Download Exam 1 Review Sheet

Review for Exam #1 (9/22/06)
Study suggestions:
1. Read (and/or re-read) the entire assignment.
2. Review your notes from lecture and from the text.
3. In addition to the important concepts listed below, make sure you understand
all of the facts and concepts Chang has summarized at the end of each
chapter along with the key words he has listed.
4. Know how to work assigned and example problems. It’s easy to look at
solution keys and work to a known answer, but remember that you won’t have
the answers on exam day. Be honest with yourself: do you really know how
to work a problem? Do you truly understand the concepts behind it?
5. If the answers to the questions posed in #4 are ‘no’ or ‘maybe not,’ you have
a number of options. In no particular order: (#1) Re-read the relevant section
of the chapter & follow along with the examples. (#2) Consult a classmate for
an explanation. (#3) Consult the evening tutors. (#4) Consult me: in person,
by e-mail, or by phone.
6. If the answers to the questions posed in #4 are ‘yes’ or ‘I think so,’ don’t be
satisfied! Practice more problems.
7. Start early!
Chapter 1:
Concepts:
Element
Atom
Compound
Molecule
SI Units
Density (know the formula: density = mass/volume)
Scientific notation
Be able to:
Calculate density given mass and volume
Calculate volume given density and mass
etc.
Convert between °C and K given that 0K = -273.15°C
Manipulate unit prefixes given Table 1.3
Use scientific notation correctly (know that the N in N x 10n should be between 1
and 10)
Pertinent problems from the book:
1.20, 24, 26, 34, 36, 38, 40, 42, 44, 48, 54, 56, 62
Chapter 2:
Concepts
Electron (negative charge)
Proton (positive charge)
Neutron (no charge)
Atomic number: # protons: defines an atom’s identity (which element?)
Mass number: total number of neutrons and protons
Isotopes: same atomic number, different mass number
Molecule
Ion (know cation (+) vs. anion (-))
Chemical formulas:
Molecular formula: exact number of atoms of each element
in the smallest unit of a substance
Empirical formula: simplest whole-number ratio of atoms
For ionic compounds: formula = empirical formula, not necessarily
true for molecules
Be able to:
Given mass number & atomic number of an atom or ion, determine
# neutrons/protons/electrons
Identify atoms, diatomic molecules, polyatomic molecules, elements,
compounds, anions, and cations.
Determine an empirical formula given a molecular formula.
Balance charges in ionic compounds
Use table 2.3 to name ionic compounds given formulas or to determine formulas
given names.
Pertinent problems from the book:
2.10, 12, 14, 16, 32, 34, 42, 44, 46, 48, 56, 59, 62, 72
Chapter 3:
Concepts
Atomic mass
Isotopes and average atomic mass
Molecular mass
Mole
Avogadro’s number
Molar mass
Percent composition
Chemical equations
Limiting reagent
Reaction yield
Theoretical yield
Percent yield
Be able to:
Use (and know) the average atomic mass equation. For example, given the
atomic masses and abundances of two (or three or four) isotopes, calculate the average
atomic mass. Or, given the average atomic mass and the masses of some isotopes,
calculate their abundances.
Determine molecular and molar masses. Use molar mass to determine the mass
of a certain number of molecules, the number of moles of a given mass of a molecule,
etc.
Use (and know) the percent composition equation (equation 3.1 on page 66).
Given a percent composition or set of masses in a sample of a compound (see
example 3.11), determine the empirical formula.
Write and balance equations.
Use balanced equations to relate quantities of reactants and products.
Given starting reactant masses or # moles, determine the limiting reagent.
Calculate the amount in excess of the excess reagent(s).
Use the limiting reagent concept to calculate the amount of product generated
(theoretical yield). Given an actual yield, calculate a percent yield.
Pertinent problems from the book:
3.5, 8, 12, 14, 16, 18, 20, 22, 24, 30, 42, 44, 48, 50, 52, 54, 60, 64, 66, 70, 72,
74, 78, 82, 84, 86, 90, 92, 94, 104, 106, 112