Honors Chemistry
Unit 3
 Electron orbital shapes
 Rules:
o Aufbau principle
o Hund’s Rule
o Pauli Exclusion principle
 Orbital notations
 Electron configuration
 Noble gas notation
 Quantum numbers
1
We are learning to:
1. Describe the quantum mechanical model.
2. Apply the quantum mechanical model.
We are looking for:
1a. Electrons can move from ground state to an excited state by gaining specific amounts of energy
(quantum) and return to the ground state by releasing a specific amount of energy (quantum) in the
form of photons.
1b. Define each of the 4 quantum numbers (principal, angular momentum, magnetic, spin).
1c. Describe the shape of the various orbital shapes (s, p, d, f).
2a. Use the Aufbau principle, Hund’s rule, and Pauli exclusion to assign electron/orbital/Noble gas
configurations for a given element.
2b. Identify the exceptions to the Aufbau principle and Hund’s rule for electron configurations.
2c.Give the 4 digit quantum number for a specific electron in an orbital notation.
2d. Indicate the specific electron in an orbital notation that is described by the given 4 digit quantum
number.
2e. Identify the s, p, d, and f blocks on the periodic table.
2
Name _______________________________ Class _______
Flame Test: Nichrome Wire
Purpose:
1. To observe the different colors emitted by ions in a flame test.
Materials:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
Barium Nitrate/Chloride
Calcium Nitrate/Chloride
Lithium Nitrate
Potassium Nitrate
Sodium Nitrate/Iodide
Strontium Nitrate/Chloride
Copper Sulfate
Matches
Nichrome Wire
Bunsen Burner
Nitric Acid
Procedure:
1. Place tip of nichrome wire in nitric acid.
2. Place tip of nichrome wire in flame until there is a constant orange/yellow color.
3. Dip the tip of the nichrome wire into a salt (only put one or two crystals on the tip) or a
solution of the salt.
4. Place the tip of the nichrome wire (with salt /solution on it) in the flame.
5. Observe the color of the salt/solution as it burns.
6. Repeat steps 1-5 for each salt/soltuion.
3
Data and Information
Metal Ion
Formula of Salt
Color of Flame
Ba+2
Ba(NO3)2
Color:
Ca+2
Ca(NO3)2
Color:
Li+
LiNO3
Color:
K+
KNO3
Color:
Na+
NaNO3
Color:
Sr+2
Sr(NO3)2
Color:
Cu+2
Cu(NO3)2
Color:
Questions:
1. What kind of colors are emitted by the ions?
2. Can a flame be used to identify a metal ion? Why, or why not?
3. What is happening to the electrons when we see color?
Unknown
Color
Metal Ion(s)
A
B
C
4
5
Schrodinger Wave Equation
Only certain frequencies satisfied his
mathematical equations, which described
the wave properties of electrons.
Orbital = 3D region around the nucleus
that indicates the probable location of an
electron
To further define the orbitals, quantum
numbers are used.
6
7
1. Principle Quantum #
(n) Energy Level
3.
2.
4.
8
9
Heisenberg’s Uncertainty Principle:
It is impossible to determine both the position and velocity of
an electron at the same time.
Aufbau Principle:
An electron occupies the lowest energy level available.
Pauli Exclusion Principle:
No 2 electrons in the same atom can have the same 4
quantum numbers.
Hund’s Rule:
Orbitals of equal energy are each occupied by one electron
before any orbital is occupied by a second electron.
All electrons in singularly occupied orbitals must have the same
spin.
10
Aufbau Principle
Filling Order
1s2
2s2
2p6
3s2
3p6
3d10
4s2
4p6
4d10
4f14
5s2
5p6
5d10
5f14
6s2
6p6
6d10
6f14
7s2
7p6
7d10
7f14
11
12
13
Name________________________________________
Write the Orbital Notation for each of these elements
1. Carbon ( C )
2. Argon (Ar)
3. Chromium (Cr)
4. Antimony (Sb)
5. Tungsten (W)
14
6. Calcium (Ca)
7. Germanium (Ge)
8. Molybdenium (Mo)
9. Tin (Sn)
10. Barium (Ba)
15
Name________________________________________
Write the Electron Configuration for each of these elements
1. Beryllium (Be)
2. Sulfur (S)
3. Scandium (Sc)
4. Copper (29)
5. Iodine (I)
16
6. Europium (Eu)
7. Osmium (Os)
8. Actinium (Ac)
9. Uranium (U)
10. Seaborgium (Sg)
17
Name __________________________________________________________________
Notation Worksheet
1. Write the orbital notation for the following elements:
Nitrogen (N)
Chlorine (Cl)
Gallium (Ga)
Cesium (Cs)
2. Write the electron configuration for the following elements:
Titanium (Ti)
Xenon (Xe)
Polonium (Po)
3. Write the Noble gas notation for the following elements:
Strontium (Sr)
Iodine (I)
18
Name __________________________________
More Practice!!!!
Fill in the table below:
Name of Quantum #
Information obtained
Symbol
1.
2.
3.
4.
5. Please write the orbital notation for arsenic, As (#33).
6. Find the 27th electron (based on filling order) in #6 and give me the four digit code
for it.
7. Please write the electron configuration for Cesium, Cs, #55.
8. Draw the electron that is represented by 4 3 +2 -1/2
19
Name __________________________________________________________________
4. Write the orbital notation for:
a. 14Si
b.
29Cu
5. Write the electron configuration for:
a. 16S
b.
39Y
6. Write the Noble gas notation for:
a. 22Ti
b.
49In
7. Given the following orbital notation; predict the 4 digit quantum number that
describes the circle electron:
a. 
1s

2s
b. 
1s

2s
  
2p
  
2p
4 digit quantum # _______________________

3s
  
3p

4s
    
3d
4digit quantum # __________________________
8. Given the 4 digit quantum number; draw the electron that it describes:
a. 2 0 0 –½
b. 3 1 1 +½
20