atomic structure

Question 1

atomic radius across period

Answer 1

-increase in no. of protons
- shielding effect remains relatively constant
-increase in effective nuclear charge
- greater nuclear attraction on the valence electrons
atomic radii decrease

Question 2

atomic radius down the group

Answer 2

-increase in number of principal quantum shells
-valence electrons further away from nucleus
-increase in shielding effect outweighs increase in nuclear charge
-decreased nuclear attractions
-atomic radius increases

Question 3

IE across the period

Answer 3

-increase in no. of protons
-shielding effect remains relatively constant
-increase in effective nuclear charge
-greater nuclear attraction on valence electrons
- more energy required to remove valence electron
- IE increases

Question 4

IE down the group

Answer 4

-increase in principal quantum shells
-valence electrons further away from nucleus
-increase in shielding effect outweighs increase in nuclear charge
-decreased nuclear attractions
-less energy required to remove valence electron
-IE decreases down the group

Question 5

successive IE of an element gradually increase

Answer 5

• more difficult to remove from a negative electron from increasingly positively charged ion
  -electron-electron repulsion decreases, ionic radius decrease
  -valence electrons closer to nucleus
  -more energy required to remove successive electrons

Question 6

large jump from 1st IE to 2nd IE

Answer 6

2nd electron removed from an inner quantum shell closer to the nucleus. element has 2 valence electrons and is from group 2