Unit 2 - Atomic Concepts - Honors - SPDF

Question 1

Definition of Sublevel (3)

Answer 1

1. A division
2. Of an e- shell
3. Contains one or more atomic orbitals

Question 2

What are the four sublevels?

Answer 2

S, P, D, F

Question 3

What is the “s” sublevel? (3)

Answer 3

1 Orbital
2 Electrons
Orbital shaped like a sphere

Question 4

What is the “p” sublevel? (3)

Answer 4

3 Orbitals
6 Electrons
Orbital shaped like a dumbell

Question 5

What is the “d” sublevel?

Answer 5

5 Orbitals
10 Electrons
Orbital shaped like a clover

Question 6

What is the “f” sublevel? (3)

Answer 6

7 Orbitals
14 Electrons
Orbital shaped like an incredibly complex shape

Question 7

Diagram for Sublevels

Answer 7

n = 1 —– 1s²
n = 2 —– 2s², 2d⁶
n = 3 —– 3s², 3p⁶, 3d¹⁰
n = 4 —– 4s², 4p⁶, 4d¹⁰, 4f¹⁴
n = 5 ——5s², 5p⁶, 5d¹⁰, 5f¹⁴

Question 8

What does this represent: 1s¹

Answer 8

1 = Principal Energy Level
S = Orbital/Sublevel
¹ = # of electrons

Question 9

When trying to determine the electron configuration of an element, what is the order of the orbitals in increasing energy? Note: This is applying the Aufbau Principle (up to PEL of 7)

(Up to 6s)

Answer 9

so, this is the orbital diagram:
n = 1 —– 1s
n = 2 —– 2s, 2p
n = 3 —– 3s, 3p, 3d
n = 4 —– 4s, 4p, 4d, 4f
n = 5 ——5s, 5p, 5d, 5f
n = 6 ——6s, 6p, 6d, 6f
n = 7 ——7s, 7p, 7d, 7f

order is:
1s

2s

2p

3s

3p

4s

3d

4p

5s

4d

5p

6s

4f

5d

6p

7s

5f

6d

7p

Question 10

How do we determine the orbital configuration?

Answer 10

Find out the final sublevel of an element, then go back and list the orbitals in increasing order up to the sublevel of the element

ex: Final Sublevel of Ca: 4s²
1s², 2s², 2p⁶, 3s², 3p⁶, 4s²

2 - 8 - 8 - 2

Question 11

Definition of Hund’s Rule (3)

Answer 11

1. Electrons occupy orbitals singly
2. Once all the orbitals are singly occupied
3. Additional electrons will pair up in orbitals

Question 12

Why do electrons occupy orbitals singly? (2)

Answer 12

1. Electrons repel each other due to - charge
2. They occupy singly to minimize repulsion

Question 13

Definition of the Aufbau Principle

Answer 13

Electrons are placed in lower orbitals first, then higher

Question 14

Definition of Pauli Exclusion Principle (5)

Answer 14

1. No two electrons
2. In an atom
3. Can have same sets
4. Of the four quantum numbers
5. This means they can’t have the same spin in the same orbital

Question 15

What is competitive exclusion in the pauli exclusion principle? (2)

Answer 15

1. Each orbital holds a max of 2 e-
2. 2 e- must have opposite spins

Question 16

How do you apply competitive exclusion to box diagrams?
Ex: 1s², 2s², 3p³

(JUST READ)

Answer 16

1. 1s² and 2s² has two electrons in 1 orbital
2. Apply the opposite spins
3. Draw a single box for 1s²
4. Because there’s only one orbital in 1s²
5. Draw both an up and down arrow
6. To indicate the opposite spins
7. Same thing for 2s²
8. For 3p³, there’s 3 electrons in 3 orbitals
9. Applying Hund’s rule
10. You need to draw 3 boxes
11. And 1 electron in each box (add 1 arrow)