1. Warm Up #6
Why do elements like potassium have a LOW ionization energy, and why do elements like chlorine have a HIGH ionization energy?
Draw the rings and rank these atoms in order of smallest to largest atomic radius: C+4, C, C-4
What are the natural charges and group names for each of the following: Na, I, Ar, Cl, Ca, Cs. These elements in order of highest to lowest electronegativity.

2. Chlorine-38, neutrally charged Aluminum-27, neutrally charged
10/19 - Warm Up # 4
Label the number of protons, neutrons and electrons for the following.
(remember, p+ = e- when neutral)
Chlorine-38, neutrally charged
Aluminum-27, neutrally charged
Sodium-23, +1 charge
Nitrogen-14, -3 charge

3. Identifying Elements
Chapter

4. Review of Electrons Negative Charge Found outside the nucleus
Arranged in Orbitals
Rings around nucleus
Octet Rule – wants 8 valance electrons

5. Electron Configurations
Niels Bohr – German chemist
Hypothesized structure of atom:
Positively charged center (nucleus)
Electrons orbit nucleus in rings

6. Rings? No. S P D F Bohr Model – Electrons move in rings
Electrons in rings = A FILTHY LIE
Electrons – move in WEIRD orbitals
Types:
S P D F

7. Weird Orbitals Pictured
S Orbital
1 variety
D Orbital
5 varieties
P Orbital
3 varieties
ELECTRONS MOVE IN THESE RED CIRCLES RANDOMLY

8. You Are Going to a Concert
Your Ticket
Row: 2
Section: P
Seat: 4

9. Electron Configuration

10. Orbitals on the Periodic Table
Remember:
Horizontal Rows = Periods
Symbol = n (principal quantum number)
When n = 1 (first row):
Hydrogen (H) and Helium (He)
When n = 2 (second row):
Lithium (Li) to Neon (Ne)

11. The 2 (major) Quantum Numbers
n = principal quantum number
Period the element is in
ℓ = orbital quantum number
Tells what section e- are in
0 = s, 1 = p, 2 = d, 3 = f

12. S – Left of Transition metals P – Right of Transition metals
S P D F On the Table
Orbital Types = S, P, D, F
S – Left of Transition metals
MAX: 2
P – Right of Transition metals
MAX: 6
D – Transition metals (rectangle)
MAX: 10
F – Lanthanides and Actinides (by themselves)
MAX: 14

13. In 1st P-orbital section
Oxygen: in n = 2, ℓ = 1
In 1st P-orbital section
Right of Transition Metals
Passes Through:
1s (2 elements)
2s (2 elements)
2p (4th element)
Notation: 1s22s22p4
OR….

14. 1s22s22p6 1s22s22p63s23p1 Other examples: 1. Neon (10):
Check:
= 10
2. Aluminum (13):
1s22s22p63s23p1
= 13

15. Write the correct notation or identify the correct element for the following:
Calcium
1s22s22p5
Sulfur
1s22s22p63s1
Quick Quiz

16. Warm Up #7 Write the orbital notation (1s2…) for the following:
Magnesium
Fluorine
Boron
Why does Silicon have a much higher electronegativity than Helium, even though Helium is in the top right corner of the table?
Which element has a larger atomic radius: Neon or Beryllium? Why is this?