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
Electrovalent (Ionic) Bond and Electrovalency
#### Ions:
** +ve ions: ** When a neutral atom loses electron(s), it becomes a positive ion. Metals have small number of electrons in their valence shells and have strong tendency to lose these electrons (low ionization energy). For example, Na has 11 protons (+11 charge) in the nucleus and 11 electrons (–11 charge) in different shells i.e K(2), L(8), M(1). When it loses one electron from the last M shell, it will have 10 electrons(–10 charge), but the +ve charge inside the nucleus remains the same i.e +11. Hence net charge is 1+ (+11–10). Same is the case with other +ve ions.
Note that the ion acquires stable octet or duplet configuration by losing electron(s).
** As many number of electrons an atom loses, same will be the magnitude of +ve charge of the ion. This is nothing but the positive elctrovalancy of the metal atom. **
Ca
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