Q.Write a balanced equation for the laboratory preparation of diborane from boron trifluoride and lithium hydride, and state one characteristic chemical property of diborane (its behaviour towards air and water).

[!TLDR] Diborane is prepared from boron trifluoride and lithium hydride, and is spontaneously flammable in air besides reacting readily with water. [!ANSWER] $2\text{BF}_3 + 6\text{LiH} \rightarrow \text{B}_2\text{H}_6 + 6\text{LiF}$; diborane is spontaneously flammabl …

A standard laboratory route to diborane uses lithium hydride as the hydride source, reacting it with boron trifluoride:\n$2\text{BF}_3 + 6\text{LiH} \longrightarrow \text{B}_2\text{H}_6 + 6\text{LiF}$\nHere each boron is reduced from the $+3$ oxidation state it holds in $\text{BF}_3$ down to a formal, average oxidation state within diborane, with fluoride displaced as lithium fluoride and hydride delivered to build up the B-H framework described in the previous answer. Diborane's most striking chemical property, a direct consequence of its electron-deficient, reactive structure, is that it is spontaneously flammable (pyrophoric) in air, igniting on contact with atmospheric oxygen and burning with a very hot flame; it is likewise rapidly and exothermically hydrolysed on contact with water, decomposing completely to boric acid and hydrogen gas:\n$\text{B}_2\text{H}_6 + 6\text{H}_2\text{O} \longrightarrow 2\text{B(OH)}_3 + 6\text{H}_2$\nBoth reactions reflect diborane's high reactivity as an electro …

Write the balanced BF3/LiH preparation equation, then state diborane's reactivity towards air (pyrophoric) a …

Leaving the preparation equation unbalanced (forgetting the 6 LiH/6 LiF stoichiometry); omitt …