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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?
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Methane is a colourless, 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.
$$C{H}_{4} + 2{O}_{2} \longrightarrow C{O}_{2} + 2{H}_{2}O$$
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.
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