JEE Main 2024 — Chemistry Inorganic Chemistry

2024mcqeasy

Given below are two statements :

Statement I : The electronegativity of group $14$ elements from $\mathrm{Si}$ to $\mathrm{Pb}$ gradually decreases.

Statement II : Group $14$ contains non-metallic, metallic, as well as metalloid elements.

In the light of the above statements, choose the most appropriate from the options given below :

Official previous-year question

Held on 29 Jan 2024 · Verified 6 Jul 2026.

Options

A
Statement I is false but Statement II is true
B
Statement I is true but Statement II is false
C
Both Statement I and Statement II are true
D
Both Statement I and Statement II are false

Did you get this right?

Solution

$\mathrm{Gr}-14\mathrm{EN}$

$C2.5$

$\mathrm{Si}1.8$

$\mathrm{Ge}1.8$

$\mathrm{Sn}1.8$

$\mathrm{Pb}1.9$

The electronegativity values for elements from $\mathrm{Si}$ to $\mathrm{Pb}$ are almost same. So Statement I is false.

Among them, Carbon and silicon are non-metals.

Germanium is metalloid in nature

Tin and lead are metal.

Reason for different metallic characteristics

The metallic character increases down the group from carbon to lead as nonmetal to metal.

The metallic character increases because the atomic size increases from Carbon to Lead.

As size increases, the ionization potential decreases down the group.

A decrease in ionization potential lead to an increase in the electropositive character of the element.

Hence, the metallic character increases down the group in group $-14$ as the ionization potential decreases to make it easier to lose an electron and increase the metallic character.

Your note

JEE Main Inorganic Chemistry in other years

Inorganic Chemistry 2026 Inorganic Chemistry 2025 Inorganic Chemistry 2023 Inorganic Chemistry 2022 Inorganic Chemistry 2021 Inorganic Chemistry 2020 Inorganic Chemistry 2019 Inorganic Chemistry 2018 Inorganic Chemistry 2017 Inorganic Chemistry 2016 Inorganic Chemistry 2015 Inorganic Chemistry 2014

Keep practicing Inorganic Chemistry

Work through every JEE Main Inorganic Chemistry PYQ, year by year.

Browse all Chemistry topics

Solution

$\mathrm{Gr}-14\mathrm{EN}$

$C2.5$

$\mathrm{Si}1.8$

$\mathrm{Ge}1.8$

$\mathrm{Sn}1.8$

$\mathrm{Pb}1.9$

The electronegativity values for elements from $\mathrm{Si}$ to $\mathrm{Pb}$ are almost same. So Statement I is false.

Among them, Carbon and silicon are non-metals.

Germanium is metalloid in nature

Tin and lead are metal.

Reason for different metallic characteristics

The metallic character increases down the group from carbon to lead as nonmetal to metal.

The metallic character increases because the atomic size increases from Carbon to Lead.

As size increases, the ionization potential decreases down the group.

A decrease in ionization potential lead to an increase in the electropositive character of the element.

Hence, the metallic character increases down the group in group $-14$ as the ionization potential decreases to make it easier to lose an electron and increase the metallic character.

JEE Main 2024 — Chemistry Inorganic Chemistry

Options

Did you get this right?

Solution

Your note

JEE Main Inorganic Chemistry in other years

More JEE Main Inorganic Chemistry questions

Other Chemistry topics for JEE Main

Physical Chemistry

Organic Chemistry

Keep practicing Inorganic Chemistry

JEE Main 2024 — Chemistry Inorganic Chemistry

Options

Did you get this right?

Solution

Your note

JEE Main Inorganic Chemistry in other years

More JEE Main Inorganic Chemistry questions

Other Chemistry topics for JEE Main

Physical Chemistry

Organic Chemistry

Keep practicing Inorganic Chemistry