Period 3 Oxides Flashcards
Give an equation and explain the reaction of Na2O with water
Na2O + H2O -> 2NaOH(aq)
The Na+ and O2- ions dissolves in water and then the O2- ions react with water: O2- + H2O -> 2 OH-
“Dissolves” (i.e. dissolves and then reacts with water to form a solution)
Reaction of MgO with water
MgO + H2O -> Mg(OH)2(aq)
Some Mg2+ & O2- ions dissolve in water (less soluble than Na2O due to higher lattice enthalpy) and then the O2- ions react with water: O2- + H2O -> 2 OH-
“Slightly soluble” (i.e. some dissolves and then reacts with water to form a solution)
The reaction between Al2O3 with water
Insoluble due to very high lattice enthalpy
Insoluble
Reaction of SiO2 with water
Insoluble due to lattice of atoms linked by strong covalent bonds that would have to be broken
Insoluble
Reaction of P4O10 with water
P4O10 + 6H2O ->4H3PO4
H2O molecules attach the delta + P atoms, leading to the release of H+ ions from the water molecules.
Reacts violently
Reaction of SO2 with water
SO2 + H2O -> H2SO3
H2O molecules attach the delta + S atoms, leading to the release of H+ ions from the water molecules.
“Dissolves” (i.e. dissolves and then reacts with water to form a solution)
SO3 with water
SO3 + H2O -> H2SO4
H2O molecules attach the delta+ S atoms, leading to the release of H+ ions from the water molecules.
Reacts violently
Na2O structure and nature of oxide
Ionic and basic
MgO structure and nature of oxide
Ionic (higher melting point than Na2O as the Mg2+ions are smaller and higher charged than Na+)
Basic
Al2O3 structure and nature of oxide
Ionic (not as high a melting point as expected due to some covalent character due to polarising nature of Al3+ ions)
Amphoteric
SiO2 structure and nature of oxide
Giant covalent
Acidic
P4O10 structure and nature of oxide
Simple molecular (but quite a big molecule)
Acidic
Structure SO2 and nature of oxide
Simple molecular
Acidic
SO3 structure and nature of oxide
Simple molecular
Acidic
SO3 structure and nature of oxide
Simple structure
Acidic
