Halogens and Their Compounds
Chemistry ⇒ Chemistry of Non-metals and Their Compounds
Halogens and Their Compounds starts at 10 and continues till grade 12.
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Compare and contrast the chemical properties of chlorine and bromine.
Describe the general physical properties of halogens and explain how these properties change as you move down the group in the periodic table.
Describe the laboratory preparation of chlorine gas and mention the chemical equation involved.
Describe the uses of chlorine and iodine in daily life.
Discuss the environmental impact of compounds containing chlorofluorocarbons (CFCs).
Discuss why halogens do not occur in the free state in nature.
Explain the term 'halide' and give examples of halide compounds formed by halogens.
Explain why fluorine is the most reactive halogen and give one industrial use of fluorine.
Explain why halogens are highly reactive and describe the trend in reactivity as you go down the group.
Write a short note on the displacement reactions of halogens with examples.
A sample of bleaching powder contains 35% available chlorine by mass. Calculate the mass of bleaching powder required to provide 21 g of available chlorine.
Chlorine reacts with cold, dilute sodium hydroxide to form sodium chloride, sodium hypochlorite, and water. Write the balanced chemical equation for this reaction. If 7.1 g of chlorine gas (Cl2) is completely reacted with excess sodium hydroxide, calculate the mass of sodium hypochlorite (NaOCl) formed. (Atomic masses: Cl = 35.5, Na = 23, O = 16, H = 1)
Fluorine is the most reactive halogen and can displace other halogens from their compounds. If 100 mL of 0.5 M potassium bromide (KBr) solution is treated with excess fluorine gas, calculate the mass of bromine (Br2) liberated. (Atomic mass: Br = 80)
Iodine can be liberated from potassium iodide (KI) solution by adding chlorine water. Write the balanced chemical equation for this reaction. If 0.2 mol of chlorine gas is bubbled through excess potassium iodide solution, calculate the number of moles of iodine (I2) formed.
When hydrogen chloride gas is dissolved in water, it forms hydrochloric acid. If 3.65 g of hydrogen chloride (HCl) is dissolved in water to make 500 mL of solution, calculate the molarity of the resulting hydrochloric acid. (Atomic masses: H = 1, Cl = 35.5)
