1.3.3, 1.3.4, 1.3.5 - Electron configurations

Question 1

What does the Quantam Mechanical Model of the atom posit

Answer 1

-even though we cannot know the exact location of an electron, we can predict a region of probability
-orbitals have different shapes, and it depends on the energy of electrons that occupy that space
-the more energetic the electron, the further from the nucleus it will be

Question 2

what is energy level (electron configurations)

Answer 2

-energy level refers to the proximity to the nucleus (the smaller the value, the closer to the nuc)
-corresponds to the horizontal row (period) of the element

Question 3

Pauli Exclusion principle

Answer 3

electrons occupying the same orbital must have opposite spins (opposite magnetic fields create an attractive force)

Question 4

Aufbau principle

Answer 4

electrons will fill lower energy levels/orbitals first

Question 5

Hund’s rule

Answer 5

when orbitals have degenerate sublevels, electrons will first occupy each seperate orbital with parallel spin

degenerate=having the same energy
parallel spin=spinning in same direction so half the arrows point in the same direction

Question 6

how many sublevel does the s orbital have

Answer 6

1

Question 7

how many sublevel does the p orbital have

Answer 7

-3 degenerate sublevels (px, py, pz)
-each sublevel hold 2 e-, hence 6e- in a p- orbital

Question 8

how many sublevels does the d orbital have

Answer 8

5 degenerate sublevels, each sublevels holds 2e-, making a total of 10 e-

Question 9

how many sublevels does the f orbital have

Answer 9

7 sublevels of degenerate energy
max of 14e-

Question 10

Electron configuration example (hydrogen)

Answer 10

H : 1s^1

s=orbital
1=energy level
^1= number of electrons

Question 11

electron configuration chart

Answer 11

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

Question 12

Noble Gas Configuration (abbreviated or shorthand)

Answer 12

-bc noble gases are found at the end of each period, they can be used to represent a complete configuration to that point

ex.
[Ar] (noble gas) = 1s2 2s2 2p6 3s2 3p6

Ca: 1s2 2s2 2p6 3s2 3p6 4s2 => [Ar] 4s2

Question 13

what happens when an electron enters a d orbital

Answer 13

it reduces the energy of that orbital so that it drops below s, so both 4s2 3dx or 3dx 4s2 are acceptable

Question 14

How to identify V e- from e- configs

Answer 14

1. locate highest energy level in your config
   ex. 1s2 2s2 2p6 3s2 3p1 => 3s2 3p1
2. identify the # of e- in a and p orbitals
3. add values tgt

Question 15

valence shell arrangement of transition metals (multi-valent)

Answer 15

they will lose e- from the s and p orbitals in the highest energy level first, then if more e- loss is required, they will lose from the highest energy d orbital

Question 16

special cases in e- config (Copper (Cu) and Chromium (Cr)

Answer 16

Cu Cr will adjust their config to increase d orbital stability, as they are more stable half filled (5) or fully fielled

ex. Cu:[Ar] 4s2 3d9 -> [Ar] 4s1 3d10

Question 17

WHat happens in ion configs

Answer 17

-metal loses v e- to form cations (empty v shell)

-non metals gain v e- to form anions (fill v shell)

-they do this to become isoelectronic with the nearest noble gas (metals w noble gases period above, non metals w the one in the same period)

Question 18

define isoelectronic

Answer 18

having the same v shell arrangement

Question 19

What are potential energy diagrams

Answer 19

-another way to model e-configs
-more detailed to show the energy differences in orbitals, all sublevels, all electrons and electron spin