Question

If the letter ‘R’ was used to represent any of the elements in the group, then the hydride and oxide of carbon would respectively be represented as ?

• A. ${\mathrm{RH}}_4,\mathrm{RO}$
• B. ${\mathrm{RH}}_4,{\mathrm{RO}}_2$
• C. ${\mathrm{RH}}_2,{\mathrm{RO}}_2$
• D. ${\mathrm{RH}}_2,\mathrm{RO}$

Answer 1

The correct option is B

${\mathrm{RH}}_4,{\mathrm{RO}}_2$

The explanation for the correct Option:

Option (B): ${\mathrm{RH}}_4,{\mathrm{RO}}_2$

• The group R is representing carbon i.e. $14\mathrm{th}$ group elements.
• The hydrides from this group would be represented as ${\mathrm{RH}}_4$.
• This is because the elements belonging to the $14\mathrm{th}$ group will have valence electron$=4$ i.e. valency is also equal to $4$ and the valency of hydrogen is $1$ so the formula of hydride is${\mathrm{RH}}_4$. $\mathrm{R}+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{RH}}_4$
• Also, the oxides from this group would be represented as ${\mathrm{RO}}_2$.
• This is because the valency of the element R is $4$ and the valency of oxygen is $2$ so the oxide form is${\mathrm{RO}}_2$. $\mathrm{R}+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{RO}}_2$

The explanation for the incorrect options:

Option (A): ${\mathrm{RH}}_4,\mathrm{RO}$

• The group R is representing carbon i.e. $14\mathrm{th}$ group elements.
• The oxides from this group would be represented as${\mathrm{RO}}_2$. This is because the valency of the element R is $4$ and the valency of oxygen is $2$ so, the oxide form is${\mathrm{RO}}_2$. $\mathrm{R}+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{RO}}_2$
• Hence, it is an incorrect option.

Option (C): ${\mathrm{RH}}_2,{\mathrm{RO}}_2$

• Hydrogen interacts with non-metals to generate compounds, which are also known as hydrides.
• The group $14\mathrm{th}$ elements have valence electron, so valency is also equal to $4$ and hydrogen has a valency of $1$ so the formula for hydride are${\mathrm{RH}}_4$. $\mathrm{R}+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{RH}}_4$
• Hence, it is an incorrect option.

Option (D): ${\mathrm{RH}}_2,\mathrm{RO}$

• Hydrogen interacts with non-metals to generate compounds, which are also known as hydrides.
• The group $14\mathrm{th}$ elements have valence electron$=4$, so valency is also equal to $4$ and hydrogen has a valency of $1$ so the formula for hydride are${\mathrm{RH}}_4$. $\mathrm{R}+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{RH}}_4$
• Hence, it is an incorrect option.

Hence, then the hydride and oxide of carbon would respectively be represented as ${\mathrm{RH}}_4$and${\mathrm{RO}}_2$.