quantum

electrons
the way atoms interact by sharing or exchanging;
electromagnetic radiation
energy embodied in oscillating magnectic and electric fields that travel thru a vaccum at constant speed of light
example: light
properties of light
exhibit both wave and partial nature; wave particle duality
wavelength
wave nature of light
interference>constuction and destruction
diffraction
diffraction
LOOK UP
Photon
particle nature of light; quantum of EM radition
packet or bundle of energy
frequency
peaks or troughts at given point, hertz per second
light equation
C= wavelength *frequency
two photon equations
e=h* frequency or E= H*C(light)/ wavelength
planks constant
relate energy of photon of light
electromagnetic spectrum
complete span of possibilites for frequency and wavelength of EM radition;
light has continous spectrum>rainbow
niels bohr
electron in hydrogen atom set of energy levels called orbitals. excited state to ground state releases energy as photon light.
energy differenc btw high and low is large
short wavelength and high energy
energy difference btw high and low is small
long wavelength and low energy
memorize this statement
restricting the energies of electrons in the hydrogen atom is a form of quantization
hisenberg’s uncertainty principle
electron have wave and particule nature so the more you know about one the less you know about another
debroglie relationshi
wavelength = H/ M *V
quantum mechanics
wavelike properties of electron
probability density
position of electron is described in these maps
difference btw energy levels equation
E= – R/ n2

1/nGO BACK AND FIX

atomic orbitals
wave functions with acceptable values of quantum numbers
wave functions
characterized by three quantum numbers
principle quantum number (n)
possible values: 1,2,3…
significance: distance from nucleus
SIZE OF THE ORBITAL
Angular quantum number (l)
possible values: 0,1,2…(n-1)
significance: SHAPE OF ORBITAL
Magnetic Quantum numnber (m)
possible values: -1,0,1….2l+1
significance: orientation fo orbital
orbitals
regions in the atom that have a high probability of containing an electron or high electron charge density
principle energy level
orbital with same value as N
subshell
same value of N and L
electron spin quantum number (m little s)
1/2 or -1/2
orbitals are defined by what
n, l, m
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