Question

Write balanced equations describing the reaction of lithium metal with each of the following: ${\mathit{o}}_{\mathbf{2}}$, ${\mathit{s}}_{\mathbf{8}}$, $\mathit{C}{\mathit{l}}_{\mathbf{2}}$, ${\mathit{P}}_{\mathbf{4}}$,${\mathit{H}}_{\mathbf{2}}$, ${\mathit{H}}_{\mathbf{2}}\mathit{O}$ and Hcl.

Short answer

The balance reaction of lithium metal is $4{\text{Li}}_{\left(s\right)}+{\text{O}}_{2\left(g\right)}\to 2{\text{Li}}_2{\text{O}}_{\left(s\right)}$ $16{\text{Li}}_{\left(s\right)}+{\text{S}}_{8\left(s\right)}\to 8{\text{Li}}_2{\text{S}}_{\left(s\right)}$ $2{\text{Li}}_{\left(s\right)}+{\text{Cl}}_{2\left(g\right)}\to 2{\text{LiCl}}_{\left(s\right)}$

$12{\text{Li}}_{\left(s\right)}+{\text{P}}_{4\left(s\right)}\to 4{\text{Li}}_3{\text{P}}_{\left(s\right)}$

$2{\text{Li}}_{\left(s\right)}+{\text{H}}_{2\left(g\right)}\to 2{\text{LiH}}_{\left(s\right)}$

$2{\text{Li}}_{\left(s\right)}+2{\text{H}}_{2\left(g\right)}{\text{O}}_{\left(l\right)}\to 2{\text{LiOH}}_{\left(aq\right)}+{\text{H}}_{2\left(g\right)}$

$2{\text{Li}}_{\left(s\right)}+2{\text{HCl}}_{\left(aq\right)}\to 2{\text{LiCl}}_{\left(aq\right)}+{\text{H}}_{2\left(g\right)}$

Step-by-step solution

Definition of lithium metal

Although its activities are unknown, trace levels of lithium are found in biological systems. Lithium salts have shown promise in the treatment of mental diseases including bipolar disorder as an antidepressant and mood stabilizer. Electrolysis is used to separate lithium metal from a solution of lithium chloride and potassium chloride.

Alkali metals

The alkali metals reduce oxygen, but the product depends on the metal.

Lithium forms the oxide, $L{i}_{2}O$

$4\text{Li}\left(s\right)+{\text{O}}_2\left(g\right)\to 2{\text{Li}}_2\text{O}\left(s\right)$

The alkali metals react with elemental sulfur to produce sulfides

$16\text{Li}\left(s\right)+{\text{S}}_8\left(s\right)\to 8{\text{Li}}_2\text{S}\left(s\right)$

Ionic halides

The alkali metals reduce halogens to form ionic halides.

$2\text{Li}\left(s\right)+{\text{Cl}}_2\left(g\right)\to 2\text{LiCl}\left(s\right)$

The alkali metals react with phosphorus to form phosphides with the general formula .

$12\text{Li}\left(s\right)+{\text{P}}_4\left(s\right)\to 4{\text{Li}}_3\text{P}\left(s\right)$

Hydrides

The alkali metals reduce hydrogen to form ionic hydrides. Therefore, we get the lithium ‘s metal reaction of balanced equation

$2\text{Li}\left(\text{s}\right)+{\text{H}}_2(\text{g})\to 2\text{LiH}\left(\text{s}\right)$

The alkali metals reduce hydrogen in $H_{2}o$from the +1 to the 0 oxidation state

$2\text{Li}\left(s\right)+{\text{H}}_2\text{O}\left(l\right)\to 2\text{LiOH}\left(aq\right)+{\text{H}}_2\text{O}\left(l\right)$

The alkali metals react with H⁺ from the dissociation at Hcl and produce hydrogen gas and the metal chloride

$2\text{Li}\left(s\right)+2\text{HCl}\left(ag\right)\to 2\text{LiCl}\left(aq\right)+{\text{H}}_2\left(g\right)$

Therefore, the lithium ‘s metal balance equations are,

$4{\text{Li}}_{\left(s\right)}+{\text{O}}_{2\left(g\right)}\to 2{\text{Li}}_2{\text{O}}_{\left(s\right)}$

$16{\text{Li}}_{\left(s\right)}+{\text{S}}_{8\left(s\right)}\to 8{\text{Li}}_2{\text{S}}_{\left(s\right)}$

$2{\text{Li}}_{\left(s\right)}+{\text{Cl}}_{2\left(g\right)}\to 2{\text{LiCl}}_{\left(s\right)}$

$12{\text{Li}}_{\left(s\right)}+{\text{P}}_{4\left(s\right)}\to 4{\text{Li}}_3{\text{P}}_{\left(s\right)}$

$2{\text{Li}}_{\left(s\right)}+{\text{H}}_{2\left(g\right)}\to 2{\text{LiH}}_{\left(s\right)}$

$2{\text{Li}}_{\left(s\right)}+2{\text{H}}_{2\left(g\right)}{\text{O}}_{\left(l\right)}\to 2{\text{LiOH}}_{\left(aq\right)}+{\text{H}}_{2\left(g\right)}$

$2{\text{Li}}_{\left(s\right)}+2{\text{HCl}}_{\left(aq\right)}\to 2{\text{LiCl}}_{\left(aq\right)}+{\text{H}}_{2\left(g\right)}$