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Chapter 12: Problem 1

In general terms, what is a chemical bond?

Short Answer

Expert verified
A chemical bond is a force of attraction between atoms or ions that holds them together in a stable structure due to the interactions between their electrons. There are three main types of chemical bonds: ionic, covalent, and metallic. Ionic bonds form between a metal and a non-metal atom and involve the transfer of electrons, creating charged ions that attract each other. Covalent bonds form between two non-metal atoms and involve the sharing of electrons, which can be in single, double, or triple pairs. Metallic bonds occur in metals where electrons are shared among all atoms in a metal lattice, leading to properties such as high conductivity and malleability.

Step by step solution

01

Understanding Chemical Bonds

A chemical bond is a force of attraction between atoms or ions that holds them together in a stable structure. These forces occur due to the interactions between electrons of the atoms or ions involved. Chemical bonds are essential for understanding the properties and behavior of compounds in chemistry.
02

Types of Chemical Bonds

There are three main types of chemical bonds: ionic, covalent, and metallic. We will provide a brief overview of each type below. 1. Ionic Bonds: Formed between a metal and a non-metal atom, ionic bonds occur when one atom transfers its electron(s) to another atom. This transfer results in both atoms forming charged particles called ions. The oppositely charged ions then attract each other, creating an ionic bond. 2. Covalent Bonds: Covalent bonds form between two non-metal atoms. This type of bond occurs when atoms share their electrons to form a bond. The electrons in this shared pair are attracted to the nuclei of both atoms, which holds them together in a molecule. Covalent bonds can be single, double, or triple, depending on the number of electron pairs shared between the atoms. 3. Metallic Bonds: Found in metals, metallic bonds involve the sharing of electrons between all the atoms in a metal lattice. The electrons are not associated with any specific atom, but instead are free to move throughout the entire structure. This "sea" of electrons leads to the unique properties of metals, such as their high conductivity and malleability.

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Key Concepts

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

Ionic Bonds
Ionic bonds form when there is a transfer of electrons between atoms, specifically between a metal and a non-metal. Metals tend to lose electrons and become positively charged ions, while non-metals gain those electrons to become negatively charged ions. These opposite charges create a strong electrostatic force that holds the ions together. One common example of an ionic bond is found in sodium chloride (NaCl), where sodium (a metal) donates an electron to chlorine (a non-metal).
  • Formation: Involves the complete transfer of valence electrons from one atom to another.
  • Resulting Ions: Positive and negative ions are formed, leading to strong attraction.
  • Properties: Ionic compounds typically have high melting and boiling points due to the strong interactions between ions.
    They are often soluble in water and can conduct electricity when dissolved.
This type of bond is essential in forming compounds with distinct properties that are vital in various applications and natural processes.
Covalent Bonds
In covalent bonds, atoms share pairs of electrons, creating a bond that holds them together. This type of bond typically occurs between two non-metal atoms. The shared electrons allow each atom to attain the electron configuration of a noble gas, achieving stability. Covalent bonds can vary in strength and are characterized by the number of electron pairs shared:
  • Single Bonds: Involves one shared pair of electrons (e.g., H2 molecule).
  • Double Bonds: Involves two shared pairs of electrons (e.g., O2 molecule).
  • Triple Bonds: Involves three shared pairs of electrons (e.g., N2 molecule).
The properties of covalent compounds depend largely on the arrangement and nature of the covalent bonds within them. They usually have lower melting and boiling points compared to ionic compounds. Depending on the substance, they can be gases, liquids, or solids at room temperature.
Metallic Bonds
Metallic bonds are unique to metals and they involve the sharing of electrons among a lattice of metal atoms. Unlike ionic or covalent bonds, metallic bonds feature a "sea of electrons" that are not tied to any specific atom. This delocalization means electrons can move freely, which is a key reason behind many of the typical properties of metals.
  • Electron Delocalization: Electrons move throughout the metal's structure, allowing for conductivity.
  • Malleability and Ductility: Metals can easily be shaped or drawn into wires because the bonding is not directional.
  • Luster: The free electrons can reflect light, giving metals their shiny appearance.
These characteristics are what make metals so valuable in electrical applications and construction, giving them a unique place among bonding types.

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Most popular questions from this chapter

Which of the following statements is false concerning bonding? Elements with extremely different electronegativities tend to form ionic bonds with each other. b. In an \(\mathrm{N}-\mathrm{O}\) bond, electron density is greater near the \(\mathrm{O}\) atom. c. An \(\mathrm{N}-\mathrm{O}\) bond is an example of a polar covalent bond. d. In general, chemical bonds form to minimize energy. e. The bond in \(\mathrm{KBr}\) is formed by sharing electrons.

Which of the following molecules contain polar covalent bonds? a. phosphorus, \(\mathrm{P}_{4}\) b. oxygen, \(\mathrm{O}_{2}\) c. ozone, \(\mathrm{O}_{3}\) d. hydrogen fluoride, HF

Give the total number of valence electrons in each of the following molecules. a. \(\mathrm{N}_{2} \mathrm{O}\) b. \(\mathrm{B}_{2} \mathrm{H}_{6}\) c. \(\mathrm{C}_{3} \mathrm{H}_{8}\) d. \(\mathrm{NCl}_{3}\)

How many electrons are involved when two atoms in a molecule are connected by a "double bond"? Write the Lewis structure of a molecule containing a double bond.

Which bond in each of the following pairs has less ionic character? a. \(\mathrm{Na}-\mathrm{O}\) or \(\mathrm{Na}-\mathrm{N}\) b. \(\mathrm{K}-\mathrm{S}\) or \(\mathrm{K}-\mathrm{P}\) c. \(\mathrm{Na}-\mathrm{Cl}\) or \(\mathrm{K}-\mathrm{Cl}\) d. \(\mathrm{Na}-\mathrm{Cl}\) or \(\mathrm{Mg}-\mathrm{Cl}\)
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