Electron structure

Question 1

Define orbital

Answer 1

A region around the nucleus (of an atom) that can hold up to two electrons with opposite spins

Question 2

What is the trend in ionisation energy from Li to Ne?

i) Explain why

Answer 2

The IE increases
i) The charge of the nucleus increases, the atomic radius gets smaller so more energy to required as there is a greater attraction between the electrons and nucleus. Shielding stays the same

Question 3

Name the 4 shapes of orbitals

For two describe what you would draw in order to represent them

Answer 3

s, p, d, and f (NOTE- the letters must be lowercase)
s- spherical
p- dumb-bell shape

Question 4

Up to how many electrons can an orbital tolerate?

Answer 4

2

Question 5

What condition is needed for 2 electrons to be held in an orbital?

Answer 5

The electrons must have opposite spins

Question 6

How do electrons fill orbitals?

Answer 6

From the lowest energy level up

Question 7

How many electrons are there in:

i) a full p subshell
ii) a half full s subshell
iii) a full 3rd electron shell

Answer 7

i) 6
ii) 1
iii) 18

Question 8

How many orbitals are there in:

i) a d sub-shell
ii) a f sub-shell
ii) a p sub-shell

Answer 8

i) 5
ii) 7
iii) 3

Question 9

Write the spdf notation of Na

Answer 9

1s1 2s2 2p6 3s1

Question 10

What does the term degenerate mean when applied to orbitals?

Answer 10

Having identical energy

Question 11

Which type of subshells contain several degenerate orbitals?

Answer 11

p, d, and f

Question 12

What order are subshells filled?

Answer 12

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

Question 13

Define subshell

Answer 13

A group of orbitals of the same type within a shell

Question 14

Define electronic configuration

Answer 14

A shorthand representation that shows how electrons occupy subshells in an atom