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Transcript
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)