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Exploring Metals: Properties and Reactions

Learn about the properties and reactions of metals, including conductivity, metallic bonding, and reactions with water and acids. Discover the amazing world of metals and their uses.

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Exploring Metals: Properties and Reactions

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  1. METALS National 5

  2. Starter Which of the following diagrams could represent the structure of a metal ? c

  3. Lesson 1: Metals Today we are learning to understand some of the properties of metals. By the end of today I can: • Complete a table to show the boiling point/melting point of metalsand conductivity of metals. • Explain metallic bonding

  4. Metals • Metals have amazed and intrigued us for thousands of years. • From tungsten, the element with the highest melting point to lithium, a metal that floats on water; from gold, a metal so unreactive it is shiny even after thousands of years, to caesium, a metal so reactive it’s stored under a vacuum. • They can be used to create electricity and convert harmful car exhaust fumes into harmless gases, they can corrode but also protect. They can be strong and rigid or soft and supple, one is even a liquid. • Some are found as pure nuggets lying at the bottom of fast flowing rivers; others are so tightly bound to other elements, huge amounts of energy are required to separate them. • Metals are truly magical!

  5. Activity 9.1

  6. Conductivity

  7. Set up either of the following electrical circuits to test the electrical conductivity of metals on the following table

  8. (9.2)Conductivity task:

  9. Metallic bonding • Most metals are SOLIDS at room temperature and HARD with high melting/boiling points • All elements want to achieve a full outer electron shell. • Metals will give up 1, 2 or 3 electrons to form +vemetal ions

  10. Metallic bonding • The greater the number of electrons in the outer shell the stronger the metallic bond. • So the melting point of Al>Mg>Na

  11. Metallic elements Strong electrostatic forces exist between the delocalised electrons (free to move) and the positive metal ions formed due to the loss of outer electrons. These electrostatic attractions are known as metallic bonds.

  12. Conducting electricity

  13. Plenary flow chart: • Pupils to complete the flow chart in their jotters. • Follow the questions and answer for (a-d) substance z in each scenario.

  14. Does it conduct electricity when solid? Does it conduct electricity when it is liquid? Does it have a high or low M.P or B.P? (a) (b) LOW (c) (d)

  15. Lesson 2: Reactions of Metals

  16. Metals Anagram • Conducting electricity is hugely important, but what other properties make metals amazing? • Unscramble these anagrams. ATHE RONOCTCDU LLAEMBEAL HSIYN TTRGHESN WLO SDNYITE LICDUTE

  17. Lesson 2: Reaction of Metals Today we are learning to understand some of the reactions of metals. By the end of today I can: • List extra properties of metals • Understand how important the reactivity series is. • List some of the alkali metals in order of reactivity due to experiment demonstration. • State some of the reactions a metal can undergo.

  18. (9.3) Coloured compounds Fill in the table to show the colour of these ions. You may remember doing the flame test and may want to use your data booklet to help you

  19. Reactions of metals • Some metals are more reactive than others. • The amount of energy given out when a metal reacts gives a measure of its reactivity. • By observing how vigorous the reaction is between a metal and: • WATER • OXYGEN • DILUTE ACID • We can begin to order the metals in a reactivity series

  20. Reactivity Series Based on their reactivity, chemists produced a table of metals as shown:

  21. Reaction with Water: The Alkali Metals (9.5) • Observe the reaction between 3 alkali metals with water. • In your jotter record the reactivity of the three metals, note which gas is produced. • Write a word equation and balanced equation for the reaction of Potassium and water

  22. Reaction with Water (9.5) • Half fill three small (100cm3) beakers with water. • Into the first place half a spatula of calcium granules, the second half a spatula of magnesium powder and the third half a spatula of zinc powder. • Observe what happens (you may need to leave them for several minutes).

  23. Metals Reacting with Water • ALL metals above aluminium in the reactivity series react with water to produce the metal hydroxide and hydrogen gas. • The metals from groups 1 and 2 react vigorously. METAL + WATERMETALHYDROXIDE + HYDROGEN

  24. Example • Lithium + Water Lithium Hydroxide + + Hydrogen

  25. Lesson 3

  26. Starter: • What is the name given to the gas given off when an alkali metal is placed in water ? • Put the 3 metals observed in order of most reactive to least reactive • What colour would the water of gone if universal indicator was dropped into the glass bowl ?

  27. (9.6)Metals with acid: Half fill six test tubes with hydrochloric acid and place them in a test tube rack. Place a piece of magnesium, aluminium, zinc, iron, tin and copper into each test tube. Observe what happens.

  28. Table of results:

  29. Metals Reacting with Dilute Acid • Metals above hydrogen in the reactivity series react with acids to produce a salt and hydrogen gas. • Metals below HYDROGEN do not react with acids. METAL + ACIDSALT + HYDROGEN

  30. Example Zinc + Hydrochloric acid Zinc Chloride + Hydrogen

  31. (9.7)Metals with oxygen:

  32. Table of results:

  33. Metals Reacting with Oxygen • Some metals react vigorously with oxygen and burn Fiercely, some react more slowly and others do not react at all. METALS react with OXYGEN to make a METAL OXIDE. METAL + OXYGENMETALOXIDE

  34. Example Magnesium + Oxygen Magnesium O Oxide

  35. Reactions of Metals and the Reactivity Series The results of experiments with Oxygen, water and dilute acids allow scientists to place metals into an order of reactivity.

  36. Which boxes show metals which react with dilute acids? • Which boxes show metals which react with dilute acid but not with cold water? • Which boxes show metals that do not react with dilute acid? • Which boxes show metals which react with oxygen but not with a dilute acid? • Which box shows the gas produced when sodium reacts with water?

  37. Lesson 4 Naming salts

  38. Naming salts Salts have both a first and second name like us. The first part comes from the alkali/metal. The second part comes from the acid.

  39. Metals and hydrochloric acid- equations Magnesium + hydrochloric Magnesium chloride + acid hydrogen Aluminium +hydrochloric ________ +___________ acid Zinc + hydrochloric ____________ +_______ acid

  40. Metal with sulfuric acid- equation Magnesium + sulfuric acid Magnesium + hydrogen sulfate Aluminium + _______ ________ + ___________ _______ + __________ _________ + __________

  41. Metals and nitric acid- equations Magnesium +________ ___________ +________ _________+_________ _________ + _________ ________ + _________ __________ + ________

  42. Challenge: • Create a word equation using any metal above hydrogen from the previous slide and one of the 3 acids we have been using.

  43. Lesson 5 Ionic equations

  44. Ionic equations Today we are learning to write ionic equations for some chemical reactions and about alloys By the end of today I can… • Write the ionic equation for some chemical reactions • State the definition for an alloy.

  45. Ionic equations • Whenever a metal reacts it always turns in to a positive charged ion by losing it’s outer electrons to whatever it is reacting with. • The other reactants must gain these electrons and form an negative charged ion.

  46. Example: Word equation: Sodium + Water Sodium hydroxide + hydrogen Chemical equation: 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) Ionic equation: 2Na(s) + 2H2O(l) 2[Na+](aq) +2[OH-](aq) +H2(g)

  47. Word equation: magnesium + hydrochloric acid magnesium chloride +hydrogen Chemical equation: Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) Ionic equation: Mg(s)+2H+(aq)+2Cl-(aq) Mg2+(aq)+2Cl-(aq) + H2(g)

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