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Chapter 10: Problem 72

Comment on the similarities and differences in the molecular structure of the following four-atom species: \(\mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}, \mathrm{SO}_{3}^{2-},\) and \(\mathrm{ClO}_{3}^{-}\).

Short Answer

Expert verified
The NO3-, CO3^2-, SO3^2-, and ClO3- ions all have similar molecular geometry (trigonal planar) and the same number of total atoms and valence electrons. The species differ considering the central atom and the number of electrons it contributes. Each species has resonance structures which explain their equal bond lengths.

Step by step solution

01

Matter Composition

First, identify the atoms that make up each species: NO3- is made up of one Nitrogen atom and three Oxygen atoms. CO3^2- is composed of one Carbon atom and three Oxygen atoms. Similarly, SO3^2- consists of one Sulfur atom and three Oxygen atoms, while ClO3- contains one Chlorine atom and three Oxygen atoms.
02

Identify the Charge

Next, identify the charge on each species due to loss or gain of electrons, NO3- has a charge of -1, CO3^2- and SO3^2- both have charges of -2, and ClO3- has a charge of -1.
03

Determine the Molecular Geometry

All of these molecules have a central atom bonded to three other atoms, resulting in a trigonal planar molecular geometry, in which the atoms make a flat triangle with the central atom in the middle.
04

Assess the Bond Length

NO3-, CO3^2-, SO3^2-, and ClO3- have double bonds and single bonds which resonate, meaning the actual bond lengths are equal and somewhere between a single and double bond length. These resonance structures explain why the bond lengths are the same within each molecule.
05

Contrast the Species

Each species differ in the central atom and the number of electrons it contributes. But, all of them have the same number of total atoms, molecular geometry, resonance structures, equal bond lengths and also, the same number of total valence electrons (24 each).

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Most popular questions from this chapter

In which of the following species is it necessary to employ an expanded valence shell to represent the Lewis structure: $\mathrm{PO}_{4}^{3-}, \mathrm{PI}_{3}, \mathrm{ICl}_{3}, \mathrm{OSCl}_{2}, \mathrm{SF}_{4}, \mathrm{ClO}_{4} ?$ Explain your choices.

Write a plausible Lewis structure for \(\mathrm{C}_{3} \mathrm{O}_{2},\) a substance known as carbon suboxide.

Each of the following molecules contains one or more multiple covalent bonds. Draw plausible Lewis structures to represent this fact, and predict the shape of each molecule. (a) \(\mathrm{CO}_{2} ;\) (b) \(\mathrm{Cl}_{2} \mathrm{CO} ;\) (c) CINO \(_{2}\).

Derive the correct formulas for the following ionic compounds by writing Lewis structures. (a) lithium sulfide; (b) sodium fluoride; (c) calcium iodide; (d) scandium chloride.

If you have four electron pairs around a central atom, under what circumstances can you have a pyramidal molecule? Similarly, how can you have a bent molecule? What are the expected bond angles in each case?
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