Statement 1 : Boron always forms covalent bond Statement 2 : The small size of B3+ favors for the formation of covalent bond.

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Statement 1 : Boron always forms covalent bond

Statement 2 : The small size of $B^{3 +}$ favors for the formation of covalent bond.

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Statement 1 is true and Statement 2 is true. Statement 2 is a correct explanation for the statement 1

Statement 1 is true and Statement 2 is false

Statement 1 is false and Statement 2 is true

Statement 1 is true and Statement 2 is true. Statement 2 is not the correct explanation for statement 1

answer is A.

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Detailed Solution

Boron is the first element of the group-13 and has the smallest size.
Ionization energy is the energy required for the removal of a valence electron from an isolated gaseous atom.
Formation of B³⁺ from boron required very high ionization energy.
Therefore, boron is more susceptible to form covalent bond than ionic bond.
Furthermore, size of B³⁺ is extremely small and a high charge density.
Considering Fajan's rule, boron has the maximum covalent character in the bond.

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