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Chapter 9: Problem 68

What hybridization do you expect for the atom that is underlined in each of the following species? (a) $\underline{\mathrm{O}}_{2}^{-} ;(\mathbf{b}) \underline{\mathrm{N}} \mathrm{H}_{4}^{+} ;$ (c) \(\mathrm{SCN}^{-}\) (d) \(\underline{\mathrm{Br}} \mathrm{Cl}_{3}\)

Short Answer

Expert verified
The hybridization for the underlined atoms in each species is as follows: (a) \(\underline{\mathrm{O}}_{2}^{-}\): sp (b) \(\underline{\mathrm{N}} \mathrm{H}_{4}^{+}\): sp3 (c) \(\mathrm{SCN}^{-}\) (Carbon is the central atom): sp (d) \(\underline{\mathrm{Br}} \mathrm{Cl}_{3}\): sp2

Step by step solution

01

Count the number of ligands surrounding the central atom

In this case, the central atom is Oxygen. We have one other oxygen atom and one extra electron due to the negative charge. The steric number equals 2.
02

Determine the hybridization

For two ligands, we'll have an electronic geometry of linear (shape). To obtain this geometry, we use one s and one p orbital to hybridize. Thus, hybridization is sp. (b) \(\underline{\mathrm{N}} \mathrm{H}_{4}^{+}\)
03

Count the number of ligands surrounding the central atom

In this case, the central atom is Nitrogen. We have four Hydrogen atoms around it and one electron less due to the positive charge. The steric number equals 4.
04

Determine the hybridization

For four ligands, we'll have an electronic geometry of tetrahedral (shape). To obtain this geometry, we use one s and three p orbitals to hybridize. Thus, hybridization is sp3. (c) \(\mathrm{SCN}^{-}\)
05

Count the number of ligands surrounding the central atom

In this case, the central atom is Carbon. We have one Sulfur atom and one Nitrogen atom attached to it. The steric number equals 2.
06

Determine the hybridization

For two ligands, we'll have an electronic geometry of linear (shape). To obtain this geometry, we use one s and one p orbital to hybridize. Thus, hybridization is sp. (d) \(\underline{\mathrm{Br}} \mathrm{Cl}_{3}\)
07

Count the number of ligands surrounding the central atom

In this case, the central atom is Bromine. We have three Chlorine atoms attached to it. The steric number equals 3.
08

Determine the hybridization

For three ligands, we'll have an electronic geometry of trigonal planar (shape). To obtain this geometry, we use one s and two p orbitals to hybridize. Thus, hybridization is sp2.

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Most popular questions from this chapter

Consider the molecule \(\mathrm{PF}_{4}\) Cl. (a) Draw a Lewis structure for the molecule, and predict its electron-domain geometry. (b) Which would you expect to take up more space, a \(\mathrm{P}-\mathrm{F}\) bond or a \(\mathrm{P}-\mathrm{Cl}\) bond? Explain. (c) Predict the molecular geometry of \(\mathrm{PF}_{4} \mathrm{Cl}\). How did your answer for part (b) influence your answer here in part (c)? (d) Would you expect the molecule to distort from its ideal electron-domain geometry? If so, how would it distort?

(a) Is the molecule \(\mathrm{BF}_{3}\) polar or nonpolar? (b) If you react \(\mathrm{BF}_{3}\) to make the ion \(\mathrm{BF}_{3}^{2-}\), is this ion planar? (c) Does the molecule \(\mathrm{BF}_{2} \mathrm{Cl}\) have a dipole moment?

Methyl isocyanate, \(\mathrm{CH}_{3} \mathrm{NCO},\) was made infamous in 1984 when an accidental leakage of this compound from a storage tank in Bhopal, India, resulted in the deaths of about 3800 people and severe and lasting injury to many thousands more. (a) Draw a Lewis structure for methyl isocyanate. (b) Draw a ball-and-stick model of the structure, including estimates of all the bond angles in the compound. (c) Predict all the bond distances in the molecule. (d) Do you predict that the molecule will have a dipole moment? Explain.

Dichloroethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{2}\right)\) has three forms (isomers), each of which is a different substance. (a) Draw Lewis structures of the three isomers, all of which have a carbon-carbon double bond. \((\mathbf{b})\) Which of these isomers has a zero dipole moment? (c) How many isomeric forms can chloroethylene, $\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}$, have? Would thev be expected to have dipole moments?

(a) An \(\mathrm{AB}_{2}\), molecule is linear. How many nonbonding electron pairs are around the A atom from this information? (b) How many nonbonding electrons surround the Xe in $\mathrm{XeF}_{2} ?(\mathbf{c})\( Is \)\mathrm{XeF}_{2}$ linear?
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