Question

(i) Explain why carbon forms strong bonds with other elements.
(ii) Why do covalent compounds have low melting and boiling points?
(iii) Draw electron dot structure of chlorine (atomic number 17).

Hint:

Carbon’s tetravalency makes it bond-rich and stable. Covalent compounds melt easily due to weak molecular forces, not ionic bonds.

Answer 1

(i) Carbon bonding explanation: Carbon has a small atomic radius and 4 valence electrons.
It can form strong covalent bonds with many elements like hydrogen, oxygen, nitrogen, chlorine, etc.
The covalent bonds are very stable due to high bond energy and ability to form single, double, and triple bonds.
(ii) Low melting and boiling points of covalent compounds:
Covalent compounds do not form ions.
Molecules are held by weak Van der Waals forces or London dispersion forces.
Less energy is required to break these weak intermolecular attractions.
(iii) Electron dot structure of Cl$_2$: \[ \text{Each chlorine atom has 7 valence electrons:} \text{Cl} \cdot \cdot \cdot \cdot \cdot \cdot \cdot \] \[ \text{They share 1 pair of electrons to form a covalent bond:} \boxed{\text{Cl} : \text{Cl}} \]