Chemistry Chapter 5

1
Chemistry Chapter 5
Electrons in Atoms
The 1998 Nobel Prize in Physics was awarded "for
the discovery of a new form of quantum fluid with
fractionally charged excitations." At the left is
a computer graphic of this kind of state.
2
Electrons in Atoms

• Thomson plum pudding
• Disproven
• Rutherford
• Bohr

3
The Puzzle of the Atom

•   Protons and electrons are attracted to each
  other because of opposite charges
•   Electrically charged particles moving in a
  curved path give off energy
•   Despite these facts, atoms dont collapse

4
So why didnt the atom collapse?? Why doesnt
the electron lose energy as it orbits???
5

• Hold onto your spectral tubes!!
• The answer actually has to do with light and
  other electromagnetic radiation.

6
Wave-Particle Duality
JJ Thomson won the Nobel prize for describing the
electron as a particle.
His son, George Thomson won the Nobel prize for
describing the wave-like nature of the electron.
The electron is a particle!
The electron is an energy wave!
So there was a difference in opinion between a
father and son. Has this ever happened to you?
7
Electrons have properties ofWaves and
Particles
So father and son BOTH right!!
8
Confused??? Youve Got Company!
No familiar conceptions can be woven around the
electron something unknown is doing we dont
know what.
Physicist Sir Arthur Eddington The Nature of the
Physical World 1934
So even the smart dudes were baffled
9
The Wave-like Electron
The electron propagates through space as an
energy wave. To understand the atom, one must
understand the behavior of electromagnetic waves.
Ok . so in order to argue with my dad I need to
understand light?
Louis deBroglie
10
Maybe I should learn about light
11
Electromagnetic radiation propagates through
space as a wave moving at the speed of light.
c ??
C speed of light, a constant (3.00 x 108 m/s)
? frequency, in units of hertz (hz, sec-1)
? wavelength, in meters
12
Types of electromagnetic radiation
13
The energy (E ) of electromagnetic radiation is
directly proportional to the frequency (?) of the
radiation.
E h?
E Energy, in units of Joules (kgm2/s2)
h Plancks constant (6.626 x 10-34 Js)
? frequency, in units of hertz (hz, sec-1)
14
Long Wavelength Low Frequency Low ENERGY
Wavelength Table
Short Wavelength High Frequency High
ENERGY
15
Spectroscopic analysis of the visible spectrum
produces all of the colors in a continuous
spectrum
16
Spectroscopic analysis of the hydrogen spectrum
produces a bright line spectrum
17
Electron transitionsinvolve jumps of definite
amounts ofenergy.
This produces bands of light with definite
wavelengths.
18
Spectral tubes, flame tests and fireworksall
colored by electrons changing energy levels.
19
The Bohr Model of the Atom
I pictured electrons orbiting the nucleus much
like planets orbiting the sun.
But I was wrong! Theyre more like bees around a
hive.
WRONG!!!
Neils Bohr
20
The electron as a standing wave

•   Standing waves do not propagate through space
•   Standing waves are fixed at both ends
•  

Only certain sized orbits can contain whole
numbers of half wave lengths.
21
Quantum Numbers
Each electron in an atom has a unique set of 4
quantum numbers which describe it.

• Principal quantum number (n)
• Angular momentum quantum number (l)
• Magnetic quantum number (m)
• Spin quantum number

22
Pauli Exclusion Principle
No two electrons in an atom can have the same
four quantum numbers.
Wolfgang Pauli
23
Principal Quantum Number
Generally symbolized by n, it denotes the shell
(energy level) in which the electron is located.
Number of electrons that can fit in a shell
2n2
24
Angular Momentum Quantum Number
The angular momentum quantum number, generally
symbolized by l, denotes the orbital (subshell)
in which the electron is located.
25
Magnetic Quantum Number
The magnetic quantum number, generally symbolized
by m, denotes the orientation of the electrons
orbital with respect to the three axes in space.
26
Assigning the Numbers

• The three quantum numbers (n, l, and m) are
  integers.
• The principal quantum number (n) cannot be zero.
  
• n must be 1, 2, 3, etc.
• The angular momentum quantum number (l) can be
  any integer between 0 and n - 1.
• For n 3, l can be either 0, 1, or 2.
• The magnetic quantum number (m) can be any
  integer between -l and l.
• For l 2, m can be either -2, -1, 0, 1, or 2.

27
Principle, angular momentum, and magnetic quantum
numbers n, l, and ml
28
Spin Quantum Number
Spin quantum number denotes the behavior
(direction of spin) of an electron within a
magnetic field.
Possibilities for electron spin
29
An orbital is a region within an atom where
thereis a probability of finding an electron.
This is a probability diagram for the s orbital
in the first energy level
Orbital shapes are defined as the surface that
contains 90 of the total electron probability.
30
Schrodinger Wave Equation
Equation for probability of a single electron
being found along a single axis (x-axis)
Erwin Schrodinger
31
Heisenberg Uncertainty Principle
One cannot simultaneously determine both the
position and momentum of an electron.
You can find out where the electron is, but not
where it is going.
OR
You can find out where the electron is going, but
not where it is!
Werner Heisenberg
32
Sizes of s orbitals
Orbitals of the same shape (s, for instance) grow
larger as n increases
Nodes are regions of low probability within an
orbital.
33
Orbitals in outer energy levels DO penetrate into
lower energy levels.
Penetration 1
This is a probability Distribution for a 3s
orbital.
What parts of the diagram correspond to nodes
regions of zero probability?
34
Which of the orbital types in the 3rd energy
level Does not seem to have a node?
WHY NOT?
Penetration 2
35
The s orbital has a spherical shape centered
around the origin of the three axes in space.
s orbital shape
36
P orbital shape
There are three dumbbell-shaped p orbitals in
each energy level above n 1, each assigned to
its own axis (x, y and z) in space.
37
Things get a bit more complicated with the five d
orbitals that are found in the d sublevels
beginning with n 3. To remember the shapes,
think of double dumbells
d orbital shapes
and a dumbell with a donut!
38
Shape of f orbitals
39
Orbital filling table
40
Slide Show                                                    
                                                   

Electron configuration of the elements of the
first three series
41
Slide Show                                                    
                                                   

Irregular confirmations of Cr and Cu
Chromium steals a 4s electron to half fill its
3d sublevel
Copper steals a 4s electron to FILL its 3d
sublevel
42
We have colors because of the movement of
electron!! Ahh ChemisTRY
43
Chemistry Chapter 5Atomic Structure
Presented by Mr. Mole You will learn about him
later
44
Mole Day 602 October 23

• Poor mister mole.we never celebrate his day
  because it takes to long to light his 6.02 x 10
  23 candles