1. Chemical Symbols of Elements
2. Valency
3. Electrovalent (Ionic) Bond and Electrovalency
4. Chemical Formula
5. Electrovalency for Some Monoatomic Negatitve Ions
6. Polyatomic Radicals/Ions (For Ionic Compounds)
7. Negative Ions (Acid radicals) Valency Table
8. Hit and Trial Method (Inspection Method)
9. Complete Chemical Equation
10. Ionic Equations
11. Solubility Rules
12. Broad Classification of Inorganic Reactions
13. Practice Questions
14. Answers to SAQs
15. Answers to Practice Questions
Polyatomic Radicals/Ions (For Ionic Compounds)
** Radicals: ** A group of atoms forming an ion is called a radical. Such a radical or ion contains more than one atoms and hence are polyatomic in nature.
There are two types of radicals, namely
(a) Acid Radicals: –ve ions(anions). Many of them are derived from acids.
(b) Basic Radicals : +ve ions(cations) They are derived from bases.
** Acids and Acid Radicals: ** The substances which can produce hydrogen ions(H+) in water or aqueous solution are called acids(Arrhenius Theory)
$$1) \hspace{0.5cm} H_2SO_4 \Longrightarrow H^+ + HSO_4^{2–}$$
HSO~4~^–^ is the acid radical called hydrogen sulphate or bisulphate radical (ion), which is a polyatomic negative ion. Sulphuric acid (H~2~SO~4~) loses one H+ ion to form HSO~4~^–^ radical.
$$H_2SO_4 \Longrightarrow 2H^+ + SO_4^{2–}$$
SO~4~^2–^ is called sulphate radical (ion). Sulfuric acid can lose two H^+^ ions to form SO~4~^2–^ ion.
So H~2~SO~4~ can form two acid radicals namely HSO~4~^–^ and SO~4~^2–^.
The
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