Question

The oxidation states of the halogens vary from -1to +7. Identify compounds of chlorine that have$\mathbf{-}\mathbf{1}\mathbf{,}\mathbf{+}\mathbf{1}\mathbf{,}\mathbf{+}\mathbf{3}\mathbf{,}\mathbf{+}\mathbf{5}$ and$\mathbf{+}\mathbf{7}$oxidation states. How does the oxyacid strength of the halogens vary as the number of oxygens in the formula increases?

Short answer

With the number of oxygen atoms, the strength of oxyacids also increases.

Examples of halogen compounds with their oxidation state are:

$\mathrm{HCl},\mathrm{Cl},{\mathrm{HClO}}_2,{\mathrm{HClO}}_3,\mathrm{and}{\mathrm{HClO}}_4.$

Step-by-step solution

Define Elements

The oxidation number is the hypothetical charge of an atom if all of its bonds to different atoms are fully ionic.

Observe how does the oxyacid strength of the halogens as the number of oxygens in the formula increases?

The oxidation states of the halogens vary from -1 to +7.

Halogens generally form four series of oxoacids.

Which are namely hypohalous acids (+1 oxidation state), halous acids (+3 oxidation state), halic acids (+5 oxidation state), and perhalic acids (+7 oxidation state).

In the oxyacid, as the number of oxygen atoms increases, it is due to the high electronegativity of oxygen; it pulls the electron density and makes the acid more acidic.

Here are examples of halogen compounds with oxidation states from -1 to +7 are shown below:

$\mathrm{HCl}$(-1 oxidation state)

$\mathrm{HOCl}$(+1 oxidation state)

role="math" localid="1663829114260" ${\mathrm{HClO}}_2$(+3 oxidation state)

${\mathrm{HClO}}_3$(+5 oxidation state)

${\mathrm{HClO}}_4$(+7 oxidation state)

Therefore,the number of oxygen atoms and the strength of oxyacids also increase.

Examples of halogen compounds with their oxidation state are:

role="math" localid="1663829210418" $\mathrm{HCl},\mathrm{Cl},{\mathrm{HClO}}_2,{\mathrm{HClO}}_3,\mathrm{and}{\mathrm{HClO}}_4$