Covalent Bonding

Unit 3

Covalent Bonding

Juan Juan
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Covalent bonding occurs when two atoms share one or more pairs of valence electrons through their inter-aetherspace.

This type of bond typically forms between nonmetal atoms with similar electronegativities. Unlike ionic bonds, covalent bonds create discrete molecules with definite shapes and sizes.

Key Characteristics

  • Electron behavior: Sharing of electron pairs
  • Bond strength: Moderate to very strong (1–10 eV per bond)
  • Melting point: Low to moderate (many are gases or liquids at room temperature)
  • Electrical conductivity: Poor (no free electrons or ions)
  • Solubility: Often soluble in nonpolar solvents
  • Structure: Distinct molecules

Covalent

Types of Covalent Bonds

Bond Type Number of Shared Pairs Example Representation
Single bond 1 pair H–H (hydrogen gas) H:H \text{H} : \text{H}
Double bond 2 pairs O=C=O (carbon dioxide) O::C::O \text{O} :: \text{C} :: \text{O}
Triple bond 3 pairs N≡N (nitrogen gas) N≡N \text{N} \equiv \text{N}

Example: Water (H₂O)

Each hydrogen shares one electron with oxygen. Oxygen shares one electron with each hydrogen, forming two single covalent bonds.

H+O+H→H−O−H \text{H} + \text{O} + \text{H} \rightarrow \text{H} - \text{O} - \text{H}

Common Examples in Daily Life:

Molecule Formula Bond Type(s) Use/Context
Methane CH₄ 4 single C–H bonds Natural gas
Carbon dioxide CO₂ Two C=O double bonds Soda bubbles, respiration
Glucose C₆H₁₂O₆ Multiple single/double bonds Blood sugar
DNA C, H, O, N, P Covalent backbone Genetic material

Polar vs. Nonpolar Covalent Bonds

  • Nonpolar: Electrons shared equally (e.g., H₂, O₂, CH₄)
  • Polar: Electrons shared unequally due to electronegativity difference (e.g., H₂O, NH₃)

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