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Chapter 10: Problem 27

How does a hybrid orbital differ from a pure atomic orbital? Can two \(2 p\) orbitals of an atom hybridize to give two hybridized orbitals?

Short Answer

Expert verified
A hybrid orbital differs from a pure atomic orbital in that it is a combination of two or more atomic orbitals, resulting in an orbital with a different characteristic shape and energy level. Yes, two \(2p\) orbitals can hybridize to give two hybridized orbitals.

Step by step solution

01

Defining Pure Atomic Orbital

A pure atomic orbital is the region in an atom where an electron with a given energy is likely to be found. They have characteristic shapes, denoted as \(s\), \(p\), \(d\), and \(f\) orbitals, each corresponding to a different shape and energy level.
02

Defining Hybrid Orbital

A hybrid orbital is a kind of atomic orbital that results from the mixing or 'hybridization' of two or more different pure atomic orbitals, resulting in a new, different orbital. They have characteristic shapes different from the pure atomic orbitals, and are often involved in covalent bonding.
03

Explaining the Difference

The key difference therefore between a pure atomic orbital and a hybrid orbital is that while the former exists alone and defines the space in which an electron is likely to be found, the latter is a combination of two or more atomic orbitals that results in an orbital with a different characteristic shape and energy level.
04

Hybridization of \(2p\) Orbitals

Indeed, two \(2p\) orbitals can hybridize to give two hybridized orbitals. In the process known as 'hybridization', different atomic orbitals mix to form new, equivalent hybrid orbitals. Therefore, two \(2p\) orbitals can mix to create two hybrid orbitals.

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Most popular questions from this chapter

What hybrid orbitals are used by nitrogen atoms in these species? (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{2} \mathrm{~N}-\mathrm{NH}_{2}\) (c) \(\mathrm{NO}_{3}^{-}\)

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

Sketch the shape of a linear triatomic molecule, a trigonal planar molecule containing four atoms, a tetrahedral molecule, a trigonal bipyramidal molecule, and an octahedral molecule. Give the bond angles in each case.

Explain why the bond order of \(\mathrm{N}_{2}\) is greater than that of \(\mathrm{N}_{2}^{+},\) but the bond order of \(\mathrm{O}_{2}\) is less than that of \(\mathrm{O}_{2}^{+}\)

Briefly compare the VSEPR and hybridization approaches to the study of molecular geometry.
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