2.2.1 Electron Structure

Question 1

Number of electrons that can fill first 4 electron shells

Answer 1

1 -> 2
2 -> 8
3 -> 18
4 -> 32

Question 2

Orbital

Answer 2

a region of space around the nucleus that can hold up to 2 electrons with opposite spins

Question 3

Shape of S orbital

Answer 3

spherical

Question 4

Shape of P orbital

Answer 4

dumbbell

Question 5

number of orbitals in s,p,d sub-shells

Answer 5

s -> 1
p -> 3
d -> 5

Question 6

number of electrons in s,p,d sub-shells

Answer 6

s -> 2
p -> 6
d -> 10

Question 7

Writing electron configuration (order)

Answer 7

1s2s2p3s3p4s3d4p4d

Question 8

Degenerate

Answer 8

Orbitals with the same energy

Question 9

Electrons in a box

Answer 9

one box is an orbital containing 2 electrons with opposite spins
fill up one electron in a box at a time

Question 10

Why does 4s come before 3d?

Answer 10

4s is at a lower energy and electrons will enter a lower energy level first

Question 11

Why do the electrons fill up one one box at a time in an energy level?

Answer 11

due to repulsion, they have the same charge and so want to stay as far away from each other as possible

Question 12

Electron spins

Answer 12

electrons have spins, 2 electrons can’t have the same spin in an orbital

Question 13

Writing ion configuration

Answer 13

cations- remove electrons from highest energy levels first
lose 4s electrons before 3d electrons
anions- just add on electrons

Question 14

Noble gases and configuration

Answer 14

use nearest past noble gas to write configuration (makes it shorter)

Question 15

Why are the electronic configurations for Cu and Cr different?

Answer 15

4s1 then fill up 3d subshell because it makes it more stable to have a full 3d shell