Question

What are the types of bonds present in $N{H_4}Cl$
A. Electrovalent, covalent and coordinate.
B. Only covalent
C. Only ionic
D. Covalent and coordinate.

Answer 1

Nitrogen has three unpaired electrons and one lone pair around it. Hence nitrogen can form only three covalent bonds. Find out the charge and electrons left in nitrogen after forming three covalent bonds with three Hydrogens.

Complete answer:
In $N{H_4}Cl$ , Nitrogen is the central atom and its valency is three and has one lone pair. If we consider that the three valence electrons form three bonds with Hydrogen atoms to form $N{H_3}$ , then those bonds would be Covalent in nature.
Now, we have one remaining lone pair which can easily be donated to one hydrogen atom forming a dative/coordinate covalent bond. Now, when this bond is formed nitrogen is losing its electrons bringing a positive charge on it forming $N{H_4}^ +$
Here, we have an $N{H_4}^ +$ ion and this ion can form a bond with $C{l^ - }$ ion to form $N{H_4}Cl$ molecule. Since both $N{H_4}^ +$ and $C{l^ - }$ are ions forming a bond, the bond would be ionic or electrovalent in nature.
Therefore the molecule $N{H_4}Cl$ contains covalent, coordinate and electrovalent bonds.

Additional information: An ionic bond is formed when two atoms/molecules with opposite charge are attracted to each other. A covalent bond is formed when both the atoms/molecules contribute one electron to form a bond. Coordinate covalent bond is formed when one atom/molecule donates its lone pair to the other atom/molecule.

So, the correct option is (A)

Note: In the given molecule, one ionic bond is formed between $N{H_4}^ +$ and $C{l^ - }$ ions, one coordinate bond is formed between Nitrogen and one Hydrogen atom and three covalent bonds are formed between Nitrogen and three Hydrogen atoms.