2010 Chemistry Final Exam Review
The
final exam will be objective (multiple choice).
Please
bring to the exam:
Two number 2
pencils, your calculator, blank notebook paper.
You
will be given reference sheets with the following:
1) Periodic table
2) Table of Common
polyatomic ions
3) Tables of
Activity series and Solubility
4) Electronegativity
Table
5) Constants
needed for equations: speed of light,
Planck’s constant
6) Equations:
E = h n c =
l n
PV = nRT V1 = V2
P1V1 = P2V2 vA =
mB
T1 T2 vB mA
Concepts to review:
Chapter 5
Measurements and Calculations
Factor-Label methodology
Significant figures
SI units
Metric conversion factors
Chapter 6 &
7 Chemical Composition and Chemical
Reactions
Chemical equations
Symbols
Skeletal
equations
Reactants/products
Balancing
chemical equations
Law
of conservation of mass
Law
of conservation of energy
Law
of definite proportions
Law
of definite composition
Types
of reactionsàBe able to recognize and identify
by equation
Determine
products of chemical reactions (Be able to predict products
from given
reactants)
Chapter 6 Chemical
Composition & Chapter 15 Solutions
Moleà definition; mole concept; Avogadro’s number
Molar
mass—what it is; how to find
Atomic
mass and Molecular mass
Molar
conversions
Concentration
Molarity
Preparing
a solution of given molarity
Percent
compositionàhow to find
Empirical
formulaà what it is, how to determine
Molecular
formulaà what it is, how to determine
Chapter 8 Reactions in Aqueous Solutions
Be able to:
1) Write and/or identify molecular
equations.
2) Write and/or identify complete ionic
equations.
3) Write and/or identify net ionic
equations.
4) Identify spectator ions.
5) Identify element in the reactions that is
oxidized.
6) Identify element in the reactions that is
reduced.
Chapter 9 Chemical Quantities and Stoichiometry
Be able to:
1) Determine the
number of moles of reactants/products in a chemical reaction using mole ratios.
2) Calculate
masses of reactants/products if you are given mole number or mass
3) Interpret given
data to determine the amounts of reactants/products in replacement reactions involving
molarity.
4) Determine the
limiting reactant in order to predict the products of a reaction (both mole and
mass amounts).
5) Calculate the
percent yield using the ratio of experimental mass to theoretical mass.
6) Be able to find
the percent error in a lab.
Chapter 13 Gases
Be able to:
1) Describe a gas
on the submicroscopic level and how it is affected by changes in pressure,
temperature, and volume.
2) Explain what
gas pressure is and describe how it can be measured.
3) Describe and
apply the gas laws:
Charle’s Law
Boyle’s Law
Graham’s Law
Ideal Gas Law
4) Determine changes in pressure, volume,
temperature, and moles of a gas sample.
5) Recognize and
use conditions of standard temperature and pressure.
6) Apply
stoichiometric principles to calculate the amount of gas produced in a chemical
reaction.
7) Differentiate
ideas gas behavior from real gas behavior.
8) Explain gas
behavior using the kinetic molecular theory.
Chapter 11 Modern Atomic Theory
Be able to:
1) Identify
factors that influence the deflection of charged particles.
2) Determine the
similarities/differences of the atomic models of
3) Determine the
difference between ions and atoms.
4) Identify the characteristics
of protons, neutrons, and electrons
(size, mass, charges).
5) Distinguish
between atomic number and atomic mass.
6) Identify
isotopes.
7) Determine the
number of protons, electrons, and neutrons in atoms and in isotopes from the
periodic table.
8) Describe/understand
the properties of waves (both water and light waves).
9) Explain the
relationship between energy and frequency of light. E = h n
10) Explain the
relationship between wavelength and frequency. c =
l n
11) Distinguish
characteristics of the electromagnetic spectrumàwavelength vs. frequency and
their relationship.
12) Describe the
quantized nature of energyàWhat does quantum mean?
13) Describe the
different quantum numbers and what each means.
14) Predict the
location of electrons in an atom using quantum numbers and orbitals.
15) Draw orbital
diagrams to show electron configurationàknow filling order by diagonal
diagram.
16) Draw/write
electron configurations for neutral atoms and ions—both longhand and shorthand.
17) Describe
sections of the periodic table (metals, nonmetals, transition metals, inner
transition metals, alkali metals, alkali earth metals, halogens, noble gases).
18) Distinguish
between periods and groups (families) of the periodic table and know
characteristics of each.
19) Relate the
electron configuration and chemical properties of an element to its position on
the periodic table.
20) Distinguish
between valence electrons and core electrons
21) Determine the
number of valence electrons for a representative element using the periodic
table.
22) Predict the
stable ion formed from an atom from its position on the periodic table.
23) Describe and
explain why periodic trends exist for: nuclear charge, shielding, atomic radii,
ion size, ionization energy, electronegativity).
Chapter 12 Chemical Bonding
Be able to:
1) Describe the
nature of a chemical bond.
2) Compare and
contrast ionic and covalent bonds.
3) Predict whether
bonds are ionic, polar covalent, or nonpolar covalent using electronegativity
values.
4) Determine
partial charge distribution of a polar covalent bond.
5) Draw Lewis dot
diagrams for atoms, molecules, and ions (using octet rule).
6) Identify
limitations and exceptions to the octet rule.
7) Predict the
shapes of molecules (Table 12-4 p. 431 plus your notes).
8) Draw dipole
moments and use it to determine if a molecule is polar or nonpolar.
Chapter 14
Intermolecular Forces
Be able to:
1) Explain how the
three types of intermolecular forces (IMF) arise.à dispersion, dipole-dipole,
hydrogen bonding
2) Compare the
solid, liquid, and gas states in terms of the intermolecular forces.
3) Analyze the
structure of molecules to determine the type of IMF that will occur.
4) Explain change
of phase terminology.
5) Interpret the
features of heating curves and explain why they occur.
6) Explain the
molecular basis for surface tension and capillary action.
7) Explain the
unique properties of water.
8) Know what heat
capacity, heat of fusion, and heat of vaporization mean.
Chapter 16 Acids and Bases
Be able to:
1) Identify common
acids and bases.
2) Describe
macroscopic properties of acids and bases..
3) Describe the
neutralization of an acid or base.
4) Describe the pH
scale as it relates to acids and bases…know what number is neutral and which
numbers represent acids and bases.
Chapter 19 Nuclear
Reactions
Be able to:
1) Complete nuclear
equations with alpha, beta minus, or beta positive particles.
2) Distinguish
between alpha, beta minus, or beta positive particles and know their symbols.
3) Explain why
nuclear reactions occur.
4) Distinguish
between nuclear fission and nuclear fusion.
5) Explain C-14
dating.