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40 Cards in this Set
- Front
- Back
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Speed of light
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c
3.00x10^8 meters/second |
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Wavelength
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h (looking)
lambda meters/nanometers |
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Frequency
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v/u (looking)
nu Hz (1/s) |
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Energy
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E
Joules |
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Plank's Constant
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h
6.626x10^-34 Joules(seconds) |
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E = h(u)
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Energy = Planks Const. X Frequency
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c = (h *lambda*)u
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Speed of light = Wavelength X Frequency
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Electromagnetic Radiation
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Radiant energy that exhibits wave like behavior and travels through space at the speed of light in a vacuum
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Photon
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Packet of Energy (Emitted when electron jumps from excited state to a lower or ground state)
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Wavelength
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The distance between two consecutive peaks or troughs in a wave
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Frequency
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The number of waves (cycles) per second that pass a given point in space
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Proportional? Wavelength and Frequency
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Inversely (Long wavelengths, less frequent)
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Proportional? Wavelength and energy
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Inversely (Long wavelengths, low energy)
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Proportional? Frequency and energy
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Directly (More frequent, more energy)
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Aufbau Princ.
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Fill lowest energy level first
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Hunds Rule
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(school bus) each orbital recieves one electron before the pair up
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Pauli exclusion Theory
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Electrons have opposite spins that attract
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Atom Size (Horizontal)
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Bigger to Smaller
---------> |
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Atom Size (Vertical)
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Smaller to Bigger
l l v |
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Element with Smallest Radius
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Helium
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Ionization energy
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The energy required to remove electron from atom (Smaller the atom, the more energy required to remove an electron)
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Excited and Ground State
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Excited: atom with excess energy
Ground: Atom in the lowest possible state (energy) |
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Bohr Model of Atom
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Electron Moves in a circular orbit (wrong)
Electrons jump between levels by absorbing and emitting photons of a particular wavelength |
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Order of wavelength
(shortest to longest) |
Radio waves - Microwaves - Infrared - ROYGBV - Ultraviolet - X rays - Gamma Rays
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Longer wavelength, less energy, less frequent, and smaller photon
RED or BLUE? |
Red
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Shorter Wavelength, more energy, bigger photon, more frequent
RED or BLUE? |
Blue
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S-block
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Far left 2 columns
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P-Block
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Far right 6 columns
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D block
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Middle 10 columns
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F Block
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Outside 14 columns
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Row wise... the d block is how many less?
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1 rows
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Row wise... the f block is hom many less?
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2 rows
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Principal energy levels
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n=1 n=2 n=3
excited electrons jump to these |
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sublevels
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each principal energy level is divide into sub levels, s, d, p, f
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orbital
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potential space for an electron, where you can probably find an electron
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Valence electrons
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the electrons in the outermost principal energy level of an atom
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core electrons
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an inner electron
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the 3 in 3p^6 corresponds to the...
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period
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the p in 3p^6 corresponds to the...
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block
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the 6 in in 3p^6 corresponds to the...
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number of electrons
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