Ionic crystals

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19 Terms

1
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What are the 4 main types of crystal structures?

  • Ionic

  • Metallic

  • Simple molecular (covalent)

  • Macromolecular (Giant covalent structures)

2
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Describe the structure of ionic compounds.

Consists of a lattice of positive and negative ions held together by strong electrostatic forces.

3
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Give examples of ionic compounds.

  • Sodium chloride (NaCl)

  • Caesium chloride (CSCl)

4
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Describe the arrangement of ions in sodium chloride.

  • Each sodium ion is surrounded by 6 chloride ions.

  • Each chloride ion is surrounded by 6 sodium ions.

<ul><li><p>Each sodium ion is surrounded by 6 chloride ions.</p></li><li><p>Each chloride ion is surrounded by 6 sodium ions.</p></li></ul>
5
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What is the coordination number of each sodium ion in NaCl?

6.

6
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What is the coordination number of each chloride ion in NaCl?

6.

7
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What is the coordination number of sodium chloride?

6:6.

8
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What is the crystalline structure of sodium chloride (NaCl)?

Face-centred cubic.

9
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Describe the arrangement of ions in caesium chloride.

  • Each caesium ion is surrounded by 8 chloride ions.

  • Each chloride ion is surrounded by 8 caesium ions.

<ul><li><p>Each caesium ion is surrounded by 8 chloride ions.</p></li><li><p>Each chloride ion is surrounded by 8 caesium ions.</p></li></ul>
10
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What is the coordination number of each caesium ion in caesium chloride?

8.

11
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What is the coordination number of each chloride ion in caesium chloride?

8.

12
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What is the coordination number of caesium chloride?

8:8.

13
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What is the crystalline structure of caesium chloride (CsCl)?

Body-centred cubic.

14
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Why does caesium chloride (CsCl) have a different structure to sodium chloride (NaCl)?

Caesium ion are larger than sodium ion hence it can be surrounded by greater number of chloride ions.

15
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State the properties of ionic compounds.

  • High melting and boiling points

  • Crystalline

  • Brittle

  • Conduct electricity only when molten or dissolved in water.

  • Soluble in polar substances i.e. water.

16
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Why do ionic compounds have high melting and boiling points?

Electrostatic forces holding the ions together are strong and require a lot of energy to break.

17
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Why are ionic compounds brittle?

When an external force is applied, the lattice arragement of ions are disrupted, causing them to break apart.

<p>When an external force is applied, the lattice arragement of ions are disrupted, causing them to break apart.</p>
18
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Why do ionic compounds conduct electricity only when molten / dissolved in water?

When molten / dissolved in water, ions are free to move and so, can transfer electrical charge.

19
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Why are ionic compounds soluble in water?

  • Positve ion from the ionic compound is attracted to the negative end of the water molecule (oxygen).

  • Negative ion is attracted to the positive end of the water molecule (hydrogen).