Question

Which of the following elements is the most electropositive?

• A. $\mathrm{Li}$
• B. $\mathrm{Be}$
• C. $\mathrm{B}$
• D. $\mathrm{C}$

Answer 1

The correct option is A

$\mathrm{Li}$

The explanation for the correct option: (a)

1. The term electropositivity denotes the tendency to donate electrons to form positive ions and it increases down the group and decreases across a period.
2. As we move from left to right along a period the tendency to lose electrons decreases and hence the electropositive character decreases.
3. Now, Lithium ($\mathrm{Li}$) belongs to Group 1 and period 2, Beryllium ($\mathrm{Be}$) belongs to Group 2 and period 2, Boron ($\mathrm{B}$) belongs to Group 13 and period 2, and Carbon ($\mathrm{C}$) belongs to Group 14 and period 2
4. Among the given elements, $\mathrm{Li}$ is found to be the most electropositive element as it is located on the extreme left of the periodic table.

The explanation for the incorrect options:

b) Among the given elements, $\mathrm{Be}$ is not the most electropositive element as it is right to $\mathrm{Li}$.

c) $\mathrm{B}$ is located on the right side of the periodic table and hence it is less electropositive than $\mathrm{Li}$.

d) $\mathrm{C}$ is a non-metal, thus it is an electronegative element.

Hence option (a) is correct and the most electropositive element is $\mathrm{Li}$.