Question

In \[sp\]hybridization, shape is
(a) Angular
(b) Tetrahedral
(c) Bipyramidal
(d) Linear
(e) None of these

Answer 1

Hint: The acetylene molecule (\[C{H_3} - C \equiv C - C{H_3}\]) is the best example of\[sp\]hybridization. Because of \[sp\]hybridization the acetylene molecule has a linear structure with a bond angle \[180^\circ \].

Complete step by step solution:The intermixing of atomic orbital (\[s,p,\]and \[d\]orbitals) of compatible energies are called hybrid orbitals and this phenomenon is known as hybridization.
Both half-and full-filled orbitals can be involved in the process of hybridization.
The hybridized molecule possesses a different shape, sizes, and energy from the unhybridized orbitals.
During the hybridization, the orbitals overlap in the proper orientation.
By employing the concept of hybridization, we can easily predict the geometry of the molecules.
The concept of hybridization can be understood by taking the example of the carbon atom. The carbon atom can form four single bonds using a valence shell \[s\] orbital and three \[p\] orbitals. The mixing of a \[s\] orbital and three \[p\] orbitals produced four \[s{p^3}\]orbital of equal energy. These four \[s{p^3}\]orbitals have tetrahedral arrangements around the carbon atom and have the tendency to form four bonds with other atoms.
Based on the intermixing hybridization can be divided into the following ways:
(1) \[s{p^{}}\]hybridization: Formed when one \[s\]and one\[p\]orbital are involved in hybridization. The \[s{p^{}}\]hybridization has 50% \[s\]and 50%\[p\]character with linear geometry. For example., the acetylene molecule.
(2) \[s{p^2}\]hybridization: Formed when one \[s\]and two\[p\]orbital are involved in hybridization. The \[s{p^2}\]hybridization has 33.33% \[s\]and 66.66%\[p\]character with trigonal planar geometry. For example., \[B{H_3}\] molecule.
(3) \[s{p^3}\]hybridization: Formed when one \[s\]and three\[p\]orbital are involved in hybridization. The \[s{p^3}\]hybridization has 25% \[s\]and 75%\[p\]character with tetrahedral geometry. For example., \[C{H_4}\] molecule.
(4) \[s{p^3}d\]hybridization: Formed when one \[s\], three\[p\]and one \[d\] orbital are involved in hybridization. The \[s{p^3}d\]hybridization has trigonal bipyramidal geometry. For example., \[PC{l_5}\] molecule.
(5) \[s{p^3}{d^2}\]hybridization: Formed when one \[s\], three\[p\]and one \[d\] orbital are involved in hybridization. The \[s{p^3}{d^2}\]hybridization has octahedral geometry. For example., sulfur hexafluoride.
Therefore from the above explanation we can say option (d) will be the correct option:

Note: In contrast to hybridization, the VSEPR helps us to determine the shape of the molecule on the bases of lone pair and bond pair interaction. For example., an ammonia molecule has a pyramidal shape due to lone pair and bond pair repulsion.