Electron Arrangement

Question 1

The configuration/ order of sub-lvls

Answer 1

1s.
2s. 2p.
3s. 3p. 4s. 3d.
4p. 4d. 4f.

S= 2 e (1[])
P = 6 e (3 [])
D = 10 e (5[])

Question 2

Sub levels

Answer 2

Because not all e- in a shell have the same Energy -> divided into sub levels with orbitals.

Question 3

Orbital

Answer 3

a region where you are most likely to find e-.
“containers” for e- in the sublevels

Question 4

Paulis exclusion principle

Answer 4

The e- in orbitals spin opposite directions -> more stable.

Question 5

Chromium electron arr.

Answer 5

instead of having 4 in 3d it takes 1 from 4s and becomes 4s1 3d5
More stable – 6 unpaired e- with lower repulsion / none have another e- repulsing them

Question 6

Copper electron arr.

Answer 6

Becomes 4s1 3d10 instead of 4s2 3d9
More stable that way