IGCSE CHEMISTRY SECTION 2 LESSON 5 Content The iGCSE Chemistry course Section 1 Principles of Chemistry Section 2 Chemistry of the Elements Section 3 Organic Chemistry Section 4 Physical Chemistry Section 5 Chemistry in Society Content Section 2 Chemistry of the Elements a) b) c) d) e) f) g) The Periodic Table Group 1 Elements Group 7 Elements Oxygen and Oxides Hydrogen and Water Reactivity Series Tests for ions and gases Lesson 5 g) Tests for ions and gases g) Tests for ions and gases 2.37 describe tests for the cations: i Li+, Na+, K+, Ca2+ using flame tests ii NH4+, using sodium hydroxide solution and identifying the ammonia evolved iii Cu2+, Fe2+ and Fe3+, using sodium hydroxide solution 2.38 describe tests for the anions: i Cl-, Br- and I-, using dilute nitric acid and silver nitrate solution ii SO42-, using dilute hydrochloric acid and barium chloride solution iii CO32-, using dilute hydrochloric acid and identifying the carbon dioxide evolved 2.39 describe tests for the gases: i hydrogen ii oxygen iii carbon dioxide iv ammonia v chlorine. What’s a cation (and now we mention it, what’s an anion?) What’s a cation (and now we mention it, what’s an anion?) What’s a cation (and now we mention it, what’s an anion?) Cations are positively charged ions What’s a cation (and now we mention it, what’s an anion?) Cations are positively charged ions Cations are positively charged ions Sodium ions, Na+, and Magnesium ions, Mg2+, are examples of cations Sodium ions, Na+, and Magnesium ions, Mg2+, are examples of cations Group 1 metals form monovalent cations Eg. Lithium forms Li+ Sodium ions, Na+, and Magnesium ions, Mg2+, are examples of cations Group 2 metals form divalent cations Eg. Calcium forms Ca2+ Sodium ions, Na+, and Magnesium ions, Mg2+, are examples of cations Group 3 metals form trivalent cations Eg. Aluminium forms Al3+ What’s a cation (and now we mention it, what’s an anion?) Anions are negatively charged ions Anions are negatively charged ions Chloride ions, Cl-, and oxide ions, O2-, are examples of anions Chloride ions, Cl-, and oxide ions, O2-, are examples of anions Group 6 elements form divalent anions Eg. sulphide forms S2- Chloride ions, Cl-, and oxide ions, O2-, are examples of anions Group 7 elements form monovalent anions Eg. fluoride forms F- Common cations Monovalent Divalent Trivalent Lithium Li+ Potassium K+ Sodium Na+ Copper(I) Cu+ Silver Ag+ Hydrogen H+ Barium Ba2+ Calcium Ca2+ Magnesium Mg2+ Zinc Zn2+ Iron(II) Fe2+ Tin(II) Sn2+ Lead(II) Pb2+ Copper(II) Cu2+ Aluminium Al3+ Iron(III) Fe3+ Common anions Monovalent Divalent Trivalent Bromide BrChloride ClIodide IHydroxide OHNitrate NO3- Oxide O2Carbonate CO32Sulphate SO42Sulphite SO32Sulphide S2- Phosphate PO43- Lesson 5 g) Tests for ions and gases g) Tests for ions and gases 2.37 describe tests for the cations: i Li+, Na+, K+, Ca2+ using flame tests ii NH4+, using sodium hydroxide solution and identifying the ammonia evolved iii Cu2+, Fe2+ and Fe3+, using sodium hydroxide solution 2.38 describe tests for the anions: i Cl-, Br- and I-, using dilute nitric acid and silver nitrate solution ii SO42-, using dilute hydrochloric acid and barium chloride solution iii CO32-, using dilute hydrochloric acid and identifying the carbon dioxide evolved 2.39 describe tests for the gases: i hydrogen ii oxygen iii carbon dioxide iv ammonia v chlorine. Li+, Na+, K+, Ca2+ using flame tests Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 1. Clean the flame test metal loop wire by dipping it into hydrochloric acid and then holding it in a hot Bunsen flame. Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 1. Clean the flame test metal loop wire by dipping it into hydrochloric acid and then holding it in a hot Bunsen flame. 2. Repeat this until the wire doesn't produce any colour in the flame. Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 1. Clean the flame test metal loop wire by dipping it into hydrochloric acid and then holding it in a hot Bunsen flame. 2. Repeat this until the wire doesn't produce any colour in the flame. 3. When the wire is clean, moisten it again with some of the acid and then dip it into a small amount of the solid you are testing so that some sticks to the wire. Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 4. Place the wire back in the flame again. Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 4. Place the wire back in the flame again. 5. If the flame colour is weak, it is often worthwhile to dip the wire back in the acid again and put it back into the flame as if you were cleaning it. You often get a very short but intense flash of colour by doing that. Li+, Na+, K+, Ca2+ using flame tests Instructions for a flame test: 4. Place the wire back in the flame again. 5. If the flame colour is weak, it is often worthwhile to dip the wire back in the acid again and put it back into the flame as if you were cleaning it. You often get a very short but intense flash of colour by doing that. RESULT? Li+, Na+, K+, Ca2+ using flame tests Li+, Na+, K+, Ca2+ using flame tests Flame test results: CATION FLAME TEST COLOUR Lithium RED Sodium STRONG PERSISTENT ORANGE Potassium Calcium LILAC (PINK) ORANGE-RED NH4+, using sodium hydroxide solution and identifying the ammonia produced NH4+, using sodium hydroxide solution and identifying the ammonia produced NH4+ is the ammonium ion. Although not a metal, it is classified as a cation because it forms a positively charged ion. NH4+, using sodium hydroxide solution and identifying the ammonia produced Test for NH4+ : All ammonium salts react with dilute alkalis, such as sodium hydroxide, to give ammonia. NH4Cl(aq) + NaOH(aq) NaCl(aq) + H2O(l) + NH3(g) NH4+, using sodium hydroxide solution and identifying the ammonia produced Test for NH4+ : All ammonium salts react with dilute alkalis, such as sodium hydroxide, to give ammonia. NH4Cl(aq) + NaOH(aq) NaCl(aq) + H2O(l) + NH3(g) Because it is an alkaline gas, ammonia will turn red litmus blue NH4+, using sodium hydroxide solution and identifying the ammonia produced Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When an iron(II) salt is added to sodium hydroxide, a dirty green precipitate of iron(II) hydroxide is formed. Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When an iron(II) salt is added to sodium hydroxide, a dirty green precipitate of iron(II) hydroxide is formed. Eg. Iron + Sodium Iron + Sodium sulphate hydroxide hydroxide sulphate FeSO4 + 2NaOH Fe(OH)2 + Na2SO4 Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When an iron(III) salt is added to sodium hydroxide, a orange / brown precipitate of iron(III) hydroxide is formed. Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When an iron(III) salt is added to sodium hydroxide, a orange / brown precipitate of iron(III) hydroxide is formed. Eg Iron + sodium chloride hydroxide iron + sodium hydroxide chloride Fe(Cl)3 + 3NaOH Fe(OH)3 + 3NaCl Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When a copper(II) salt is added to sodium hydroxide, a pale blue precipitate of copper(II) hydroxide is formed. Cu2+, Fe2+ and Fe3+ using sodium hydroxide solution When a copper(II) salt is added to sodium hydroxide, a pale blue precipitate of copper(II) hydroxide is formed. Eg. Copper + Sodium Copper + Sodium sulphate hydroxide hydroxide sulphate CuSO4 + NaOH Cu(OH)2 + Na2SO4 Lesson 5 g) Tests for ions and gases g) Tests for ions and gases 2.37 describe tests for the cations: i Li+, Na+, K+, Ca2+ using flame tests ii NH4+, using sodium hydroxide solution and identifying the ammonia evolved iii Cu2+, Fe2+ and Fe3+, using sodium hydroxide solution 2.38 describe tests for the anions: i Cl-, Br- and I-, using dilute nitric acid and silver nitrate solution ii SO42-, using dilute hydrochloric acid and barium chloride solution iii CO32-, using dilute hydrochloric acid and identifying the carbon dioxide evolved 2.39 describe tests for the gases: i hydrogen ii oxygen iii carbon dioxide iv ammonia v chlorine. Cl-, Br- and I- using dilute nitric acid and silver nitrate solution Cl-, Br- and I- using dilute nitric acid and silver nitrate solution STANDARD PROCEDURE: Add dilute nitric acid to a solution of the halide, and then add silver nitrate solution. Cl-, Br- and I- using dilute nitric acid and silver nitrate solution RESULT: With a chloride solution, a white precipitate of silver chloride is formed: NaCl + AgNO3 AgCl + NaNO3 Cl-, Br- and I- using dilute nitric acid and silver nitrate solution RESULT: With a bromide solution, a pale yellow precipitate of silver bromide is formed: NaBr + AgNO3 AgBr + NaNO3 Cl-, Br- and I- using dilute nitric acid and silver nitrate solution RESULT: With an iodide solution, a yellow precipitate of silver iodide is formed: NaI + AgNO3 AgI + NaNO3 Cl-, Br- and I- using dilute nitric acid and silver nitrate solution Halide Results: Chloride Bromide Iodide SO42- , using dilute hydrochloric acid and barium chloride solution SO42- , using dilute hydrochloric acid and barium chloride solution STANDARD PROCEDURE: Dilute hydrochloric acid is added to a solution of the sulphate and then barium chloride solution is added. SO42- , using dilute hydrochloric acid and barium chloride solution RESULT: A white precipitate shows the presence of a sulphate BaCl2(aq) + Na2SO4(aq) BaSO4(s) + 2NaCl(aq) SO42- , using dilute hydrochloric acid and barium chloride solution Barium sulphate precipitate CO32- , using dilute hydrochloric acid and identifying the carbon dioxide evolved CO32- , using dilute hydrochloric acid and identifying the carbon dioxide evolved STANDARD PROCEDURE: Dilute hydrochloric acid is added to a solution of the carbonate. CO32- , using dilute hydrochloric acid and identifying the carbon dioxide evolved RESULT: A gas, carbon dioxide, is produced which will turn limewater cloudy (then clear again) CO32- , using dilute hydrochloric acid and identifying the carbon dioxide evolved RESULT: CaCO3(aq) + 2HCl(aq) CaCl2(aq) + H2O(l) + CO2(g) Calcium + Hydrochloric Calcium + water + carbon Carbonate Acid Chloride dioxide CO32- , using dilute hydrochloric acid and identifying the carbon dioxide evolved Limewater Calcium carbonate + Hydrochloric acid Lesson 5 g) Tests for ions and gases g) Tests for ions and gases 2.37 describe tests for the cations: i Li+, Na+, K+, Ca2+ using flame tests ii NH4+, using sodium hydroxide solution and identifying the ammonia evolved iii Cu2+, Fe2+ and Fe3+, using sodium hydroxide solution 2.38 describe tests for the anions: i Cl-, Br- and I-, using dilute nitric acid and silver nitrate solution ii SO42-, using dilute hydrochloric acid and barium chloride solution iii CO32-, using dilute hydrochloric acid and identifying the carbon dioxide evolved 2.39 describe tests for the gases: i hydrogen ii oxygen iii carbon dioxide iv ammonia v chlorine. Tests for gases You need to know these! Tests for gases 1. Hydrogen Hydrogen gas Hydrochloric acid Magnesium ribbon Tests for gases 1. Hydrogen Hydrogen gas Hydrochloric acid Magnesium ribbon Tests for gases 1. Hydrogen POP! Hydrogen gas Hydrochloric acid Magnesium ribbon Tests for gases 1. Hydrogen POP! To test for hydrogen, use a burning splint. The gas will explode with a squeaky ‘pop’. Hydrogen gas Hydrochloric acid Magnesium ribbon Tests for gases 2. Oxygen Oxygen gas Hydrogen peroxide Manganese (IV) oxide Tests for gases 2. Oxygen Glowing splint Oxygen gas Hydrogen peroxide Manganese (IV) oxide Tests for gases 2. Oxygen Splint re-lights Oxygen gas Hydrogen peroxide Manganese (IV) oxide Tests for gases 2. Oxygen To test for oxygen, use a glowing splint. The gas will cause the splint to re-light. Splint re-lights Oxygen gas Hydrogen peroxide Manganese (IV) oxide Tests for gases 3. Carbon dioxide Delivery tube Bubbles of carbon dioxide Hydrochloric acid Calcium carbonate Limewater Tests for gases 3. Carbon dioxide Delivery tube Bubbles of carbon dioxide Hydrochloric acid Calcium carbonate Limewater Tests for gases 3. Carbon dioxide To test for carbon dioxide, bubble the gas through limewater. After a short while the limewater will go milky-white. Delivery tube Bubbles of carbon dioxide Hydrochloric acid Calcium carbonate Limewater Tests for gases 3. Carbon dioxide To test for carbon dioxide, bubble the gas through limewater. After a short while the limewater will go milky-white. Delivery tube If carbon dioxide continues to be bubbled through limewater, the liquid will eventually go clear again. Bubbles of carbon dioxide Hydrochloric acid Calcium carbonate Limewater Tests for gases 4. Ammonia Tests for gases 4. Ammonia Tests for gases 4. Ammonia Ammonia gas will turn moist litmus paper from RED to BLUE Tests for gases 5. Chlorine Tests for gases 5. Chlorine Tests for gases 5. Chlorine Chlorine gas will turn moist litmus paper from BLUE to RED, and will then bleach it WHITE Tests for gases Summary Test Positive result Hydrogen Burning splint Burns with a squeaky pop Oxygen Glowing splint Relights a glowing splint Carbon dioxide Bubble through Limewater Limewater turns cloudy Ammonia Moist red litmus paper Turns from red to blue Chlorine Moist blue litmus paper Bleaches the paper Gas End of Section 2 Lesson 5 In this lesson we have covered: Tests for Cations Tests for Anions Tests for the gases