Electron Configuration Quantum Mechanical Model Quantum mechanics was developed by Erwin Schrodinger Estimates the probability of finding an e in a certain position Electrons are found in an electron cloud or orbital ID: 307509
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Slide1
Ch. 13 Quantum Mechanical Model
Electron ConfigurationSlide2
Quantum Mechanical Model
Quantum mechanics was developed by Erwin Schrodinger
Estimates the probability of finding an e
- in a certain positionElectrons are found in an “electron cloud” or orbitalSlide3
Radial Distribution Curve
Orbital
Orbital
(“electron cloud”)
Region in space where there is 90% probability of finding an e
-Slide4
Each orbital letter has a different shape.Slide5
“s” orbital
spherical
shaped, and holds up to 2e-Slide6
“p” orbital
Dumbbell shaped
Arranged x, y, z
axes, and can
hold up to 6e- Slide7
“d” orbital
clover
shaped, and can hold up
to 10e-Slide8
“f” orbital
f
Orbitals
combine to form a spherical shape
.
This orbital can hold up to
14e-
2s
2p
z
2p
y
2p
xSlide9
Hog Hilton
You are the manager of a prestigious new hotel in downtown Midland—the “Hog Hilton”. It’s just the “snort of the town” and you want to keep its reputation a cut above all the other hotels. Your problem is your clientele. They are hogs in the truest sense.
Your major task is to fill rooms in your hotel. The Hog Hilton only has stairs. You must fill up your hotel keeping the following rules in mind:
1) Hogs are lazy, they don’t want to walk up stairs!
2) Hogs want to room by themselves, but they would rather room with another hog than walk up more stairs.
3) If hogs are in the same room they will face in opposite directions.
4) They stink, so you can’t put more than two hogs in each room.Slide10
Hog Hilton
Your hotel looks like the diagram below:
6th floor ______
5th floor ______ ______ ______
4th floor ______
3rd floor ______ ______ ______ 2nd floor ______
1st floor ______Book 7 hogs into the rooms.Slide11
Hog Hilton
Your hotel looks like the diagram below:
6th floor ______
5th floor ______ ______ ______ 4th floor ______
3rd floor ______ ______ ______ 2nd floor ______ 1st floor ______
Book 14 hogs into the rooms.Slide12
Let’s play Hog Hilton!!Slide13
Rules for e
-
configurations
1. Aufbau principle
: e- enter orbitals of lowest energy level (
Hogs are lazy, they don’t want to walk up stairs!)2.
Pauli exclusion principle: an atomic orbital may have at most 2 e-, e-
in the same orbital will spin in opposite directions
(
They stink, so you can’t put more than two hogs in each room. & If hogs are in the same room they will face in opposite directions.)
3.
Hund’s
rule
: when e
-
occupy
orbitals
of = energy, 1 enters each orbital until all the
orbitals
contain 1 e
-
w/parallel spins
(
Hogs want to room by themselves, but they would rather room with another hog than walk up more stairs.)Slide14
Now you will relate the “Hog Hilton” to electron
orbitals
. Electron
orbitals are modeled by the picture on the left and are grouped into principal energy levels.1. Compare their similarities and differences.
2. To go between floors on the Hog Hilton did the hogs need to use energy? Would electrons need to use the energy to go between orbitals.
3d ___ ___ ___ ___ ___ n=3(4s ____) n=43p ___ ___ ___ n=3
3s ___ n=3
2p ___ ___ ___ n=2
2s ___ n=2
1s ___ n=1
6th floor ___
5th floor ___ ___ ___
4th floor ___
3rd floor ___ ___ ___
2nd floor ___
1st floor ___Slide15
A. The principle quantum numbers
,
(n)
Electrons are in designated energy levels
.
Organization of e- in the
Quantum Mechanical model
The ground state- the lowest energy state of the atomSlide16
B. Within the energy level are sublevels, designated by letters.
Principle energy level (n)
Number of sublevels
Type of Orbital
1
st
energy level
1 sublevel
“s” (1 orbital)
2
nd
2 sublevels
“s” (1) & “p” (3 orbitals)
3
rd
3 sublevels
“s”(1) , “p” (3) & “d” (5 orbitals)
4
th
4 sublevels
“s”(1), “p”(3) , “d”(5), and “f” (7)Slide17
1s
2s
2p
3p
3s
4s
3d
4p
5s
4d
5p
6s
4f
5d
6p
7s
7s 7p
6s 6p 6d 6f 6g
5s 5p 5d 5f 5g
4s 4p 4d 4f
3s 3p 3d
2s 2p
1sSlide18
Filling in orbitals then writing the electron configuration
4p _
↑↓
_ _ ↑↓ _ _
↑↓ _ 3d _ ↑↓ _ _
↑↓ _ _ ↑↓ _ _
↑↓ _ _ ↑↓ _
4s _
↑↓
_
3p _
↑↓
_ _
↑↓
_ _
↑↓
_
3s _
↑↓
_
2p _
↑↓
_ _
↑↓
_ _
↑↓
_
2s _
↑↓
_
1s _
↑↓
_
1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
6Slide19
1. Noble Gases – outermost
s
&
p
sublevels filled
Because they have their s
2
& p
6
orbitals filled they follow the:
2 + 6 =
OCTET RULE
D. According to their e- configs, elements can be classified into 4 main groupsSlide20
2. Representative Elements – outermost
s
or
p sublevel is only partially filled, energy level same as period #
The pink elements excluding the Noble Gases.
s
1
s
2
p
1
p
2
p
3
p
4
p
5Slide21
3. Transition metals – outermost
s
sublevel & nearby
d sublevel contain e
- , energy level is the same as the period # minus 1
d
1
d
2
d
3
d
4
d
5
d
6
d
7
d
8
d
9
d
10Slide22
4. Inner Transition metals - outermost
s
& nearby
f generally contain e
-
f
1
f
14Slide23
d
1
d
2
d
3
d
4
d
5
d
6
d
7
d
8
d
9
d
10
f
1
f
14
s
1
s
2
p
1
p
2
p
3
p
4
p
5
s
2
p
6
Your Periodic Table should look like this.Slide24
How many electrons are present in the d sublevel of a neutral atom of Manganese?
Learning Check
1 2 3 4 5
5 electronsSlide25
What element has the electron configuration 1s
2
2s
22p63s23p4?
Add together all the exponents, then find that atomic number. = Sulfur 16Slide26
E.
Using the Noble Gases to write Shorthand
Write the noble gas that is in the previous row.
Use the symbol of the noble gas, put it in brackets, then write the rest of the configuration.
Write the e- config for Tin (Sn).
[Kr]
5s
2
4d
10
5p
2
Write the e- config using Noble Gas notation for Cobalt.
It would be written [Ar] 4s2 3d7Slide27
Learning Check
Using the Noble Gas Shorthand write the
e
- configuration 1. Cr
2. Br
3. Te4. Ba
[Ar] 4s
2
3d
4
[Ar] 4s
2
3d
10
4p
5
[Kr] 5s
2
4d
10
5p
4
[Xe] 6s
2Slide28
Electromagnetic Spectrum
The electromagnetic spectrum (see p. 373) includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, x-rays, and gamma rays.
Visible light is in the middle of the spectrum.
The speed of light is 3.0 X 108 m/s.The formula for light is c =ƛʋ
C = speed of light, ƛ = wavelength, ʋ = frequencyVisible light has many wavelengths of light that can be separated into red, orange, yellow, green, blue, indigo, and violet (ROY G BIV)Slide29
Atomic Emission Spectrum
Every element gives off light when it is excited by the passage of an electric current through its gas or vapor.
The atomic emission spectrum occurs when the light that is given off by an element in its excited state is passed through a prism. It consists of a few lines called a line spectra or discontinuous spectra. Each line on the spectra corresponds with a frequency.
See page 374.Work problems # 11 and 12 on page 375.Slide30
Planck’s Constant
In 1900, German Physicist Max Planck used math to explain why objects, such as iron, that are heated change color.
He said energy can be quantized. The size of an emitted or absorbed quantum depends on the size of the energy change. A small energy change involves the emission or absorption of low frequency radiation. A large energy change involves the emission or absorption of high frequency radiation.Slide31
Planck’s constant cont.
The math formula used is:
E = h x vE = radiant energy of a unit (quantum)h = Planck’s constant = 6.6262 x 10 -34v = frequency of radiationSlide32
Planck’s constant cont.
In 1905, Albert Einstein used Planck’s work to call quanta of light photons. He then used this information to explain the photoelectric effect (metals eject/emit electrons called photoelectrons when light shines on them).
Work problems 13 and 14 on p. 379.