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Chapter 5: Problem 111

How does a polar covalent bond differ from. a covalent bond? Give examples of diatomic molecules that contain a polar covalent bond and of diatomic molecules that contain a covalent bond.

Short Answer

Expert verified
A polar covalent bond is a subtype of a covalent bond that occurs when the electronegativity difference between the two atoms is significant but not large enough to form an ionic bond, resulting in unequal sharing of electrons and a partial positive/negative charge on each atom. In contrast, a covalent bond has more or less equal sharing of electrons due to similar electronegativity values. Examples of diatomic molecules with covalent bonds include H2, N2, and O2, while examples of diatomic molecules with polar covalent bonds include HF, HCl, and NO.

Step by step solution

01

Understanding Covalent Bonds

A covalent bond is formed when two atoms share electrons to achieve a stable electronic configuration. In general, atoms within a covalent bond have similar electronegativity values. Examples of diatomic molecules with covalent bonds include H2, N2, and O2.
02

Understanding Polar Covalent Bonds

A polar covalent bond is a subtype of the covalent bond. It occurs when the electronegativity difference between the two atoms involved in the bond is significant but not large enough to form an ionic bond. In a polar covalent bond, electrons are not shared equally, resulting in a polarity where one atom has a partial positive charge, and the other has a partial negative charge. Examples of diatomic molecules with polar covalent bonds include HF, HCl, and NO.
03

Comparing Covalent and Polar Covalent Bonds

Covalent bonds and polar covalent bonds share electrons between atoms. However, in a covalent bond, electrons are shared more or less equally due to similar electronegativity of the atoms involved. In polar covalent bonds, electrons are shared unequally because of the significant electronegativity difference between the atoms, causing the bond to have a polar nature.
04

Examples of Diatomic Molecules with Covalent Bonds

In diatomic molecules with covalent bonds, the atoms have similar electronegativity values, resulting in equal sharing of electrons. Examples of such diatomic molecules include: 1. Hydrogen molecule (H2) 2. Nitrogen molecule (N2) 3. Oxygen molecule (O2)
05

Examples of Diatomic Molecules with Polar Covalent Bonds

In diatomic molecules with polar covalent bonds, the atoms have a significant electronegativity difference, resulting in the unequal sharing of electrons and creating poles within the molecule. Examples of such diatomic molecules include: 1. Hydrogen fluoride (HF) 2. Hydrogen chloride (HCl) 3. Nitrogen monoxide (NO)

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Most popular questions from this chapter

The acetate ion has the formula \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}\). Draw a dot diagram for it given the following atomic connections. (Hint: Watch for resonance forms.)

Consider the following: \(\begin{array}{llllll}\mathrm{Cl}_{2} & \mathrm{CF}_{4} & \mathrm{MgO} & \mathrm{NaCl} & \mathrm{PH}_{3} & \mathrm{SCl}_{2}\end{array}\) (a) Which of these substances is ionic? (b) Which of these substances has nonpolar bonds? (c) Which of these substances has polar covalent bonds?

\(\mathrm{P}\) is immediately under \(\mathrm{N}\) in the periodic table. Both react with three atoms of chlorine to form \(\mathrm{NCl}_{3}\) and \(\mathrm{PCl}_{3} .\) However, phosphorus also forms \(\mathrm{PCl}_{5}\), whereas nitrogen does not. Draw dot diagrams for all three molecules. In doing so, you will have to violate the octet rule for \(\mathrm{PCl}_{5}\). That is OK. Do it. Then explain why phosphorus can do this but nitrogen can't. (Hint: Nitrogen has only \(2 \mathrm{~s}\) and \(2 p\) orbitals in its valence shell, which together can hold a maximum of eight electrons. Read section \(5.8\) about expanded octet atoms.) Then postulate what kind of atoms might be expected to exceed the octet rule.

How many electrons does the nickel atom lose when forming nickel(II) nitrate? When forming nickel(II) sulfate?

What is a binary compound? Is atmospheric oxygen an example of a binary compound?
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