1. Models of the Atom

2. Goals for this Lesson
Recognize that there are 3 different models for the atom
DO NOT NEED TO KNOW MANY SPECIFICS!!
Decipher the 4 different atomic orbital shapes
Be able to know, in general, what they look like and how many shapes there are for each orbital
Recall how many electrons can fit in each atomic orbital

3. Rutherford’s Model of the Atom
Great at showing the relationship between protons, neutrons and electrons
Lacking a major detail
Couldn’t show the chemical properties of elements
Example
Why, when heated, metals turn red, than orange, than yellow, than white
Need a better model to show these properties

5. Neils Bohr and the Bohr Model
Danish physicist
Student of Rutherford
What he proposed (used the Hydrogen atom for his experiment = 1 e-)
Electrons exist in specific circular paths, or orbits, around the nucleus
Each electron orbit has a fixed energy
Energy level
Electrons can jump from one energy level to the next

6. The Bohr Model What it did not prove
What happens with an element that has more than 1 electron?
Do the electrons collide, do they dance with each other?
Bohr’s Model couldn’t predict this

7. Quantum Mechanical Model
The amount of energy it takes to propel an electron from one energy level to the next
Erwin Schrodinger
Used math to figure out the energy levels of electrons
Where electrons are at any given point in time
What did Schrodinger prove?
Electrons exist in clouds around the nucleus
Used math to say what the probability it is to find an electron in any specific area of the cloud

8. Quantum Mechanical Model
What does the quantum mechanical model prove?
Gives you the energy levels of the electrons
Tells you where each electron is for any element
Located in the energy levels (the quantum levels)
Explains why elements have certain chemical properties
We excite electrons up and down energy levels

10. Goals From Now On! Decipher the 4 different atomic orbital shapes
Recall how many electrons can fit in each atomic orbital

11. Take a Deep Breath Energy Levels Within each energy level
There are 4 energy levels
n = 1, 2, 3, or 4
Within each energy level
We have atomic orbitals
The region of space where there is a high probability you will find an electron
4 Atomic orbitals (also called sublevels)
s orbital
p orbital
d orbital
f orbital

12. s orbital

13. p orbitals

14. d orbitals

15. f orbitals

16. Energy Levels Energy Level 1 ( n =1) Energy Level 2 (n = 2)
s orbital (1 shape)
2 possible electrons in this level
Energy Level 2 (n = 2)
s orbital (1 shape) and p orbitals (3 shapes)
2 possible electrons in the s orbital
6 possible electrons in the p orbital
8 total

17. Energy Levels Energy Level 3 ( n = 3) Energy Level 4 ( n = 4)
s orbital (1 shape), p orbitals (3 shapes) and d orbitals (5 shapes)
2 electrons in the s orbital
6 electrons in the p orbital
10 electrons in the d orbital
18 total
Energy Level 4 ( n = 4)
s orbital (1 shape), p orbitals (3 shapes), d orbitals (5 shapes), and f orbitals (7 shapes)
14 electrons in the f orbital
32 electrons