4-2: P Orbitals

Question 1

What are the different orbital shapes?

Answer 1

s, p, d

Question 2

Types of p orbitals

Answer 2

Px, Py, Pz
(all as subscripts)

Question 3

Types of d-orbitals

Answer 3

d(x^2-y^2), dxy, dyz, dxz, d(z^2)
(All as subscripts)

Question 4

Aufbau Principle

Answer 4

• an electron occupies the lowest-energy orbitals that can receive it
• shows order in which electrons occupy orbitals

Question 5

Pauli Exclusion Principle

Answer 5

• no two electrons in the same atom can have the same set of four quantum numbers
• reflects importance of the spin quantum number
• energy, shape, and orientation comes from the principle, angular momentum, and magnetic quantum numbers.

Question 6

Hunds Rule

Answer 6

• Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron.
• All electrons in singly occupied orbitals must have the same spin state.

Question 7

Number of energy levels

Answer 7

Highest coefficient

Question 8

Numbers of sublevels

Answer 8

Number of letters in total

Question 9

What are all the different orbitals in order?

Answer 9

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

Question 10

What are the exceptions for the orbitals?

Answer 10

First lanthanide is 5d
First two actinides are 6d