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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

Give the empirical formulas and names of the compounds formed from the following pairs of ions: (a) \(\mathrm{Rb}^{+}\) and \(\mathrm{I}^{-},\) (b) \(\mathrm{Cs}^{+}\) and \(\mathrm{SO}_{4}^{2-}\) (c) \(\mathrm{Sr}^{2+}\) and \(\mathrm{N}^{3-},(\mathrm{d}) \mathrm{Al}^{3+}\) and \(\mathrm{S}^{2-}\).

What is a coordinate covalent bond? Is it different from a normal covalent bond?

Draw four reasonable resonance structures for the \(\mathrm{PO}_{3} \mathrm{~F}^{2-}\) ion. The central \(\mathrm{P}\) atom is bonded to the three \(\mathrm{O}\) atoms and to the \(\mathrm{F}\) atom. Show formal charges.

Define electronegativity, and explain the difference between electronegativity and electron affinity. Describe in general how the electronegativities of the elements change according to position in the periodic table.

Write Lewis structures for these ions: (a) \(\mathrm{O}_{2}^{2-}\), (b) \(\mathrm{C}_{2}^{2-},\) (c) \(\mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.
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