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Chapter 10: Problem 86

Estimate the lengths of the following bonds and indicate whether your estimate is likely to be too high or too low: (a) I \(-\mathrm{Cl} ;\) (b) \(\mathrm{C}-\mathrm{F}\).

Short Answer

Expert verified
The estimated bond lengths are approximately 232 pm for I-Cl and 149 pm for C-F. These estimates may be too high because of reasons related to electron shell count in case of I-Cl and high electronegativity of Fluorine in case of C-F.

Step by step solution

01

Gather atomic radius information

Research the atomic radii of iodine (I), chlorine (Cl), carbon (C), and fluorine (F). For example, according to the periodic table, the covalent radii of iodine, chlorine, carbon, and fluorine are approximately 133 pm, 99 pm, 77 pm, and 72 pm respectively.
02

Estimate the bond lengths

To estimate the bond length, one can add the atomic radii of the two atoms forming the bond. The estimated bond length of I-Cl is therefore approximately \(133 pm + 99 pm = 232 pm\) and the estimated bond length of C-F is \(77 pm + 72 pm = 149 pm\). These are estimates and can contain some error.
03

Assess the estimates

These estimates may be too high or too low. I-Cl bond is a single bond within halogens. However, iodine has more electron shells than chlorine, so the bond length might be overestimated. For C-F, it's a single bond between a non-metal and a halogen. The bond might be shorter due to fluorine's high electronegativity pulling electrons closer, hence these estimations might be overestimated.

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Most popular questions from this chapter

Write plausible Lewis structures for the following molecules that contain only single covalent bonds. (a) \(\mathrm{FCl} ;\) (b) \(\mathrm{I}_{2} ;\) (c) \(\mathrm{SF}_{2} ;\) (d) \(\mathrm{NF}_{3} ;\) (e) \(\mathrm{H}_{2} \mathrm{Te}\).

Explain the important distinctions between (a) ionic and covalent bonds; (b) lone-pair and bond-pair electrons; (c) molecular geometry and electron-group geometry; (d) bond dipole and resultant dipole moment; (e) polar molecule and nonpolar molecule.

Use the VSEPR theory to predict the shape of (a) the molecule OSF \(_{2} ;\) (b) the molecule \(\mathrm{O}_{2} \mathrm{SF}_{2} ;\) (c) the ion \(\mathrm{SF}_{5}^{-} ;\) (d) the ion \(\mathrm{ClO}_{4}^{-} ;\) (e) the ion \(\mathrm{ClO}_{3}^{-}\).

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

One of the isomers of chloromethanol has the formula $\mathrm{ClCH}_{2} \mathrm{OH} .$ Sketch, by using the dash and wedge symbolism, this isomer of chloromethanol, and indicate the various bond angles.
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