ELECTRON CONFIGURATION AND IONISATION

Question 1

The sub shells in order of increasing energy up to 4p

Answer 1

1s 2s 2p 3s 3p 3d 4s 4p

Question 2

How many electrons does each subshell contain when full

Answer 2

s - 2
p - 6
d - 10
f - 14

Question 3

how are chromium and copper behaved differently

Answer 3

they donate one of their 4s electrons to the 3d sub-shell because they are much happier with a more stable full or half full d sub shell
Cr (24e) - 1s2 2s2 2p6 3s2 3p6 3d5 4s1
Cu (29e) - 1s2 2s2 2p6 3s2 3p6 3d10 4s1

Question 4

What happens to transition metals when they turn into ions

Answer 4

they lose their 4s electrons before 3d electrons

Question 5

What is ionisation energy

Answer 5

minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms in the gaseous state.

Question 6

What process is ionisation energy

Answer 6

endothermic as it always requires energy and has a + value

Question 7

3 factors that affect ionisation energy

Answer 7

shielding
atomic size
nuclear charge

Question 8

what is shielding

Answer 8

the more electron shells between the + nucleus and negative electron that is being removed the less energy is required .there is a weaker attraction

Question 9

what is nuclear charge

Answer 9

the more protons in the nucleus the bigger the attraction between the nucleus and outer electrons . this means more energy is required to remove the electron

Question 10

what is atomic size

Answer 10

the bigger the atom the further away the outer electrons are from the nucleus . the attractive force between nucleus and outer electron reduces - easier to remove electrons

Question 11

what is successive ionisation

Answer 11

the removal of more than 1 electron from the same atom

Question 12

formula for 1st 2nd and 3rd ionizing energy

Answer 12

Na (g) - Na+ (g) + e-
Na+ (g) - Na2+(g) + e-
Na2+ (g) - Na3+(g) + e-

Question 13

From the 1st to 2nd ionization energy there is a jump in energy why

Answer 13

we are removing electrons from shell closest to the nucleus.

Question 14

1st ionisation trends in groups

Answer 14

ionisation decrease as we go down a group

• the atomic radius increases as we go down the group outer electrons further from the nucleus. attractive force is weaker. Energy required to remove an electron decrease
• shielding increases as we go down the group most shells between nucleus and outer shell attractive force is weaker .energy required to remove an electron decrease

Question 15

1st ionisation trends in periods

Answer 15

ionisation increases as we go across a period

• as we go across the period there is an increasing number of protons in the nucleus . This increases the nuclear attraction.
• shielding is similar and distance from nucleus marginally decreases
• more energy is required to remove an outer electron

Question 16

Why is there a decrease in ionisation energy in aluminium

Answer 16

Aluminium is an exception and the outer most electron in aluminium sits at a higher energy sub shell slightly further from the nucleus than the outer electron in Mg

Question 17

why is there a decrease in sulfur

Answer 17

electron repulsion
phosphorus and sulfur both have outer electrons in the 3p orbital so the shielding is the same
removing an electron from sulfur involves taking it from and orbital with 2 electrons in
electrons repel each other so less energy is required to remove an electron from an orbital with 2 in than a one with 1 in like phosphorus