1. OXIDES AND OXOANIONS OF SULPHUR and NITROGEN
Dr. S.B.Misal
S.M.Joshi College, Hadapsar, Pune-28

2. Oxides of Sulphur
Sulfur oxides(SOx) are the compounds of sulfur and oxygen molecules.
Sulfur has a rich chemistry with oxygen. Sulfur forms strong double bonds to oxygen.
Oxides with sulfur in low oxidation states occur.
Oxides of sulfur
Sulfur dioxide (SO2)
Sulfur trioxide (SO3)
Sulfuric acid (H2SO4)

3. Sulfur dioxide
Sulfur trioxide
Sulfuric acid

4. Oxoanions of Sulfur Oxoanion : Sulphite (SO3)2- Sulphate(SO4)2-
Thiosulphite(S2O3)2-

5. Sulfate ion Oxdn state of sulfur : +6 Oxdn state of each oxygen : -2
Tetrahedral molecular shape
The symmetry is the same as that of methane. The sulfate ion carries a negative two charge and is the conjugate base of the bisulfate (or hydrogen sulfate) ion, HSO−4, which is the conjugate base of H2SO4
The tetrahedral molecular geometry of the sulfate ion is as predicted by VSEPR theory

6. Trigonal pyramidal shape
Sulphite ion
Trigonal pyramidal shape
(like ammonia)
The sulfur atom is double-bonded to one oxygen atom with a formal charge of zero (neutral),
and sulfur is singly bonded to the other two oxygen atoms, which each carry a formal charge of −1, together accounting for the −2 charge on the anion.

7. Tetrahedral molecular shape
Thiosulfate
 Tetrahedral molecular shape
Oxdn state +2
The prefix thio- indicates that the thiosulfate ion is a sulfate ion with one oxygen replaced by sulfur.

8. Dithionite
reducing agent
The dithionite anion ([S2O4]2−), is an oxoanion of sulfur [1] formally derived from dithionous acid, H2S2O4.
Oxdn state +3

9. Oxidation state of sulfur is +5
Dithionate
Oxidation state of sulfur is +5
Resist oxdn and redn
Strong oxidants oxidise them to sulfates and strong reducing agents reduce them to sulfites and dithionites

10. OXIDES & OXOANIONS OF NITROGEN
NAME : YELE POOJA RAMDAS
CLASS : M.Sc (1)
SUBJECT : INORGANIC CHEMISTRY

12. Nitric oxide ,NO
When exposed to oxygen, ·NO is converted into nitrogen dioxide.
2 ·NO + O2 → 2 NO2
This conversion has been speculated as occurring via the ONOONO intermediate. In water, ·NO reacts with oxygen and water to form HNO2 or nitrous acid. The reaction is thought to proceed via the following stoichiometry:
4 ·NO + O2 + 2 H2O → 4 HNO2

13. Nitrogen dioxide NO2
Nitrogen dioxide is the chemical compound with the formula NO 2. It is one of several nitrogen oxides. NO 2 is an intermediate in the industrial synthesis of nitric acid, millions of tons of which are produced each year. At higher temperatures it is a reddish-brown gas that has a characteristic sharp, biting odor and is a prominent air pollutant.[7] Nitrogen dioxide is a paramagnetic, bent molecule with C2v point group symmetry.

14. Nitrous oxide,N2O
Nitrous oxide, commonly known as laughing gas, nitrous, nitro, or NOS [1] is a chemical compound with the formula N 2O. It is an oxide of nitrogen. At room temperature, it is a colorless, non-flammable gas, with a slightly sweet odor and taste. It is used in surgery and dentistry for its anaesthetic and analgesic effects. It is known as "laughing gas" due to the euphoric effects of inhaling it, a property that has led to its recreational use as a dissociative anaesthetic. It is also used as an oxidizer in rocket propellants, and in motor racing to increase the power output of engines. At elevated temperatures, nitrous oxide is a powerful oxidizer similar to molecular oxygen.

15. Dinitrogen trioxide N2O3
Dinitrogen trioxide is the chemical compound with the formula N2O3. This deep blue solid[1] is one of the binary nitrogen oxides. It forms upon mixing equal parts of nitric oxide and nitrogen dioxide and cooling the mixture below −21 °C (−6 °F):[2]
NO + NO2 ⇌ N2O3

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