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Analyse the relationship between the position of elements in the Periodic Table, and the acid–base behaviour of their oxides. - HSC - SSCE Chemistry - Question 18 - 2004 - Paper 1
Question 18
Analyse the relationship between the position of elements in the Periodic Table, and the acid–base behaviour of their oxides.
Worked Solution & Example Answer:Analyse the relationship between the position of elements in the Periodic Table, and the acid–base behaviour of their oxides. - HSC - SSCE Chemistry - Question 18 - 2004 - Paper 1
Step 1
Position in the Periodic Table
Answer
The position of an element in the Periodic Table influences its properties significantly. As you move from left to right across a period, the elements transition from metals to nonmetals. This shift affects the nature of their oxides. Metallic oxides generally exhibit basic properties, while nonmetallic oxides are often acidic or amphoteric.
Step 2
Acid-Base Behavior of Oxides
Answer
Metal oxides, such as sodium oxide (Na2O) and calcium oxide (CaO), tend to react with acids to form salts and water, showcasing their basic nature. For instance, they react with hydrochloric acid (HCl) to produce salt and water:
ightarrow 2 ext{NaCl} + ext{H}_2 ext{O}$$. In contrast, nonmetal oxides, like sulfur trioxide (SO3) or carbon dioxide (CO2), react with bases to form salts and water, indicating their acidic behavior. For example, sulfur trioxide reacts with sodium hydroxide (NaOH): $$ ext{SO}_3 + 2 ext{NaOH} ightarrow ext{Na}_2 ext{SO}_4 + ext{H}_2 ext{O}$$.Step 3
Step 4