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Example problems from previous quizzes and assignments.
Matter Review
Classify each of the following as a physical or a chemical
property of matter.
_____1.
_____2.
_____3.
_____4.
_____5.
_____6.
_____7.
_____8.
Iron and oxygen form rust
Oil and water do not mix
Aluminum has a silvery color
Silver tarnishes
Water boils at 1000 C
Gold has a density of 19 g/ml
Sodium ignites when dropped in water
Magnesium burns brightly when ignited
9. Create a graphic organizer using the following words: Matter,
Mixtures, elements, sugar, water, oxygen, pure substance,
solution, homogeneous, gold, heterogeneous, compounds
The Atom
1. Discuss Rutherford’s experiment. What was he testing for? What
was his hypothesis? What did he discover? How did this change
the theory of the atom?
2. Give the number of protons, neutrons and electrons in the
following elements:
a. C-12
b. Cu-63
c. Ni-58
d. U-235
3. Give the noble gas configuration of the following elements. Try
not to use the atomic number while doing so. (HINT: use the s, p,
d, and f blocks we discussed).
a. Cl
b. Co
c. Al
d. I
4. What element has the following electron configuration?
a. [Kr] 5s2 4d5
b. [Ar] 4s2 3d10 4p4
c. [Xe] 6s2 4f14 5d4
5. Fill the following table out about quantum levels and sublevels
Quantum level
Sub levels
Orbitals in sub
Total electrons
present
level
in sub level
1
2
3
4
Periodic Table
1. On the periodic table below, label the following items (use the
letter given to label):
a. two elements in the same group (A)
b. two elements in the same period (B)
c. a transition metal (C)
d. A lanthanide (D)
e. An alkali Earth Metal (E)
f. A non-metal (F)
g. A metalloid (G)
2. On the periodic table above, draw in the following trends, showing
how the particular trend increases, both across and up/down (ex –
if atomic radius increases across, draw an arrow from left to right
and label it increasing, atomic radius). Explain WHY the trends are
the way they are.
a. Atomic radius, ionic radius, ionization energy,
electronegativity
3. What is the difference between ionization energy and
electronegativity?
Ionic and Covalent Compounds
1. How does a cation form? An anion?
2. Using the following list of ions, create 10 ionic compounds AND
name them.
Au +1
Fe+2
Na+1
Ca+2
Al+3
NH4+1
BrO-1
Cl-1
OH-1
NO2-1
SO4-2
N-3
O-2
ClO4-1
BO3-3
C2H3O2-1
3. Describe the difference between ionic and covalent compounds.
4. Name the following covalent compounds:
a. NO ________________________________________
b. NF3 ________________________________________
c. P2F4 _______________________________________
d. SeO3 _______________________________________
4. Draw the following molecular structures for the covalent
compounds.
5. a. SeBr2
b. PO3-3
c. CO3-2
Chemical Reactions
Write out the correct, balanced chemical equation given the following
word equations. Also, determine the type of reaction that is occurring.
1. Sodium sulfide and silver nitrate react to form sodium nitrate and
silver sulfide.
2. Carbon monoxide and oxygen react to form carbon dioxide.
3. Potassium chlorate decomposes into potassium chloride and
oxygen.
4. Iron (III) chloride reacts with sodium hydroxide producing solid
iron (III) hydroxide and sodium chloride.
5. How can you determine whether a single replacement reaction will
occur?
Moles and Molar Conversions
Convert the following numbers to either moles, grams or particles in the
following elements or compounds.
1. X mol in 5.5 x 1026 atoms of Bi
2. X grams in 4.67 mol Li
3. X mol in 25 g Zn
4. X atoms 3.54 mol Hg
5. X mol of CO2 in 3.2 x 1020 molecules
6. X g of CaCO3 in 1.9 mol
7. X particles in 44.5 g H2O
8. X g KMnO4 in 2.54 X 1024 formula units
Stoichiometry
1. One of the main ingredients of pearls is calcium carbonate. If
pearls are put in an acidic solution, they dissolve.
CaCO3 + HCl  CaCl2 + H2O + CO2
How many moles of CaCO3 can be dissolved in .0250 mol HCl?
2. The fuel methanol (CH3OH) is made by the reaction of carbon
monoxide and hydrogen. How many grams of hydrogen are needed
to produce 45.0 g of methanol?
3. Hydrogen cyanide is produced industrially from the reaction of
gaseous ammonia, oxygen and methane.
NH3 + O2 + CH4  HCN + H2O
If 5.0 X 103 kg of CH4 are used, what mass of HCN and H2O would be
produced?
**Density and isotope problems – very little on the final, look over
previous tests and quizzes for example problems**