Positive Radicals (Cations) — Explanation
What they are: Positive radicals are single atoms or groups of atoms that carry a net positive charge. They form when an atom or group loses electrons.
How they form: Metals (Na, Ca, Al) and some polyatomic species (NH4+) lose electrons in reactions such as ionization, acid–base reactions, or salt formation.
Valency & charge: The valency equals the magnitude of the charge (e.g., Na+ has valency 1, Ca2+ has valency 2). Higher charges mean higher valency.
Naming: Use the element name plus oxidation state if needed. Traditional names may use suffixes -ous (lower) and -ic (higher), or IUPAC Roman numerals in brackets.
Common examples (with valency):
- H+ (1), Li+ (1), Na+ (1), K+ (1), Ag+ (1), NH4+ (1)
- Mg2+ (2), Ca2+ (2), Zn2+ (2), Fe2+ (2), Cu2+ (2)
- Al3+ (3), Fe3+ (3), Cr3+ (3)
Role in salts: Cations combine with negative radicals (anions) to make neutral compounds, e.g., Ca2+ + SO42− → CaSO4.
Quick lab hints: Many metal cations give characteristic flame colors (Na: yellow, K: lilac, Ca: brick-red) or distinctive precipitates with reagents (e.g., NH4OH, NaOH).
Negative Radicals (Anions) — Explanation
What they are: Negative radicals are single atoms or groups of atoms that carry a net negative charge. They form when an atom or group gains electrons.
How they form: Non-metals (Cl, O, S, N) and many polyatomic groups (SO42−, NO3−) gain electrons or result from acid deprotonation (e.g., HCl → Cl−).
Valency & charge: The valency equals the magnitude of the negative charge (e.g., Cl− has valency 1, SO42− has valency 2, PO43− has valency 3).
Naming: Monoatomic anions usually end with -ide (chloride, oxide, sulfide). Oxyanions use -ate / -ite (more/less oxygen) and may take prefixes per- (most O) and hypo- (least O).
Common examples (with valency):
- Cl− (1), Br− (1), I− (1), OH− (1), NO3− (1), HCO3− (1), CH3COO− (1)
- SO42− (2), CO32− (2), S2− (2), SO32− (2), CrO42− (2), Cr2O72− (2)
- PO43− (3), BO33− (3)
Role in salts: Anions pair with cations to form neutral salts, e.g., NH4+ + NO3− → NH4NO3.
Quick lab hints: Many anions give characteristic tests: CO32− effervesces with acids (CO2), SO42− forms a white BaSO4 precipitate with BaCl2, Cl− gives white AgCl with AgNO3 (soluble in NH3).
Positive Radicals (Cations)
S.No | Radical Name | Formula | Valency | हिंदी नाम |
---|---|---|---|---|
1 | Ammonium | NH₄⁺ | 1 | अमोनियम |
2 | Sodium | Na⁺ | 1 | सोडियम |
3 | Potassium | K⁺ | 1 | पोटैशियम |
4 | Silver | Ag⁺ | 1 | चांदी |
5 | Hydrogen | H⁺ | 1 | हाइड्रोजन |
6 | Copper(I) | Cu⁺ | 1 | तांबा(I) |
7 | Copper(II) | Cu²⁺ | 2 | तांबा(II) |
8 | Calcium | Ca²⁺ | 2 | कैल्शियम |
9 | Magnesium | Mg²⁺ | 2 | मैग्नीशियम |
10 | Iron(II) | Fe²⁺ | 2 | लोहा(II) |
11 | Iron(III) | Fe³⁺ | 3 | लोहा(III) |
12 | Aluminium | Al³⁺ | 3 | एल्युमिनियम |
13 | Zinc | Zn²⁺ | 2 | जस्ता |
14 | Lead(II) | Pb²⁺ | 2 | सीसा(II) |
15 | Manganese(II) | Mn²⁺ | 2 | मैंगनीज(II) |
Negative Radicals (Anions)
S.No | Radical Name | Formula | Valency | हिंदी नाम |
---|---|---|---|---|
1 | Chloride | Cl⁻ | 1 | क्लोराइड |
2 | Bromide | Br⁻ | 1 | ब्रोमाइड |
3 | Iodide | I⁻ | 1 | आयोडाइड |
4 | Fluoride | F⁻ | 1 | फ्लोराइड |
5 | Hydroxide | OH⁻ | 1 | हाइड्रॉक्साइड |
6 | Nitrate | NO₃⁻ | 1 | नाइट्रेट |
7 | Nitrite | NO₂⁻ | 1 | नाइट्राइट |
8 | Sulphate | SO₄²⁻ | 2 | सल्फेट |
9 | Sulphite | SO₃²⁻ | 2 | सल्फाइट |
10 | Carbonate | CO₃²⁻ | 2 | कार्बोनेट |
11 | Bicarbonate | HCO₃⁻ | 1 | बाइकार्बोनेट |
12 | Phosphate | PO₄³⁻ | 3 | फॉस्फेट |
13 | Acetate | CH₃COO⁻ | 1 | एसीटेट |
14 | Permanganate | MnO₄⁻ | 1 | परमैंगनेट |
15 | Dichromate | Cr₂O₇²⁻ | 2 | डाइक्रोमेट |
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