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Chapter 1: Problem 25

Which compounds have nonpolar covalent bonds, which have polar covalent bonds, and which have ions? (a) LiF (b) \(\mathrm{CH}_{3} \mathrm{~F}\) (c) \(\mathrm{MgCl}_{2}\) (d) \(\mathrm{HCl}\)

Short Answer

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Question: Categorize the following compounds as having nonpolar covalent bonds, polar covalent bonds, or ionic bonds: (a) LiF, (b) CH3F, (c) MgCl2, (d) HCl. Answer: (a) LiF has ionic bonds, (b) CH3F has both nonpolar and polar covalent bonds, (c) MgCl2 has ionic bonds, and (d) HCl has polar covalent bonds.

Step by step solution

01

(a) LiF

The electronegativity difference between lithium (Li) and fluorine (F) is 3.98 - 0.98 = 3.0, which is greater than 1.7. Therefore, LiF has ionic bonds.
02

(b) \(\mathrm{CH}_{3} \mathrm{~F}\)

In this compound, we have two types of bonds: C-H and C-F. For the C-H bond, the electronegativity difference is 2.55 - 2.20 = 0.35, which is less than 0.4, so it is considered nonpolar covalent. For the C-F bond, the electronegativity difference is 3.98 - 2.55 = 1.43, which is between 0.4 and 1.7, so it is considered polar covalent. Overall, \(\mathrm{CH}_{3} \mathrm{~F}\) has both nonpolar and polar covalent bonds.
03

(c) \(\mathrm{MgCl}_{2}\)

The electronegativity difference between magnesium (Mg) and chlorine (Cl) is 3.16 - 1.31 = 1.85, which is greater than 1.7. Therefore, \(\mathrm{MgCl}_{2}\) has ionic bonds.
04

(d) \(\mathrm{HCl}\)

The electronegativity difference between hydrogen (H) and chlorine (Cl) is 3.16 - 2.20 = 0.96, which is between 0.4 and 1.7. Therefore, \(\mathrm{HCl}\) has polar covalent bonds.

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Most popular questions from this chapter

Classify each bond as nonpolar covalent or polar covalent or state that ions are formed. (a) \(\mathrm{S}-\mathrm{H}\) (b) \(\mathrm{P}-\mathrm{H}\) (c) \(\mathrm{C}-\mathrm{F}\) (d) \(\mathrm{C}-\mathrm{Cl}\)

Use VSEPR to predict the geometry of these ions. (a) \(\mathrm{NH}_{2}{ }^{-}\) (b) \(\mathrm{NO}_{2}{ }^{-}\) (c) \(\mathrm{NO}_{2}^{+}\) (d) \(\mathrm{NO}_{3}^{-}\)

Draw Lewis structures for these functional groups. Be certain to show all valence electrons on each. (a) Carbonyl group (b) Carboxyl group (c) Hydroxyl group (d) Ester group (e) Amide group

Draw a Lewis structure for the azide ion, \(\mathrm{N}_{3}{ }^{-}\). (The order of atom attachment is \(\mathrm{N}-\mathrm{N}-\mathrm{N}\), and they do not form a ring.) How does the resonance model account for the fact that the lengths of the \(\mathrm{N}-\mathrm{N}\) bonds in this ion are identical?

Draw condensed structural formulas for all compounds with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{8} \mathrm{O}\) that contain (a) A carbonyl group (there are two aldehydes and one ketone). (b) A carbon-carbon double bond and a hydroxyl group (there are eight).
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