these sides for those students who's studying in class ninth. it is very important topic of chemistry

1. *BINARY*
COMPOUNDS OF
OXYGEN
Edited by → Waseem Ahmed Bhatti (M.Sc Chemistry)
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Contact No: → 0302-3095007 – 0314-7732937

2. OXIDES
- The binary compounds of oxygen
with metals and non-metals are called
as oxides.
Example
CaO, CO2, Fe2O3, H2O etc

3. CLASSIFICATION OF OXIDES
- On the basis of valence number of oxidation
state of oxygen, oxides are classified into
several groups, namely
✓ Normal Oxides
✓ Peroxides
✓ Super Oxides
✓ Sub Oxides.

4. I- NORMAL OXIDES
- Normal oxides are those
oxides in which oxygen
shows normal oxidation state
or valence number – 2.

5. CLASSIFICATION OF NORMAL OXIDES
- Normal oxides are further classified into
four types on the basis of their chemical
characteristics.
✓Basic oxides
✓Acidic oxides
✓Amphoteric oxides
✓Neutral oxides

6. 1- BASIC OXIDES
- The normal oxides of metal are the examples of basic oxides
4Na(s) + O2(g) → 2Na2O(s)
2Pb(s) + O2(g) → 2PbO
▪ Most of these oxides are soluble in water and produce their
hydroxides and turn red litmus blue
CaO(s) + H2O(l) → Ca(OH)2(s)
▪ They also react with acids to form salt and water
MgO(s) + 2HCl → MgCl2(aq) + H2O(l)

7. II- ACIDIC OXIDES
- The normal oxides of non-metal are generally acidic
S(s) + O2(g) → SO2(s)
C(s) + O2(s) → CO2(g)
▪ These oxides are react with water to form acids and turn blue litmus red
SO2(s) + H2O(l) → H2SO3(aq)
▪ Acidic oxides of non-metal react with alkalies to form salts and water
CO2(g( + 2NaOH(s) → Na2CO3

8. III- AMPHOTERIC OXIDES
- Oxygen with less electropositive metals like aluminum, zinc and
tin etc form oxides that posses dual characteristics acidic as well
as basic. These oxides are known as amphoteric oxides.
4Al(s) + 3O2(g) → 2Al2O3(s)
2Zn(s) + O2(g) → 2ZnO(s)
Amphoteric oxides can react with acids and alkalies to form salts
and water.

9. AMPHOTERIC PROPERTIES OF ACIDIC AND
BASIC
With Acid
- Amphoteric oxides react with acids, behaving just like
bases to form salts and water.
Al2O3(s) + 6HCl(g) → 2AlCl3(s) + 3H2O(l)
With Base
- Amphoteric oxides react with alkalies behaving just lie acids
to form salts and water.
Al2O3(s) + 2NaOH(aq) → 2NaAlO2(aq) + H2O(l)

10. IV- NEUTRAL OXIDES
- Neutral oxides are neither acidic nor basic.
They are neutral to litmus in aqueous
solution.
- For Example
→ Water (H2O)
→ Nitric acid (NO)
→ Carbon monoxide (CO)

11. II- PEROXIDES- Peroxides are oxides containing higher proportion of oxygen
as compared to normal oxides.
In these oxides, oxygen has an oxidation state or valence
number -1.
Example
- Sodium peroxide (Na2O2)
- Barium peroxide (BaO2)
- Hydrogen peroxide (H2O2)
- They produce hydrogen peroxide with acids
Na2O2(s) + 2HCl(aq) → 2NaCl(aq) + H2O2(aq)

12. III- SUPER OXIDES
- The elements of group IA potassium, rubidium and cesium form super
oxide. These contain more oxygen than peroxides.
In these oxides, oxygen has an oxidation state or valence number - ½.
They do not produce hydrogen peroxide with acid, rather they show the
tendency to release oxygen (O2) on heating and are powerful oxidizing
agents.
Example
- Potassium superoxide (KO2)
- Rubidium superoxide (RbO2)
- Cesium superoxide (CsO2)

13. IV- SUBOXIDES
- Suboxides have less quantity of oxygen
than the normal oxides.
- They are unstable.
- Very few suboxides are known.
Example
→ Carbon suboxide (C3O2)