Question

Describe the type and nature of the bonding that often occurs between two nonmetals.

Short answer

Nonmetals usually form covalent bonds by sharing electron pairs. These bonds can be single, double, or triple, leading to the formation of stable molecules.

Step-by-step solution

Identify the Type of Bonding

When two nonmetals bond together, they typically form a covalent bond. This type of bond involves the sharing of electron pairs between atoms.

Describe Covalent Bonding

Covalent bonding occurs when two nonmetal atoms share one or more pairs of electrons to achieve a stable electron configuration. This is because nonmetals generally have high electronegativities and similar affinities for electrons.

Differentiate Between Single, Double, and Triple Bonds

Covalent bonds can be single (one pair of shared electrons), double (two pairs of shared electrons), or triple (three pairs of shared electrons). The more pairs of electrons shared, the stronger and shorter the bond.

Explain Electron Sharing and Molecular Formation

In a covalent bond, the shared electrons allow each atom to attain the electron configuration of noble gases, thus forming a stable molecule. For example, in a water molecule (H₂O), each hydrogen atom shares one electron with the oxygen atom, resulting in two single covalent bonds.

Illustrate with Examples

Examples of covalent bonding include the formation of H₂ (hydrogen gas), O₂ (oxygen gas), and CH₄ (methane). In each of these molecules, the atoms share electrons to achieve stability.

Key concepts

nonmetals

In the periodic table, nonmetals are located on the right side. They include elements like hydrogen, carbon, nitrogen, oxygen, fluorine, and chlorine. Nonmetals have unique properties:

• They are often poor conductors of heat and electricity.
• They can exist in different states: gases (like oxygen), liquids (like bromine), or solids (like carbon).
• Nonmetals usually have high electronegativities, meaning they attract electrons more strongly.

When nonmetals interact with each other, their tendency is to share electrons rather than transfer them completely. This electron sharing leads to covalent bonding.

electron sharing

Electron sharing is the hallmark of covalent bonding. In a covalent bond, nonmetal atoms share pairs of electrons to create a stable outer electron shell. This shared pair of electrons belongs to both atoms in the bond.

Why do atoms share electrons? Nonmetals have similar electron affinities and high electronegativities, which means they do not easily give up electrons. Instead, they share to fill their valence shells, achieving a stable electron configuration, much like noble gases.

For example, two chlorine atoms (each needing one electron) will share one pair of electrons to form a covalent bond, creating a Cl₂ molecule.

molecular formation

Molecular formation involves atoms bonding together to create molecules. Nonmetal atoms commonly form molecules by sharing electrons in covalent bonds. The stable arrangement of electrons achieved through sharing creates a molecule.

Consider the water molecule (H₂O) as an example:

• Each hydrogen atom shares one electron with the oxygen atom.
• This results in two single covalent bonds.
• The oxygen atom now has a full outer shell, and each hydrogen atom feels like it has two electrons, resulting in a stable configuration.

Different combinations of nonmetals and electron sharing patterns lead to a vast diversity of molecules with unique properties.

single bond

A single bond involves one pair of shared electrons between two atoms. This is the simplest type of covalent bond. Single bonds are found in numerous molecules. They are generally represented by a single line between two atoms. Example:

• In a hydrogen molecule (H₂), two hydrogen atoms share one pair of electrons, forming a single bond.
• In methane (CH₄), each hydrogen atom shares one electron pair with a carbon atom, creating four single bonds around the carbon atom.

Single bonds provide a strong and stable connection between atoms while allowing flexibility in the molecule's structure.

double bond

A double bond involves two pairs of shared electrons. It is stronger and shorter than a single bond. You can represent a double bond by drawing two lines between the bonded atoms.

Here are some examples:

• In an oxygen molecule (O₂), each oxygen atom shares two pairs of electrons with the other oxygen atom, forming a double bond.
• In carbon dioxide (CO₂), carbon forms double bonds with two oxygen atoms.

Double bonds affect the molecule's shape and reactivity. The additional shared electrons create a more rigid and stable bond compared to a single bond.

triple bond

A triple bond involves three pairs of shared electrons. It is the strongest and shortest of the covalent bonds. Triple bonds are depicted by three lines between atoms.

Examples include:

• In a nitrogen molecule (N₂), two nitrogen atoms share three pairs of electrons, forming a very strong triple bond.
• In acetylene (C₂H₂), each carbon atom shares three pairs of electrons with another carbon atom, forming a triple bond.

Triple bonds create very stable and rigid structures. However, they also make the molecules less flexible in terms of shape and movement.