Download The Quantum Mechanical Model and Electron

The Quantum Mechanical Model and
Electron Configuration Notes
I. Light and the Electromagnetic Spectrum
{Scientists were trying to understand how ___________ behave. They first
looked at how __________ interacts with _____________.}
Light travels in waves called ________________ waves.
Light is a form of __________________________ (a form of radiation which
exhibits _________________ behavior as it travels through ______________.)
A. Parts of a Wave
_______________: the ___________ of a wave measured from the origin to the
crest or peak; determines the _____________ and ________________.
________________ ( ): _____________ between two adjacent crests (or
troughs) of a wave, or the ____________ a wave travels in _______________;
measured in units of cm, m or nm.
__________________ ( ): indicates how __________ a wave ____________ up
and down; measured by the number of times a light passes a given point in one
-1
second, or the number of _________________; units are 1/s, s , or Hertz (Hz)
8
________________ (c): all light moves at a _________ speed of 3.00 X 10 m/s;
represents a relationship between _____________ and _____________ by the
equation ________________
This wave has a ____ wavelength and a _____ frequency
This wave has a ____ wavelength and a _____ frequency
B. ELECTROMAGNETIC SPECTRUM
C. WAVELENGTH AND FREQUENCY PROBLEMS
1. Microwaves are used to transmit information. What is the wavelength of a
microwave having a frequency of 3.44 X109Hz?
2. A radio station broadcasts at a frequency of 94.7 MHz. What is the
wavelength of the broadcast? (1MHz = 1 X 106 Hz)
3. An x-ray has a wavelength of 1.15 X 10-10 m. What is its frequency?
4. A beam of light has a wavelength of 595nm. What is its frequency? (1 m = 1X
109nm)
II. Quantum Theory
In 1900, __________ and _____________ were seen as different from each
other in fundamental ways.
Matter was ______________.
Energy could come in ______________, with any frequency.
Scientists at the time did not understand why the color of an object changed
when ______________ it up (change _____________________). At this time,
scientists believed that as energy _______________, the amplitude or
_______________ also increased.
A. Max Planck
_________________ found that the cooling of _______ objects couldn’t be
explained by viewing energy as a __________.
Max Planck developed a theory that said energy depends on _____________(or
frequency). He explained how the __________m of radiation emitted by an
object changes with _________________.
_____________ absorbed or given off by an object is released in ___________
called _____________ (or quantum). Developed the equation ________ (h is
Plancks constant, h = 6.626 x 10-34 J s) (__________-the minimum amount of
____________ that can be gained or lost by an ___________ or object)
Planck's theory relates to the atom because ___________ can absorb or release
certain specific amounts of _____________.
When we heat a piece if metal and the color changes from orange to red to
white, the objects color is actually _____________ from one color to the next.
We cannot see the ___________s between these bits of light, or quanta,
because they are _______________ for our eyes to perceive.
B. Einstein's Contribution:
__________________: when high frequency light (violet) can causes electrons
to be knocked off of a piece of metal, while lower frequency light (red) cannot.
Einstein explained this photoelectric effect using ___________ theory.
He said that __________ is divided into little packets called _________.
Electrons can absorb ________e photon at a time, and must absorb _______ of
the _________ in the photon.
If enough _________ is present in the ___________, the electron will be
____________ from the metal. If there is ______ enough _________ in the
photon, the electron will ________ be removed from the metal, no matter how
many ___________ energy photons are absorbed.
There must be the _________ sized photon in order for the metal to be
__________. The photons cannot be ________________ to the total amount of
energy needed.
C. Compton:
Showed that a ___________ could collide with and electron and change the
_____________ of both the _________ and the __________, therefore light can
transfer momentum and behaves as a ______________.
Is energy a wave like light, or a particle?
__________
Concept is called the ___________________________.
***Scientists now believe that light behaves as both a ___________ and as a
_________________.
What about the other way, is matter a wave?
At this point, scientists believe matter behaves as a _______________ only.
D. de Broglie
Did experiments which showed that matter behaves as a ________ as well.
E. 1925 Erwin Schroedinger
Described the __________ function of the electron.
Solutions to the equation are called __________ which are tied to a certain
_________.
F. The Heisenberg Uncertainty Principle.
There is a limit to how well we can know both the __________ and the
______________ of an object.
__________________________________ states that we cannot know the exact
location and exact momentum of an object at a given time.
***Now Scientists believe matter behaves as a ______________ and a
________.
III. QUANTUM MECHANICAL MODEL OF THE ATOM
So far we have learned:
-energy of an electron is ____________ or can have only __________
amounts of energy
-electrons exhibit __________ behavior
-cannot determine the exact __________ and _____________ of an
electron at a given instant
All of these things together make-up the Quantum Mechanical Model of the atom.
Characteristics of the Quantum Mechanical Model
Quantum numbers
Angular momentum quantum number _____.
_______ of orbital.
integer values from 0 to n-1
l =0 is called s
l =1 is called p
l =2 is called d
l =3 is called f
Magnetic quantum number ______
integer values between -l and +l
tells ___________ in each shape.
Electron spin quantum number _________
Can have 2 values.
either +1/2 or -1/2
A. Electrons are found in _____________ (not orbits as Rutherford's model
described) (Angular Momentum Quantum Number, l)
An ___________ is a region around the nucleus of an atom where an
____________ with a certain amount of ___________ is likely to be found
An orbital looks like a __________ cloud of _____________ charge which is
____________ dense where the electron is more likely to be found and
________ dense where the electron is less likely to be found. The density of
an electron cloud is called the _____________________.
There are different types of orbitals, _______________.
Each orbital corresponds to a certain amount of __________. The main
or principal energy levels in an atom are designated by the principle
quantum number, _____.
The lowest energy state is called the ___________________.
B. Each principle energy level is divided into one or more _____________.
The ____________ of sublevels in each principle energy level is equal to
the quantum number, ______, for that energy level.
The sublevels are labeled with a ______________ (the value of the quantum
number) and a __________ (the type of sublevel, s, p, d, or f).
For example:
First energy level (n=1) has _________ sublevel which contains a single
____ orbital. The sublevel is therefore called the ___ sublevel.
Second energy level (n=2) has ______ sublevels which contain a single
____ orbital and three ____ orbitals of equal energy.
The sublevels are called the ___ and the ____.
Third energy level (n=3) has _______ sublevels which contain a single
____ orbital, three _____ orbitals, and five ____ orbitals of equal
energy.The sublevels are called ________________.
Fourth energy level (n=4) has ______ sublevels which contain a single
___ orbital, three ____ orbitals, and five ____ orbitals, and seven ____
orbitals of equal energy. Called-_________________
C. Electron Spin (Electron spin quantum number (ms))
_________ behave as if they were ___________ on their own axis.
Electrons spin either ____________ or ____________________.
________________________: states that each orbital in an atom can hold a
maximum of ______________ and these electrons must have ___________
spins.
___________ electrons have opposite spins. A single electron is called
_______________.
Therefore each sublevel can hold only a certain number of electrons
s sublevel has ___________ and can hold a maximum of ___________
p sublevel has __________ and can hold a maximum of ___________
d sublevel has __________ and can hold a maximum of ___________
f sublevel has __________ and can hold a maximum of ___________
D. DETERMINING ELECTRON CONFIGURATIONS
The electron configuration is the __________ of electrons among the
__________ of the atom. It describes ________ the electrons are found and
__________ energy they possess.
Orbital Energy Diagram
-------------------------4d __ __ __ __ __
------5s __
----------------4p __ __ __
------------------------3d __ __ __ __ __
-----4s __
----------------3p __ __ __
-----3s __
----------------2p __ __ __
-----2s __
-----1s __
The _____________ Principle:
Electrons are added _________ at a time to the ____________ energy
orbital available until _________ electrons have been accounted for.
The Pauli Exclusion Principle
See above
_______________ Rule
Electrons occupy ______________ orbitals so that a maximum
number of ________________ electrons result.
Orbital Diagram
Element symbol __ __
1s 2s
__ __ __
2p
3s
__ __ __ __
3p
Simplified Electron Configuration
Write the label for each occupied sublevel and add a __________ to
indicate the number of __________s in each sublevel. The ________ of the
superscripts represents the total number of ____________ in the atom.
Uncle Wiggly's Chart (or the Diagonal Rule)
1s
2s
3s
4s
5s
6s
7s
2p
3p
4p
5p
6p
7p
3d
4d
5d
6d
7d
4f
5f
6f
7f
Exceptions to the Aufbau Principle
Cr and Cu
IV. Another Look at the Atom
Pure elements, when heated up, only emit __________ wavelengths of
radiation. This ______________ is different for every element.
___________ attended a lecture given by Rutherford in which Rutherford
described his ____________ model of the atom. Bohr realized that
_____________ idea about quanta could be applied to the ______________
atom.
He didn’t know why but only ____________ energies were allowed.
He called these allowed energies __________ levels.
Putting Energy into the atom moved the electron away from the nucleus.
From ____________ state to ____________ state.
When it returns to ______________ state it gives off light of a certain
____________.
Bohr developed the quantum model of the ____________ atom.
He said the atom was like a ___________ system.
The electrons were attracted to the nucleus because of ____________ charges.
Bohr said that when an atom is heated up, or supplied with energy, the electrons
will __________ certain specific sized packets of __________. The electron will
then become “_____________” and will jump to a __________ energy level.
The electron does not like the __________ "__________" state. The electron
will then ___________ the absorbed energy in the form of __________ of a
specific wavelength and return to the original low energy ___________ state.
Each ______________ can absorb a certain sized __________ of energy. This
is what we see when looking through the ______________ at a specific element.
We see the different colors which represent the __________ of energy absorbed
by each specific electron in the atom. When we do the flame test (not looking
through the spectroscope), we see a ___________ of the colors found in the line
spectrum for that particular element.
Hydrogen spectrum
Emission spectrum because these are the colors it gives off or emits.
Called a ________ spectrum because there are just a few discrete __________
showing
Only certain energies are allowed for the hydrogen atom.
Can only give off certain energies.
Energy in the in the atom is _________________.