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
Complete Chemical Equation
If the balanced equation is to look complete in all respects, then we have to put all the states of the species, the conditions of reactions.
(s) : solid(insoluble solid)
(l) : liquid
(g) : gas
(aq.): aqueous (soluble in water)
$$CaCO_3(s) + heat \xrightarrow{1070-1270K} CaO(s) + CO_2(g)$$
$$N_2(g) + 3H_2(g) \xrightarrow[700K/200 atm]{FeO(k_2O + Al2O_3)} 2NH_3(g) + 22.4 Kcals$$
$$NaOH(aq.) + HCl(aq) \rightarrow NaCl(aq.) + H_2O(l) + 13.6 kcals$$
In the first example, heat is absorbed (endothermic reaction) and the in the 2^nd^ and 3^rd^ examples, heat is liberated (exothermic reactions).
**IMPORTANCE OF A BALANCED CHEMICAL EQUATION:**
Besides giving the reactants and products, a balanced equation gives the following.
(a) Reaction Stoichiometry: How many atoms or molecules of the reactants undergo chemical reactions to produce how many atoms or molecules of the products.
$$2KClO_3 \rightarrow 2KCl + 3O_2$$
From the above example, we understand that 2 molecules (actually 2
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