1. You have learned how to write electron configuration… Let’s learn exactly what they represent!

2. Match the following atomic model with sicentists
Bohr
Thomson
Dalton
Rutherford

3. John Dalton
Atom=solid indivisible mass

4. J.J. Thomson Plum-pudding model
Negatively charged electrons stuck into a lump of positively charged material
Explain about electrical properties of atom

5. Ernest rutherford
Most of atom’s mass is concentrated in a small positively charged region called nucleus
But doesn’t explain why atom doesn’t collapse

6. Niels Bohr Electrons travel in definite orbits around the nucleus
Energy level; region around the nucleus where the electron is likely moving
Quantum =amt of energy required to move an electro from its present energy level to the next higher one
Higher energy level>>more energetic

7. Quantum Mechanical Model-Schrodinger
Doesn’t define exact path an e- takes place
Energy level=principal quantum numbers (n)
Estimates the probability of finding an electron in certain position
Thicker the cloud>>more likely to find e-

8. Principal quantum number
=energy level
N=1,2,3…..
N increase>>farther from nucleus
Within each principal energy level, the e- occupy …

9. Energy sublevels Principal Energy Levels Number of sublevels Sublevels1 S
N=2 2
S,P
N=3 3
S,P,D
N=4 4
S,P,D,F

10. Atomic orbitals
Different shape of electron cloud where you are more likely to find
How many orbital are in the 2nd energy level?
How many e- in 3rd energy level?
Type of sublevel
Number of orbitals S 1 P 3 D 5 f 7

11. For the rest of the class
Let’s practice more on electron configuration!
Electron configuration battleship
wkst