Question

What is methane? Draw its electron dot structure. Name the type of bonds formed in this compound. Why are such compounds (i) Are poor conductors of electricity and (ii) Have low melting and boiling points? What happens when this compound burns in oxygen?

Answer 1

Methane

• ${\mathrm{CH}}_4$ is the molecular formula of methane.
• Methane is a saturated hydrocarbon.
• It is a colorless and odorless gas.

Electron dot structure

• The electron dot structure of methane is as follows:

Type of bond

• The single carbon atom in the center of the molecule and the four hydrogen atoms are connected by covalent bonds.
• Structure of methane:

Conductivity of methane

• Methane is a poor electrical conductor.
• All of the bonds in methane are covalent.
• Hence the molecule has no free electrons that may aid in electrical conductivity.

Melting and boiling point of methane

• Covalent compounds have low melting and boiling points due to the molecules' low intermolecular forces of attraction.
• Methane has a relatively low melting and boiling point since it is also a covalent compound.

Burning of methane in oxygen

• Methane produces carbon dioxide $\left({\mathrm{CO}}_2\right)$ and water $\left({\mathrm{H}}_2\mathrm{O}\right)$ as a byproduct of burning when it is exposed to oxygen.
• The reaction is as follows:
• ${\mathrm{CH}}_4\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$