Question

Which of the following has covalent radius more than germanium?

• A. Tin
• B. Lead
• C. Phosphorus
• D. Iodine

Answer 1

Answer: (A), (B), (D)

Iodine

Explanation for the correct options:

Atomic size

• Generally on going down the group in a periodic table, atomic size increases.
• Generally, ongoing left to right in a periodic table, atomic size decreases.

(a) Tin

• Covalent radius of germanium is equal to $121\mathrm{pm}$
• Tin has a covalent radius equal to $140\mathrm{pm}$.
• Tin is present in the fifth period and group 14 in the periodic table.
• Germanium is present in the fourth period and group 14 in the periodic table.
• As the covalent radius increases on going down the group.
• So, tin has a covalent radius more than germanium.

(b) Lead

• Covalent radius of germanium is equal to $121\mathrm{pm}$
• Lead has covalent radius equal to $146\mathrm{pm}$
• Lead is present in the sixth period and group 14 in the periodic table.
• So, lead has a covalent radius more than germanium.
• Thus, this option is correct.

(d) Iodine

• Covalent radius of germanium is equal to $121\mathrm{pm}$
• Iodine has a covalent radius equal to $139\mathrm{pm}$
• Iodine is an element of the halogen family.
• It is present in group 17 and fifth period.
• Tin, lead, and iodine are all below compared to germanium in the periodic table. As the covalent radius increases on going down the group.

Explanation for the incorrect options:

(c) Phosphorus

• Covalent radius of germanium is equal to $121\mathrm{pm}$
• Phosphorus has a covalent radius equal to $107\mathrm{pm}$
• Thus, this option is incorrect.

Hence the correct option is (a) Tin (b) Lead and (d) Iodine