1. Chemistry – Nov 14, 2016 P3 Challenge- Objective –
Which is smaller? N or P
Which is larger? K+ or K
Which has the higher ionization energy? K or Br
Which has the higher electronegativity? O or Br
Objective –
Quantum Mechanics / Atomic Structure (Get out your colored periodic table)
Get out Periodic Trends Worksheet for Hmk Check

2. Chemistry – Nov 14, 2016 Objective – Agenda
Atomic Structure / Quantum Mechanics
Agenda
Homework Review
Bohr model review, QM overview
Orbital Shapes
Organization of orbitals
Filling order
2D images (given time)
Assignment: Quantum Numbers Worksheet

3. Homework Review 1. O, C, Al, K 2. Ne, Al, S, O (noble gases = 0)
3. F is smaller atom, higher on PT, harder to remove electron from F than I
4. same group
5. a. decrease b. increase c. increase
6. Atomic Radii increase going down PT, Re: more electrons repel each other
7. Ionization E increase going L R, Re: same size, but Z is increasing.

4. Homework Review 8. a. Al Al is lower on PT
b. Na same period, Al is smaller due to higher Z
c. S S is lower on PT
d. O same period, O is larger because it’s to the left
e. Br Br lower on PT
f. Ca Ca lower on PT
9. a. Be I.E increases L R
b. Ca Ca is smaller
c. Na Na is smaller
d. Ar Ar noble gas, I.E increases L R
e. Cl I.E increases L R
f. Li Li is smaller

5. Homework Review 10. a. Ga Ga to the right b. Br Br to the right
c. O O to the right
d. Sr Sr is above Ba
e. Cl Cl is to the right
f. O O is above S
11. a. Ca Cations get smaller
b. Br– anions get larger
c. Na+ Isoelectronic, Na has lower Z
d. Ba+2 Ba is below Sr
e. Cl– isoelectronic, Cl has lower Z
f. S–2 S is below O

6. Bohr model and Quantum models
Recall the Bohr model that uses quantized orbits
Recall Quantum Mechanics that uses quantized orbitals
Orbitals that we draw represent a 90% probability of finding an electron in that space.
Any single orbital can contain up to two electrons (0, 1, or 2)

7. Quantum Mechanics
Same as Bohr model except for how the energy levels are described.
Electrons located in orbitals.
Mathematical description is a “wave function” - Schrödinger
Explains the wave property of matter.
Strategy to understand QM:
Learn what the orbitals look like and how they’re organized on H atom
Populate the orbitals with electrons to describe other atoms

8. Shapes of Orbitals The bigger an orbital, the higher the energy level
The more complicated the shape, the higher the energy level.
Using different shapes is how QM creates its quantized energy levels.
Four different basic orbital shapes: s p d f
Basic shapes double the number of lobes for each level:

9. P, D, and F Orbitals

10. Quantum Mechanics Atomic Model -
Electrons organized on 4 levels
1) Shells 1, 2, 3, 4, 5, 6, 7
2) Subshells s, p, d, f
3) Orbitals
4) An orbital can hold up to two electrons.
S subshells contain 1 orbital (room for 2 e)
P subshells contain 3 orbitals (6 e)
D subshells contain 5 orbitals (10 e)
F subshells contain 7 orbitals (14 e)
Shell 1 – s (2e)
Shell 2 – s and p (8e)
Shell 3 – s and p and d (18e)
Shell 4 – s and p and d and f (32e)
Shell 5 – s and p and d and f (32e)
Shell 6 – s and p and d (18e)
Shell 7 – s and p (8e)
= 118
Structure for all 118 known elements.

11. Each small box with a 2 represents a single empty orbital that has a capacity of 2 electrons.

12. Subscripts (x, y, z, xy, yz etc…
Quantum Numbers
Four Quantum Numbers used to describe the structure. Memory items.
Quantum Number
Name
Allowed Values
Determines
Specifies a
Common labels n
Principle
1, 2, 3, 4…..
Size and Energy
Shell
1,2,3,4…
(Period #)
Angular Momentum
0, 1, 2… (only up to n-1)
Shape
Subshell
s, p, d, f ml
Magnetic
Orientation
Orbital
Subscripts (x, y, z, xy, yz etc… ms
Spin
+½ or -½
Electron
Up ↑, Down ↓

13. How Electrons Fill the Orbitals – the rules
The orbitals are present on every atom, but only some have electrons located in them depending on how many electrons the atom has.
Three guiding principles to use:
1) Aufbau Principle: Electrons live in the lowest energy orbitals possible. (Higher energy orbitals remain empty.)
2) Hund’s Rule: Electrons would rather not live with another electron, but its better to be paired up than to live at a higher energy. If paired, they have opposite spins.
3) Pauli Exclusion principle: No two electrons can occupy the same space. No two electrons can have the same 4 quantum numbers

14. Orbital Energy Levels
Energy levels are not intuitive because the energy levels of the shells overlap.
Order of filling:
1s…2s, 2p…3s, 3p….
Then the shells start to overlap.
…4s, 3d, 4p…5s, 4d, 5p…
…6s, 4f, 5d, 6p…7s, 5f, 6d, 7p
If that seems hard to remember, try this…

15. Shells 1-7 S block P block D block F block Periods 1 – 2 H = 1s 13-18
**actinides
*lanthanides
Shells 1-7
Periods
S block
1 – 2
H = 1s
P block
13-18
B = 2p
D block
3-12
Sc = 3d
F block
Lanthanides
Actinides
La = 4f
Lanthanum 57 La
138.91
Cerium 58 Ce
140.12
Praseodymium 59 Pr
140.91
Neodymium 60 Nd
144.24
Promethium 61 Pm
(145)
Samarium 62 Sm
150.36
Europium 63 Eu
151.97
Gadolinium 64 Gd
157.25
Terbium 65 Tb
158.93
Dysprosium 66 Dy
162.50
Holmium 67 Ho
164.93
Erbium 68 Er
167.26
Thulium 69 Tm
168.93
Ytterbium 70 Yb
173.04
Actinium 89 Ac
(227)
Thorium 90 Th
232.04
Protactinium 91 Pa
231.04
Uranium 92 U
238.03
Neptunium 93 Np
(237)
Plutonium 94 Pu
(244)
Americium 95 Am
(243)
Curium 96 Cm
(247)
Berkelium 97 Bk
Californium 98 Cf
(251)
Einsteinium 99 Es
(252)
Fermium
100 Fm
(257)
Mendelevium
101 Md
(258)
Nobelium
102 No
(259)

16. s p d f 1 1s 2 2s 2p 3 3s 3p 3d 4 4s 4p 4d 4f 5 5s 5p 5d 5f 6 6s 6p 6d 7 7s 7p

17. Exit Slip - Homework Exit Slip:
Determine the highest energy subshell for Strontium and Silicon
What’s Due? (Pending assignments to complete.)
Quantum Numbers Worksheet
What’s Next? (How to prepare for the next day)
Read Holt p