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i) Describe the variation in behavior of the following oxides in water: Na2O, MgO, Al2O3, SiO2, P4O10 , SO2, and Cl2O
ii) Recognise the variations of acid-base properties of the oxides of elements from Na to Cl as exemplified by Na2O, Al2O3 and SO2
Part I- Behaviour in Water
Na2O *ionic oxide
Na2O(s) + H2O(l) → 2NaOH(aq)
❗️❕Na2O reacts with water to form a strongly alkaline solution
MgO *ionic oxide
MgO(s) + H2O(l) → Mg(OH)2(s)
❗️❕MgO reacts slightly with cold water and moderately with hot water to form a slightly alkaline solution
❗️❕Al2O3 does not react with water
❗️❕SiO2 is insoluble in water as it is a covalent oxide with a giant covalent structure
P4O10*covalent oxide
❗️❕Reacts vigorously with cold water to form metaphosphoric acid
P4O10 + 2H2O(l) → 4HPO3(aq)
Reacts with warm water to form phosphoric acid
P4O10 + 6H2O(l) → 4H3PO4 (aq)
SO2*covalent oxide
SO2(g) + H2O(l) → H2SO3(aq)
❗️❕ SO2 reacts with water to form sulphurous acid
Cl2O*covalent oxide
Cl2O(g) + H2O(l) → 2HOCl(aq)
❗️❕Cl2O dissolves in water to form hypochlorous acid
Part II- Acid-base Properties
Na2O⇒ Strongly basic
MgO ⇒ Basic
Al2O3 ⇒Amphoteric
SiO2 ⇒ Acidic
P4O10 ⇒ Acidic
SO2 ⇒ Acidic
Cl2O ⇒ Acidic
❗️❕Compounds which can act as both acids and bases like Al2O3 are called amphoteric
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