Assertion (A): [B(OH_2)_6]^{3+} and [B(OH)_4] | vedclass

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(D) The assertion is false because boron has a small atomic size and lacks $d$-orbitals in its valence shell,which prevents it from expanding its coor

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$A$ is false but $R$ is true

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(D) The assertion is false because boron has a small atomic size and lacks $d$-orbitals in its valence shell,which prevents it from expanding its coordination number beyond $4$. Therefore,the formation of an octahedral $[B(OH_2)_6]^{3+}$ complex is impossible.However,the reason is true because boron is electron-deficient ($sextet$ of electrons) and acts as a Lewis acid,reacting with Lewis bases like $OH^{-}$ to form the stable tetrahedral $[B(OH)_4]^{-}$ ion.Thus,$A$ is false but $R$ is true.

Assertion $(A)$: $[B(OH_2)_6]^{3+}$ and $[B(OH)_4]^{-}$ form octahedral and tetrahedral structures.
Reason $(R)$: Being electron deficient,boron readily reacts with Lewis bases like $H_2O$ and $OH^{-}$.
The correct option among the following is

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Assertion $(A)$: $[B(OH_2)_6]^{3+}$ and $[B(OH)_4]^{-}$ form octahedral and tetrahedral structures.Reason $(R)$: Being electron deficient,boron readily reacts with Lewis bases like $H_2O$ and $OH^{-}$.The correct option among the following is