CHEMISTRY 222
Rogue Community College
STUDY GUIDE FOR EXAM #1 (Thursday, 1/30/14)
A periodic table and a list of equations will be provided for you with the exam.
Chapter 8:
Vocabulary: valence electrons, Lewis structure, octet rule, single bond, double bond, triple bond,
lone pair, electronegativity, bond polarity, molecular polarity, polar, nonpolar, formal charge,
resonance, incomplete octet, expanded octet, VSEPR, linear, trigonal planar, bent, tetrahedral,
trigonal pyramidal, trigonal bipyramidal, see-saw, T-shaped, octahedral, square pyramidal, square
planar, isomer, structural isomer, stereoisomer, geometric isomer, optical isomer, chiral,
stereospecific, axial, equatorial
Skills: use and distinguish between vocabulary terms; draw Lewis structures (you may need to
review Ch. 7); determine whether a bond is polar or nonpolar based on electronegativity differences
(0.4 is the dividing line between polar and nonpolar bonds); determine the shape of a molecule or
polyatomic ion from its Lewis structure; determine the polarity of a molecule from its
electronegativity differences and shape; classify isomers; determine the number of isomers for a
given molecule with a given shape
Chapter 9:
Vocabulary: sigma bond, pi bond, internuclear axis, hybridized atomic orbitals (sp3, sp2, sp, sp3d and
sp3d2), molecular orbitals (, *, , *), bonding & antibonding orbitals, constructive & destructive
interference, bond order, photodissociation, paramagnetic, diamagnetic, delocalized electrons, cis
isomer, trans isomer
Skills: use and distinguish between vocabulary terms; determine the hybridization of central atoms in
Lewis structures; determine the numbers of sigma bonds and pi bonds in a molecule or polyatomic
ion; calculate the bond order of a homonuclear diatomic molecule or ion and determine whether it is
paramagnetic or diamagnetic; recall that in benzene (C6H6), the molecule has a planar hexagonal
shape, each carbon is sp2 hybridized and the  electrons are delocalized
Chapter 13:
Vocabulary: gas, pressure, barometer, manometer, volume, temperature, mole, density, molecular
weight, STP (273.15 K, 1 atm), Boyle’s Law, Charles’ Law, Avogadro’s Law, mm Hg, torr, atm,
molar volume, Dalton’s Law, mole fraction, partial pressure, vapor pressure, ideal gas, real gas,
kinetic theory of gases, kinetic energy, speed, root mean square speed, diffusion, effusion, Graham’s
Law, mean free path, van der Waals equation, direct vs. inverse proportion
Skills: use and distinguish between vocabulary terms; perform calculations using Boyle’s Law,
Charles’ Law, Avogadro’s Law, the ideal gas equation, density and molecular weight, Dalton’s Law,
Graham’s Law, the equations of kinetic molecular theory and the van der Waals equation; perform
stoichiometry calculations in which at least one of the reactants or products is a gas; describe the
conditions under which a gas will behave more ideally; use the concepts of kinetic molecular theory
to compare gases in terms of average kinetic energy, average molecular speeds and diffusion/effusion
rates; describe how molecular speeds are distributed at different temperatures
Chapter 15:
Vocabulary: intermolecular forces; kinetic molecular theory; solid; liquid; gas; fluid; condensed
phase; vaporization; condensation; melting; freezing; heat of vaporization; heat of fusion; dipole;
induced dipole; London forces; dipole-dipole interactions; hydrogen bonding; surface tension;
viscosity; crystalline; amorphous; x-ray diffraction; unit cell; simple cubic cell; body-centered cubic
cell; face-centered cubic cell; metals; ionic compounds; molecular covalent solids; network covalent
solids; conductor; insulator; semiconductor; band gap; valence band; conduction band; phase
diagram; triple point; critical temperature (Tc); critical pressure (Pc); vapor pressure; dynamic
equilibrium; melting point (Tm); boiling point (Tb); liquid crystal; colloid; micelle; sol; aerosol; foam;
emulsion; gel; Tyndall effect;
Skills: use and distinguish between vocabulary terms; place substances in order of increasing or
decreasing surface tension, viscosity and/or boiling point on the basis of relative polarity, H-bonding
and molecular weight; distinguish between solids, liquids and gases on the basis of definite
volume/shape, fluidity, density, compressibility, and molecular motion; find the total number of
atoms in a given unit cell; interpret phase diagrams to give triple point, critical temperature and
pressure, melting point and boiling point and to explain the effect that pressure changes have on Tm
and Tb; perform heat flow calculations that include temperature changes or phase changes or both;
calculate the triple point of a substance, given equations for the vapor pressure of its solid and liquid;
recall that sols, aerosols, foams, emulsions and gels are all examples of colloids
Interchapter I:
The main group metals are the alkali metals, alkaline earth metals, Al, Ga, In, Tl, Sn, Pb, and Bi.
Be is found in gemstones. Mg is found in seawater, fireworks (white), flashbulbs and automobile and
aircraft parts. Ca is found in milk, bones, teeth, egg shells and plaster. Sr is found in signal flares and
fireworks (red). Sr-90 from radioactive fallout mimics Ca in the body and is a major health hazard.
Ba is found in signal flares, fireworks (green) and rat poison. All isotopes of Ra are radioactive. Al is
the most abundant metal in the earth’s crust, is highly reactive and forms a protective oxide coating in
air that resists corrosion. Ga will melt in your hand (Tm = 30oC). Pb is found in the mineral galena. It
is found in paints and batteries, used to be found in pipes and as a gasoline additive, and it is very
poisonous. (Pencil “lead” is C, not Pb.) Sn is found in the mineral cassiterite. It is used in tin-plated
food cans, solders, pewter and bronze. Bi is used in a variety of alloys such as pewter. Bi alloys tend
to be low-melting, making them useful for fuses and fire-extinguisher sprinkler-head plugs.
Interchapter J:
Sulfur is a crumbly, yellow solid that exists as S8 molecules which have rhombic and monoclinic
allotropes. Large deposits are found on Io, a moon of Jupiter. Melted sulfur thickens as it is heated,
due to the S8 rings breaking, forming long chains and becoming entangled. Sulfuric acid (H2SO4) is
the #1 industrial chemical worldwide, and it is a powerful dehydrating agent. Hydrogen sulfide (H2S)
smells like rotten eggs. The tarnish that forms on silver surfaces is silver sulfide.
Lab:
Give examples of molecules and/or polyatomic ions with a given geometry. Use formal charges to
explain why O3 is polar and CO is nonpolar. Use isomer logic to explain why CH2Cl2 and CHFClBr
are tetrahedral. Give examples of polar molecules with polar bonds, nonpolar molecules with polar
bonds and nonpolar molecules with nonpolar bonds.
Describe the liquid oxygen demo, and explain why oxygen is paramagnetic. Describe the Boyle’s
Law, Charles’ Law, Pressure-Temperature relationship, and air pressure demos, and give
explanations or graph data, as appropriate.
Describe observations, perform calculations and do error analysis from the Atomic Weight of
Magnesium Lab.
Describe and explain the basic set-up of the Thin Layer Chromatography experiment, and explain
how it can be used to separate compounds in mixtures.