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Chapter 11: Q4P (page 432)

How many hybrid orbitals form when four atomic orbitals of a central atom mix? Explain

Short Answer

Expert verified

Hybrid orbitals are formed only by combining atomic orbitals. These are very different from the atomic orbitals in isolated atoms in shapes and orientations.

Step by step solution

01

How hybrid orbital form

In isolated atoms, hybrid orbitals do not exist.These are formed only by the combination of atomic orbitals which are equivalent in shape and energy.

02

Step2:Number of hybrid orbitals formed

The number of hybrid orbitals formed depends upon the number of atomic orbitals that combines.This means that when four atomic orbitals of a central atom mix formation of four hybrid orbitals take place.

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Most popular questions from this chapter

The illustrations below depict differences in orbital hybridization of some tellurium ( Te ) fluorides.

(a) Which depicts the difference, if any, between TeF₆ (left) and TeF₅ (right)? (b) Which depicts the difference, if any, between TeF₄ (left) and TeF₆ (right)?

Certain atomic orbitals on two atoms were combined to form the following MO’s. Name the atomic orbitals used and the MO’s formed, and explain which MO has higher energy:

Tryptophan is one of the amino acids found in proteins:

(a) What is the hybridization of each of the numbered C, N, and O atoms?

(b) How many sigma bonds are present in tryptophan?

(c) Predict the bond angles at points a, b, and c.

Predict the shape, state the hybridization of the central atom, and give the ideal bond angle(s) and any expected deviations for:

${BrO}_{3}^{-}$
${AsCl}_{4}^{-}$
${SeO}_{4}^{2 -}$
${BiF}_{5}^{2 -}$
${SbF}_{4}^{+}$
${AlF}_{6}^{3 -}$
${IF}_{4}^{+}$

Which types of atomic orbitals of the central atom mix to form hybrid orbitals in

(a) CI₂O ; (b) BrCI₃ ; (c) PF₅ ; (d) SO₃²?

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