Chapter 3 Part II: The Electron
Name_______________________________
3.3
1. Waves:
Period______Date_____________________
A. Amplitude: _________________ of the wave. The higher the wave the _______________ intensity.
B. Wavelength: (λ , lambda) in nanometers (1 x 10-9m) Measured from ______________ to _____________
or from ________________ to _________________.
C. Frequency: (ν , nu) The ____________________ of times a wave passes a fixed point. Measured in
____________/___________ (1/s) 1 cycle/second = __________________(Hz)
ex) Radio FM 93.3 megahertz (MHz) is ________________________ cycles/sec.
D. Speed of Light: (c) = __________________________ or 186,000 miles/sec. The relationship
between wavelength and frequency can be shown with the following equations:
λ= c or ν = c
ν
λ
This is an ____________________ relationship. If λ ↑ then ν _______
2. Quantum Theory:
A. Planck’s Hypothesis:
(Max Planck 1900)
1. An object absorbs or emits ___________________ in a little packet or bundle called a
________________________ (quanta - plural).
2. Energies are __________________________.
3. Equation relating energy (E) to frequency (, nu) h = _________________________________
(6.6262 x 10-34J*sec)
E = h
This is a __________________ relationship, as ν  , E _____
B. Light (Electromagnetic Radiation):
1. A quantum of light is called a _______________________.
2. Light travels through space in ____________________.
3. Light acts like a ____________________ when it interacts with matter.
4. This shows the __________________________________________________________
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3. The Atom:
A. Atomic Emission Line Spectra: contains only certain colors or _________________________ (  )
of light.
1. Every _______________ has its own ___________ ______________________ (fingerprint).
B. Bohr Model of Hydrogen: (1911)
1. Bohr said the energy of an electron was _______________________
(only certain __________________ that represented different amounts of energy.)
2. Bohr labeled each __________________ ____________________ with a
__________________________ _________________________ (n).
3. n=1 lowest level or ______________________ _____________________.
4. When electrons _____________________ energy they jump to a higher
(__________________________) state. n=2
n=3
n=4
n=5
n=6
n=7
5. Radiation (_________________) is emitted when an _______________________
falls back from a _____________________ level to a _____________________level.
C. Werner Heisenberg:
(1927)
1. Heisenberg’s Uncertainty Principle: states the ___________________ and
_______________________ (speed, direction & mass) of a moving object cannot simultaneously
be measured and known exactly.
2. You cannot predict _______________________ locations of particles.
3. He found a problem with the __________________________ - no way to observe or measure
the orbit of an ______________________.
4. Quantum Mechanics
A. Quantum Mechanical Model of the atom combines previous ideas and treats the electron
like a ________________ that has ____________________ _____________________.
Impossible to state the exact _______________________ or _________________________
of an electron, but you can state a _______________________ of where the electron is located.
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B. Electron Density – Where the density of an electron cloud is high – there is a ___________
probability that is where the electron is located. If the electron density is __________ then
there is a ___________ probability.
C. Atomic Orbitals – region around the ____________ where an ______________ with a given
_______________ is likely to be found (not the same as Bohr’s orbits!)
1. Orbitals have characteristic ______________, ______________, & _________________.
2. Orbitals do _______ describe how the ________________ _______________.
3. The drawing of an orbital represents the ______________________________ within which
the electron is found _____________ of the time.
4. Sublevels can have 4 different __________________.
s-orbital
p-orbital
d-orbital
f-orbital
D. Quantum Numbers – Finding an address for the electrons from general to specific.
1. state:
Principal Quantum Number (n) or the _________________ ranges from _______
2. city:
Sublevel _____________________ either ______, ______, ______ or _______.
3. street:
Orbital The __________________________ in space ex) __________________
4. house:
Spin The ___________ or __________ motion of the electrons.
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5. The number of Sublevels in an energy level _______________ the Principal Quantum Number.
6. Orbital: There are always an ___________ number of orbitals.
s-sublevel has _____ orbital.
p-sublevel has _____ orbitals.
d-sublevel has _____ orbitals.
f-sublevel has _____ orbitals.
Orbitals in higher principal levels get ___________________.
A max of ________ electrons fit in each orbital.
7. Electron Spin
a. Two electrons in each orbital have _______________________ spins.
(_______________________ and ____________________________________)
b. The opposite spin is written:
______
or
______
c. Pauli Exclusion Principle:
1. Each orbital can only hold _______ electrons.
2. The electrons must have ________________________ spins.
s-sublevel = max ________ electrons
p-sublevel = max ________ electrons
d-sublevel = max ________ electrons
f-sublevel = max ________ electrons
3. Incorrect: _____
Incorrect: _____
Correct: _____
d. Hund’s Rule: Electrons will ________________ __________ among the orbitals
before they ____________ ______.
Incorrect: ____ ____ ____ Correct: ____ ____ ____
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E. Electron Configurations:
1. Shows the distribution of electrons among the _________________________.
Describes where the electrons are found and what _____________________ they possess.
2. The Aufbau Principle: electrons are added one at a time to the __________________
energy orbital.
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Ex) electron configuration for Na:
_________________________________________
Ex) orbital filling diagram for Na:
_________________________________________
3. Electron Dot Diagrams:
Write _________________ for the element.
Place dots around the symbol to represent________________ _____ & _____ electrons only.
Do NOT include ______ + ______ orbitals in the diagram.
Electron Configuration
16
8
O
35
17
Cl
Orbital Box Diagram
Electron-dot Diagram
127
52
Te
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