Metals and Non-metals
What are amphoteric oxides? Give two examples. Write balanced chemical equations showing the reaction of aluminium oxide ($Al_2O_3$) with both hydrochloric acid ($HCl$) and sodium hydroxide ($NaOH$).
Show the formation of magnesium chloride ($MgCl_2$) by the transfer of electrons between magnesium and chlorine atoms. Why do ionic compounds have high melting points?
Differentiate between Roasting and Calcination with suitable chemical equations. In which step of metallurgy are these processes used?
What are amphoteric oxides? Identify two amphoteric oxides from the following list: $\text{Na}_2\text{O}$, $\text{Al}_2\text{O}_3$, $\text{CaO}$, $\text{ZnO}$. Write balanced chemical equations showing the reaction of one of these amphoteric oxides with both an acid and a base.
Explain the formation of Magnesium Chloride ($\text{MgCl}_2$) by the transfer of electrons. State two general physical properties of ionic compounds.
What is the Thermite Process? Write the chemical equation for the reaction involved. State one important practical application of this process and explain why it is highly exothermic.
What is the thermite reaction? Write the balanced chemical equation for the reaction of iron(III) oxide with aluminium. State two practical applications of this reaction.
What are amphoteric oxides? Give two examples of amphoteric oxides and write balanced chemical equations to show the reaction of aluminium oxide with both an acid and a base.
Explain the process of extraction of metals of medium reactivity from their carbonate and sulphide ores with balanced chemical equations. Also, describe the process of refining impure copper by the electrolytic method with a neat diagrammatic description.
Answer the following questions regarding the chemical properties of metals and non-metals: (a) What are amphoteric oxides? Give two examples of amphoteric oxides and write balanced chemical equations for their reactions with both acids and bases. (b) Explain how metals react with water. Compare the reactions of Sodium, Calcium, Magnesium, and Iron with water, providing balanced chemical equations for each.
Explain the extraction process of metals from their ores based on their position in the activity series. Specifically detail:
- Extraction of metals low in the reactivity series (with suitable chemical equations).
- Differentiate between Roasting and Calcination with chemical equations for metals in the middle of the reactivity series.
(a) What is corrosion? Explain the conditions required for the rusting of iron, and describe three effective methods used to prevent corrosion. (b) Numerical Problem: A blast furnace process uses pure Hematite ore ($Fe_2O_3$) to extract iron metal according to the reaction: $$Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)$$\nCalculate the maximum theoretical mass of pure iron (in grams) that can be extracted from $800\text{ g}$ of pure Hematite ($Fe_2O_3$). (Given atomic masses: $Fe = 56\text{ u}$, $O = 16\text{ u}$)
Explain the steps involved in the extraction of metals of medium reactivity from their carbonate and sulphide ores. Support your answer with balanced chemical equations. Additionally, explain the process of electrolytic refining of impure copper with a step-by-step description and electrode reactions.
(a) Differentiate between roasting and calcination with balanced chemical equations using zinc ores as examples.
(b) Explain the process of electrolytic refining of copper with a clear description of the setup, electrodes used, and the chemical reactions involved at both electrodes.