Question

Write equations describing the reactions of$\mathit{S}$ with each of the following:role="math" localid="1663850037443" $\mathit{C}{\mathit{l}}_{\mathbf{2}}\mathbf{,}{\mathit{O}}_{\mathbf{2}}$, and$\mathit{H}\mathit{C}\mathit{l}$

Short answer

The required equation describing the reaction of S with each of them$C{l}_2,O_2$, and$HCl$ is

$$\begin{gathered} Sn\left(s\right)+C{l}_2\left(g\right)\to SnC{l}_2\left(s\right) \\ Sn\left(s\right)+2C{l}_2\left(g\right)\to SnC{l}_4\left(s\right) \end{gathered}$$

$Sn\left(s\right)+O_2\left(g\right)\to Sn{O}_2\left(s\right)$

$Sn\left(s\right)+HCl\left(ag\right)\to SnC{l}_2\left(aq\right)+H_2\left(g\right)$

Step-by-step solution

Definition of oxidation states

The total number of electrons that an atom gains or loses in order to create a chemical connection with another atom is known as the oxidation number, also known as the oxidation state.

Calculate the Amount of Pb

Group 4A elements are oxidised by halogens.

Because Group 4A elements have common oxidation states of +2 and +4, tin can produce +2 and +4 halides. The +2 halides of tin, on the other hand, are more stable.

$$\begin{gathered} Sn\left(s\right)+C{l}_2\left(g\right)\to SnC{l}_2\left(s\right) \\ Sn\left(s\right)+2C{l}_2\left(g\right)\to SnC{l}_4\left(s\right) \end{gathered}$$

The elements of Group 4A are oxidised by the elements$O_2$

Except for $Pb$, which produces a +2 oxide, all Group 4A elements create +4 oxides.

$Sn\left(s\right)+O_2\left(g\right)\to Sn{O}_2\left(s\right)$

From the dissociation of $HCl$, group 4A metals react with $H^{+}$to create hydrogen gas and metal chloride.

$Sn\left(s\right)+HCl\left(ag\right)\to SnC{l}_2\left(aq\right)+H_2\left(g\right)$