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Review for exam 1:
Chapter 1
Definitions - chemistry, matter, mass, energy, kinetic energy, potential energy
Conservation of mass, conservation of energy
States of matter (solid, liquid, gas) and their general properties; condensed phase, fluid
Crystalline and amorphous solids
Pure substances and mixtures, homogeneous mixtures (solutions), heterogeneous mixtures
Elements and compounds; atoms and molecules
Physical properties, chemical properties
Scientific notation
SI units; the seven base units; derived units
The metric system, metric prefixes, their size and symbol
Volume units, m3, cm3, L, mL
Temperature scales (Celsius, Fahrenheit, Kelvin); conversion among these scales
Precision and accuracy; intensive and extensive properties
Rules for counting significant figures
Significant figures for addition/subtraction and multiplication/division, and combinations of these
Rounding off numbers
Conversion factors and dimensional analysis
Chapter 2
Early theories of matter - continuous or discrete
Dalton's atomic theory
Electrons - discovery and properties; charge to mass ratio
The plum pudding model and the nuclear model; Rutherford experiment and explanation
Protons, neutrons, electrons and their general properties
Atomic structure, the nucleus, electron cloud charge
Redefinition of an element
Atomic number (Z), mass number (A), isotopes, notation for isotopes of atoms
Number of protons, neutrons, and electrons, and approximate atomic mass (in amu) for an isotope
Radioactivity; alpha, beta, and gamma rays
Nuclear stability
Atomic mass units (amu); definition and use
Mass spectrometry and its use to find atomic and molecular mass
Atomic mass for unstable elements; average atomic mass for stable elements and its calculation
The periodic table
general organization of the table, rows (periods) and columns (groups)
main group, transition metals, lanthanides, actinides
alkali metals, alkali earth metals, halogens, noble gases
metals, nonmetals, metalloids (semimetals); general properties and location
The mole; definition, Avogadro’s number; molar mass
Use of the mole concept in calculations; conversion from moles to number of atoms
Chapter 3
Mass and energy; kinetic energy and potential energy
Units for energy; conversion between energy units
Properties of waves; wavelength, frequency, and speed; intensity and amplitude
Light; the electromagnetic spectrum; regions of the spectrum from highest to lowest energy
(gamma ray, X-ray, ultraviolet, visible, infrared, microwave, radio frequency)
Relationship between wavelength (), frequency (), and speed of light c; (c = )
Constructive and destructive interference
Wave properties of light; double slit experiment
Particle properties of light; the photoelectric effect and its explanation
Quantization of energy; photon energy formula E = h = (hc/)
Atomic spectra; spectrum for hydrogen atoms
Rydberg formula and relation to energy levels, quantum number n
De Broglie wavelength; electron diffraction
Heisenberg Uncertainty Principle (x) (p)  h/4
Quantum numbers for the electron in hydrogen; restrictions and meaning
n - principle quantum number; relationship to energy and distance from nucleus
 - angular momentum quantum number; relationship to orbital type (s, p, d, ...)
shapes of s, p and d orbitals
radial nodes
m - magnetic quantum number; relationship to the number of different orbitals
ms - spin quantum number; relationship to electron spin
Determining possible values for n, , m, and ms
n = 1, 2, 3, …
Examples:
If n = 3,  = 0, 1, 2
 = 0, 1, 2, … (n-1)
If  = 2, m = -2, -1, 0, +1, +2
m = -, …, +
ms = - 1/2, +1/2
Electron configuration for atoms
Pauli principle
Aufbau principle (ground states of atoms)
Hund's rule (diamagnetic and paramagnetic)
Order of energy for orbitals 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < …; mnemonic device
Shorthand notation for electron configuration (using noble gases)
Orbital filling diagrams; counting unpaired electron spins; diamagnetic and paramagnetic
Electron configuration and the periodic table; core and valence electrons
Anomolous electron configurations; transfer of one s electron to give a half-filled or filled d
orbital (Cr, Mo, Cu, and Ag)