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Chapter 6: Problem 107

What is it about the trigonal bipyramidal shape that distinguishes it from all the other molecular shapes that we have covered? (Hint: Think about lone pairs of electrons.)

Short Answer

Expert verified
The trigonal bipyramidal shape is distinguished from other molecular shapes by the absence of lone pairs of electrons on the central atom. Instead, all five electron pairs are involved in bonding with the surrounding atoms, leading to its distinct geometry with bond angles of 90 degrees between axial and equatorial atoms and 120 degrees between equatorial atoms. This configuration optimizes stability and minimizes repulsion between the electron pairs.

Step by step solution

01

Understanding the trigonal bipyramidal shape

The trigonal bipyramidal shape is a molecular geometry that occurs when a central atom is bonded to five other atoms. This shape consists of three atoms (forming an equatorial plane) surrounding the central atom, with two additional atoms (the axial atoms) positioned directly above and below the central atom. The bond angles in this shape are 90 degrees between the axial and equatorial atoms and 120 degrees between the equatorial atoms.
02

Identifying major molecular shapes

There are several molecular shapes that we can consider for comparison with the trigonal bipyramidal shape, such as linear, bent, trigonal planar, trigonal pyramidal, tetrahedral, and octahedral. Each of these molecular shapes are associated with unique geometries and bond angles.
03

Role of lone pairs of electrons

One crucial aspect that characterizes molecular shapes is the presence or absence of lone pairs of electrons on the central atom. Lone pairs are valence electrons that are not shared by any other atom in the molecule. The distribution of these lone pairs can affect the molecular geometry, as the electron pairs will repel each other and alter bond angles.
04

Comparing the trigonal bipyramidal shape to other molecular shapes

The most significant feature that distinguishes the trigonal bipyramidal shape from other molecular shapes is that it has no lone pairs of electrons on the central atom. Instead, all five electron pairs are involved in bonding with the surrounding atoms, resulting in the distinct geometry. The trigonal bipyramidal shape has electron pair repulsion between five bonding electron pairs, which helps to minimize repulsions and achieve optimal stability.
05

Conclusion

In conclusion, the trigonal bipyramidal shape differs from other molecular shapes due to the absence of lone pairs of electrons on the central atom. The distinct geometry and favorable bond angles of this shape result from having five bonding electron pairs repel each other, leading to increased stability and minimum repulsion.

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Most popular questions from this chapter

Consider the molecule \(\mathrm{N}_{2} \mathrm{O}\) (connected \(\mathrm{N}-\mathrm{N}-\mathrm{O})\) (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this molecule? (d) Draw in the individual bond dipole moments. (e) Is the molecule polar? If yes, draw the molecular dipole moment vector.

Consider the molecule \(\mathrm{BrCl}_{3}\). (a) Draw a dot diagram for the molecule. (b) Predict the molecule's electron group geometry. (c) Predict the molecule's shape (name the shape and draw it using wedges, lines, and broken lines, and indicate the ideal value of the bond angles). (d) Predict if the molecule is polar or nonpolar. If polar, draw the dipole moment for the molecule.

Consider the phosphonium ion, \(\mathrm{PH}_{4}^{+}\). (a) Draw the dot diagram. (b) Draw the ion's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this polyatomic ion? (d) Draw in the individual bond dipole moments.

What is the difference between intermolecular forces and intramolecular forces? Which are stronger?

Under what conditions is the electron-group geometry for a molecule the same as the molecular shape?
See all solutions

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