Electronic Structure of the Atom
Unit 1: Lecture 3
Lecture 3: Electron Configuration
Electron Configuration
Pauli Exclusion Principle:
o No two electrons can have exactly the same energy
o Therefore,
Electron configuration shows the distribution of all el
Electronic Structure of the Atom
Unit 1: Lecture 1
Lecture 1: Wave and Particle Nature of Matter
Niels Bohr tried to explain the location of electrons
Based his ideas on the relationship between matter and light
There are two theories that can explain li
Electronic Structure of the Atom
Unit 1: Lecture 2
Lecture 2: Quantum Numbers
Quantum Mechanics
Schrodinger developed quantum mechanics: a mathematical treatment into which both the wave
and particle nature of matter could be incorporated.
He mathematical
Electronic Structure of the Atom
Unit 1: Lecture 4
Lecture 4: Photoelectron Spectroscopy (PES)
Photoelectron Spectroscopy (PES)
Spectroscopy
How it works:
1. Sample is exposed to electromagnetic radiation
2. Electrons jump out of sample and go through an
Unit 2: Thermochemistry
Lecture 1: Energy and How Its Transferred
Vocabulary:
Thermodynamics
Energy
Work Energy used to move an object over some distance. w = _
w is work, F is the force, d is the distance over which the force is exerted.
Heat Energy tr
Unit 2: Thermochemistry
Lecture 4: Calculating Enthalpy
HOW DO WE FIGURE OUT H TO INCLUDE IN OUR EQUATION?
Method #1 to find H: Calorimetry
When H
=q, you can calculate q like you did in your first year class when given
the proper information!
Specific he
Unit 2: Thermochemistry
Lecture 2: The First Law of Thermodynamics
Internal Energy The sum of all kinetic and potential energies of all components of
the system. (We call it E)
Usually we dont measure E, we measure _.
By definition, the change in internal
Unit 2: Thermochemistry
Lecture 3: Enthalpy
P-V Work
When a chemical reaction occurs, commonly the only work done is a change in volume
of a gas pushing on the surroundings (or being pushed on by the surroundings).
We can measure the work done by the gas
6. The PES spectrum for element X is shown below.
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E {Mjg’mol}
a. What is the group number of this element?
b. What is the maximum positive charge that this atom is likely to have under norma
Unit 1 Lecture 1: In Class Practice
. ., ,r , ,.
The yellow light given off by a sodium vapor lamp used for public lighting has a wavelength of 589 am.
What is the freguency of this radiation? \ 7‘
a Mela/s = (5.3% 10 '7 ml T v mesa.
Practice: E; {Doggy
-6
,7 Name KL
Period: 1/2 3 4 5/6
(“1.
' "'1. List the common kinds of radiation in the electromagnetic spectrum in order of increasing energy:
Radio < Min/0mm“ “24 visiblc Mgr/1+4 W4 X'myj gamma
[sour most
2. Given an electro gnetic wave] gth of 5.7 thﬁ