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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

List these molecules in order of increasing dipole moment: \(\mathrm{H}_{2} \mathrm{O}, \mathrm{CBr}_{4}, \mathrm{H}_{2} \mathrm{~S}, \mathrm{HF}, \mathrm{NH}_{3}, \mathrm{CO}_{2}\)

Use valence bond theory to explain the bonding in \(\mathrm{Cl}_{2}\) and \(\mathrm{HCl}\). Show how the atomic orbitals overlap when a bond is formed

Predict the geometry of these molecules and ion using the VSEPR method: (a) \(\operatorname{HgBr}_{2}\), (b) \(\mathrm{N}_{2} \mathrm{O}\) (arrangement of atoms is NNO), (c) SCN \(^{-}\) (arrangement of atoms is SCN).

The ionic character of the bond in a diatomic molecule can be estimated by the formula $$ \frac{\mu}{e d} \times 100 \% $$ where \(\mu\) is the experimentally measured dipole moment (in \(\mathrm{C} \mathrm{m}\) ), \(e\) is the electronic charge \((1.6022 \times\) \(10^{-19} \mathrm{C}\) ), and \(d\) is the bond length in meters. (The quantity \(e d\) is the hypothetical dipole moment for the case in which the transfer of an electron from the less electronegative to the more electronegative atom is complete.) Given that the dipole moment and bond length of \(\mathrm{HF}\) are \(1.92 \mathrm{D}\) and \(91.7 \mathrm{pm},\) respectively, calculate the percent ionic character of the molecule.

Draw a potential energy curve for the bond formation in \(\mathrm{F}_{2}\).
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