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Chapter 8: Problem 113

Predict the molecular structure (including bond angles) for each of the following. a. \(\mathrm{SeO}_{3}\) b. \(\mathrm{SeO}_{2}\)

Short Answer

Expert verified
The molecular structure of \(\mathrm{SeO}_{3}\) is square pyramidal with bond angles of approximately 90 degrees, and the molecular structure of \(\mathrm{SeO}_{2}\) is bent with a bond angle of less than 120 degrees.

Step by step solution

01

a. Determination of the electron geometry of \(\mathrm{SeO}_{3}\)

To determine the electron geometry of \(\mathrm{SeO}_{3}\), we first need to find the number of electron pairs around the central atom, Se. 1. Determine the total number of valence electrons: Se has 6 valence electrons and O has 6. Since there are 3 O atoms, the total valence electrons are: 6 (Se) + 3x6 (O) = 24 2. Determine the number of electron pairs: There are 6 electron pairs as Se forms 3 single bonds with 3 O atoms and has 1 lone pair. Now, since there are 6 electron pairs around the central atom Se, the electron geometry of \(\mathrm{SeO}_{3}\) is octahedral.
02

b. Determination of the molecular geometry of \(\mathrm{SeO}_{3}\)

Since the electron geometry is octahedral, and there is 1 lone pair of electrons on the central atom, the molecular geometry should be derived from the octahedral geometry by removing one vertex from the octahedron. That will create a molecular geometry called square pyramidal.
03

c. Predicting bond angles for \(\mathrm{SeO}_{3}\)

In a square pyramidal molecular geometry, the bond angles are approximately 90 degrees between the equatorial oxygen atoms and 90 degrees between each equatorial oxygen and the apical oxygen atom.
04

d. Determination of the electron geometry of \(\mathrm{SeO}_{2}\)

To determine the electron geometry of \(\mathrm{SeO}_{2}\), we first need to find the number of electron pairs around the central atom, Se. 1. Determine the total number of valence electrons: Se has 6 valence electrons and O has 6. Since there are 2 O atoms, the total valence electrons are: 6 (Se) + 2x6 (O) = 18 2. Determine the number of electron pairs: There are 5 electron pairs as Se forms 2 single bonds with 2 O atoms and has 2 lone pairs. Now, since there are 5 electron pairs around the central atom Se, the electron geometry of \(\mathrm{SeO}_{2}\) is trigonal bipyramidal.
05

e. Determination of the molecular geometry of \(\mathrm{SeO}_{2}\)

Since the electron geometry is trigonal bipyramidal and there are 2 lone pairs of electrons on the central atom, the molecular geometry should be derived from the trigonal bipyramidal geometry by removing two vertices from the bipyramid. That will create a molecular geometry called bent or angular.
06

f. Predicting bond angles for \(\mathrm{SeO}_{2}\)

In a bent molecular geometry, the bond angle between the two oxygen atoms is approximately less than 120 degrees due to the presence of the two lone pairs on the central atom which compress the angle. In conclusion, the molecular structure of \(\mathrm{SeO}_{3}\) is square pyramidal with bond angles of approximately 90 degrees, and the molecular structure of \(\mathrm{SeO}_{2}\) is bent with a bond angle of less than 120 degrees.

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Most popular questions from this chapter

One type of exception to the octet rule are compounds with central atoms having fewer than eight electrons around them. \(\mathrm{BeH}_{2}\) and \(\mathrm{BH}_{3}\) are examples of this type of exception. Draw the Lewis structures for \(\mathrm{BeH}_{2}\) and \(\mathrm{BH}_{3}\).

Give the formula of a negative ion that would have the same number of electrons as each of the following positive ions. a. \(\mathrm{Na}^{+}\) c. \(\mathrm{Al}^{3+}\) b. \(\mathrm{Ca}^{2+}\) d. \(\mathrm{Rb}^{+}\)

Consider the following reaction: $$ \mathrm{A}_{2}+\mathrm{B}_{2} \longrightarrow 2 \mathrm{AB} \quad \Delta H=-285 \mathrm{~kJ} $$ The bond energy for \(\mathrm{A}_{2}\) is one-half the amount of the \(\mathrm{AB}\) bond energy. The bond energy of \(\mathrm{B}_{2}=432 \mathrm{~kJ} / \mathrm{mol}\). What is the bond energy of \(\mathrm{A}_{2}\) ?

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