peridocity

Question 1

how are elements arranged in the periodic table

Answer 1

via proton number

Question 2

what do elements in the same period have

Answer 2

same number of electron shells

Question 3

what are the different blocks on the periodic table

Answer 3

s,p,d,f

Question 4

what happens to atomic radius across period 3

Answer 4

decreases

Question 5

what happens to nuclear charge across period 3

Answer 5

increases as there are more protons

Question 6

what happens to melting points in group 3 in the first 3 elements

Answer 6

first three elements (Na, Mg, Al increase due to metallic bonding which causes an increase +ve charge, and increased delocalised electrons and smaller ionic radius. Stronger metallic bonding

Question 7

what happens to the melting point of silicon

Answer 7

increased a lot. giant covalent structures so lots of energy required to overcome these strong bonds

Question 8

what happens to the last 4 elements melting points in period 3

Answer 8

p4 decreases- simple molecular structure weak VDW
s increases slightly - bigger molecular structure, more VDW
cl2 decreases - simple molecular, weaker VDW
argon decreases- individual atom, weak Vdw

Question 9

define ionisation

Answer 9

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

Question 10

how does shielding effect ionisation energy

Answer 10

the more shielding there is the lower the ionisation

Question 11

how does atomic size affect ionisation

Answer 11

the larger the atomic size the lower ionisation energy

Question 12

how does nuclear charge affect ionisation?

Answer 12

The higher the nuclear charge the higher ionisation energy

Question 13

define successive ionisation

Answer 13

the removal of more than 1 electron from the same atom

Question 14

what happens to ionisation energy down a group

Answer 14

• decreases due to atomic radias increases so outer electrong furthur so weaker attractive force
• shielding increases