Which of the following species acts as the st | vedclass

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(C) An oxidising agent is a species that gains electrons and gets reduced. The strength of an oxidising agent is determined by its standard reduction

Vedclass · Accepted Answer

$F_2$

Vedclass · Answer

(C) An oxidising agent is a species that gains electrons and gets reduced. The strength of an oxidising agent is determined by its standard reduction potential $(E^{\circ}_{red})$. Higher positive values of $E^{\circ}_{red}$ indicate a stronger tendency to gain electrons,making the species a stronger oxidising agent.Among the given options:$1$. $Li$ is a strong reducing agent (it loses electrons easily).$2$. $Li^{+}$ has a very negative reduction potential and is a very weak oxidising agent.$3$. $F_2$ has the highest standard reduction potential $(+2.87 \ V)$,making it the strongest oxidising agent among the options.$4$. $F^{-}$ is the reduced form of fluorine and cannot be further reduced,so it acts as a reducing agent.Therefore,$F_2$ is the strongest oxidising agent.

Which of the following species acts as the strongest oxidising agent?

Similar Questions

Why does the following reaction occur?
$XeO_6^{4-}{(aq)} + 2F^{-}{(aq)} + 6H^{+}{(aq)} \rightarrow XeO_{3_{(g)}} + F_{2_{(g)}} + 3H_2O_{(l)}$
What conclusion about the compound $Na_4XeO_6$ (of which $XeO_6^{4-}$ is a part) can be drawn from the reaction?

An oxidising agent is a substance,which

$(A) \ HOCl + H_2O_2 \rightarrow H_3O^{+} + Cl^{-} + O_2$
$(B) \ I_2 + H_2O_2 + 2 OH^{-} \rightarrow 2 I^{-} + 2 H_2O + O_2$
Choose the correct option.

Which of the following is not a reducing agent?

Which acts as an oxidising agent in the following reaction?
$2H_2O_{(l)} + 2Na_{(s)} \to 2NaOH_{(aq)} + H_{2_{(g)}}$

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