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Chapter 10: Problem 46

Explain the significance of bond order. Can bond order be used for quantitative comparisons of the strengths of chemical bonds?

Short Answer

Expert verified
Bond order, which indicates the number of bonds between atoms in a molecule, is significant as it suggests the stability, strength, and length of these bonds. Higher bond orders generally indicate stronger, shorter bonds. However, while bond order can indicate relative bond strength, it is not entirely accurate for precise quantitative comparisons; other factors also influence bond strength.

Step by step solution

01

Definition

Define bond order. Bond order is the number of chemical bonds between a pair of atoms. It gives an indication of the stability of a bond. In general, the higher the bond order, the more stable the bond.
02

Significance

Explain the significance of bond order. Bond order indicates the strength and length of bonds between atoms in a molecule. Higher bond orders mean that there are more bonds, and as a result, these bonds are generally stronger and shorter.
03

Quantitative Comparison

Explain whether or not bond order can be used for quantitative comparisons of the strengths of chemical bonds. It is important to note that while bond order can indicate relative bond strength, it may not always be accurate for quantitative comparisons - other factors like electronegativity, molecule geometry, and atomic size also influence bond strength.

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Most popular questions from this chapter

The geometries discussed in this chapter all lend themselves to fairly straightforward elucidation of bond angles. The exception is the tetrahedron, because its bond angles are hard to visualize. Consider the \(\mathrm{CCl}_{4}\) molecule, which has a tetrahedral geometry and is nonpolar. By equating the bond moment of a particular \(\mathrm{C}-\mathrm{Cl}\) bond to the resultant bond moments of the other three \(\mathrm{C}-\mathrm{Cl}\) bonds in opposite directions, show that the bond angles are all equal to \(109.5^{\circ}\)

Draw a potential energy curve for the bond formation in \(\mathrm{F}_{2}\).

Draw a molecular orbital energy level diagram for each of these species: \(\mathrm{He}_{2}, \mathrm{HHe}, \mathrm{He}_{2}^{+} .\) Compare their relative stabilities in terms of bond orders. (Treat HHe as a diatomic molecule with three electrons.)

Draw Lewis structures and give the other information requested for the following molecules: (a) \(\mathrm{BF}_{3}\). Shape: planar or nonplanar? (b) \(\mathrm{ClO}_{3}^{-}\). Shape: planar or nonplanar? (c) \(\mathrm{H}_{2} \mathrm{O}\). Show the direction of the resultant dipole moment. (d) \(\mathrm{OF}_{2}\). Polar or nonpolar molecule? (e) \(\mathrm{SeO}_{2}\). Estimate the OSeO bond angle.

Which of these pairs of atomic orbitals of adjacent nuclei can overlap to form a sigma bond? Which overlap to form a pi bond? Which cannot overlap (no bond)? Consider the \(x\) -axis to be the internuclear axis, that is, the line joining the nuclei of the two atoms. (a) \(1 s\) and \(1 s,\) (b) \(1 s\) and \(2 p_{x},\) (c) \(2 p_{x}\) and \(2 p_{y}\) (d) \(3 p_{y}\) and \(3 p_{y},\) (e) \(2 p_{x}\) and \(2 p_{x}\), (f) 1 s and 2 s.
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