electron structure

Question 1

define first ionisation energy

Answer 1

the energy required to remove one mole of electrons from one mole of gaseous atoms

Question 2

what are the 3 factors that affect ionisation energy

Answer 2

position of electron
proton number
shielding

Question 3

how will the proton number affect ionisation energies

Answer 3

the more protons the greater the force of attraction so the harder it is to remove electrons.
(higher IE)

Question 4

how will the amount of shielding affect the ionisation energies

Answer 4

the more complete inner shells (more shielding) the easier it is to remove electrons
(lower IE)

Question 5

how does the distance between the electron and the nucleus affect the IE

Answer 5

the further the electron from the nucleus the less energy required to remove it
(lower IE)

Question 6

how do electron shells affect the IE

Answer 6

electrons in the same shell have similar attraction to the nucleus
(similar IE)

Question 7

which is easier to remove P electrons or S electrons

Answer 7

P electrons are easier to remove

Question 8

why are P subshell electrons easier to remove that S subshell electrons

Answer 8

P subshell is shielded by the full S subshell and is higher in energy

Question 9

how do paired electrons affect the IE

Answer 9

paired electrons are easier to remove as they are both negative so the repel each other
(lower IE)

Question 10

why does the IE increase when moving to a PQS that is closer to the nucleus

Answer 10

electrons in shells closer to the nucleus experience much less shielding therefore have a greater attraction to the nucleus.