chem 6/7
wave particle duality
light behaves as particle and eave
electromagnetic radiation
light and radiation generated by particles moving through space
wavelength
width between peaks (distance)
frequency
amount of times waves repeats cycle (Hz or 1/s)
wavelength×frequency (problem)
(wavelength×10^-9m)÷ 1
v=c/wavelength
2.99x10^8 m/s ÷ (wavelength found m)
angstrom (unit)
10^-10 & Xray
nanometer (unit) nm
10^-9 & ultraviolet
micrometer (unit) um
10^-6 & infrared
millimeter (unit) mm
10^-3 & microwave
centimeter (unit) cm
10^-2 & microwave
meter (unit) m
1 & television/radio
kilometer (unit) km
10^3 & radio
particle/quantized energy
planck constant: 6.626x10^-34 Js
photoelectric effect
minimum frequency of light required for one e- emission -- photons E= hc/wavelength
photoelectric effect (problem)
E=(planck contant)(2.99x10^8 m/s) ÷ [solution - found by finding wavelength]
absorption
energy absorbed (high quanta)
emission
photon emitted (low quanta)
continuous spectrum
spectrum w continuous colors
line spectrum
spectrum containing only radiation (specific radiation)
Bohr Model (energy change between energy levels)
Efinal-Einitial ~ (+)= absorbed, (-)=emitted
Erwin Schrodinger
quantum mechanics - orbitals
principal # (n)
state ~ high # = high energy
angular # (l)
city
magnetic # (ml)
street
spin # (ms)
address
s orbital
l=0 ~ 0 nodes
p orbital
l=1 ~ 1 node
d orbital
l=2 ~ 2 nodes
f orbital
l=3 ~ 3 nodes
magnetic QN (ml)
if l=2 ~ ml= -2,-1,0,1,2
pauli exclusion principal
(1 spin up and 1 spin down) - arrows
hund's rule
for same l, fill spin up first then continue w spin down - arrows
electron configurations & periodic table
row 4:
4s2 3d10 4p6
d= -1 from main #
valence e-
e- involved in chemical bonding
elecron configuration (d)
d4 and d9 (will rearrange filling all boxes equally)
d4 original (arrows): 2 1 1 1 = 5
d4 new: 1 1 1 1 1 = 5
> turns to d5
> turns to d10
effective nuclear charge
net electric field ~ core e- shield outer e-
Zeff= Z-S
Z=actual nuclear charge (# of protons)
S= valence e- (screening constant)
anions
larger than neutral element
cations
smaller than neutral element
isoelectric
same e- arrangement
Na: 1s2 2s2 2p6 3s1 (not)
Na+: 1s2 2s2 2p6 (iso)
Ne: 1s2 2s2 2p6 (iso)
firsr ionization energy
energy required to move first e-
increase: left to right
decrease: top to bottom
affinity
more negative = more affinify
more positive = unstable
alkali metals
+1 ~ very reactive
alkaline earth metals
+2 ~ less reactive (further from iso w noble gas)
halogens
-1 ~ very reactive
F= most
noble gas
happy ~ no reaction