Download Quantum Theory - developed by German physicist Max Planck

TP - Ws
Quantum Theory - developed by German physicist Max Planck: atoms emit
energy in small discrete bundles called ~
E = hv
(quantum of energy in j~ 6.63x1~34 j-s x wave frequency)
(planck’s constant)
Wave - vibrating disturbance by which energy is transmitted
Wavelength - k (lambda) distance between two successive peaks or crests of
waves, units = nm, m, era, etc.
Fre ueo~u_~ - v (nu) number of waves that pass a given point per second
(cycles per second:/s) SI unit is hertz (Hz) 1Hz -- lcyele/s
Amplitude - vertical distance from the midline of a wave to the crest
S~ed of a wave = wavelength x freauenc~: ~ = Lv
All electromagnetic radiation waves travel at the sarae speed in a vacuum.:
Speed of light- "c" = 3.00 x 108 m/s
Substituting "c" for rt in the above equation: c = kv
P__hotoelectric effect -when electrons are ejected fromthe surface of certain
metals exposed to light of a certain frequency, light is a stream of particles
called photons
TP-Ws
_Quantum Numbers
("L" will be used to replace °T’ to better differentiate the letter from the
number1)
There are 4 quantum numbers that can describe the distribution of electrons:
1 - ~antum number (n) describes the average distance the
electron is from the nucleus of the atom (energy levels or shells)
**’~n values = 1, 2,
2 - Azimuthal (Angular Momentum) quantum number: (L) describes the
shape of the orbitals (s=spherical, p=dmnbell, d=clover leaf, f=too complex)
**~’L = 0 to (n-l)
values = 0, 1, 2, 3, .....
(s) (p) (d) (f)
Example: n = 1 L = 1-1 = 0 (s) ls subshell
n = 2 L = 2-1 = l& 0 (s,p) 2s, 2p subshells
(also designates the number of subshells)
3 - Ma.=~Ngneiic quantum number: (NIL) describes the orientation of the
orbiltal in space (# of orbitals in a subshell: s=l, p=3, d=5, f=-7 )
***ML = 2L + 1
-L, (-L + 1) ..... 0 .... (+L -1), +L
Example: n = 2, L = 1 2p subshell
ML= 2(1) + 1 = 3 values or orbitals
4 - Electron S in uantum number: (Ms) value = +1/2 or -1/2
+1/2 = elockwise~-~
-1/2 = counterclockwise ~-~
ELECTRON iN AN S ORBITAL:
ELECTRON iN Py, Pz, AND P× ORBITALS:
Z
Py
Use Type |25, |27 or 133 Film
SCIENCE - I~H
(~COPYRIGHT 1965 BY REINHOLD
PUBLISHING CORPORATION
ELECTRONS IN dz~, dyz, dxz, dxy, AND dx2 y20RBITALS
Z
Y
X
Z
Z
~X
lyz
Z
d×z
Z
X
dxy
Use Type ’125, 127 or 133 Film
SCIENCE (~ COPYRIGHT 1965 BY REINHOLD
PUBLISHING CORPORATION
Principal
Azimuthal
Quantufn Quantum
Number, n Number, 1
(Shell)
(Subshell)
Subshell
Designation
Number, m
(Orbital)
Number of
Orbitals in
Subshell
lS
0
1
0
0
1
-1,0,+1
1
3
0
2
3
4
0
35
0
1
1
3p
-1,0,+ 1
3
2
3d
0
5
1
1
4~
4p
=2,=1,0, +1,+2
0
ml, O, +1
2
4d
3
5
3
4~
-3,-2,-1, O, +1,+2, +3
7
main energy level
1
2
3
number of sublevels(n)
number of orbita~s (n~)
1
1
s
1
2
4
sp
13
3
9
spd
135
4
16
spdf
1357
2610
261014
18
32
kind and no. of orbitais
per subJevel
maximum no. of electrons
per sublevel
maximum no. of eleo{rons
per main leve~ 2~~)
3 Rules to Follow When Wfitin~ Eo Confi~ratio~
1o Aulban Princi~
electrons’enter/fillup orbitals of lowest energy first
orbitals in the same sublevel are equal in energy
e×. p (orbital)- O×OyOz are all equal in energy
sometimes energy levels ~ each other
2. Pauli Ex~elusion Princi.p.~le
there is a maximum of 2eo in any one orbital
these 2e- (paired) must be of opposite spins
one positive/clockwise and the other negative/counterclockwise
3. Hund’s Rule.
when ~ling orbitals of equal energy (spdf) one eo enters each
orbital first (unpaired), until all of the orbi~als eontain one ewith spins parallel
then the 2nd. eo will enter eaeh orbital to form paired spins
o ex.p= ~