METAL + METAL (or pure metal) → METALLIC bonding (electron sea)
The Three Types of Chemical Bond
IONIC BONDING:
Occurs between a METAL and a NON-METAL.
The metal TRANSFERS one or more electrons to the non-metal.
Metal becomes a POSITIVE ION (cation). Non-metal becomes a NEGATIVE ION (anion).
OPPOSITE CHARGES ATTRACT — strong electrostatic force holds the ions together.
Example: sodium chloride (NaCl) — Na transfers 1 electron to Cl.
COVALENT BONDING:
Occurs between NON-METALS.
Atoms SHARE pairs of electrons — each shared pair counts as one covalent bond.
Both atoms count the shared electrons as their own — achieving full outer shells.
Example: water (H₂O) — oxygen shares electrons with two hydrogen atoms.
METALLIC BONDING:
Occurs in PURE METALS and ALLOYS.
Metal atoms release their outer electrons into a 'SEA' of delocalised electrons.
Positive metal ions (left behind) are surrounded by and attracted to these free electrons.
The delocalised electrons can move freely throughout the structure.
Example: copper (Cu), iron (Fe), all metals.
Bond Type and Properties
The type of bonding directly determines the properties of the substance:
IONIC compounds:
High melting and boiling points (strong electrostatic forces between ions).
Conduct electricity when molten or dissolved (ions can move).
Usually soluble in water.
COVALENT substances:
Simple molecules: low melting/boiling points (weak forces BETWEEN molecules).
Giant covalent: very high melting points (strong covalent bonds throughout).
Generally do not conduct electricity.
METALLS:
High melting/boiling points (strong metallic bonds).
Excellent electrical and thermal conductors (delocalised electrons).
Malleable and ductile (layers of ions can slide).
⚠️ Common Mistake
The strong bond in a covalent MOLECULE is between atoms within the molecule. The WEAK forces between separate molecules (intermolecular forces) are what give simple molecular substances their LOW melting points. Students often confuse the strong covalent bond (within a molecule) with the weak intermolecular forces (between molecules).
📌 Key Note
Metal + non-metal → ionic (electron transfer). Non-metal + non-metal → covalent (electron sharing). Metal → metallic (electron sea). Bond type determines properties: ionic = high MP, conducts when molten/dissolved; simple covalent = low MP; metallic = conducts, malleable.
🎯 Matching Activity — Match the Bond Type
Match each substance to its bond type and why it forms that way. — drag the symbols on the right to match the component names on the left.
Ionic
Drop here
Covalent
Drop here
Metallic
Drop here
Ionic
Drop here
Covalent
Drop here
Copper wire — metal atoms releasing electrons into a delocalised sea
Water (H₂O) — two non-metals sharing electrons
Carbon dioxide (CO₂) — two non-metals sharing electron pairs
Sodium chloride (NaCl) — metal Na transfers electron to non-metal Cl
Magnesium oxide (MgO) — metal + non-metal, electron transfer
🎯 Test Yourself
Question 1 of 2
1. Which type of bonding occurs between a metal and a non-metal?
2. Magnesium (Group 2) reacts with oxygen (Group 6) to form magnesium oxide. What type of bonding does MgO have?
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