Atomic structure 2 : electron configuration and ionisation energies notes

Question 1

why is 4s filled before 3d

Answer 1

it has lower energy

Question 2

what are orbitals

Answer 2

regions of space where electrons can move

Question 3

how many electrons can each orbital contain

Answer 3

2

Question 4

how many orbitals in sub level s

Answer 4

1

Question 5

how many orbitals in sub level p

Answer 5

3

Question 6

how many orbitals in sub level d

Answer 6

5

Question 7

how many orbitals in sub level f

Answer 7

7

Question 8

what does the s block have in reference to electrons

Answer 8

highest energy electrons in an orbital

Question 9

s block

Answer 9

2 in each period

Question 10

p block

Answer 10

6 in each period

Question 11

d block

Answer 11

10 in each period

Question 12

f block

Answer 12

14 in each period

Question 13

why would you re over electrons from 4s before 3d

Answer 13

because 4s electrons are further from nucleus

Question 14

1st factor that effect ionisation energies

Answer 14

• distance between nucleus and outer electrons/ atomic radius
  as the force of attraction increases between nucleus, the outer electrons decreases

Question 15

2nd factor that effect ionisation energies

Answer 15

• charge on nucleus/ num of protons in nucleus
  electrons are attracted to + protons in nucleus
  greater the number of + the greater the force of attraction between outer electrons and nucleus

Question 16

3rd factor that effect ionisation energies

Answer 16

• amount of shielding
  electrons in the outer shell are repelled b electrons in inner shell
  shielding effect reduces attraction between outer electrons and nucleus

Question 17

what is first ionisation energy

Answer 17

energy needed to remove 1 mole of electrons from 1 mole of atoms in their gaseous state to form 1 mole of 1+ ions

Question 18

what else increases as the attraction between outer electrons and nucleus increases

Answer 18

ionisation energy

Question 19

why do successive ionisation energies increase

Answer 19

every time you lose an electron the ion gets a bit smaller

Question 20

atomic radius across the period

trends in first ionisation energies

Answer 20

decreases

as across a period atoms are getting smaller since there are more proton

trends in first ionisation energies

Question 21

atomic radius down a group

trends in first ionisation energies

Answer 21

increases

atoms get bigger
more shells added

trends in first ionisation energies

Question 22

electron shells down a group

trends in first ionisation energies

Answer 22

increases

outer electron is further from nucleus
more shielding

trends in first ionisation energies

Question 23

electron shells across a period

trends in first ionisation energies

Answer 23

stays the same

same shielding

trends in first ionisation energies

Question 24

across period ionisaiom energy generally increases because..

Answer 24

more protons in nucleus
atomic radius decreases
electron have same shielding

Question 25

down a group the IE decreases and when moving into a new period because..

Answer 25

atomic radius increases
more shielding
less attraction between nucleus and electron to be removed