3.1.1 Periodicity

Question 1

first ionisation energy

Answer 1

amount of energy needed to remove 1 mole of electrons from 1 mole of atoms in a gaseous state

Question 2

successive ionisation energy (definition)

Answer 2

amount of energy needed to remove 1 mole of electrons from 1 mole of ion in a gaseous state

Question 3

first ionisation energy equation

Answer 3

X(g) -> X(g)+ + e-

Question 4

Trends in ionisation energy

Answer 4

increases as you go across periods

decreases as you go down groups

Question 5

factors that affect IE ( charge)

Answer 5

charge- number of protons in a nucleus
the bigger the charge, the greater the attractive forces between the nucleus and the outer electron, the higher the ionisation energy

Question 6

factors that affect IE (atomic radius)

Answer 6

atomic radius- distance from the nucleus to the outer electron
the bigger the atomic radius, the weaker the attraction between the nucleus and the outer electron,making it easier to remove the outer electron meaning lower ionisation energy

Question 7

factors that affect IE (shielding)

Answer 7

shielding- the effect on inner electrons to lose outer electrons
lots of electron shells and inner electrons between the nucleus and the outer electrons, the more shielding meaning lower IE

Question 8

anomalies in IE trend (G2 and 3) (Mg and Al)

Answer 8

drops between Mg and Al, Al has a 3p sub-shell, which is more than a 3s sub-shell therefore the outer electron has more shielding (draw electron diagram)

Question 9

anomalies in IE trend (G5 and 6) (P and S)

Answer 9

drops at S, this is because it has an electron pair orbital in it’s 3p orbital, repulsion between the pair will make them easier to separate (easier to separate electrons from paired orbitals)

Question 10

Reading IE graphs and interpreting data

Answer 10

look for large increase in IE data, shows removal from an electron in another shell closer to nucleus