Why is BiH3 a good reducing agent?

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Why is BiH3 a good reducing agent?

The nitrogen hydride is more stable and bismuth hydride is least stable. Due to the least stability of bismuth hydride, it is the strongest reducing agent among all the hydrides of group \[15\] elements. Thus, \[Bi{H_3}\] the stronger reducing agent amongst all the hydrides of group \[15\] elements.

Why is BiH3 a strong reducing agent than NH3?

From N to Bi the size of atom increases and tendency to form covalent bonds with H decreases. As a result their tendency to liberate hydrogen increases for hydrides down the group. Hence NH3 is a mild reducing agent while BiH3 is a very strong reducing agent.

What is the oxidation state of Bi in BiH3?

See, the oxidation state of Bi hasn’t changed, in BiH3(+3) and in Bi(OH)3 is also,(+3, but oxidation state of H^- ion is oxidized from -1 in BiH3 to +1 and 0 in Bi(OH)3 and H2, respectively.

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Why is 3 the strongest reducing agent among all the hydrides of group 15 elements?

Doen the group (↓) i.e, from N to Bi, the atomic size increases, hence the bond length A-H increases consequently A-H bond strength decreases and tendency to behave as reducing agent increases i.e., BiH3 is the strongest reducing agent amongst all the hydrides of group 15 elements.

Why is BiH3 least basic?

Since BiH3 is a drago compound, the lone pair it has, is stereochemically inactive and hence cannot be donated. This makes it less basic as compared to NH3 (NH3 can donate its electron ).

Why is BiH3 unstable?

Since,the BiH3 is the least stable (because the size of central atom is greatest & therefore its tendency to form stable covalent bond with small hydrogen atom decreases,as a result the bond strength decreases) in this series,hence the reducing character increases.

Why is bih3 least stable?

Why are the compounds of bismuth more stable in +3 oxidation state?

Bismuth compounds are more stable in +3 oxidation state because ‘Bi’ exhibits +3 stable oxidation state instead of +5 due to inert pair efffect.

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Which among the following is the strongest reducing agent a BiH3 B PH3 C SbH3 and NH3?

NH3 < PH3 < AsH3 < SbH3 < BiH3. therefore BiH3 is the strongest reducing hydride.

How do you know if a compound is oxidizing agent or reducing agent?

Break the reaction down into a net ionic equation and then into half-reactions. The substance that loses electrons is being oxidized and is the reducing agent. The substance that gains electrons is being reduced and is the oxidizing agent.

Why is BiH3 the strongest reducing agent among all hydrides BiH3 not highly stable B HH BiH3 is less stable Hydide group group elements BiH3?

The reducing character of the hydrides of Group 15 elements increases from NH3 to BiH3(Bismuthine) because the reducing character depends upon the stability of the hydride. The greater the unstability of anhydride,the greater is the its reducing character.

Why does BiH3 act as a reducing agent in this reaction?

See, the oxidation state of Bi hasn’t changed, in BiH3 (+3) and in Bi (OH)3 is also, (+3, but oxidation state of H^- ion is oxidized from -1 in BiH3 to +1 and 0 in Bi (OH)3 and H2, respectively. So, BiH3 act as reducing agent in this reaction with water.

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Why is NH3 not a strong reducing agent?

So, NH3 is not strong reducing agent, but it works as reducing agent under severe condition, this is because the NH3 is stable compound dissolve in water, inonized slightly into NH4^+ and OH^- giving alkaline solution, nitrogen in this ionization reaction didn’t change its oxidation state (-3). So, reaction of NH3 with water is acid-base reaction.

Why is the reducing character of anhydride bismuthine?

(Bismuthine) because the reducing character depends upon the stability of the hydride.The greater the unstability of anhydride,the greater is the its reducing character.Since,the BiH

Why does PH3 have a maximum oxidation number of +5?

Since,PH3 has maximum oxidation no. Of +5 which others elements of the same group possess as well but they don’t lose 5 electrons easily,like Sb and Bi (they show +3 oxidation state due to inert pair effect) and nitrogen due to small size also don’t lose 5 electrons easily. So PH3 which has -3 oxidation state can easily increase its O.N. to +5