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Chapter 10: Problem 26

What is the hybridization of atomic orbitals? Why is it impossible for an isolated atom to exist in the hybridized state?

Short Answer

Expert verified
Hybridization of atomic orbitals is the intermixing of atomic orbitals of slightly different energies to distribute energy more evenly. This occurs only when atoms are in the process of forming covalent bonds in a molecule, as they require the necessary energy and proximity to another atom for this to occur. Therefore, an isolated atom cannot exist in the hybridized state.

Step by step solution

01

Define Hybridization of Atomic Orbitals

Hybridization is the concept of intermixing of the atomic orbitals of slightly different energies so as to redistribute the energy more evenly among them. The resulting orbitals are called hybrid orbitals. Mathematically, hybridisation can be explained by the linear combination of atomic orbitals.
02

Describe Types of Hybridization

Different types of hybridization involve combinations of orbitals. For example, in carbon, the 2s and all the three 2p orbitals mix together forming four new orbitals that are equivalent known as the SP3 hybrid orbitals, involved in the formation of methane.
03

Explain Why Hybridization Cannot Occur in Isolated Atoms

Hybridization occurs when atoms are forming covalent bonds in a molecule. Isolated atoms, not forming bonds, don't have the necessary energy and proximity to another atom to undergo intermixing of their atomic orbitals. Therefore, isolated atoms will not display hybridization.

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Most popular questions from this chapter

The compound 1,2 -dichloroethane \(\left(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}\right)\) is nonpolar, while cis-dichloroethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}\right)\) has a dipole moment: The reason for the difference is that groups connected by a single bond can rotate with respect to each other, but no rotation occurs when a double bond connects the groups. On the basis of bonding considerations, explain why rotation occurs in \(1,2-\) dichloroethane but not in \(c i s\) -dichloroethylene.

Compare the relative stability of these species and indicate their magnetic properties (that is, diamagnetic or paramagnetic): \(\mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}\) (superoxide ion), \(\mathrm{O}_{2}^{2-}\) (peroxide ion).

Specify which hybrid orbitals are used by carbon atoms in these species: (a) \(\mathrm{CO},\) (b) \(\mathrm{CO}_{2},\) (c) \(\mathrm{CN}^{-}\).

The allene molecule \(\mathrm{H}_{2} \mathrm{C}=\mathrm{C}=\mathrm{CH}_{2}\) is linear (the three \(\mathrm{C}\) atoms lie on a straight line). What are the hybridization states of the carbon atoms? Draw diagrams to show the formation of sigma bonds and pi bonds in allene.

Does the molecule OCS have a higher or lower dipole moment than \(\mathrm{CS}_{2} ?\)
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