Periodicity + Period 3

Question 1

What elements are s block elements?

Answer 1

Groups 1 and 2 (up to Ra)

Question 2

What elements are d block elements?

Answer 2

Middle section (Sc column to Zn column)

Question 3

What elements are p block elements?

Answer 3

Groups 3 to 0

Question 4

What happens to atomic radius as you go across period 3?

Answer 4

Decreases - nucleus has more protons so greater attraction + shielding effect stays same

Question 5

What happens to first ionisation energy as you go across period 3?

Answer 5

General trend - Increases
Mg to Al and P to S it decreases

Question 6

Why does 1st I.E. decrease as you go from Mg to Al?

Answer 6

Mg outer electron in 3s shell
Al outer electron in 3p shell
3p higher energy level, less attraction, more shielding, less energy needed to remove

Question 7

Why does 1st I.E. decrease as you go from P to S?

Answer 7

Both have outer electrons in 3p shell
In one of sulfur’s 3p subshells, there is an electron pair, that repel each other, making it easier to remove

Question 8

What type of bonding do Na to Al have and how does it change as you go across?

Answer 8

Metallic bonding - Increases as number of delocalised electrons increases, so greater attraction between metal ions and delocalised electrons

Question 9

What type of bonding does Si have?

Answer 9

Covalent - Giant covalent structure, many covalent bonds, very strong and hard to overcome

Question 10

What type of bonding do P to Cl have and how does it change?

Answer 10

Covalent - simple molecular
Weak VdW forces, however order of strength is S8, P4, Cl2 (bigger the molecule greater the VdW)

Question 11

What type of bonding does Ar have?

Answer 11

weak VdW - monatomic molecule, gas at room temp