Definition: Dipoles form in polar covalent bonds when specific conditions are met, including appropriate electronegativity differences (0.4 < ΔE < 1.4) and molecular geometry.

Example: Water (H₂O) is a dipole molecule with a bent structure at 105°, while CO₂ is non-polar due to its linear structure.

Highlight: Ionic bonds form between cations and anions when the electronegativity difference exceeds 1.9.

Vocabulary: Coordination (donor-acceptor) bonds form when one atom donates both electrons for sharing.

Example: The formation of Na+ and Cl- ions demonstrates ionic bonding, where complete electron transfer occurs between atoms.

Definition: Non-polar covalent bonds form between identical non-metal atoms through equal sharing of valence electrons.

Example: In nitrogen molecules (N₂), electrons are shared equally between atoms, represented as :N≡N:

Highlight: For non-polar covalent bonds, the electronegativity difference (ΔE) must be less than 0.4.

Vocabulary: Polar covalent bonds occur between different non-metal atoms with electronegativity differences between 0.4 and 1.7.

Example: In HCl molecules, the electron pair shifts toward chlorine due to its higher electronegativity (Cl: 3.0 > H: 2.1).