Q10 E
Question
Give the shape that describes each hybrid orbital set:
(a) \({\rm{s}}{{\rm{p}}^{\rm{2}}}\)
(b) \({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{d}}\)
(c) sp
(d) \({\rm{s}}{{\rm{p}}^{\rm{3}}}{{\rm{d}}^{\rm{2}}}\)
Step-by-Step Solution
Verified(a) The shape is trigonal planar.
(b) The shape is trigonal bipyramidal.
(c) The shape is linear.
(d) The shape is octahedral.
Hybridization: When two or more different pure orbitals with comparable energy are mixed together to produce an equivalent amount of impure orbitals with equal energy and definite geometry, this is referred to as hybrid orbitals, and the phenomenon is referred to as hybridization.
This type of hybridization entails combining one s-orbital and two p-orbitals from the valence shell to form three \({\rm{s}}{{\rm{p}}^{\rm{2}}}\)hybrid orbitals. These hybrid orbitals form a trigonal planar shape when directed towards the corners of an equilateral triangle.
Therefore, it has a trigonal planar shape.
This type of hybridization entails combining one s-orbital, three p-orbitals, and one d-orbital from the valence shell to form the \({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{\;d}}\) hybrid orbital. Three hybrid orbitals are oriented toward the corners of an equilateral triangle, and two are oriented axially. As a result, the shape is trigonometric bipyramidal.
Therefore, trigonal bipyramidal is the shape.
This type of hybridization involves combining one s-orbital and one p-orbital of the valence shell to form a sp hybrid orbital. These hybrid orbitals are oriented in space at a 180-degree angle, forming a linear shape.
Therefore, the form is linear.
The valence shell's one s-orbital, three p-orbitals, and two d-orbitals are mixed to form the \({\rm{s}}{{\rm{p}}^{\rm{3}}}{\rm{\;}}{{\rm{d}}^{\rm{2}}}\) hybrid orbital. These hybrid orbitals are oriented toward the corners of a regular octahedron, forming an octahedral shape.
Therefore, it is octahedral in shape.