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
Electrovalency for Some Monoatomic Negatitve Ions
| Valency = 1- | Valency = 2- | Valency = 3- | Valency = 4- | | :--- | :--- | :--- | :--- | | (Monovalent) | (Divalent) | (Trivalent) | Tetravalent | | F^1–^ (Fluoride) | O^2–^ (oxide) | N^3–^ (nitride) | C^4–^ (carbide) | | Cl^1–^ (Chloride | S^2–^ (sulphide) | P^3–^ (phosphide) | | | Br^1–^ (Bromide) | | | | | I^1–^ (Iodide) | | | | | H^1–^ (Hydride) | | | | ** Writing Empirical Formula of Binary Ionic compounds: ** The basic principle for writing the formula (empirical formula) of an ionic compound(neutral) is to make *charge balance*. The total +ve charge of the +ve ions should be equal to the total –ve charge of the –ve ions. The positve ion is written first follwed by the negative ion. **Cross-over Rule: Aluminium oxide:** While writing formula of an
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