Ionic and Covalent Bonds in Chemical Bonding
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Ionic and covalent bonds are two fundamental types of chemical bonds that hold atoms together to form molecules.

1. Ionic Bonds:
Ionic bonds form between atoms when there is a large difference in electronegativity, typically between a metal and a nonmetal.
In an ionic bond, one atom essentially donates an electron (or electrons) to another atom, resulting in the formation of positively charged ions (cations) and negatively charged ions (anions).
These oppositely charged ions are then attracted to each other due to electrostatic forces, forming an ionic compound.
Example: Sodium chloride (NaCl), where sodium (Na) donates an electron to chlorine (Cl), resulting in the formation of Na⁺ and Cl⁻ ions, which are attracted to each other to form the ionic compound sodium chloride.

2. Covalent Bonds:
Covalent bonds form between atoms when they share one or more pairs of electrons.
Covalent bonds typically occur between nonmetal atoms with similar electronegativities.
In a covalent bond, each atom contributes one or more electrons to the shared pair, resulting in the formation of a molecule.
Covalent bonds can be further classified into single, double, or triple bonds based on the number of electron pairs shared between atoms.
Example: Hydrogen molecule (H₂), where each hydrogen atom shares a pair of electrons, forming a covalent bond and resulting in the stable molecule of hydrogen gas.

In summary, ionic bonds involve the transfer of electrons from one atom to another, resulting in the formation of ions, while covalent bonds involve the sharing of electrons between atoms to achieve a stable electron configuration.

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