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HSC Chemistry

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Module 2 | Acidic environment

Focus 2: While we usually think of the air around us as neutral, the atmosphere naturally contains acidic oxides of carbon, nitrogen and sulfur. The concentrations of these acidic oxides have been increasing since the Industrial Revolution.

Lesson 1 | Oxides and Periodic Table

  • Identify oxides of non-metals which act as acids and describe the conditions under which they act as acids

  • Analyse the position of these non-metals in the Periodic Table and outline the relationship between position of elements in the Periodic Table and acidity/basicity of oxides

Lesson 2 | Increasing atmospheric concentration of oxides of sulfur and nitrogen

  • Identify natural and industrial sources of sulfur dioxide and oxides of nitrogen

  • Analyse information from secondary sources to summarise the industrial origins of sulfur dioxide and oxides of nitrogen and evaluate reasons for concern about their release into the environment

  • Describe, using equations, examples of chemical reactions which release sulfur dioxide and chemical reactions which release oxides of nitrogen

Lesson 3 | Acid rain and its effects

  • Explain the formation and effects of acid rain

  • Assess the evidence which indicates increases in atmospheric concentration of oxides of sulfur and nitrogen

Lesson 4 | Calculating gas volumes

  • Calculate volumes of gases given masses of some substances in reactions, and calculate masses of substances given gaseous volumes, in reactions involving gases at 0˚C and 100 kPa or 25˚C and 100 kPa

Lesson 5 | Le Chatelier's Principle

  • Define Le Chatelier’s principle

  • Identify factors which can affect the equilibrium in a reversible reaction

Lesson 6 | Decarbonation of soft drink

  • Identify data, plan and perform a first-hand investigation to decarbonate soft drink and gather data to measure the mass changes involved and calculate the volume of gas released at 25˚C and 100 kPa

  • Describe the solubility of carbon dioxide in water under various conditions as an equilibrium process and explain in terms of Le Chatelier’s principle

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