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Chapter 9: Problem 32

What is a polar covalent bond? Name two compounds that contain one or more polar covalent bonds.

Short Answer

Expert verified
A polar covalent bond is a type of chemical bond where the shared pair of electrons is unequally distributed between two atoms due to a difference in electronegativity, creating a slight electrical imbalance in the molecule. Two compounds that contain polar covalent bonds are water (H_2O) and hydrogen fluoride (HF).

Step by step solution

01

Define Polar Covalent Bond

A polar covalent bond is a type of chemical bond where a pair of electrons is unequally shared between two atoms. This is due to a difference in electronegativity between the two atoms. The atom with the higher electronegativity will pull the electrons closer to itself, creating a slight electrical imbalance or polarity in the molecule.
02

Identify Compound 1 with Polar Covalent Bond

One example of a compound with polar covalent bonds is water (H_2O). In a water molecule, the oxygen atom shares a pair of electrons with each hydrogen atom. However, oxygen is more electronegative than hydrogen, so it pulls the shared electrons closer to itself, creating a polarity in the molecule.
03

Identify Compound 2 with Polar Covalent Bond

Another example of a compound with polar covalent bonds is hydrogen fluoride (HF). In a hydrogen fluoride molecule, the fluorine atom is more electronegative than the hydrogen atom, creating an electronegativity difference. As a result, the fluorine atom attracts the shared electrons more strongly, leading to a polar covalent bond.

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Most popular questions from this chapter

Match each of these energy changes with one of the processes given: ionization energy, electron affinity, bond enthalpy, standard enthalpy of formation. (a) \(\mathrm{F}(g)+e^{-} \longrightarrow \mathrm{F}^{-}(g)\) (b) \(\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{~F}(g)\) (c) \(\mathrm{Na}(g) \longrightarrow \mathrm{Na}^{+}(g)+e^{-}\) (d) \(\mathrm{Na}(s)+\frac{1}{2} \mathrm{~F}_{2}(g) \longrightarrow \mathrm{NaF}(s)\)

Draw three resonance structures for the molecule \(\mathrm{N}_{2} \mathrm{O}\) in which the atoms are arranged in the order NNO. Indicate formal charges.

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Classify these bonds as ionic, polar covalent, or covalent, and give your reasons: (a) the SiSi bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (b) the \(\mathrm{SiCl}\) bond in \(\mathrm{Cl}_{3} \mathrm{SiSiCl}_{3},\) (c) the CaF bond in \(\mathrm{CaF}_{2},\) (d) the \(\mathrm{NH}\) bond in \(\mathrm{NH}_{3}\).

Most organic acids can be represented as \(\mathrm{RCOOH}\), in which \(\mathrm{COOH}\) is the carboxyl group and \(\mathrm{R}\) is the rest of the molecule. (For example, \(\mathrm{R}\) is \(\mathrm{CH}_{3}\) in acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH}\).) (a) Draw a Lewis structure of the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures of the carboxylate group.
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