CC6 Covalent bonding mind map

Shared electrons

• Bond: Shared electron pair attracted to both nuclei
• Pairs: Single / double / triple bonds share 1 / 2 / 3 pairs
• Dot and cross: Count shared and lone pairs; symbols distinguish origin
• Double bonds: O₂: O=O; CO₂: O=C=O, four shared pairs total
• Element / compound: O₂ contains one element; CO₂ contains two

Single bonds

• H₂ / Cl₂: One shared pair; Cl has three lone pairs per atom
• Water: Two O–H bonds; oxygen has two lone pairs
• Ammonia: Three N–H bonds; nitrogen has one lone pair
• Methane: Four C–H bonds; no lone pairs on carbon
• Shape / scale: Molecules not necessarily flat; HCl shares one pair; tiny scale

Molecular matter

• State changes: Overcome weak intermolecular forces, not covalent bonds
• Electricity: Usually no mobile ions / electrons; neutral motion ≠ current
• Conditions: Solubility varies; HCl ionises in water and conducts
• Exception: Giant covalent networks differ from small molecules

Polymers / models

• Chains: Monomers chemically link into polymer molecules
• Addition: Ethene → poly(ethene); C=C becomes C–C links
• Properties: Strong chain bonds; between-chain attractions matter
• Models: Ball / stick shows bonds; space filling shows occupied space
• Limits: Dot / cross counts electrons, not real shape or bond length

Connections

• Shared electrons → Single bonds: Shared pairs build the bonds in molecules.
• Shared electrons → Molecular matter: Strong bonds within molecules differ from forces between them.