Chemistry 1st Semester Final Exam Review – ANSWER KEY
READ THE FOLLOWING PARAGRAPH BEFORE YOU START! This worksheet is meant to be a
“practice test” to help you prepare for your final exam.
Suggestions on how to prepare: I would first order my notes and homework by the dates on them.
Then I would look at the topic statement below (the capital letter phrases) for the first topic. Find this
topic and all related information or materials in your possession and study them thoroughly! I would
suggest you re-read your textbook/notes and re-work old problems. When you feel you have the topic
well reviewed and understood THEN work the topic problems or questions on this sheet. If you don’t
get the answers right, go back and spend more time reviewing your old materials. If you do get them
right, go on to the next topic and repeat the process. After you do all topics this way, start over!
As always, remember to use and report answers to the correct significant figures and to include units!
FUNDAMENTALS OF CHEMISTRY: MATTER AND CHANGE
 Define chemistry.
 Discuss the steps in the scientific method.
 Which of the following observations is evidence used to imply that a chemical reaction has
occurred? a – f
a. gas evolution
b. a precipitate forms (solid formed from aqueous solutions)
c. the color changes
d. the temperature changes
e. the odor changes
f. a sound is produced (i.e. fireworks)
g. change in taste (but lets not taste anything during lab class!)
 Describe a physical property vs. a chemical property.
 What is the difference between a physical change and a chemical change?
 Identify each type of change (physical or chemical).
a. boiling water P
b. rusting iron C
c. burning candles C (produces new products  H2O + CO2 )
d. breaking glass P
e. melting wax P (solid to liquid – change in state only)
 Be able to classify matter: mixtures (homogeneous, heterogeneous) vs. pure substances
(compounds or elements)
 Identify each as an element, compound or mixture.
a. lead - element
b. water - compound
c. kool-aid - mixture
d. table salt - compound
e. soda - mixture
f. oxygen - element
 What are the characteristic of a metal, metalloid and non-metal? Identify each type of
element:
a. Zn - metal
b. As - metalloid
c. S - nonmetal
d. Ne - nonmetal
e. Na - metal
MEASUREMENTS AND CALCULATIONS (Sig. Figs., Scientific Notation, SI Units)
 What are the rules/guidelines of determining significant figures?
 How many significant figures in: 4 sig. figs. In all (a. – e.)
a. 1234
b. 123.0
c. 123400
d. 0.001234 e. 0.01230
 Report the above problems (a-e) in correct scientific notation.
o a. 1.234 x 103
b. 1.230 x 102
d. 1.234 x 10-3
 What are the common SI Units? Know the prefixes from milli to kilo and be able to convert
between units in the metric system.
 What is the difference between mass and weight?
 Multiply: 5.98 mm x 3.2 mm = 19 mm
 Add 3.258 cm + 12.0 cm = 15.3 cm
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 Give an example of a qualitative observation. Describes color, odor, shape or some other
physical characteristic (i.e. hot)
 Give an example of a quantitative observation. numerical information (i.e. temperature,
pressure, volume, the quantity of a chemical formed or used up in a reaction)
 What is the difference between accuracy and precision?
 How many grams of mercury would you have if you had 32 cm3 of mercury? The density of
mercury is 13.6 g/cm3. D = m/V  m = D x V = 13.6 g/cm3 x 32 cm3 = 440 g
 Ronnie has a piece of aluminum which has a mass of 10.8 grams and a volume of 4 cubic
centimeters. Calculate the density of aluminum. D = m/V = 10.8 g / 4 cm3 = 3 g/cm3
ATOMIC THEORY AND NUCLEAR CHEMISTRY
 Describe Dalton’s Atomic Theory.
 What did we learn from Rutherford’s Gold Foil Experiment and how did it work?
 What did J. J. Thomson discover with his Cathode Ray experiment?
 Define the atomic number, mass number, average atomic mass and isotopes.
 Explain the difference between atoms, ions, cations, anions.
 Know the charge, location and size of the three subatomic particles.
29
 Fill in the blanks for the following:
79
137
37 Al
Br
Ba2+
Cl
35
56
17
atomic number
__35_
__56_
__17__
__13_
mass number
_79__
_137__
_37__
_29__
# protons
_35__
__56_
_17___
_13__
# neutrons
_44__
_81__
_20__
_16__
# electrons
_35__
_54__
_18__
_13__
neutral or type of ion? neutral
cation
anion
neutral
 An element has 30 protons, 35 neutrons, and 30 electrons. What element is this? Zn
 An ion of an element has 29 protons, 35 neutrons, and 27 electrons. What ion is this? Write its
symbol with the correct charge. Cu2+
 State the Law of Conservation of Mass (Matter).
 Most of the volume of the atom is taken up by the electron cloud. True or False?
 How many particles are there in 1 mole of anything? What is the name for this number of
particles?
 What is the molar mass of sodium? 22.99 g/mol Na
What is the molar mass of Na2SO4? 142.05 g/mol
 Indicate the number of molecules, and the total number of each type of atom for each of the
following:
4H2O 4 molecules of water, 8 H atoms, 4 O atom
2Al2(SO4)3 2 formula units of aluminum sulfate; 4 Al atoms, 6 S atoms, 24 O atoms
 Be able to convert: Grams to Moles
or
Moles to Grams
Grams to Atoms
or
Atoms to Grams
 How many moles are in 222 g of copper? 3.49 moles Cu
 How many atoms are in 4.00 g of sulfur? 7.51 x 1022 atoms S
 What is Avogadro’s number? What is the significance of it?
 Be able to balance simple nuclear equations.
 What is radioactive decay? Half-life? (no equations)
 Describe the process of nuclear fission and nuclear fusion?
 What are the penetrating strength differences between alpha particles, beta particles and
gamma rays? alpha < beta < gamma (gamma is most penetrating)
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 Balance the following nuclear reactions, using the following choices:
a.
b.
c.
1.
238
92
U 
234
90
Th +

a
2.
234
90
Th 
234
91
d.
Pa +

d
ELECTRON CONFIGURATIONS
 What is the frequency of an electromagnetic wave traveling at the speed of light with a
wavelength of 6.80 x 10-7 m? 4.41 x 1014 s-1
 All types of electromagnetic radiation have the same _traveling speed (in a vacuum)__.
 Identify the parts of an electromagnetic wave on a diagram (i.e. wavelength, amplitude, etc.).
 What is a quantum of electromagnetic energy called? a photon
 Write the full electron configuration for: C, As, and S2 How many outer electrons does each of the following have? Na As
Br
O2K+
 How many electrons must each of the following lose or gain to achieve an octet? (State
whether it loses or gains and how many)
Cl = gains 1
Ca = loses 2
Xe = none, noble gas!
P = gains 3
 Which element has similar chemical properties like Si? Why?
At
Al
N
C
both have four valence electrons (both found in group 14)
 When electrons absorb energy, what is the result?
 What color of light has the most energy?
 What is the probability map for an electron called? an orbital (90% probability)
 What occurs when an electron moves from a higher energy level to a lower energy level in an
atom? a photon is released
 The
principle quantum number
indicates the main energy level occupied by the
electrons (n).
 How many electrons can occupy an s orbital, p orbital, d and f orbitals? S=2, p=6, d=10, f=14
 Which atom would have an octet of electrons (full s and p orbitals): Ar (He only has 2 electrons)
PERIODIC TABLE
 Who is Dmitri Mendeleev?
 What charge do all elements in the following columns form when they are ions?
1, 2, 13, 15, 17, 18
 What is the chemical family name for column: 1, 2, 17 and 18?
 What are the following groups most characteristic properties?
1, 2, 17, 18
Group 1: alkali metals (except H), soft, very reactive metal (usually exists as compounds;
easily lose their one valence electron); forms a “base” (or alkali) when reacting with water (not
just dissolved!)
Group 2: alkaline earth metals; also form bases with water; do not dissolve well, reactive
(loses two valence electrons)
Group 17: halogens, most highly reactive of nonmetals
Group 18: noble gases, unreactive
 Write the complete electron structure for a neutral sodium atom. According to its electron
structure, what period of the periodic table should sodium be in? How many valence electrons
does it have? What ion will sodium tend to form?
 What is meant by a noble gas electron configuration? Why are they more stable? filled outer
shell – octet rule
 Define:
electronegativity
ionization energy
electron affinity
 Describe the trends (across a period, down a group) in the periodic table for:
Atomic radius
Ionization energy
Electronegativity
 State the periodic law.
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CHEMICAL BONDING
 What is a chemical bond?
 What are valence electrons and why are they important?
 State the octet rule.
 What is the difference between ionic, covalent and metallic bonding?
 What type of bond (ionic or covalent) will form in the following compounds? How do you know?
CO2 -covalent
NaCl - ionic
F2 – covalent
Ionic – metal and nonmetal
Covalent – two nonmetals
 Using an electronegativity chart identify each type of bonding (ionic, polar covalent, nonpolar
covalent):
Cs – Cl ionic
H–O
polar covalent
Br – I
polar covalent
Cl – Cl
nonpolar covalent
 List the seven diatomic molecules. BrINClHOF
 What is a polar molecule?
 What is VSEPR theory? Is a model for predicting the shape of molecules
 Use VSEPR theory to predict the molecular geometry of the following (common geometries:
linear, trigonal planar, tetrahedral): CO2 linear
CH4 tetrahedral
BF3
trigonal planar
NOMENCLATURE AND USING CHEMICAL FORMULAS
 Use the following ions and write the correct formula for the compound made from them:
a. Na+ and BrNaBr
sodium bromide
b. Mg2+ and IMgI2
magnesium iodide
2+
c. Ca and NO3
Ca(NO3)2
calcium nitrate
d. Fe3+ and SO42Fe2(SO4)3
iron(III) sulfate
 Name the above compounds (a-d) and the following:
e. KOH
potassium hydroxide
f. CuF
copper(I) fluoride
g. CuSO4
copper(II) sulfate
 Which compounds below are ionic? Which are molecular (covalently bonded)?
a. N2
molecular compound (nonmetals)
b. CaF2
ionic compound (metal and nonmetal)
c. NO2
molecular compound
d. CuSO4
ionic compound
e. CCl4
molecular compound
 Given SO42- and the compound Zr2(SO4)3 , what is the charge on Zirconium? 3+
 What is the chemical formula for potassium chloride? KCl
 What is the formula for iron(III) sulfide? Fe2S3
 What is the formula for lithium carbonate? Li2CO3
 What is the molar mass of an element?
 What is the molar mass of CuSO4?
 What is the percent composition of carbon in carbon dioxide?
[12.011 g C / [12.011 g C + (2 x 16.00 g O)]] x 100 = 27.29%
 Name each of the following acids:
a. HCl
hydrochloric acid
b H2SO4
sulfuric acid
c. HNO3
nitric acid
d. HI
hydriodic acid
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