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Chapter 4: Problem 99

What is meant by the term polar covalent bond?

Short Answer

Expert verified
Answer: A polar covalent bond is a type of covalent bond where the electrons are shared unequally between the two atoms due to a significant difference in electronegativity. This results in an uneven distribution of electron density across the bond, creating bond polarity with a positive (未+) end and a negative (未-) end of the bond. In contrast, a regular covalent bond involves equal sharing of electrons between the two atoms, with no significant difference in electronegativity and no bond polarity.

Step by step solution

01

Explain Covalent Bonds

Covalent bonds are chemical bonds formed by sharing pairs of electrons between atoms. The shared pair of electrons is attracted to the nuclei of both atoms that are participating in the bond, effectively holding them together.
02

Define Bond Polarity

Bond polarity arises due to the difference in electronegativity between the two atoms participating in the covalent bond. Electronegativity is the measure of an atom's ability to attract shared electrons in a covalent bond. When there is a significant difference in electronegativities between the two atoms in the bond, the electrons will be more attracted to the atom with the higher electronegativity, causing an uneven distribution of electron density. This creates a slightly positive (未+) end on the less electronegative atom and a slightly negative (未-) end on the more electronegative atom.
03

Define Polar Covalent Bond

A polar covalent bond is a type of covalent bond where the electrons are shared unequally between the two atoms due to a significant difference in electronegativity. This results in an uneven distribution of electron density across the bond, creating bond polarity with a positive (未+) end and a negative (未-) end of the bond. The polarity of polar covalent bonds leads to the formation of dipole moments, which affect the physical and chemical properties of the molecules containing those bonds.

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Most popular questions from this chapter

Draw Lewis structures for the following oxoanions: (a) \(\mathrm{ClO}_{2}^{-} ;\) (b) \(\mathrm{SO}_{3}^{2-} ;\) (c) \(\mathrm{HCO}_{3}^{-}\)

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Carbon disulfide, \(\mathrm{CS}_{2},\) is a flammable, low-boiling liquid. Draw the Lewis structure for \(\mathrm{CS}_{2}.\)

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In the typical Lewis structure of \(\mathrm{BF}_{3}\) there are only six valence electrons on the boron atom and each \(\mathrm{B}-\mathrm{F}\) bond is a single bond. However, the length and strength of these bonds indicate that they have a small measure of doublebond character-that is, their bond order is slightly greater than 1. a. Draw a Lewis structure of \(\mathrm{BF}_{3}\), including all resonance structures, in which there is one \(\mathrm{B}=\mathrm{F}\) double bond. b. What is the formal charge on the \(\mathrm{B}\) atom, and what is the average formal charge on each \(\mathrm{F}\) atom? c. Based on formal charges alone, what should be the bond order of each \(\mathrm{B}-\mathrm{F}\) bond in \(\mathrm{BF}_{3} ?\) d. What factor might support a bond order slightly greater than \(1 ?\)
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