CHEMISTRY TEST #1 REVIEW: MATTER
* the test will check what you have understood of all the topics discussed in class so far, YOU WILL
NOT BE ASKED TO GIVE DEFINITIONS, you will be expected to use your knowledge of chemical
concepts
* Prepare a Cheat-Sheet: on one side of the given paper assemble hand-written information to bring
to the test. This will be submitted (but not evaluated) with the test.
* You will be allowed to use the following (unmarked) handouts: Periodic Table, list of polyatomic ions,
solubility rules
Topics Covered
-the atom: proton, neutron, electron
-classifying elements: metal, nonmetal, atom, molecule, atomic number, mass number, pure substance,
mixture, halogens, alkali metals, alkaline earth metals, transition metals, semimetals/metalloids, noble
gases
-models of atom: Bohr-Rutherford diagrams, energy level, precipitate, solubility, electron
configuration, ion, group, electronegativity, Lewis formulas and structures, valence electrons
-spectroscopy: continuous and line spectrum
-nomenclature for ionic and covalent compounds
-polarity of covalent bonds
-intermolecular forces (London dispersion forces, dipole-dipole interactions, hydrogen bonding),
intramolecular forces (covalent, ionic)
-properties of matter: physical property, chemical property, qualitative, quantitative, physical change,
chemical change, element, compound, solute, solvent, solution
-types of chemical reactions
-chemical equations
- total/net ionic equations, spectator ions, precipitate
SUGGESTED QUESTIONS
p.18
1. Describe the difference between radio waves and
X rays using the concepts of wavelength, frequency,
and energy.
2. What range of wavelengths of electromagnetic
radiation can the human eye detect?
4. Distinguish between a continuous spectrum and a
line spectrum.
5. When an X ray is taken, the X-ray technician
leaves the room, but the patient is exposed to the X
ray.
(a) Why is it not safe for the technician to be in the
room when the X ray is taken?
(b) What precautions are followed to minimize the
patient’s and the technician’s exposure to X rays?
p.22
4. Electrons can be found in the ground state or in
the excited state. What is different about an
electron in each state?
6. Why do electrons emit light energy when they
drop from a higher energy level to a lower energy
level?
p. 35
1. Distinguish between an electrolyte and a
nonelectrolyte.
2. Explain why some atoms have a tendency to form
ions. Which combinations of atoms tend to form
ions? Why?
3. Which types of elements form ionic bonds? How?
4. Draw a Lewis symbol for each of the following
atoms:
(a) potassium(b) cesium(c) iodine(d) silicon(e)
antimony(f) krypton(g) barium
5. Predict the charge on the most stable ion that is
formed by each of the following elements. Write
theion’s symbol, including its charge.
(a) hydrogen(b) potassium(c) fluorine(d)
magnesium(e) sulfur
6. Draw Lewis symbols for the element ions in
question 5. What similarity do you notice? State the
rule that is being followed.
7. Using Lewis symbols and the octet rule,
illustratehow each of the following pairs of atoms
bond:
(a) potassium and chlorine(b) magnesium and sulfur
p.39
1. Draw Lewis symbols for the reaction between two
bromine atoms.
2. Draw Lewis symbols for the reaction between one
nitrogen atom and three hydrogen atoms. Draw the
Lewis structure for the resulting ammonia molecule.
3. Draw Lewis symbols for the reaction between one
carbon atom and four hydrogen atoms. Draw the
Lewis structure for the resulting methane molecule.
4. Draw Lewis symbols for the reaction between one
silicon atom and two oxygen atoms. Draw the Lewis
structure for the resulting silicon dioxide molecule.
p.45
1. Which of the following pairs of atoms form
covalent bonds, and which form ionic bonds? How do
you know?
(a) sulfur and oxygen (b) sodium and iodine (c)
bromine and bromine
2. Draw a Lewis structure for each of the following
molecules:
(a) F2 (b) H2 (c) O2 (d) H2S (e) CO2
3. Which of the molecules in question 2 are polar
molecules? Which are nonpolar?
4. How are a covalent bond and an ionic bond
different? How are they similar?
6. Identify the more polar bond in each of the
following pairs.
(a) H—F and H—Cl (b) N—O and C—O (c) S—H
and O—H (d) P—Cl and S—Cl
(e) C—H and N—H (f) S—O and P—O (g) C—N and
N—N
8. (a) What is an intermolecular bond?
(b) What type(s) of intermolecular forces of
attraction may form between nonpolar molecules?
What type(s) may form between polar molecules?
Give reasons in both cases.
10. How do intermolecular bonds help to explain why
the boiling point of methane, CH4, is much lower
than the boiling point of hydrogen bromide, HBr?
p.53
1. Classify each of the following reactions as a
synthesis reaction or a decomposition reaction. Give
reasons for your classification.
(a) 2 KI(s) → 2 K(s) + I2(s)
(b) H2(g) + Cl2(g) → 2 HCl(g)
(c) ZnCO3(s) →ZnO(s) + CO2(g)
4. Complete each of the following single
displacement reactions. Make sure that your final
equation is balanced.
(a) Zn(s) + CuCl2(aq) →
(b) Ca(s) + HCl(aq) →
(c) Na(s) + H2O(l) →
7. Classify each of the following reactions as a
single displacement reaction or a double
displacement reaction. Predict the products of each
reaction, and write the balanced chemical equation.
(a) Silver metal is recovered in a laboratory by
placing aluminum foil into aqueous silver nitrate:
Al(s) + AgNO3(aq) →
(b) Hydrogen gas can be produced in the lab from
the reaction of zinc and sulfuric acid (H2SO4):
zinc + sulfuric acid →
(c) The presence of chloride ions in a water sample
is indicated by the formation of a white precipitate
when aqueous silver nitrate is added to the sample:
aqueous magnesium chloride + aqueous silver nitrate →
(d) Sodium metal reacts vigorously with water to
produce a flammable gas and a basic (hydroxide)
solution:
sodium + water→
(e) Aqueous potassium hydroxide is added to a
sample of well water. The formation of a rusty
brown precipitate indicates the presence of an
iron(III) compound in the water:
KOH(aq) + FeCl3(aq) →
p.57
1. Determine the products (if any). If a reaction
occurs, summarize the reaction as a balanced
chemical equation. For each, write the total/net
ionic equations, identify the spectator ions.
(a) a solution of lead(II) nitrate mixed with a
solution of sodium chloride
(b) a solution of sodium sulfate mixed with a
solution of calcium chloride
(c) a solution of magnesium acetate mixed with a
solution of silver nitrate
(d) a solution of sodium acetate mixed with a
solution of potassium chloride
p.62
1. Using the solubility rules, determine whether
each of the following compounds is soluble in water:
(a) lead(II) sulfate
(b) ammonium sulfide
(c) silver nitrate
(d) silver chloride
(e) calcium carbonate (f) ammonium hydroxide
(g) barium hydroxide