Ch 221 Exam #1 Study Outline
Fall, 2016
NOTE: Use this outline at your own risk. Hopefully I haven't forgotten anything, but sometimes I do! It is meant to be a study
aid and is not meant to be a replacement for actually reviewing the lecture notes and homework assignments.
Ch 1 - Matter, Energy, and the Origins of the Universe
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chemistry, matter, substance, energy
states of mater - solids, liquids, gases
forms of energy: work=force x distance, kinetic and potential energy, Law of Conservation of Energy
classes of matter – elements, compounds, mixtures (hetero- and homogeneous)
separating mixtures: distillation, filtration, chromatography
memorize the names and symbols of the first 38 elements PLUS Ba, Pt, Pb, Sn, Ag, Cd, Hg, Au, I, Xe, U
physical and chemical properties
physical and chemical changes
extensive vs. intensive properties
scientific method - data, hypothesis, law, theory
Early Chemical discoveries NOTE: this material is not found in the book in any organized fashion, so use your lecture
notes to study these: Law of Definite Proportions, Law of Multiple Proportions, Law of Conservation of Mass
Dalton's Atomic Theory
Chemical, molecular and structural formulas
Metric System - SI units, base and derived units
SI prefixes (memorize Table 1.1 from pico to tera)
metric-metric conversions
accuracy and precision
Significant figures, rounding off rules mult/div and add/sub
Dimensional Analysis (Factor-Label method) and conversion factor calculations. All English-metric conversions will be
given to you and whether or not they are exact
density
2 and 3-D conversions
percent as a conversion factor
temperature scales
Ch 2 - Atoms, Ions and Compounds
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Thomson's experiments with cathode rays and the results
Thomson's model of the atom (“plum pudding”)
Millikan oil drop experiment and determination of the charge and therefore mass of the electron
Radioactivity and associated particles
Rutherford's gold foil experiments and the results
Rutherford’s Nuclear atom nuclear atom
atomic mass units
p and n about 2000X more massive than the electron, so most of the mass of the atom is the nucleus
isotopes
Z = atomic number, A = mass number, X = element symbol
Calculating atomic mass
Mendeleev’s periodic table - arranged elements by atomic mass, predicted presence of new elements
The Modern Periodic table - arranges elements by increasing atomic number, not mass
groups (families) and periods (rows)
the seven nonmetals that are always found as diatomics
molecular mass (molecular weight), formula units, formula mass
the mole, Avogadro’s Number (given)
calculations between, moles, mass and particles
continued on the back 
Ch 3 – Atomic Structure: Explaining the Properties of Elements
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Electromagnetic radiation
Properties of waves – u =  (memorize)
Atomic spectra – absorption (dark lines) and emission (light lines)
Quantum Theory: Blackbody radiation and photoelectric effect – explained by quantizing light as particles or photons
Calculation photon energies using E = h = hc/ (memorize)
Hydrogen spectrum
The Rydberg Equation (given)
The Bohr Model of Hydrogen – emission and absorption of a photon, the energy gap between levels has to equal the
photon energy, or E =  h
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Wave-Particle duality – standing waves, DeBroglie Wavelength DB = h/mv
Quantum Mechanics – wavefunction , atomic orbitals, shells, subshells, quantum numbers
Atomic orbitals as probability regions within which the electron is 90% probable of being found.
rd
Memorize and be able to draw all of the orbitals in the 3 shell (including coordinate axes and names)
Quantum Numbers