ionisation energy

Question 1

def ionisation energy (no mol!!)

Answer 1

amount of energy needed to remove 1 electron from a GASEOUS atom

Question 2

def FIRST ionisation energy

Answer 2

minimum energy (/mol) needed to remove the 1st electron from 1 mol of gaseous atoms to form 1 mol of gaseous singly positive IONS!!

Question 3

factors affecting i.e (2)

Answer 3

nuclear charge (number of protons), atomic size (electron shells)

Question 4

how does nuclear charge (number of protons) affect i.e

Answer 4

more protons –> nuclear charge becomes more +ve

attraction btw +vely charge nucleus & -vely charged electrons increases

–> i.e increases

Question 5

how does atomic size (electron shells) affect i.e

Answer 5

more electron shells, dist of valence electrons from nucleus increases

attraction of +vely charged nucleus & -vely charged valence electrons decreases

–> i.e decreases

Question 6

i.e across periods

Answer 6

same number of e shells, 1 additional proton

–> nuclear charge increases, increased force of attraction on all -vely charged electrons –> stronger force of attraction to protons

–> more energy needed to remove v electrons

–> i.e increases

Question 7

i.e down groups

Answer 7

1 additional electron shell

–> atomic size increases, +vely charged nucleus further away from -vely charged v electrons

–> weaker force of attraction btw +vely charged nucleus & -vely charged v electrons

less energy needed to remove v electrons

–> i.e decreases

Question 8

successive i.e’s

Answer 8

more energy is needed to remove an electron from a singly +ve ion

electrons are being removed from increasingly +ve ions

–> greater electrostatic foa btw +vely charged nucleus & -vely charged v electrons (2nd i.e > 1st i.e)