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Chapter 4: Problem 26

In a covalent bond, of electrons takes place between the two atoms.

Short Answer

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Question: Explain the concept of a covalent bond and describe the process of electron sharing between two atoms in a covalent bond. Answer: A covalent bond is a chemical bond formed between two atoms by sharing one or more pairs of electrons. This electron sharing allows both atoms to achieve stable electron configurations, usually with filled outer electron shells. The process of electron sharing in a covalent bond involves identifying the atoms involved, determining the number of electrons to be shared, illustrating the electron sharing process using electron-dot (Lewis) structures, and identifying the type of covalent bond based on the number of electron pairs shared (single, double, or triple covalent bond).

Step by step solution

01

Understand Covalent Bonds

A covalent bond is a chemical bond formed between two atoms by sharing one or more pairs of electrons. This allows both atoms to achieve stable electron configurations, usually with a filled outer electron shell.
02

Identifying Atoms Involved in a Covalent Bond

The atoms involved in a covalent bond are typically nonmetals with similar electronegativities. Examples of covalent bonds can be found in molecules like hydrogen gas (\(H_2\)), water (\(H_2O\)), and carbon dioxide (\(CO_2\)).
03

Determine the Number of Electrons to be Shared

The number of electrons each atom needs to achieve a stable configuration (usually a full outer electron shell) is determined. This will give us the number of electrons that need to be shared between the atoms in the covalent bond.
04

Illustrate the Electron Sharing Process

Using electron-dot (Lewis) structures, show the electron sharing process for each atom. The shared electrons are represented as a pair of dots or a line between the atoms, indicating a covalent bond.
05

Identify the Type of Covalent Bond

Based on the number of electron pairs shared between the two atoms, we can identify the type of covalent bond formed. There are three types of covalent bonds: 1. Single covalent bond - one pair of electrons is shared 2. Double covalent bond - two pairs of electrons are shared 3. Triple covalent bond - three pairs of electrons are shared For example, in a water molecule (\(H_2O\)), each hydrogen atom forms a single covalent bond with the oxygen atom by sharing one electron pair.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Electron Sharing
In a covalent bond, electron sharing is the key process that occurs between two atoms. This involves the mutual sharing of electrons, allowing each atom to complete its outer electron shell.
This sharing happens because atoms strive to achieve an environment where they feel more stable, which usually means having a full set of electrons in their outermost shell.
By sharing these electrons, the atoms form a connection or bond, known as a covalent bond. This type of bond is particularly important in molecules made up of nonmetals, where the electrons are shared fairly equally.
Stable Electron Configurations
A stable electron configuration is a state where an atom's outer electron shell is filled, which usually means having eight electrons, known as an octet.
Atoms naturally seek to achieve this balanced and stable energy level through electron sharing.
This quest for stability and having a full outer shell are the main reasons atoms form covalent bonds in the first place.
For example, when hydrogen atoms form a covalent bond, they each achieve a stable configuration by fulfilling the duet rule, which means having two electrons, unlike the octet rule generally applied to most other elements.
Nonmetals
Nonmetals are the primary participants in forming covalent bonds due to their position on the periodic table.
Typically found on the right side of the periodic table, these elements have similar properties such as high electronegativities, which explains their tendency to pull electrons toward themselves.
As they share electrons, nonmetals efficiently create stable covalent bonds, forming molecules.
  • Hydrogen ( S ) and oxygen ( O ), as in water ( H_2O ).
  • Carbon ( C ) and oxygen ( O ) as in carbon dioxide ( CO_2 ).
These examples demonstrate how nonmetals come together to share and balance their electrons, resulting in stable covalent compounds.
Lewis Structures
Lewis structures, also known as electron-dot structures, are diagrams that show the bonding between atoms in a molecule and the lone pairs of electrons that may exist.
These structures are a valuable visual tool in chemistry that help illustrate the way electrons are shared in covalent bonds.
Each dot represents an electron, and pairs of dots or lines represent shared electron pairs or bonds. This method gives a clear picture of how the atoms achieve stable electron configurations.
For instance, in the water molecule ( H_2O ), the Lewis structure shows two pairs of dots between the oxygen and hydrogen atoms, depicting the shared electron pairs that form the covalent bonds.

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Most popular questions from this chapter

compounds conduct electricity in fused state or in aqueous solution.

Mention the oxidizing agent, reducing agent in the following redox reactions and give reason in support of your answer. (i) \(\mathrm{Mg}+2 \mathrm{HCl} \rightarrow \mathrm{MgCl}_{2}+\mathrm{H}_{2}\) (ii) \(2 \mathrm{ZnS}+3 \mathrm{O}_{2} \rightarrow 2 \mathrm{ZnO}+2 \mathrm{SO}_{2}\) (iii) \(2 \mathrm{KMnO}_{4}+16 \mathrm{HCl} \rightarrow 2 \mathrm{KCl}+2 \mathrm{MnCl}_{2}+8 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{Cl}_{2}\) (iv) \(2 \mathrm{H}_{2} \mathrm{~S}+\mathrm{SO}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+3 \mathrm{~S}\) (v) \(4 \mathrm{HCl}+\mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{Cl}_{2}\)

What are van der Waal's forces of attraction?

Why is the density of the ionic compounds high and that of covalent compounds low?

Name one solvent in which most of the ionic compounds dissolve.
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