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A molecule of ammonia $(N{H_3})$ has:
A. Only single bonds
B. Only double bonds
C. Only triple bonds
D. Two double bonds and one single bond

Last updated date: 20th Jun 2024
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Hint: Ammonia molecule has \[A{B_3}\] molecular geometry with a lone pair in which the three hydrogen atoms and an unshared pair of electrons are attached to the central nitrogen atom.

Complete step-by-step solution:
Ammonia is a colourless gas, consisting of hydrogen and nitrogen. It has a pungent smell and it is dangerous in its concentrated form. It behaves as a weak base as it forms salts with many acids. Ammonia is also called azane or nitrogen trihydride. It is a polar molecule due to the presence of lone pairs and readily forms hydrogen bonds.
Ammonia is a covalent atom because of the overlap of orbitals of three hydrogen atoms and three \[s{p^3}\] hybrid orbitals of nitrogen in the structure. The fourth \[s{p^3}\] hybrid orbital is denoted by a lone pair. The lone pair exerts an extra repulsion on the three-bonding hydrogen atoms and creates a slight compression to a ${107.3^\circ }$ bond angle. The H-N-H bond angle is ${107.3^\circ }$ , which results in bond pair-lone pair repulsions that push the N-H bonds inward.

Such a molecule tends to have a trigonal pyramidal molecular geometry because the lone pair although invisible when looking at structure yet exert its influence. Therefore, it has three single bonds and a lone pair.

Hence, the correct option is (A).

Note: The nitrogen has five valence electrons and gets three more electrons from three hydrogen atoms to complete its octet. It leaves a lone electron pair on nitrogen that is not bonded to any other atom and freely available for binding. This might also resemble tetrahedral geometry, having a somewhat similar bond angle of ${109^\circ }$.