TEST:
overview
Topics covered:
Electrons
- Bohr Model & Atomic Emission Spectra
- Quantum-Wave Mechanical Theory
- 4 Quantum Numbers
- Ground State Electron Configuration
- Aufbau Principle
- Noble Gas Notation
- Orbital Diagram
- S,P,D,F – Blocks (periodic table)
The
Quantum-Wave Mechanical Model (Theory)
- It determines the allowed energies (quantum) an electron can have
&
How likely it is to find the electron orbiting the nucleus.
Also, electrons move around the nucleus in a wave pattern, having a specific
frequency & wavelength (which determines the energy of an electron).

looks something like a composite of quarks surrounded by clouds of uncertainty 
The
Quantum-Wave Mechanical Model (Theory)



•  This model does not have orbitals, rather regions of probability.
•  Atomic orbitals are regions of space in which there is a high
probability (90%) of finding an electron. Except the s orbital (only 10%).
** The theory states that any electron in an atom can be
completely described(located) by 4 Quantum Numbers.
4 Quantum #’s –
(describe the electrons location)
1.  Principle Quantum Level
2.  Sub-levels
3.  Orbital’s
4.  Spin of Electrons
( …..How electrons fill in each orbital)
1. Principal Quantum Numbers
also called “Energy Levels”
- symbol
“n”
- “n” are always integers 1 ,2 ,3 ,4…7
-
And are related to Periods on the Periodic Table

see below.
2. electron
Sub-levels
.
S
~ sublevel………..holds a total of
2 e-
P
~ sub-level.……….holds a total of
6 e-
d
~sub-level…………holds a total of
10 e-
f
~ sub-level………. holds a total of
14 e-
________________________________________________________
Below – a atomic model with Energy Levels,
2e-
Sublevels, &
the maximum amount of
2e-
6e-
electrons they can hold.
2e-
6e-
10e-
Quantum Numbers
#1 = Energy Levels
+
1&2
#2 = Sublevels
1st energy level has one sublevel
2nd
(sublevel breakdown, below)
 1s
energy level has two sublevels  2s , 2p
3rd energy level has three sublevels
 3s , 3p , 3d
4th
energy level has four sublevels
 4s , 4p , 4d , 4f
5th
energy level has four sublevels
 5s , 5p , 5d , 5f
6th
energy level has four sublevels
 6s , 6p , 6d , 6f
7th
energy level has four sublevels
 7s , 7p , 7d , 7f
•  3rd Quantum Number
•  All orbital’s hold 2 electrons only
.
deals with electron Orbital’s.
(no exceptions).
S~
has 1 orbital .……holds a total of 2 e-
P ~
has 3 orbitals ……holds a total of 6 e-
d
~
has 5 orbitals ……holds a total of 10 e-
f
~
has 7 orbitals ……holds a total of 14 e-
•
All orbital’s in any one sublevel (of the same element) are
For example,
of equal energy
all three, 2p orbital’s for all elements are of equal energy.
•  the energy sublevels within an energy level have different energies.
for the same energy level….
low Energy
s  p  d  f
high Energy
For example, the 2p orbitals are of higher energy than the 2s orbital.
Quantum Sublevels are labeled S, P, D, F
S – orbital’s
(has a Spherical shape)
P - orbital’s
(has a figure 8 shape)
or “dumbbell”
D - orbital’s
(has a Clover leaf shape)
4th Quantum Number, deals with electrons filling orbital’s.
Each box (below) represents one orbital
- Pauli Exclusion Principle = States that a maximum of two electrons
may occupy a single atomic orbital, but only if the electrons have opposite spins.
Sublevels and orbitals
S sub-level has 1 orbital ….
P sub-level has 3 orbital’s …………..
D sub-level has 5 orbital’s …………………………
F sub-level has 7 orbital’s
- Hund’s Rule = States that single electrons with the same spin must occupy each equalenergy orbital before additional electrons with opposite spins can occupy the same orbital’s.

P sub-level how do all 6 electrons fill in?