Types of Chemical Bonds

Types of Chemical Bonds

Ionic Bonds

• Formed between two atoms with a large difference in electronegativity (≥ 1.7)
• One atom loses an electron(s) to become a cation, while the other atom gains an electron(s) to become an anion
• Electrons are transferred from one atom to another, resulting in the formation of ions with opposite charges
• Attractive forces between the oppositely charged ions hold them together
• Typically found in compounds between metals and nonmetals

Covalent Bonds

• Formed between two atoms with a small difference in electronegativity (≤ 1.7)
• Atoms share one or more pairs of electrons to form a bond
• Electrons are shared between atoms, resulting in a covalent bond
• Can be polar or nonpolar, depending on the difference in electronegativity between the atoms
• Found in molecules, including those composed of nonmetals and some metals

Characteristics of Bonds

• Bond Strength: Ionic bonds are generally stronger than covalent bonds
• Bond Polarity: Covalent bonds can be polar, while ionic bonds are always polar
• Bond Formation: Ionic bonds involve electron transfer, while covalent bonds involve electron sharing
• Bond Type: Ionic bonds are typically found in solids, while covalent bonds are found in molecules (gases, liquids, and solids)

Examples

• Ionic bond: NaCl (sodium chloride), where sodium loses an electron to become a cation and chlorine gains an electron to become an anion
• Covalent bond: H2 (hydrogen gas), where two hydrogen atoms share a pair of electrons to form a bond
• Polar covalent bond: HCl (hydrogen chloride), where the difference in electronegativity between hydrogen and chlorine results in a partial positive charge on hydrogen and a partial negative charge on chlorine

Chemical Bonds

• Ionic bonds form between atoms with a significant difference in electronegativity (≥ 1.7).
• In ionic bonds, one atom loses an electron(s) to become a cation, while the other atom gains an electron(s) to become an anion.
• Ionic bonds involve the transfer of electrons from one atom to another, resulting in the formation of ions with opposite charges.
• Attractive forces between the oppositely charged ions hold them together.
• Ionic bonds are typically found in compounds between metals and nonmetals.

Covalent Bonds

• Covalent bonds form between atoms with a small difference in electronegativity (≤ 1.7).
• Covalent bonds involve the sharing of one or more pairs of electrons between atoms.
• The sharing of electrons results in a covalent bond.
• Covalent bonds can be polar or nonpolar, depending on the difference in electronegativity between the atoms.
• Covalent bonds are found in molecules, including those composed of nonmetals and some metals.

Bond Characteristics

Bond Strength

• Ionic bonds are generally stronger than covalent bonds.

Bond Polarity

• Covalent bonds can be polar, while ionic bonds are always polar.

Bond Formation

• Ionic bonds involve electron transfer, while covalent bonds involve electron sharing.

Bond Type

• Ionic bonds are typically found in solids, while covalent bonds are found in molecules (gases, liquids, and solids).

Examples of Bonds

• NaCl (sodium chloride) is an example of an ionic bond, where sodium loses an electron to become a cation and chlorine gains an electron to become an anion.
• H2 (hydrogen gas) is an example of a covalent bond, where two hydrogen atoms share a pair of electrons to form a bond.
• HCl (hydrogen chloride) is an example of a polar covalent bond, where the difference in electronegativity between hydrogen and chlorine results in a partial positive charge on hydrogen and a partial negative charge on chlorine.