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67 Cards in this Set
- Front
- Back
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femto (f)
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10^(-15)
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pico (p)
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10^(-12)
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tera (T)
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10^12
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giga (G)
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10^9
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mega (M)
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10^6
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kilo (k)
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10^3
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centi (c)
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10^(-2)
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milli (m)
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10^(-3)
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micro (mu)
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10^(-6)
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nano (n)
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10^(-9)
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joule
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kg*m^2*s^(-2)
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coulomb
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A*s
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hertz
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s^(-1)
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electron mass m
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9.11 × 10^(-31) kg
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speed of light c
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2.998 x 10^8 m/s
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equation for speed, wavelength, and frequency of electromagnetic radiation
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c = lambda*nu
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order of electromagnetic spectrum
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gamma, X, UV, visible (violet to red), infrared, microwave, radio
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along the electromagnetic spectrum, wavelength _____
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increases
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along the electromagnetic spectrum, frequency _______
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decreases
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along the electromagnetic spectrum, energy ________
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decreases
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range of wavelengths of visible light spectrum
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390 nm (blue) to 760 nm (red)
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constructive interference
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in-phase, amplitudes combine
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destructive interference
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out-of-phase (by 1/2 lambda), amplitudes cancel
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diffraction
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dispersion of a light beam into different wavelength components because of interference
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refraction
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bending of light (due to change in speed) when it passes from one medium to another
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Lyman series
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(UV emission lines for H) nf=1
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Balmer series
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(visible emission lines for H) nf = 2
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Pashen series
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(IR emission lines for H) nf = 3
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blackbody radiation
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light emitted by heated solids
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Rayleigh-Jeans law for blackbody
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equation predicts inverse relationship between energy density and wavelength
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Planck's constant h
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h = 6.62607 x 10^(-34) J s
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Planck's equation for energy of a photon given frequency
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E = h*nu
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Planck's equation for energy of a photon given wavelength
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E = h*c/lambda
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photoelectric effect
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when light hits the surface of some metals, electrons are ejected
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kinetic energy of emitted electron given velocity
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KEe = (1/2)m*u^2
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work function definition
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energy binding electron to surface
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work function phi given threshold frequency
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phi = h*nu0
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kinetic energy of emitted photoelectrons given work function, frequency
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KEe = h*nu - phi = h*nu - h*nu0
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bohr radius a0
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a0 = 52.9 pm
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radius rn of orbit n given Z
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rn = n^2 *a0/Z
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energy of orbit n given Z
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En = -Z^2*h*c*Rh/n^2
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Davisson & Germer (and Thompson) experiment
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confirm wave properties of electrons using electron diffraction
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de Broglie equation for wavelength of matter given velocity, mass
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lambda = h/u*m
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uncertainty in momentum given uncertainty in position, or vice versa
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dx*dp >/= h/4pi
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the square of the wavefunction describes _________
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the probability of finding the electron in space (this probability determines orbital shape)
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principle quantum number n
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n=1, 2, 3, 4,... determines numbers of principal electronic shells
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orbital angular momentum l
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l may be zero or a positive integer, but not larger than n-1. determines shape. (s=0, p=1, d=2, f=3)
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magnetic quantum number ml
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may be integer from -l to l. determines orientation. (e.g. d=-2, -1, 0, 1, 2. so d has 5 orbitals)
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s type orbitals
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1 orbital. sphere. l = 0
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p type orbitals
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3 orbitals, represented as px, py, pz. two balloons tied together. l = 1
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d type orbitals
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5 orbitals. four balloons tied together. l = 2
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f type orbitals
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7 orbitals. l=3
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spin quantum number ms
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ms = +/- (1/2). determines electron spin
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paramagnetic
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atom has unpaired electrons
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stern-gerlach experiment
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demonstrates magnetic fields generated by electrons. atoms with unpaired electrons go up or down, while diamagnetic atoms go straight
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exception to rule of minimum energy configuration
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groups starting with chromium and copper: electron abandons s orbital for the d orbital
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Pauli exclusion principle
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all electrons in an atom have different quantum numbers
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Hund's rule
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an atom tends to have as many unpaired electrons as possible
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ultraviolet catastrophe
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(failure of Rayleigh-Jeans law for blackbody) energy density goes to infinity as wavelength gets smaller
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orbital energy En given effective nuclear charge Zeff
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En = -Zeff^2*h*c*Rh/n^2
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ionization energy
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absorption energy for ni=1, nf=infinity
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ionization energy given Z
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dEie = Z^2*h*c*Rh
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atomic radius increases
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left and down
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ionization energy increases
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right and up
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electron affinity increases
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right and up
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for isoelectronic cations, the more positive the charge, the _______ the ionic radius
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smaller
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