Question

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

Answer 1

Answer:

Methane is a colorless, odourless and highly flammable gas which is the main component of natural gas.

Electron dot structure of methane is- (Image attached)

The covalent bonds are present in between four hydrogen atoms and the single carbon atom at the centre of the molecule.

(i) Methane is a poor conductor of electricity because in methane all bonds are covalent bonds and therefore no free electrons are present in the molecule that can help in conducting electricity.

(ii) Covalent compounds have low intermolecular forces of attraction between the molecules and thus show low melting and boiling points. Since methane is also a covalent compound thus methane has very low melting and low boiling point.

When methane is burned in the presence of oxygen, it forms $$C{O}_{2}$$ with water as the product of the reaction.

$$C{H}_{4} + {O}_{2} \longrightarrow C{O}_{2} + {H}_{2}O$$

solution

Answer 2

Methane and its property

Explanation:

• Methane could be a colorless, odorless and extremely ignitable gas that is that the main element of gas.
• The valence bonds are gift in between four atomic number 1 atoms and also the single atom at the centre of the molecule.
• Methane series could be a poor conductor of electricity as a result of in methane series all bonds ar valence bonds and so no free electrons are gift within the molecule which will facilitate in conducting electricity.
• Valence compounds have low unit forces of attraction between the molecules and so show low melting and boiling points. Since methane series is additionally a valence compound so methane series has terribly low melting and low boiling purpose.