(a) What is the difference between a mineral and an ore?
(b) Which metal is extracted from cinnabar ore?
(c) Name one ore of sodium. Name the sodium compound present in this ore and write its chemical formula.
(d) How is sodium metal extracted? Explain with the help of the equation of the reaction involved.
(e) Name three other metal s which are extracted in a manner similar to sodium.

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Solution

(a) The differences between a mineral and an ore are listed below:

Mineral Ore

1. Naturally occurring metals or their compounds are called minerals. Minerals containing a good quantity of metals that can be profitably mined are called ores.

2. Minerals may or may not contain metals in large percentages. Ores always contain metals in large percentages.

3. Minerals may or may nor contain objectionable impurities. Ores do not contain objectionable impurities.

4. All minerals are not ores. All ores are minerals.

(b) Mercury is extracted from cinnabar ore. It is the sulphide ore of mercury and its chemical formula is HgS. The name of the compound present in cinnabar is mercury (II) sulphide. It is a sulphide ore; therefore, it is first heated in the presence of surplus air (roasting). This converts mercury (II) sulphide to mercury (II) oxide.

$2 H g S + 3 O_{2} R o a s t i n g (s u r p l u s o f a i r) - -------------- \to 2 H g O + 2 S O_{2}$

Mercury (II) oxide is then heated again to around $300^{0} C$ . On heating, it gets reduced to mercury.
2 $2 H g O H e a t i n g u p t o 300^{0} C - ----------- \to 2 H g + O_{2}$

(c) The ore of sodium is rock salt. The sodium compound present in this ore is sodium chloride. The chemical formula of the ore is NaCl.

(d) Sodium is extracted by the electrolytic reduction of molten sodium chloride. On passing electricity through molten sodium chloride, decomposition occurs and sodium metal and chlorine gas are formed.
$2 N a C l (l) e l e c t r o l y s i s - ------ \to 2 N a (s) + C l_{2} (g)$
Molten sodium chloride contains sodium and chloride ions. The reactions that occur during electrolysis are:

1. The cathode produces electrons to reduce sodium ions to sodium atoms (or sodium metal) by acting as a reducing agent. Sodium ions are cations; therefore, they are attracted to the negatively-charged cathode and get deposited there.

$C a t h o d e :$

$2 N a^{+} S o d i u m i o n s (from molten NaCl) + 2 e^{-} E l e c t r o n s (from cathode) ⟶ 2 N a S o d i u m a t o m s (or sodium metal)$

2. Chloride ions are anions; therefore they are attracted to the positively-charged anode. These chloride ions are oxidised to chlorine gas. Chlorine gas is produced at the anode.

$A n o d e :$

$2 C l^{-} C h l o r i d e i o n s (from molten NaCl) - 2 e^{-} E l e c t r o n s (to anode) ⟶ 2 C l Chlorine gas$

(e) Potassium, calcium and aluminium are highly reactive metals like sodium and are also placed on the top of the reactivity series. These metals are not reduced by other reducing agents such as coke, carbon monoxide etc. Like sodium, these metals are also extracted by electrolytic reduction of their molten chlorides or oxides.

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Mineral	Ore
1. Naturally occurring metals or their compounds are called minerals.	Minerals containing a good quantity of metals that can be profitably mined are called ores.
2. Minerals may or may not contain metals in large percentages.	Ores always contain metals in large percentages.
3. Minerals may or may nor contain objectionable impurities.	Ores do not contain objectionable impurities.
4. All minerals are not ores.	All ores are minerals.