Lecture 9 & 10: Orbitals, Electron Configurations Flashcards
1
Q
L = 0
A
s
2
Q
L = 1
A
p
3
Q
L = 2
A
d
4
Q
L = 3
A
f
5
Q
electrons states
A
orbital x2 (2 in each orbital)
6
Q
how are magnetic fields generated
A
electron spin charges
7
Q
mL (m subscript L) is the # of
A
orbitals
8
Q
nodes are
A
region of space with a zero percent chance of an electron wave being there
9
Q
total nodes in orbital
A
(n-1)
10
Q
planar nodes
A
L (special L)
11
Q
radial nodes
A
(n-1)-L
12
Q
Pauli Exclusion Principle
A
only 2
electrons can be placed in each
orbital
13
Q
Aufbau (‘to build”) Principle
A
electrons are placed in lowest energy orbitals first (lowest n + l )
14
Q
Hund’s Rule
A
BUS RULE electrons fill all degenerate orbitals singly (and with same spin) before pairing up (it costs energy to put two electrons in the same orbital because they repel each other)
15
Q
diamagnetic
A
all electrons paired (arrows up and down in all boxes)
