State how the acid/base character of the Period 3 oxides changes from Na to S.
State and explain how the maximum oxidation number of the Period 3 elements in their oxides changes from Na to S.
Sodium oxide and phosphorus(V) oxide each react with water. State the product formed in each case.
Explain why phosphorus(V) oxide melts at about $300^{\circ}\text{C}$, yet magnesium oxide melts at about $2850^{\circ}\text{C}$.
Write an equation for the reaction of aluminium oxide, $\text{Al}_2\text{O}_3$, with excess aqueous hydrochloric acid.
Write an equation for the reaction of aluminium oxide, $\text{Al}_2\text{O}_3$, with excess aqueous sodium hydroxide.
Describe the lattice structure of silicon(IV) oxide. Your response should refer to the arrangement of the silicon and oxygen atoms and the bonds joining them.
Sodium oxide and silicon(IV) oxide combine to make sodium silicate(IV), $\text{Na}_2\text{SiO}_3$. Write an equation for the reaction between sodium oxide and silicon(IV) oxide.
Sodium oxide is produced by the thermal decomposition of sodium carbonate. Write an equation for the thermal decomposition of sodium carbonate to form sodium oxide and carbon dioxide.