Quantum Theory test
visible
ROYGBIV; only particle we can see; wavelength is comparable to hair
exceptions
d-1# less than the period # f block-2# less than the period #
photoelectric effect
einstein; energy is not continuous at all frequencies
Hund's rule
electrons are placed in seperate orbitals of the same energy before pairing up (bus rule)
Aufbau principle
electrons enter the orbitals of the lowest energy first
Schrödinger
electrons move around the nucleus as waves; electrons probably around nucleus; orbitals
general information provided by quantum numbers
energy level, shape, location, and electrons
quantum
finite quantity of energy in discrete units that are gained or lost by an atom
electromagnetic spectrum
forms of radiant energy that show wavelike behavior as it travels through space; forms of waves- both electrial and magnetic properties
gamma rays
harmful; penetrating
microwaves
heating
infared (ir)
heating; red coloring; night vision goggles
amplitude
height of the wave
excited state
higher energy levels than ground state
electron dot notation
how many electrons are in the highest energy level
laser
light amplification by stimulated emission of radiation; scanning playing music
orientations per sublevel
s-1 p-3 d-5 f-7
shapes
s-sphere; p-dumbell; d-4leaf clover and dumbell with donut; f 6leafed flower
orbital quantum number
shape of orbital; s,p,d,f
ground state
state of lowest energy level of an atom
de Broglie
the electron can act like a wave or particle
frequency
the number of waves that pass by a particular point in one second (cycles/second)
x-rays
used to see bones
wavelength
distance between 2 identical points on successive waves
planck
e=hv where h=6.626x10^-34 Jxs
speed of light
c=wavelength (lambda) x frequency (v)
speed of light constant
3.00x10^8 m/s and 3.00x10^10 cm/s
planck constant
6.626x10-34 Js
quantum theory
(physics) a physical theory that certain properties occur only in discrete amounts (quanta)
unit of frequency
("v") 1/s=Hz or s^-1
unit for wavelength
(lambda) cm or m
spin quantum number
+1/2 -1/2; electrons do opposites
possible values for quantum number
1-7
electron configuration pattern
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d10 7p6
shortcomings of the bohr model
cant work for any atoms except single electron atoms and ions; cant explain chemical bonds
electron configuration
arrangement of electrons of an atom
Octet of electrons
atoms combine so there are eight electrons in valence shells
ultraviolet
black lights; suntan/burn; spf; uva and uvb
radiowaves
music/sound; heihrich hertz
principal quantum number
n; main energy level; periods of the periodic table
Pauli exclusion principle
no 2 electrons in the same atom can have the same set of quantum numbers (opposite spins)
Heisenberg-Uncertainity principle
not possible to measure the velocity and position of the electron exactly; waves are bigger than electron so it gives energy
magnetic quantum number
orientation; x,y,z
photon
particle or packets or particular energy
four quantum numbers
principle quantum number; orbital quantum number; magnetic quantum number; spin quantum number
orbital
probable location of electron
radar
radio detection and ranging; navigation/collision avoidence
