4.7Chemistry 01. Materials And Their Structure
Describe an ionic bond as an attraction between a positively… — Cambridge Checkpoint Science 0893 Revision Notes & Topical Questions
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4.7 Ionic bonds and ionic compounds — CHECKPOINT - Lower Secondary Science 0893 notes: Describe an ionic bond as the electrostatic attraction between a positively charged ion and a negatively charged ion, and relate the giant structure to the properties of ionic compounds.Ionic b…
- Strong forces
- High melting and boiling points
- Brittle crystals
- Electrical conduction
- Sodium chloride
- Ionic bond — the attraction between a positively charged ion and a negatively charged ion.It is an electrostatic force
Section 1 of 6Ionic bond
- Ionic bond
- the attraction between a positively charged ion and a negatively charged ion.
- It is an electrostatic force.
- Ionic compounds
- compounds made of ions, formed when a metal reacts with a non-metal.
Section 2 of 6Formation of sodium chloride
- A sodium atom loses one electron and becomes a Na+ ion.
- A chlorine atom gains that electron and becomes a Cl- ion.
- The oppositely charged ions attract each other.
- The ionic bond holds them together as sodium chloride, NaCl.
Section 3 of 6Other ionic compounds
| Compound | Ions | Formula |
|---|---|---|
| Sodium chloride | Na+ and Cl- | NaCl |
| Magnesium oxide | Mg2+ and O2- | MgO |
| Magnesium chloride | Mg2+ and two Cl- | MgCl2 |
| Lithium fluoride | Li+ and F- | LiF |
| Potassium chloride | K+ and Cl- | KCl |
- The total positive charge equals the total negative charge in the formula.
Section 4 of 6Giant ionic lattice
- Lattice
- the ions are arranged in a regular pattern in a giant structure.
- In sodium chloride each Na+ ion is surrounded by six Cl- ions.
- Strong forces
- the electrostatic forces act in all directions, so many strong ionic bonds hold the lattice together.
- Crystals
- the regular arrangement gives crystals with a regular shape.
Section 5 of 6Properties of ionic compounds
- High melting and boiling points
- a lot of energy is needed to overcome the strong ionic bonds.
- Brittle crystals
- the regular lattice breaks along flat surfaces.
- Electrical conduction
- they conduct electricity when molten or dissolved because the ions are free to move, but not as solids.
Section 6 of 6Comparison of ionic and covalent bonding
| Feature | Ionic bond | Covalent bond |
|---|---|---|
| Atoms involved | Metal and non-metal | Non-metals |
| Electrons | Transferred | Shared |
| Particles | Ions | Molecules |
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