Covalent Bonding

Definition

Covalent bonding is a type of chemical bond that involves the sharing of one or more pairs of electrons between atoms. This type of bond is responsible for the formation of many stable molecules and is a fundamental concept in understanding the structure and properties of various substances, including those covered in the topics of 8.3 Multiple Bonds, 18.1 Periodicity, 18.3 Structure and General Properties of the Metalloids, 18.5 Occurrence, Preparation, and Compounds of Hydrogen, and 18.7 Occurrence, Preparation, and Properties of Nitrogen.

5 Must Know Facts For Your Next Test

1. Covalent bonds are formed by the sharing of one or more pairs of electrons between atoms, which allows them to achieve a stable electron configuration.
2. The strength of a covalent bond is determined by the number of shared electron pairs, with multiple bonds being stronger than single bonds.
3. Covalent bonds play a crucial role in the structure and properties of metalloids, which exhibit characteristics intermediate between metals and nonmetals.
4. Hydrogen forms covalent bonds with other elements, such as oxygen and nitrogen, to create a variety of important compounds, including water and ammonia.
5. Nitrogen's ability to form multiple covalent bonds is responsible for its diverse range of compounds and its importance in biological processes.

Review Questions

• Explain how the concept of covalent bonding is relevant to the understanding of multiple bonds (topic 8.3).
  • Covalent bonding is the foundation for understanding multiple bonds, which occur when atoms share more than one pair of electrons. In multiple bonds, such as double and triple bonds, the increased number of shared electron pairs results in stronger and more stable connections between atoms. This knowledge is crucial for comprehending the structure and properties of various molecules, as the presence of multiple covalent bonds can significantly influence their reactivity and behavior.
• Describe how the periodic trends in electronegativity (topic 18.1) can affect the nature of covalent bonds.
  • The periodic trends in electronegativity, which is the ability of an atom to attract shared electrons in a covalent bond, can impact the polarity and strength of covalent bonds. As you move across a period (row) in the periodic table, electronegativity generally increases, leading to the formation of more polar covalent bonds. Conversely, as you move down a group (column), electronegativity typically decreases, resulting in more nonpolar covalent bonds. Understanding these periodic trends is essential for predicting the properties and behavior of covalently bonded substances.
• Analyze how the covalent bonding characteristics of metalloids (topic 18.3) contribute to their unique properties and applications.
  • Metalloids, such as silicon and germanium, exhibit a combination of metallic and nonmetallic properties due to their covalent bonding patterns. The ability of metalloids to form both covalent and metallic bonds allows them to display intermediate characteristics, such as moderate electrical conductivity and the ability to form semiconductors. This versatility in covalent bonding is a key factor in the diverse applications of metalloids, ranging from electronic devices to solar cells. Understanding the relationship between covalent bonding and the structure-property relationships of metalloids is crucial for understanding their unique role in various technological and scientific fields.

Related terms

Polar Covalent Bond:

A covalent bond in which the shared electrons are unequally distributed between the bonded atoms, resulting in a slightly positive and slightly negative charge on the atoms.

Nonpolar Covalent Bond:

A covalent bond in which the shared electrons are equally distributed between the bonded atoms, resulting in no net charge separation.

Sigma (σ) Bond: A type of covalent bond formed by the head-on overlap of atomic orbitals, providing the strongest type of covalent bond.