Which reagent acts as the best electrophile?

Bromine cation,

B r^{+}

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Tribromide,

B r_{3}^{-}

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Bromide,

B r^{-}

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Bromine radical,

B r^{\cdot}

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Solution

The correct option is A Bromine cation, $B r^{+}$
$\begin{matrix} Electrophile is a chemical species deficient of electrons. So, as to bond with nucleophile B r^{+} is a electrophile. \end{matrix}$

$\begin{matrix} {B r_{3}}^{-}, B r^{-}, are nucleophiles. where as B r is neither electrophile nor nucleophile. In simple words electrophile is an electron loving species. \end{matrix}$

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Similar questions

2 M n O_{4}^{-} + B r^{-} + H_{2} O \to 2 M n O_{2} + B r O_{3}^{-} + 2 O H^{-}

- 1

{B r O_{3}}^{-} (a q .) + 5 {B r}^{-} (a q .) + 6 H^{+} (a q .) ⟶ 3 {B r}_{2} (l) + 3 H_{2} O (l)

({B r}_{2})

B r O_{3 (a q)}^{-} + 5 B r_{(a q)}^{-} + 6 H_{(a q)}^{+} \to 3 B r_{2 (l)} + 3 H_{2} O_{(l)}

In the following reaction, how is the rate of appearance of the product Bromine related to the rate of disappearance of the reactant Bromide?

$B r O_{3 (a q)}^{⊝} + 5 B r_{(a q)}^{⊝} + 6 H_{(a q)}^{\oplus} \to 3 B r_{2 (l)} + 3 H_{2} O_{(l)}$

B r O_{4}^{-}

1.82 V - -- \to

B r O_{3}^{-} 1.50 V - -- \to

H B r O 1.595 V - --- \to

B r_{2} 1.06552 - --- \to B r^{-}

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