periodicity

Question 1

what is the first ionisation energy?

Answer 1

energy required to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

Question 2

what are the factors affecting ionisation energy?

Answer 2

1) atomic radius
2) nuclear charge
3) electron shielding

Question 3

what are the trends in first ionisation energy across each periods?

Answer 3

Increase in first ionisation energy across each period ( H-He, Li-Ne, Na-Ar)
A decrease in first ionisation energy between the end of one period and start of next period( He - Li)

Question 4

What is the trend in first ionisation energy down a group?

Answer 4

first ionisation energy decrease down a group as there are increased shielding and increased atomic radius

Question 5

what is the trend in first ionisation energy across period 2?

Answer 5

a rise from lithium to beryllium,
a fall to boron as electron is 2p sub shell is easier to remove than 2s subshell in beryllium
rise to carbon and nitrogen
fall to oxygen as the paired electrons in 2p orbitals repel on another decreasing ionisation energy

Question 6

properties of metals

Answer 6

strong metallic bond, high electrical conductivity, high mp and bp point

Question 7

what non-metals form giant covalent lattice?

Answer 7

boron,carbon,silicon

Question 8

properties of giant covalent structures?

Answer 8

high mp/bp points
insoluble
non-conductors of electricity except graphene and graphite

Question 9

what is the trend in period 2 melting points?

Answer 9

melting point increases from Li to Carbon and large decrease between Nitrogen and Neon due to change from giant to simple molecular structures with london forces

Question 10

what is the trend in melting points in period 3 ?

Answer 10

Increase from Na to Si but slow increase from Mg to AI
Decrease from Si to Ar due to change from giant structure to simple molecular structure