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Chapter 9: Problem 28

Use an example to illustrate each of the following terms: lone pairs, Lewis structure, the octet rule, bond length.

Short Answer

Expert verified
The key concepts are explained as follows: Lone Pairs are pairs of valence electrons which are not shared, example being the Oxygen atom's lone pairs in water. A Lewis structure shows the bonding and non-bonding electrons of a molecule or ion, such as the H-O-H arrangement for water. The Octet Rule states that atoms aim to have eight electrons in their outer shell, as seen in the water molecule where Oxygen atom achieves 8 electrons. Bond length is the distance between the nuclei of two bonded atoms, e.g. it's about 0.74 angstroms for Hydrogen molecule.

Step by step solution

01

Lone Pairs

Lone pairs refer to the pair of valence electrons that are not shared with another atom in a chemical bond. As Example, consider water molecule \(H_2O\). Each Oxygen atom has 6 electrons in the outer shell where 2 electrons participate in bonding with Hydrogen atoms, and the remaining 4 are two lone pairs.
02

Lewis Structure

Lewis structures represent the bonding and non-bonding electrons for a molecule or ion. It helps to visualize how the valence electrons are distributed in the molecule. For instance, for water molecule \(H_2O\), the Lewis Structure represents two single bonds between Hydrogen atoms and the Oxygen atom and two lone pairs on the Oxygen atom.
03

The Octet Rule

The Octet rule states that atoms tend to form bonds in such a way that they achieve an electron configuration of the nearest noble gas, typically having eight electrons in their outer shell. For example, in the water molecule, the Oxygen atom follows the octet rule as it has 8 electrons in its outer shell (4 from its own, 2 shared with one Hydrogen atom and 2 shared with another Hydrogen atom).
04

Bond Length

The bond length refers to the distance between the nuclei of two bonded atoms in a molecule. It reflects the type of bond and strength between the atoms. For instance, in a Hydrogen molecule \(H_2\), the bond length is approximately 0.74 angstroms.

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Most popular questions from this chapter

Which of the following are ionic compounds? Which are covalent compounds? \(\mathrm{RbCl}, \mathrm{PF}_{5}, \mathrm{BrF}_{3},\) \(\mathrm{KO}_{2}, \mathrm{CI}_{4}\)

Summarize the essential features of the Lewis octet rule.

Most organic acids can be represented as \(\mathrm{RCOOH}\) where \(\mathrm{COOH}\) 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 for the carboxyl group. (b) Upon ionization, the carboxyl group is converted to the carboxylate group, \(\mathrm{COO}^{-}\). Draw resonance structures for the carboxylate group.

Write Lewis structures for the following species, including all resonance forms, and show formal charges: (a) \(\mathrm{HCO}_{2}^{-},\) (b) \(\mathrm{CH}_{2} \mathrm{NO}_{2}^{-}\). Relative positions of the atoms are as follows:

Give a brief description of the medical uses of the following ionic compounds: \(\mathrm{AgNO}_{3}, \mathrm{BaSO}_{4},\) \(\mathrm{CaSO}_{4}, \mathrm{KI}, \mathrm{Li}_{2} \mathrm{CO}_{3}, \mathrm{Mg}(\mathrm{OH})_{2}, \mathrm{MgSO}_{4}, \mathrm{NaHCO}_{3}\) \(\mathrm{Na}_{2} \mathrm{CO}_{3}, \mathrm{NaF}, \mathrm{TiO}_{2}, \mathrm{ZnO} .\) You would need to do a Web search of some of these compounds.
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