Ionic lattices and their properties
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Question
What is a giant ionic lattice?
Answer
A regular, repeating **3-D array** of oppositely charged ions, with each ion surrounded by ions of the opposite charge.
Question
What holds an ionic lattice together?
Answer
**Strong electrostatic forces of attraction** between the oppositely charged ions (this is the ionic bond).
Question
Why do ionic compounds have high melting points?
Answer
Many **strong electrostatic attractions** between the ions must be broken, which needs a **large amount of energy**.
Question
What two factors make an ionic bond stronger?
Answer
**Higher ionic charge** and **smaller ionic radius** — both increase the electrostatic attraction.
Question
When does an ionic compound conduct electricity?
Answer
When **molten** or **dissolved in water (aqueous)** — the ions are then **free to move**. Not as a solid.
Question
Why doesn't a solid ionic compound conduct?
Answer
The ions are held in **fixed positions** in the lattice, so no charged particles are free to move.
Question
Why are ionic solids brittle?
Answer
A force makes layers **shift**, bringing **like charges** next to each other; they **repel** and split the crystal.
Question
Why do many ionic compounds dissolve in water?
Answer
Water is **polar**: its δ⁻ oxygen attracts cations and δ⁺ hydrogens attract anions, pulling ions out of the lattice (hydration).
Question
Compare a solid and molten ionic compound for conductivity.
Answer
Solid = ions **fixed**, does **not** conduct. Molten = lattice broken, ions **free to move**, **conducts**.
Question
How can you identify an ionic compound from its properties?
Answer
High melting point + does **not** conduct as a solid + **conducts when molten/aqueous** = ionic.
Question
Why does MgO melt higher than NaCl?
Answer
Mg^{2+} and O^{2−} carry **higher charges** than Na^{+} and Cl^{−}, so the electrostatic attraction is much stronger.
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Topic 2.1 hub
The ionic model
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