Unit 2: Electron configuration

Question 1

State the electron configuration

Answer 1

Shell/energy level: 1,2,3,4
Sub shell: S,P,D,F
Orbital: 1,3,5,7
No of electrons: 2,6,10,14

Question 2

What are orbitals

Answer 2

Areas of an atom where electrons are likely to be found

Question 3

What is the bus seating rule

Answer 3

Each orbital is filled before the electrons pair up

Question 4

What are the exceptions to the rule

Answer 4

CR: 1S2, 2S2, 2P6, 3S2, 3P6, 4S1, 3D5
CU: 1S2, 2S2, 2P6, 3S2, 3P6, 4S1, 3D10

Question 5

What is the definition for first ionisation energy

Answer 5

The energy needed to remove 1 electron from 1 mole of gaseous atoms resulting in 1 mole of gaseous ions

Question 6

What are the 2 rules for the ionisation formula

Answer 6

always include state symbols. monatomic atoms

Question 7

What factor effect ionisation energy

Answer 7

Charge of nucleus- increase in charge increase in IE
Distance from nucleus- increase in distance decrease in IE
Shielding- Increase in shielding decrease in IE
Repulsion- single pairing in an orbital results in repulsion and decrease IE
Consecutive IE- IE increased- especially between energy levels

Question 8

What is the trend across the period and down the group

Answer 8

Across the period, there is the same level of shielding but the charge of the nucleus gets bigger so the atomic radius decreases. IE increases
Down the group, distance from the nucleus increases as does shielding so IE decreases