Download Essential Question: What is the current model of the atom? How

CP Chemistry
Unit 2A and Chapter 4 Notes: Quantum Theory
Electromagnetic energy
Plank’s constant
Excited state
Principal Q #
Hund’s rule
Heisenberg Uncertainty Prin
Orbital notation
d orbitals
Atomic number
Protons
Important Vocabulary
Wavelength
Frequency
Bohr model
Energy levels
ground state
Photoelectric effect
Azimuthal Q#
Magnetic Q#
Quantum model
Electron cloud
Pauli Exclusion Prin
Electron configuration
Orbital
S orbital
f orbitals
sublevels
Atomic mass
Mass number
Neutrons
Electrons
Speed of light
Quantized
Aufbau principle
Spin Q#
Photon
p orbitals
Hertz
Isotopes
Nucleus
Essential Question: What is the current model of the atom? How does it
function?
2-1
Before the advent of quantum theory (quantum mechanics or quantum physics), considerable work was
done to gain an understanding of atomic structure. Here is a summary of what was learned about atoms
prior to 1924:
The first three models of the atom:
Dalton 1803
Thompson 1897
The Bohr model of the atom looks like:
Rutherford 1911
How does this model compare to a ladder?
What was wrong with the Rutherford model that necessitated the Bohr model?
What experimental evidence was this model based on? (video)
The ground state is:
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The excited state is:
How is energy related to the Bohr model?
How do electrons move between the levels?
How many total electrons can fit on each level of the Bohr model?
The parts of the Bohr Model that are correct are:
It has a _________________, which contains ______________ and ___________________.
Electrons are ordered by energy on _____________________________
What was found to be incorrect about the Bohr model? Why?
What are some analogies that help us to understand the size of the atom:
a.
b.
To summarize: atoms are mostly ___________________________, with a small dense and positively
charged ______________
The three basic subatomic particles
Name
Where it is located
Atomic number:
Ex:
2
relative mass (u)
Actual mass (g)
relative charge
Actual charge (C)
Mass number:
Ex:
Isotopes:
Ex: Chlorine
Ex: Hydrogen
Nuclear symbols:
Ex:
a.
b.
How do we determine the number of protons, electrons and neutrons are in an atom?:
a.
b.
c.
d.
Fill in the following table (check projector for filled in information)
Name
Symbol Atomic #
Mass #
# protons #
neutrons
1
2
3
4
5
6
7
8
9
3
#
electrons
Charge
How does one calculate the average atomic mass (or atomic mass)? à weighted average
Ex:
a. Chlorine
b.
c.
d.
How is this different from a normal average?
Ex: test scores
2-2 (quiz on section 2-1)
What is electromagnetic radiation?
What is light?
What is a wave? (draw a picture and label it)
Frequency:
unit:
symbol:
Wavelength:
unit:
symbol:
A picture of the electromagnetic spectrum:
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Highest ν
Highest energy
Largest λ
Uses for gamma rays:
Uses for microwaves:
Uses for X rays:
Uses for radiowaves:
Uses for UV light:
How are wavelength and frequency related? (equation provided on exams)
What does inversely proportional mean?
What is the speed of light?
Symbol:
Which type of light has the longest wavelength? Smallest frequency?
Which type of visible light has the shortest wavelength? Highest frequency?
Why is the color red used for stop lights?
Sample calculations of wavelength and frequency:
a.
c.
b.
d.
The photoelectric effect is:
A picture of what this might look like:
Why is the photoelectric effect important?
What is the current theory of light?
A particle of light is called a:
It is also called a :
5
The equation to calculate the energy of a photon is:
h is called and is equal to :
Sample calculations using the equation E = hν (equation provided on exams)
a.
b.
c.
d.
Matter waves are:
Who came up with the idea of matter waves?
Why are electrons acting as waves important?
The Heisenberg Uncertainty Principle:
What does the H.U.P really mean?
An analogy for the principle is:
Why do we think the H.U.P. is correct?
The current model for the atom is:
Draw a picture of what we think the atom looks like today:
Does the atom have a boundary?
Has the quantum theory ever been proved wrong?
What is the key word for the quantum model?
How do we determine where the electron is probably found?
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Quantum Numbers
The first quantum number is called:
The symbol is
It can have values of
It represents
The third quantum number is called
The symbol is
It can have values of
It represents
The second quantum number is called
The symbol is
It can have values of
It represents
The fourth quantum number is called
The symbol is
It can have values of
It represents
This is very confusing! What is an analogy for these crazy quantum numbers??
What are some helpful “rules of thumb” for these quantum numbers:
What do I really need to know about these quantum numbers for the exam?
Example A
Example B
Example C
Orbitals
An orbital:
What does the s orbital look like?
What do the p orbitals look like?
What do the d orbitals look like?
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Example D
2-3 (quiz on section 2-2)
Electron configurations are:
Examples:
There are three “laws” governing electron configurations
Aufbau principle:
Ex:
Pauli Exclusion Principle:
Ex:
Hund’s rule:
Ex:
How do we write electron configurations? What are some examples?
Diagonal Rule:
What is the “best” way to write electron configurations?
What are orbital diagrams or orbital notation?
Example A:
Example B:
What shortcuts can one take to write electron configurations?
Examples of electron configurations:
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