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Chapter 8: Problem 134

What do each of the following sets of compounds/ions have in common with each other? a. \(\mathrm{SO}_{3}, \mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}\) b. \(\mathrm{O}_{3}, \mathrm{SO}_{2}, \mathrm{NO}_{2}^{-}\)

Short Answer

Expert verified
The common property among the compounds/ions in set a (\(\mathrm{SO}_{3}, \mathrm{NO}_{3}^{-}, \mathrm{CO}_{3}^{2-}\)) is that they are all Trigonal Planar molecules and ions with three Oxygen atoms surrounding the central atom with double or coordinate covalent bonds. In set b (\(\mathrm{O}_{3}, \mathrm{SO}_{2}, \mathrm{NO}_{2}^{-}\)), the common property is that they are all Bent (V-shaped) molecules and ions, featuring two atoms of either Oxygen or Sulfur surrounding the central atom with double and single bonds or two double bonds.

Step by step solution

01

Observation of Bonding Patterns

From the given compounds/ions, we notice that all of them have three atoms surrounding the central atom. Also, we can see that they share Oxygen atoms. Now, let's look for any common bonding pattern.
02

Valence Electrons

In all three compounds/ions, the three Oxygen atoms are bonded to the central atom (Sulfur, Nitrogen, or Carbon) using double bonds or coordinate covalent bonds (in the case of the negative ions). The double bonds are formed due to the sharing of a pair of valence electrons by both the central atom and the Oxygen atom.
03

Common Property

After analyzing the valence electrons and bonding patterns in these compounds/ions, we can conclude that the common property among these is that they are all Trigonal Planar molecules and ions, featuring three Oxygen atoms surrounding the central atom with double or coordinate covalent bonds. #b. Identify the common property of \(\mathrm{O}_{3}, \mathrm{SO}_{2}, \mathrm{NO}_{2}^{-}\)#
04

Observation of Bonding Patterns

In this set of compounds/ions, we notice that all of these species have two atoms connected to the central atom. One is an Oxygen atom, and another can be either Oxygen or Sulfur. Let's investigate the bonding patterns.
05

Valence Electrons

All three compounds/ions have a central atom (Oxygen, Sulfur, or Nitrogen) sharing valence electrons with the other atoms. In the case of \(\mathrm{O_3}\) (Ozone) and \(\mathrm{NO}_{2}^{-}\), the central atom is linked by double bonds and single bonds to the other atoms, while \(\mathrm{SO}_{2}\) has two double bonds between the central Sulfur atom and the two Oxygen atoms.
06

Common Property

After analyzing the bonding patterns and valence electrons in these compounds/ions, we can conclude that the common property among these is that they are all Bent (V-shaped) molecules and ions, featuring two atoms of either Oxygen or Sulfur surrounding the central atom with double and single bonds or two double bonds.

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Most popular questions from this chapter

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 \(\mathrm{A}_{2}\) ?

Draw a Lewis structure for the \(N, N\) -dimethylformamide molecule. The skeletal structure is Various types of evidence lead to the conclusion that there is some double bond character to the \(\mathrm{C}-\mathrm{N}\) bond. Draw one or more resonance structures that support this observation.

Two different compounds have the formula \(\mathrm{XeF}_{2} \mathrm{Cl}_{2} .\) Write Lewis structures for these two compounds, and describe how measurement of dipole moments might be used to distinguish between them.

Use Coulomb's law, $$ V=\frac{Q_{1} Q_{2}}{4 \pi \varepsilon_{0} r}=2.31 \times 10^{-19} \mathrm{~J} \cdot \mathrm{nm}\left(\frac{Q_{1} Q_{2}}{r}\right) $$ to calculate the energy of interaction for the following two arrangements of charges, each having a magnitude equal to the electron charge.

Oxidation of the cyanide ion produces the stable cyanate ion, \(\mathrm{OCN}^{-}\). The fulminate ion, \(\mathrm{CNO}^{-}\), on the other hand, is very unstable. Fulminate salts explode when struck; \(\mathrm{Hg}(\mathrm{CNO})_{2}\) is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in \(\mathrm{OCN}^{-}\) and \(\mathrm{N}\) is the central atom in \(\mathrm{CNO}^{-} .\).)
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