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Chapter 12: Problem 3

What is meant by a chemical bond?

Short Answer

Expert verified
A chemical bond is the attractive force that holds atoms or ions together in a molecule or crystal to achieve stability and fulfill the octet rule in their outermost electron shell. Atoms bond to lower their potential energy and achieve a more stable electron configuration. There are three main types of chemical bonds: ionic bonds, which involve the transfer of electrons between atoms; covalent bonds, where atoms share electrons; and metallic bonds, where valence electrons move freely through a crystal lattice.

Step by step solution

01

Definition of Chemical Bond

A chemical bond is the attractive force that holds atoms or ions together in a molecule or crystal. Chemical bonds result from the sharing or transfer of electrons between atoms to achieve stability and fulfill the octet rule in their outermost electron shell.
02

Why Atoms Form Bonds

Atoms form bonds to become more stable and achieve the octet rule in their valence electron shell. The octet rule states that elements tend to combine in such a way that they each have eight electrons in their valence shell, similar to the electronic configuration of a noble gas. By forming bonds, atoms can lower their potential energy and achieve a more stable electron configuration.
03

Types of Chemical Bonds

There are three main types of chemical bonds: ionic, covalent, and metallic bonds.
04

Ionic Bonds

Ionic bonds occur when atoms transfer one or more electrons from one atom to another, resulting in the formation of positively-charged and negatively-charged ions. These opposite charges attract each other and form an ionic bond. For example, sodium and chlorine form an ionic bond in table salt (NaCl) due to the transfer of an electron from sodium to chlorine.
05

Covalent Bonds

Covalent bonds are formed when atoms share their valence electrons, allowing both atoms to achieve a stable electron configuration. This shared electron pair is attracted to the nuclei of both atoms, holding them together in a bond. There can be single, double, or triple covalent bonds depending on the number of shared electron pairs. For example, in a water molecule (H2O), the oxygen atom shares electrons with two hydrogen atoms, forming two covalent bonds.
06

Metallic Bonds

Metallic bonds occur in metals, where valence electrons can move freely through the crystal lattice. These free-moving electrons, often referred to as a "sea of electrons," create a strong bond between metal ions. Metallic bonds are responsible for the conductivity and malleability of metals.

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Key Concepts

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

Ionic Bonds
Ionic bonds are a type of chemical bond formed through the complete transfer of one or more electrons from one atom to another. This transfer typically occurs between atoms with significantly different electronegativities, such as metals and non-metals.
  • When the electron is transferred, it results in two ions: one positively charged (cation) and one negatively charged (anion).
  • The electrostatic attraction between these oppositely charged ions forms a strong ionic bond.
  • This type of bonding is commonly seen in compounds like sodium chloride (NaCl) or table salt, where the sodium atom donates an electron to the chlorine atom.
This electron transfer helps both participating atoms achieve a stable electronic configuration resembling the nearest noble gas, in line with the octet rule. Ionic compounds generally have high melting and boiling points due to the strong attractions between ions. Additionally, when dissolved in water, they conduct electricity due to the free-moving ions.
Covalent Bonds
Covalent bonds occur when two or more atoms share pairs of electrons. It allows each atom involved to achieve a stable electron configuration. Typically, this type of bond forms between non-metal atoms.
  • An electron pair is shared between two atoms, creating a bond that holds them together.
  • Depending on the number of shared electron pairs, covalent bonds can be classified as single, double, or triple bonds.
  • For instance, a water molecule (H鈧侽) is formed when oxygen shares electrons with two hydrogen atoms, resulting in two single covalent bonds.
Covalent bonds are characterized by the overlapping of atomic orbitals, which significantly influences the molecule鈥檚 shape and physical properties. These bonds are vital in organic molecules like DNA and proteins, as they offer the flexibility required for biological functions. Molecular compounds composed of covalent bonds have lower melting and boiling points compared to ionic compounds, and they do not conduct electricity in their solid or liquid state.
Metallic Bonds
Metallic bonds are unique to metals, where electrons can move freely across the entire structure. This type of bonding gives metals their characteristic properties.
  • The valence electrons in metallic bonds are not associated with any specific atom and are free to move within the "sea of electrons."
  • This electron mobility allows metals to conduct electricity and heat efficiently.
  • It also affords metals their malleability and ductility, enabling them to be shaped and stretched without breaking.
In a metallic bond, the positively charged metal ions are held together by the negatively charged "sea" of delocalized electrons. This collective attraction between the metal ions and the electron cloud accounts for the strong and flexible nature of metals. This is why metals are commonly used in construction and manufacturing industries where durability and flexibility are crucial.

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Most popular questions from this chapter

True or false? In general, a larger atom has a smaller electronegativity. Explain.

How do we determine the total number of valence electrons for an ion? Provide an example of an anion and a cation, and explain your answer.

How do we deal with multiple bonds in VSEPR theory?

The molecules \(\mathrm{NH}_{3}\) and \(\mathrm{BF}_{3}\) have the same general formula \(\left(\mathrm{AB}_{3}\right)\) but different shapes. a. Find the shape of each of the above molecules. b. Provide more examples of real molecules that have the same general formulas but different shapes.

In a bond between fluorine and iodine, which has more attraction for an electron? Why?
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