Chemistry 108 - Review Sheet for Exam #3
As a guide for studying, you should be familiar with the concepts listed below.
Chapter 6: Energy
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Chapter 7: Gases
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Chapter 10: Modern Atomic Theory
orbital
principal energy levels
orbital sublevels
electron configuration
valence electrons
metals
non-metals
Sample problems: 25, 26, 27, 30, 41, 42, 45
Chapter 11: Chemical Bonding
bond
ionic bonding
ionic compound
covalent bonding
polar covalent bond
electronegativity
Lewis Structures
duet rule (H)
octet rule
bonding pair of electrons
lone pair of electrons
single bond
double bond
molecular geometry
linear
trigonal structure
tetrahedral structure
VSEPR theory
Sample problems: 5, 6, 12, 14, 18, 26, 38, 56, 60, 63, 66, 68, 77, 82, 83
Chapter 12: Gases
barometer
mm Hg
torr
standard atmosphere
Boyle's Law
absolute zero
Charles' Law
Avagadro's Law
universal gas constant
ideal gas law
molar volume
standard temperature pressure (STP)
Sample problems: 3,8,18,24,25,32,36,42,52,56,62,70,79,82,86,100
Chapter 15: Acids and Bases
Acid
Base
Bronsted-Lowry model
Proton Donor/Acceptor
Lewis acid
Electron pair donor/acceptor
Conjugate acid-base pair
conjugate acid
conjugate base
Strong Acid/Base
weak acid/base
neutral solution
[H+] concentration
pH = -log[H+]
hydronium ion
pH scale
buffered solution
Chapter 18:
oxidation
reduction
oxidation-reduction
half-reaction
anode
cathode
battery
oxidizing agent
reducing agent
oxidation number
electron-transfer reaction
activity series
Chapter 3
binary ionic compound (type I & II ionic; metal-nonmetal compounds)
type III binary compounds with only nonmetals
polyatomic ion (sulfate, nitrate, carbonate, phosphate)
naming acids (nitric, sulfuric, HCl, phosphoric)
memorize the chemical symbols of atoms 1-18
Dalton's atomic theory
atom (what subatomic particles are present in an atom?)
compound (difference between an element, or diatomic molecule)
chemical formulas (diatomic, monoatomic, binary, polyatomic)
electron (relative mass & number in atom)
nucleus (protons & neutrons and number of each in an atom)
isotopes (definition & designation - 126C)
periodic table & groups (similarity in chemical reactivity, valence, etc.)
alkali & alkaline earth metals (what groups are these? what is their valence?)
halogens & noble gases (group & valence)
transition metals (where are these in the periodic chart?)
nonmetals & metalloids (semimetals) (where are these in the periodic chart?)
diatomic molecules (e.g., H2 vs Ne vs Na)
ions, cations, & anions (valence of different elements & names of each)
matter & states of matter (solids, liquids & gases)
physical & chemical properties (what is the difference? give examples)
physical & chemical changes (what is the difference? give examples)
element, molecule, compound & mixtures (how do these differ?)
pure substance & solutions (definitions & examples)
homogeneous & heterogenous mixtures (give example)
distillation & filtration (differences & definitions)
energy - calorie, joule & specific heat capacity (values & definitions)
measurements, units, SI units (what are these units?)
mass, volume, length & density (what are the units of each?)
Fahrenheit & Celsius temperature conversions (can you convert between each?)
scientific notation & significant figures
Chemistry 60 - Review Sheet for Exam 3
November 16, 1998
Chapter 6: Chemical Reactions
chemical reaction
chemical equation
reactant
coefficient
product
balancing a chemical equation
Sample problems: 37, 40, 44, 74, 68
Chapter 7: Reactions in Aqueous Solution
Solubility Table 7.1
precipitation reaction
strong electrolyte
soluble solid
insoluble solid
molecule equation
complete ionic equation
spectator ions
net ionic equation
acid - strong acid
base - strong base
salt
Sample problems: 7, 14, 15, 16, 18, 25, 30, 33, 39, 40
Chapter 8: Classifying Chemical Reactions
oxidation-reduction reaction
combustion reaction
synthesis (combination) reaction
decomposition reaction
Sample problems: 4, 5, 10, 12, 14, 17, 21, 26
Other Concepts:
binary ionic compound (type I & II ionic)
type III binary compounds - nonmetals
polyatomic ion (sulfate, nitrate, carbonate, phosphate)
acids (nitric, sulfuric, HCl, phosphoric)
chemical symbols of atoms 1-18
chemical formulas (diatomic, monatomic, binary, polyatomic)
diatomic molecules (e.g., H2)
ions, cations, & anions
matter & states of matter
You should be familiar with each of the terms listed for each chapter. You should also solve the problems indicated. Study hard. Make certain you understand the concepts and problems. Exam is scheduled for November 18, 1998
Chapter 8: Chemical Composition
atomic mass unit (amu)
average atomic mass
mole
Avogadro's number
molar mass
mass percent
empirical formula
molecular formula
Sample problems: 5, 8, 9, 12, 14, 22, 27, 31, 35, 38, 39, 42, 45, 51, 55, 60, 61, 69, 75, 77, 89
Chapter 9: Chemical Quantities
mole ratio
stoichiometry
stoichiometric quantities
theoretical yield
percent yield
Sample problems: 4, 7, 9, 11, 13, 19, 25, 27, 32, 41, 45, 51
Chapter 10: Modern Atomic Theory
orbital
principal energy levels
orbital sublevels
electron configuration
valence electrons
metals
non-metals
Sample problems: 25, 26, 27, 30, 41, 42, 45
Chapter 11: Chemical Bonding
bond
ionic bonding
ionic compound
covalent bonding
polar covalent bond
electronegativity
Lewis Structures
duet rule (H)
octet rule
bonding pair of electrons
lone pair of electrons
single bond
double bond
molecular geometry
linear
trigonal structure
tetrahedral structure
VSEPR theory
Sample problems: 5, 6, 12, 14, 18, 26, 38, 56, 60, 63, 66, 68, 77, 82, 83
Chapter 12: Gases
barometer
mm Hg
torr
standard atmosphere
Boyle's Law
absolute zero
Charles' Law
Avagadro's Law
universal gas constant
ideal gas law
molar volume
standard temperature pressure (STP)
Sample problems: 3,8,18,24,25,32,36,42,52,56,62,70,79,82,86,100
Chapter 15: Acids and Bases
Acid
Base
Bronsted-Lowry model
Proton Donor/Acceptor
Lewis acid
Electron pair donor/acceptor
Conjugate acid-base pair
conjugate acid
conjugate base
Strong Acid/Base
weak acid/base
neutral solution
[H+] concentration
pH = -log[H+]
hydronium ion
pH scale
buffered solution
Chapter 18:
oxidation
reduction
oxidation-reduction
half-reaction
anode
cathode
battery
oxidizing agent
reducing agent
oxidation number
electron-transfer reaction
activity series