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Chapter 14: Problem 7

Consider the series \(\mathrm{Cl}_{2}, \mathrm{Br}_{2}, \mathrm{I}_{2}\). a) What is the bond order for each X-X bond? b) What trend is observed in bond energy? c) Considering the relative size of \(\mathrm{Cl}, \mathrm{Br}\), and \(\mathrm{I}\), what trend would you predict in \(\mathrm{X}-\mathrm{X}\) bond length?

Short Answer

Expert verified
a) The bond order for each X-X bond is 1. b) The bond energy decreases from \(Cl_2\) to \(I_2\). c) The bond length increases from Cl-Cl to I-I.

Step by step solution

01

Determine the Bond Order

The bond order is calculated by subtracting the number of bonding electrons from the number of antibonding electrons, all divided by 2. For diatomic halogens like Cl-Cl, Br-Br, and I-I, there are no unpaired electrons. Therefore, all electrons are involved in bonding, so the bond order for all of these is 1.
02

Understand the Trend in Bond Energy

As we go down a group on the periodic table, the size of the atoms increases; hence, the bonds become longer and weaker. Therefore, the bond energy decreases. So, starting with \(Cl_2\) and going to \(I_2\), bond energy decreases.
03

Predict the Trend in Bond Length

Bond length, in general, increases with the size of the atom. Considering the size of the halogens Cl, Br, and I, it will be expected that the bond length increases from Cl-Cl to I-I.

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Most popular questions from this chapter

Consider the series \(\mathrm{HF}, \mathrm{HCl}, \mathrm{HBr}, \mathrm{HI}\). a) What is the bond order for each H-X bond? b) What trend is observed in bond energy? c) Considering the relative size of \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}\), and \(\mathrm{I}\), what trend would you predict in H-X bond length? Bond length is defined as the distance between the nuclei of two bonding atoms.

What is the relationship between the bond order of a bond and the designation of single, double, and triple bonds?

What is the relationship between the bond order and the number of electrons shared by two adjacent atoms?
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