Ionisation Energy

Question 1

What is ionisation energy

Answer 1

How easily an atom looses electrons tp form positive ion is

Question 2

1st ionisation energy

Answer 2

The energy required to remove 1 electron from each atom, is 1 mole of gaseous atoms of an element to form 1 mole of gaseou 1+ ions

Question 3

Is removing an electron from an atom/ ion EXO or ENDO ther mic

Answer 3

ENDOTHERMIC

Question 4

2nd ionisation energy

Answer 4

The differnence between 1+ and 2+

The energy required to remove one electron from each ion is 1 mole fo gaseous 1+ ions of an element to form 1 mole gaseous 2+ ions

Question 5

Write the 1st and 2nd ionisation energy equations for al

Answer 5

1. Al(g) — al+ (g) + e-

2. Al+(g)— al2+(g) + e-

Question 6

Why are successive ionisation energies larger

Answer 6

The 2nd ionisation energy of an element is ALWAYS bigger than the 1st ionisation
Due to the ion formed- smaller than the atom
The proton to the electron ratio in the 2+ ion is greater than in the 1+ ion - so the attraction between nucleus adn electron is stronger

Question 7

What a re the factors that effect ionisation. Energy

Answer 7

Nuclear charge
Electron shielding
Atomic radius

Question 8

Nuclear charge - factors effecting ionisation energy

Answer 8

The more protons there are in the nucleus, the stronger the attraction between nucleus and electrons

Question 9

Electron shielding

Answer 9

Inner shel electrons repel outer shell electrons

- repulsion reduces attraction between the nucleus and outer electons - SHIELDING AFFECT

Question 10

Atomic radius

Answer 10

Greatest effect

Greater distance between the nucleus and outer electons - less nuclear attraction

Question 11

Trend in ionisation energy down a group

Answer 11

Atomic radius increases
More inner shells so shielding increases
Nuclear attack on on outer electron decreases
1st ionisation energy decrease

Question 12

Trend across a period

Answer 12

Nuclear charge increases( no. Of protons) 
Same no. Of shells- shielding the same 
Nuclear attraction increases 
Atomic radius decreases
First ionisation energy increases

Question 13

Subs hell structure - affect on ionisation energy

Answer 13

Drop between group 2 and 3
- the 2p subs hell has a higher energy than the 2s subs hell, so the 2p elecron is EASIER to remove- atom will have a lower 1st ionisation energy than 1 with its electron in its 2s sub sell

• the electron is further away in HGIHER energy level
• p has additional shielding

Question 14

Pairing

Answer 14

Between group 5 and 6

Having electrons PAIRED in an orbital - easier to remove tha as there’s repulsion between the 2 electrons, spin paired = easier to remove

Question 15

What are the 5 trends in ionisation energy

Answer 15

High ionisation energy of noblel gases- full outer shell
General increase across each period
Drop in ionisation energy between group 2 and 13( subs hell structure)
Drop in ionisation energy between group5 and 16( pairing)
Sharp decrease in 1st ionisation energy between end of 1 period and start of the next

Question 16

Describe metallic bonding

Answer 16

The electrons in the outermost she’ll of the atom are DELOCALSED

Metal cation electrostatically attracted to the delocalised electrons, form a lattice of closely packed cations in a sea of DELOCALSED electrons

Question 17

Features of a giant metallic lattice

Answer 17

The more delocalised electrons- the higher the melting and boiling not point ( mg 2+ has 2 electrons per atom so has a HGIHER melting poitn than na+)

Size of the metal io and lattice structure - smaller ionic radius will hold delocalise electrons closer to the nucleus

No bonds holding specific ions together- metal ions can slide past each other when the structure is pulled- a malleable and ductile

Question 18

Ductile meaning

Answer 18

Can be pulled into a wire

Question 19

MALLEALE MEANING

Answer 19

Can be hammered into sheets

Question 20

Are metals insoluble or soluble

Answer 20

Insoluble due to strength of metallic bonds

Question 21

Trend in MP and BP across period ( 1-13) metals

Answer 21

Ionic charge increases and size decereases
Number of outer shell electrons increases
Attraction increases - mp + BP increases

Question 22

Giant COVALENTLY structures - properties

Answer 22

High melting and boiling points- strong covalent bonds

Solubility-insoluble as covalent bonds can’t be broke by interactions with solvent s

Electrical conductivity - 2 exceptions of graphite and graphene( only use 3 of carbons outer electrons- delocalised)

Question 23

BP AND MP across the periodic table

Answer 23

MELTING poitn increases for group 1-14( metallic bonds get stronger, ionic radius decreases number of delocalised electrons increases)

High melting points of group 14 ( carbon and silicon )

Low melting points of group 15-18(week London dispersion forces)