Saturday, 17 January 2015

5.2.1 - Laboratory Activity : Preparation of ionic compounds

Laboratory Activity 5.2.1:
Preparation of ionic compounds
Aim: To prepare ionic compounds

» Sodium
» Chlorine gas
» Copper powder
» Magnesium tape
» Iron wool

» Gas jar
» Gas jar spoon
» Crucible
» Forceps
» Bunsen burner

The animation below shows the procedures and observation of the experiment.

(A) Preparation of magnesium oxide
1. A sandpaper is used to clean the magnesium tape which is then rolled into a coil and placed in a crucible.
2. The crucible is heated strongly.
3. All observation are recorded.

(B) Preparation of sodium chloride
1. A small piece of sodium is cut and dry with filter paper.
2. The sodium piece is placed in a gas jar spoon with a forceps.
3. The sodium is gently heated until it starts to burn.
4. The gas jar spoon is placed in a gas jar filled with chlorine gas.
5. All observation are recorded.

(C) Preparation of iron (III) oxide
1. The iron wool is heated strongly until it glows red hot.
2. Dry chlorine gas is passes through the tube for a while.
3. All observation are recorded.
Experiment Observation
(A) Preparation of magnesium oxide Magnesium tape burns with a bright flame to form a white ash.
(B) Preparation of sodium chloride Sodium burns with a bright yellow flame and forms a white powder. The greenish-yellow colour of chlorine disappears.
(C) Preparation of iron (III) oxide Iron glows slowly and forms a reddish-brown substance.

Magnesium combines with oxygen present in air to form a compound called magnesium oxide.
2Mg(s) + O2(g) → 2MgO(s)
Magnesium oxide is an ionic compound made up of Mg2+ and O2- ions.

Sodium chloride is obtained when sodium burns in chlorine.
2Na(s) + Cl2(g) → 2NaCl(s)
Sodium chlorine is made up of Na+ and Cl- ions. NaCl is an ionic compound.

Iron (III) chloride is produced when iron reacts with chlorine.
2Fe(s) + 3Cl2(g) → 2FeCl3(s)
Iron (III) chloride is an ionic compound made up of Fe3+ and Cl- ions. FeCl3 is an ionic compound.

Metals react chemically with non-metals to form ionic compounds.
Metal + non-metal → Ionic compound

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