Honors Chemistry: Final Exam Study Topics
law of
conservation of mass
law of
conservation of energy
pure science
vs. technology
organic /
inorganic compounds
scientific
law
theory
phlogiston vs. combustion theory of burning
hypothesis
properties
of acids and bases
the
scientific method
controlled experiment
avoid bias (Drunken Goldfish book)
conclusions must follow logically from data
quantitative
and qualitative observations
graphing
(line, bar, pie)
laboratory
equipment
SI System
(Metric System)
base units [meter, second, liter, gram]
derived units
prefixes [kilo-, base, deci-, centi, milli-, micro, atomo-]
Measurement
scientific notation
Accuracy vs.
precision
Conversion
Factors
safety
Material
Safety Data Sheet
Chronic
vs. Acute exposure
LD50 values
reactants
and products
chemical and
physical properties
extensive vs. intensive properties
color, boiling point, density, mass
chemical and
physical changes
states of
matter (solid, liquid, gas)
phase diagram
sublimation (solid --> gas)
energy:
potential and kinetic
KE = ½ mv2
endothermic
and exothermic reactions
effect of catalyst (activation energy)
Nuclear
energy
fission (splitting atoms) & fusion (joining nuclei)
half-life (radioactive decay)
heat vs.
temperature
temperature scales (Celcius, Kelvin, Farenheit)
oF
32 = 1.8 oC &
oC + 273
= K
absolute
zero
calorimetry problems heating curve
(specific
heat, latent heat, heat of fusion, heat of vaporization)
latent
heat
Classification of Matter
pure
substances: elements and compounds
vs. mixtures
heterogeneous
and homogeneous mixtures
solution (alloys), colloid, suspension
atoms
HOBrFINCl twins (diatomic), P4 S8 (polyatomic), allotropes
SI base
units
conversions
density
Archimedes Principle water displacement method
metals,
nonmetals, metalloids
Separation techniques
magnetism, distillation, chromatography, centrifugation, decant,
evaporation, electrolysis
Problem solving
Fermi approximations
development
of model of atom
Greek, Dalton, Thomson, Rutherford, Bohr, Quantum mechanical model
Cathode Ray tube electrons
Gold-foil experiment nucleus (atom mostly empty space)
alpha particles (He2+ nucleus) deflected away
Geiger-counter
Bohr model electrons in fixed orbit
Quantum mechanical model electrons in orbitals (s, p, d,
and f-orbitals)
electrons, protons, neutrons
electron
configuration
1s22s22p63s23p64s23d104p65s24d10
[shorthand configuration]
excited state vs. ground state
Filling
order of electrons in atom
Aufbau
Principle (bottom to top);
Pauli
Exclusion Principle (two electrons per orbital);
Hunds
Rule (most unfilled orbitals)
light (dual
nature...particle & wave)
electromagnetic spectra ...IR...ROYGBIV...UV...
high frequency...short wavelength (high energy)
c = f / l
(c = 3 x 108 m/s)
E = h f (h = 6.6 x 10-34 J/Hz)
continuous vs. quantized energy
emission spectra
lyman series (UV), balmer series (visible), paschen series (IR)
periodic
table
atomic
number (# protons), mass number (# protons +
# neutrons)
isotopes
(same element (# protons) but different # neutrons)
isotope notation: C-12 vs.
C-14
ions
(same element (# protons) but different number of electrons
cations
(+) charge: formed from metals that
lose electrons
anions
(-) charge: formed from non-metals
that gain electrons
average
atomic mass
AAM = (% A)(mass A) +
(%B)(mass B) + ...
Periodicity
(Periodic Table Trends)
Mendeleev & Mosely
atomic mass vs. atomic number
group,
period
names of
elements (Greek, location, planets, people, Latin, synthetic)
names of
families and groups...alkali metals, alkaline earth metals, transition metals,
halogens, noble
gases,
lanthanide and actinide series, coinage metals, metalloids, essential elements
trends in
atomic / ionic radius
down a column (family) atoms get larger due to increasing shielding
effect
across a period (horizontally) atoms get smaller due to increased
coulombic attraction
valence
electrons
ionization
energy
cations,
anions
electronegativity
nuclear
fission and nuclear fusion
Avogadro's
number
molar mass,
moles, atoms
properties
of metals
salts
metal & non-metal
properties
of ionic compounds
strong bonds, high melting points, rigid
oxidation
number
apparent
charge
finding
formulas from oxidation number
naming
compounds
binary (with fixed charge Group 1, 2, Ag, Zn, Al)
binary (with variable charge)
Stock system (uses Roman numeral to signify charge on metal ion)
Old system -ic (higher oxidation state) & -ous
(lower oxidation state)
polyatomic ions
memorize ates PO43-,
SO42-, CO32-, NO31-
& CN1-, OH1-
-ites one less oxygen
hypo ___-ite two less oxygen
per___-ate one more oxygen
percentage
composition (by mass)
formula of a
hydrate MN. XH2O
properties
of covalent compounds
ionic
(transfer electrons), covalent (share electrons), hydrogen bonds
Lewis
dot structures
single,
double, triple covalent bonds
structural
diagrams
empirical
formula / molecular formula
mole island
1 mole = 22.4 L @ STP =
6.02 x 1023 particles
= Molar Mass
The following is a brief list of many of the topics we covered first semester. All topics covered on the final man not be listed below. Use your own notes to check for completeness.