Ionisation enthalpy

Question 1

What happens to the amount of energy (ionisation enthalpy value) needed to remove the electron as you go down the group

Answer 1

it decreases as the number of protons in the nucleus increase but so do the amount of electron shells meaning there is a weaker attraction, more shielding and further away between the electrons and positive nucleus meaning it requires less energy to remove the electron

Question 2

What happens to the amount of energy (ionisation enthalpy value) needed to remove the electron as you go along the period

Answer 2

it increases because the number of protons increase as well as the electrons but these go into the same shell so there is a higher attraction because the positive nucleus attracts the outer electron more strongly and more energy is required to remove the electron

Question 3

Which group has the lowest ionisation enthalpy value and what does it mean

Answer 3

group 1 which means it is easy for them to lose an electron so they are very reactive

Question 4

What has the highest ionisation enthalpy value and what does it mean

Answer 4

noble gases which means they are very unreactive

Question 5

First ionisation enthalpy meaning

Answer 5

it is the energy required to remove one electron from every atoms in one mole of sperate, gaseous atoms of the element

Question 6

Why does in ionisation enthalpy increase when you remove the 2nd, 3rd… electron

Answer 6

as once you remove one electron from an atom we have the same number of protons attracting fewer electrons so the attraction is stronger so more energy is required to remove the second electron

Question 7

Why are there large jumps in the amount of ionisation enthalpy` value at 2,8,3

Answer 7

the first 3 electrons are from the outer shell but the 4th electron is from the next shell in so it is much closer and less shielded from the positive nucleus so attraction is stronger and more energy is required to remove it