cl
#15
For the diatomic molecule Cl2,
how many electron(s) does each
chlorine share with the other
chlorine?
A.
 B.
 C.
 D.

1
2
7
8
#16
How many pairs of shared and
unshared electrons does the
Lewis dot structure for water
have?
A.
 B.
 C.
 D.

4, 0
3, 1
2, 2
4, 4
#17
In a double bond between two
atoms, the number of shared
electrons is:
A.
 B.
 C.
 D.

2
4
6
8
#18
In the compound ammonia, NH3:
A. Each hydrogen has a partial negative charge
 B. The nitrogen has a full positive charge
 C. The N-H bond is ionic
 D. The Lewis structure will have one unshared
pair of electrons

#19
What kind of compound would
form between nonmetallic atoms
and non metallic atoms?
A. Nonpolar covalent
 B. Polar covalent
 C. Ionic
 D. Covalent

#20
What kind of compound would
form between polyatomic ions
and metallic ions?
A. Nonpolar covalent
 B. Polar covalent
 C. Ionic
 D. Covalent

#21
What kind of compound would
form between metallic ions and
nonmetallic ions?
A.
 B.
 C.
 D.

Nonpolar covalent
Polar covalent
Ionic
Covalent
#22
What kind of compound would
form between potassium and
bromine?:
A.
 B.
 C.
 D.

Nonpolar covalent
Polar covalent
Ionic
Macromolecular covalent
#23
Predict the physical state of the
compound formed between
magnesium and oxygen:
A.
 B.
 C.
 D.

Probably a gas
Probably a liquid
Probably a solid
Impossible to determine from the given data
#24
The physical state of nearly all
ionic compounds at
room temperature is:
A. Solid
 B. liquid
 C. Gas
 D. Different for each ionic compound

#25
Ionic Compounds are generally:
A. Conductors of electricity in the solid state
 B. Gases at room temperature
 C. Formed when a metal transfers its valence
electron to a nonmetal
 D. Electrically charged

#26
How does a covalent bond differ
from an ionic bond?
A. Ionic: transfer of e-; covalent: sharing of e B. Ionic: involves 2 e-; covalent: involves 4 e C. Ionic: btw metals; covalent btw nonmetals
 D: Ionic: usually acids; covalent: usually bases

#27
Which theory is used to account
for the shape of molecules?
A. theory of relativity
 B. thermodynamic theory
 C. kinetic theory
 D. VSEPR theory

#28
Which of the following does a
ball and stick model reveal about
chemical bonds?
A. their arrangement in space
 B. their presence and type
 C. both A and B
 D. neither A or B

#29
What shape does an ammonia ,
NH3, molecule have?
A. pyramidal
 B. trigonal planar
 C. tetrahedral
 D. bent

#30
What shape does a water
molecule have?
A. pyramidal
 B. trigonal planar
 C. tetrahedral
 D. bent

#31
In a molecule of carbon dioxide,
what kind of bonds connect the
carbon atom to the 2 oxygen
atoms?
A. two single bonds
 B. one single and one double bond
 C. one double and one triple bond
 D. two double bonds

#32
What shape is a carbon dioxide
molecule?
A. linear
 B. bent
 C. trigonal planar
 D. pyramidal

#33
What shape is a methane, CH4
molecule?
A. tetrahedral
 B. bent
 C. trigonal planar
 D. pyramidal

#34
What is the bond angle of a
molecule of ammonia , NH3?
A.
 B.
 C.
 D.

107o
109.5o
120o
180o
#35
What is the bond angle of a
molecule of carbon dioxide?
A.
 B.
 C.
 D.

107o
109.5o
120o
180o
#36
What is the bond angle of a
molecule of methane?
A.
 B.
 C.
 D.

107o
109.5o
120o
180o
#37
What is the bond angle of a
molecule of water?
A.
 B.
 C.
D

90o
105o
107o
109.5o
Which of the following
properties would you expect to
find in a small nonpolar
molecule?
#38
A.
 B.
 C.
D

Gas at room temperature
Solid at room temperature
Very high melting point
Very high boiling point
In a pyramidal molecule, how
many unshared pairs of valence
electrons does the central atom
have?
#39
A.
 B.
 C.
 D.

None
One
Two
Three
In a tetrahedral molecule, how
many unshared pairs of valence
electrons does the central atom
have?
#40
A.
 B.
 C.
 D.

None
One
Two
Three
#41
In polar bonds electrons are:
A.
 B.
 C.
 D.

Shared unequally
Shared equally
Completely transfered
Not shared at all
#42
Dipoles are:
A.
 B.
 C.
 D.

Nonpolar bonds
Polar bonds
Nonpolar molecules
Polar molecules
#43
What determines the polarity of a
bond?
A.
 B.
 C.
 D.

Electronegativity difference only
Molecular shape only
Both A and B
Neither A and B
#44
What determines the polarity of a
molecule?
A.
 B.
 C.
 D.

Electronegativity difference only
Molecular shape only
Both A and B
Neither A and B
#45
How are the electrons shared in a
bond between carbon & oxygen?
A.
 B.
 C.
 D.

They are shared equally
Carbon attracts them more
Oxygen attracts them more
Electrons are completely transferred
#46
All solutions have the following
properties except that the:
A. Dissolved particles are very small
 B. Particles in a solution are evenly distributed
 C. Solution particles do not settle out
 D. Final physical state of a solution is a liquid

Which of the following
statements applies to the
dissolved solute particles in a
solution?
#47
A.
 B.
 C.
 D.

They can be seen with the unaided eye
They will be in the same phase as the solvent
They will settle out when left standing
There is always less solute than solvent
#48
An alloy is an example of a:
A.
 B.
 C.
 D.

Gaseous mixture
Liquid solution
Solid solution
Solid mixture
#49
Solutions with water as the
solvent are called:
A.
 B.
 C.
 D.

Liquids
Miscible solutions
Aqueous solutions
Electrolytes
#50
Molarity is expressed as:
A.
 B.
 C.
 D.

Moles of solvent / Liters of solute
Moles of solute / Liters of solvent
Moles of solute / Liters of solution
Moles of solute / moles of solution
A solution that contains as much
solute as can possibly be
dissolved under existing
conditions is said to be:
#51
A.
 B.
 C.
 D.

saturated
supersaturated
soluble
concentrated
#52
Which of the following is NOT
an important factor influencing
solubility?
A.
 B.
 C.
 D.

Chemical nature of solute
Temperature
Chemical nature of solvent
Volume of solution
#53
Common nonpolar solvents
include all of the following
except:
A.
 B.
 C.
 D.

Salt water
Carbon tetrachloride
Hexane
Vegetable oil
#54
Ionic solids best dissolve in
liquid solvents that are:
A.
 B.
 C.
 D.

polar
nonpolar
viscous
transparent
#55
Which of the following’s
solubility is most affected by
pressure?
A.
 B.
 C.
 D.

Ionic solids
Supersaturated solutions
Gases
Alloys
#56
Why can water dissolve NaCl,
whereas hexane cannot?




A. Hexane is attracted to the sodium, but not to the
chlorine
B. As a polar solvent, water is attracted to both anions
and cations
C. Both water and salt are inorganic, while hexane is
organic
D. Water can form hydrogen bonds with NaCl
#57
The rate at which a solid can be
dissolved in a liquid solvent can
be increased by:
A.
 B.
 C.
 D.

Lowering the temperature of the solvent
Grinding the solute into smaller pieces
Increasing the air pressure on the liquid
Lowering the temperature of the solute
#58
To identify the strongest acid,
compare the Ka and:
A.
 B.
 C.
 D.

The highest Ka value is the strongest acid
The lowest Ka value is the strongest acid
The Ka closest to pH 7 is the strongest acid
The Ka closest to pH 0 is the strongest acid
#59
Substances that change color
when added to acids or bases are
called:
A. indicators
 B. electrolytes
 C. insulaotrs
 D. capacitators

#60
The ionic compound formed in
acid-base neutralization reactions
is:
A. water
 B. a salt
 C. hydride
 D. hydroxide

#61
A substance that can act as either
an acid or a base is described as:
A. neutral
 B. ambidextrous
 C. conjugate
 D. amphoteric

#62
Which of the following is least
able to donate a proton?
A. HF
 B. H2O
 C. HCO3 D. F
#63
Which of the following could be
a conjugate acid-base pair?
A. strong acid –strong base
 B. weak acid - weak base
 C. strong acid – weak base
 D. need more information

#64
The acid dissociation constant, Ka,
measures an acid’s:
A. concentration
 B. strength
 C. number of protons
 D. degree of sourness

#65
HNO3 reacts with magnesium
metal to give off the gas:
A. oxygen
 B. nitrogen
 C. hydrogen
 D. no gas is given off

#66
HNO3 turns litmus paper:
A. blue
 B. red
 C. no color change
 D. green

#67
What is the pH of 0.00100M
HCl?
A.
 B.
 C.
 D.

3
2
1.3
4
#68
What affect does increasing the
pH by 2 have on the
hydronium ion concentration?
A.
 B.
 C.
 D.

Doubles it
Halves it
Increases by power of 2 (100 times more)
Decreases by power of 2 (100 times less)
#69
What is the pH of an acid if the
hydronium ion concentration is
1 x 10-4 M?
A.
 B.
 C.
 D.

1
4
10
10000
#70
Determine the pH of a
0.00100M NaOH solution.
A.
 B.
 C.
 D.

3
4
11
14
#71
Pure water contains which of the
following species?
A. H2O molecules
 B. H3O+ ions
 C. OH- ions
 D. all of these

#72
Determine the hydroxide ion
concentration of a solution with a
pH of 13.
A. 1.0 x 10-13
 B. 13
 C. 1
 D. 1.0 x 10-1

#73
The definition of pH is:
A. –log[H3O+]
 B. the percent of hydronium ions
 C. the parts per million of hydronium ions
 D. log[OH-]

#74
Two common ways to measure
pH are:
A. with indicators and thermometers
 B. with indicators and a pH meter
 C. by taste and color
 D. by electric conductivity and by temperature

#75
The equivalence point of a
strong acid-strong base
titration curve is:
A. at a pH of 7
 B. at the steepest part of the curve
 C. when the solution is neutral
 D. all of the above

Chemistry Final Exam
Good Luck!


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