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Chapter 6: Problem 2

Describe the difference between a shared pair and an unshared pair of electrons.

Short Answer

Expert verified
Shared pairs of electrons, also called bonding pairs, are the pairs of electrons that are shared between two atoms in a chemical bond, each atom contributes one electron to form this pair. Unshared pairs of electrons or lone pairs are not involved in bonding and belong entirely to one atom, thus reside in one atom only.

Step by step solution

01

Define Electron Pairs

Electronic pairs refer to two electrons occupying the same orbital in an atom. These pairs of electrons may exist in an atom independently, or they can also be part of a chemical bond with another atom. Here differentiates a shared pair and an unshared pair of electrons.
02

Explain a Shared Pair of Electrons

Shared pairs of electrons, often referred to as bonding pairs, are the pairs of electrons that are shared between two atoms, and thus, participate in bond formation. They create covalent bonds, which means both atoms in the bond contribute one electron to form a pair.
03

Explain an Unshared Pair of Electrons

An unshared pair of electrons, otherwise known as lone pairs, nonbonding pairs, or lone pairs, are two electrons that reside on one atom only. These pairs of electrons do not participate in bond formation and belong entirely to one atom.

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Key Concepts

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

Shared Pair of Electrons
Shared pairs of electrons are at the heart of many chemical bonds, particularly covalent bonds. When two atoms come together, they can form a strong connection by sharing a pair of electrons.
  • Each atom involved in the bond contributes one electron to the shared pair.
  • These shared electrons orbit both nuclei, creating a stable link between the atoms.
  • This sharing often leads to the filling of the outer electron shells, bringing stability to the molecule.
Sharing electrons allows atoms to achieve a more stable electronic arrangement, often resembling the nearest noble gas configuration. This process is fundamental in forming molecules such as H鈧侽, where each hydrogen atom shares one of its electrons with the oxygen atom, leading to two shared pairs of electrons between them.
Unshared Pair of Electrons
Unshared pairs of electrons, also known as lone pairs, are electrons that are not involved in chemical bonding. They typically belong solely to one atom in a molecule and can influence a molecule's shape and reactivity.
  • Lone pairs occupy space and can push away bonding pairs, affecting molecular geometry.
  • They play a crucial role in defining the physical and chemical properties of molecules.
  • While they do not form bonds, lone pairs can participate in chemical reactions.
For instance, in a water molecule, the oxygen atom has two unshared pairs of electrons. These lone pairs create a bent shape for the water molecule and affect properties like boiling point and solubility. The presence of lone pairs often leads to interesting molecular behaviors, influencing how molecules interact in a solution.
Covalent Bonds
Covalent bonds are a type of chemical bond where atoms share electrons to achieve stability. They are pivotal in forming the structures of many substances we encounter daily, such as plastics, proteins, and diamond.
  • In a covalent bond, each pair of shared electrons counts towards the valence shell of both bonded atoms.
  • These bonds are generally quite strong and need a significant amount of energy to break.
  • There can be single, double, or even triple covalent bonds, depending on the number of electron pairs shared.
Covalent bonding creates molecules, with shared pairs of electrons being responsible for holding the atoms together. For example, in carbon dioxide (\( CO_2 \)), each oxygen atom forms a double covalent bond with the carbon atom, sharing two pairs of electrons. Understanding covalent bonds helps explain molecular structure, polarity, and interactions within compounds.

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Most popular questions from this chapter

Draw the Lewis structures for boron, nitrogen, and phosphorus.

Draw Lewis structures for the following polyatomic ions. a. \(\mathrm{OH}^{-}\) b. \(\mathrm{O}_{2}^{2-}\) c. \(\mathrm{NO}^{2-}\) d. \(\mathrm{NO}^{2+}\) e. \(\mathrm{AsO}_{4}^{3-}\)

How does a Lewis structure show a bond between two atoms that share four electrons?

a. What causes \(\mathrm{H}_{2} \mathrm{O}\) to have a bent shape rather than a linear shape? b. How does this bent shape relate to the polarity of the water molecule?

How are the inner-shell electrons represented in a Lewis structure?
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