Elements Compounds Mixtures
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- Nancy Gordon
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2 Elements Compounds Mixtures
3 Comment on what you observe in this photograph. How do the sweets in this photograph model the idea of elements, compounds and mixtures?
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5 By the end of this topic students should be able to Identify elements, compounds and mixtures. Define and explain the terms element, compound and mixture. Give examples of elements, compounds and mixtures. Describe the similarities and differences between elements, compounds and mixtures.
6 How can I classify the different materials in the world around me?
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12 What other classification systems do scientists use? One example is the classification of plants and animals in biology.
13 Could I have a brief introduction to elements, compounds and mixtures?
14 Iron and sulfur are both chemical elements. A mixture of iron and sulfur can be separated by a magnet because iron can be magnetised but sulfur cannot.
15 Duration 10 seconds. Elements, Compounds & Mixtures Iron and sulfur are both chemical elements. A mixture of iron and sulfur can be separated by a magnet because iron can be magnetised but sulfur cannot.
16 Iron and sulfur react to form the compound iron(ii) sulfide. The compound iron(ii) sulfide has new properties that are different to those of iron and sulfur, e.g. iron(ii) sulfide is not attracted towards a magnet.
17 Duration 25 seconds. Elements, Compounds & Mixtures Iron and sulfur react to form the compound iron(ii) sulfide. The compound iron(ii) sulfide has new properties that are different to those of iron and sulfur, e.g. iron(ii) sulfide is not attracted towards a magnet.
18 iron (metal) + sulfur (non-metal) chemical reaction iron(ii) sulfide
19 Elements (found in the Periodic Table) iron (metal) + sulfur (non-metal) chemical reaction Mixture of two elements Compound (not found in the Periodic Table) iron(ii) sulfide
20 Elements (found in the Periodic Table) iron (metal) Grey powder (attracted towards magnet) + sulfur (non-metal) Yellow powder (not attracted towards magnet) chemical reaction Mixture of two elements Compound (not found in the Periodic Table) iron(ii) sulfide Black solid (not attracted towards magnet) A reaction causes a change in the properties of the chemicals.
21 A mixture of the two elements, iron and sulfur. The atoms of iron and sulfur are not bonded together. The mixture can be easily separated by a physical process. The ratio between iron and sulfur can vary, i.e. it is not fixed. The compound iron(ii) sulfide. The atoms of iron and sulfur are bonded together and cannot be easily separated by a physical process. Properties of the compound are different to those of the mixture. The ratio between iron and sulfur is fixed.
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23 How can models help me to understand elements, compounds and mixtures?
24 Models are often used in Chemistry to represent, explain and understand things that cannot be observed directly. methane + oxygen carbon dioxide + water CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) Carbon atom = white brick. Hydrogen atom = yellow brick. Oxygen atom = red brick.
25 In the diagram shown below, Lego bricks are used to represent atoms to illustrate the reaction between methane and oxygen. methane + oxygen carbon dioxide + water CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l) Carbon atom = white brick. Hydrogen atom = yellow brick. Oxygen atom = red brick.
26 What are elements, compounds and mixtures? To develop the ideas of elements, compounds and mixtures into concepts, we need to consider examples of each one and then identify the ways in which they are similar to each other.
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28 All matter is composed of tiny particles that are in a constant state of motion. The smallest particles are given names such as proton, neutron and electron. These are arranged into slightly larger (but still very small) particles called atoms, ions and molecules.
29 Here are some diagrams that Chemists might use to represent atoms and molecules. The letters are symbols that are used by Chemists to identify different atoms. There are many different types of atoms and molecules, and these diagrams show just a few examples.
30 This is an example of A pure chemical element. Kr = Krypton (Group 0)
31 This is an example of A pure chemical element. Br 2 = Bromine (Group VII)
32 This is an example of A pure compound. HCl = Hydrogen Chloride
33 This is an example of A pure chemical element. I 2 = Iodine (Group VII)
34 This is an example of A pure compound. H 2 S = Hydrogen Sulfide
35 This is an example of A mixture of two chemical elements. He = Helium (Group 0) Xe = Xenon (Group 0)
36 This is an example of A mixture of a chemical element and a compound. I 2 = Iodine (Group VII) C 6 H 6 = Benzene
37 This is an example of A pure chemical element. S (or S 8 ) = Sulfur (Group VI)
38 This is an example of A pure compound. CH 4 = Methane
39 This is an example of A mixture of two compounds. CH 4 = Methane C 6 H 6 = Benzene
40 This is an example of A pure compound. C 2 H 6 = Ethane
41 This is an example of A mixture of two chemical elements. Br 2 = Bromine (Group VII) Cl 2 = Chlorine (Group VII)
42 Now describe the properties of elements, compounds and mixtures using clear and concise scientific language.
43 Summary of the properties of elements: A chemical element is a pure substance. A chemical element is composed of only one type of atom. A chemical element cannot be converted into anything more simple by a chemical reaction or electrolysis (can not be broken down by electricity). All known chemical elements are listed in the Periodic Table.
44 Period Elements, Compounds & Mixtures The Periodic Table of Chemical Elements 1 2 Group H He 2 Li Be B C N O F Ne 3 Na Mg Al Si P S Cl Ar 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac = Metallic elements. = Non-metallic elements. Element Song
45 The General Properties of Metals Good conductors of electricity, in both the solid and molten states. Good conductors of heat. Shiny in appearance (metallic lustre). Sonorous (ring when struck). Malleable (can be bent without breaking). Ductile (can be drawn-out to form wires). High melting and boiling points (except Group I metals). Hard and strong (except Group I metals). High density (except Group I metals). Metal oxides tend to be basic in nature. Note: Not all metals are magnetic.
46 The General Properties of Non-metals Do not conduct electricity in either the solid or molten states (except graphite). Usually poor conductors of heat. Usually dull in appearance (except crystals). Not sonorous (do not ring when struck). Not malleable or ductile. Non-metals are usually brittle and break easily when bent or stretched. Usually have low melting and boiling points (compared to metals). Usually weak and soft (compared to metals). Usually have low densities (compared to metals). Non-metal oxides tend to be acidic in nature.
47 Summary of the properties of compounds: A compound is a pure substance. A compound is composed of two or more different chemical elements that react and bond together in a fixed ratio. The ratio is given by the compound s formula, e.g. the formula of ammonia is NH 3 which means that one atom of nitrogen (N) is bonded to three atoms of hydrogen (H). A compound can only be converted into more simple substances by a chemical reaction.
48 Summary of the properties of compounds: A compound has unique chemical and physical properties that are different from those of the chemical elements that it is composed of. For example, sodium is a highly reactive metal that would burn your skin on contact and chlorine is a highly reactive non-metal that would also burn your skin on contact. When sodium and chlorine react, they form the compound sodium chloride (common table salt) which is safe enough to eat!
49 Duration = 51 seconds. Elements, Compounds & Mixtures The extremely reactive and harmful elements sodium and chlorine react to form the compound sodium chloride (common table salt) which is safe enough to eat!
50 Duration = 51 seconds. Elements, Compounds & Mixtures The extremely reactive and harmful elements sodium and chlorine react to form the compound sodium chloride (common table salt) which is safe enough to eat!
51 Summary of the properties of compounds: A crystal of sodium chloride (common table salt, NaCl) is composed of positive sodium ions (Na + ) and negative chloride ions (Cl ). Compounds that contain a metallic element bonded to a non-metallic element are described as ionic. They contain positive metal ions (cations) and negative non-metal ions (anions) arranged in a crystal lattice.
52 Summary of the properties of compounds: A molecule of carbon dioxide CO 2 A molecule of water H 2 O Compounds that contain a non-metallic element bonded to another non-metallic element are described as covalent molecules. They are composed of neutral atoms held together by shared pairs of electrons.
53 Summary of the properties of mixtures: A mixture is not a pure substance. Two or more different chemicals (elements or compounds) are added together, but do not react and chemically bond together. The components of a mixture can be easily separated by a physical process, e.g. distillation or filtration.
54 Summary of the properties of mixtures: The ratio of chemicals in a mixture can vary, i.e. it is not fixed. The mixture has the same chemical and physical properties as the individual chemicals that it is composed of.
55 Did you know? A pure chemical has a sharp melting point and a sharp boiling point.
56 Did you know? Adding an impurity to a pure chemical will lower the melting point of the chemical.
57 Did you know? m.p. Adding an impurity to a pure chemical will lower the melting point of the chemical.
58 Did you know? Adding an impurity to a pure chemical will increase the boiling point of the chemical.
59 Did you know? b.p. Adding an impurity to a pure chemical will increase the boiling point of the chemical.
60 Question: Why is table salt (sodium chloride) added to water that is used for cooking? Question: Why is table salt (sodium chloride) added to snow and ice on frozen roads during winter time?
61 Question: Why is table salt (sodium chloride) added to water that is used for cooking? Answer: The sodium chloride is an impurity that will increase the boiling point of the water. The food will cook at a faster rate. Question: Why is table salt (sodium chloride) added to snow and ice on frozen roads during winter time? Answer: The sodium chloride is an impurity that will decrease the melting point of the ice. The ice will therefore melt, even at low temperatures, thus making the roads safer to drive on.
62 A chemical melts at 20 C and boils at +40 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C
63 A chemical melts at 20 C and boils at +40 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C Solid Liquid Gas Liquid
64 A chemical melts at +40 C and boils at +80 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C
65 A chemical melts at +40 C and boils at +80 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C Solid Liquid Gas Solid
66 A chemical melts at 60 C and boils at 10 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C
67 A chemical melts at 60 C and boils at 10 C. What is the chemical s physical state (solid, liquid or gas) at room temperature (25.0 C) and pressure? Room Temperature 25.0 C Solid Liquid Gas Gas
68 What is an alloy?
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70 An alloy is a mixture of two or more metals, or a mixture containing a metallic element and a non-metallic element. Common alloys include... Brass copper (70%) and zinc (30%). Bronze copper (88%) and tin (12%). Pewter tin (94%), copper (2%) and antimony (4%). Stainless Steel iron (88%) and chromium (12%).
71 What is the difference between a solution and a suspension?
72 A solute, e.g. CuSO 4 (s) Dissolves in a solvent, e.g. H 2 O(l) To form a solution, e.g. CuSO 4 (aq)
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74 A solution is a mixture of a solvent and a solute (a chemical that dissolves in the solvent). The solvent is usually a liquid but the solute maybe a solid, liquid or a gas. If the solvent is water, then the solution is described as an aqueous solution. A solution is a homogenous mixture, meaning that it is the same composition throughout.
75 All solutions are clear, i.e. it is possible to see through a solution. Solutions can either be colourless or coloured. Sodium chloride (table salt) dissolved in water is an example of a colourless solution. Examples of coloured solutions include copper(ii) sulfate (blue) and potassium manganate(vii) (purple).
76 Solubility is a chemical property. It measures the ability of a substance (solute) to dissolve in a liquid (solvent). Solubility is normally expressed as the mass of solute, in grams, that will dissolve in 100 g of solvent. For most chemicals, solubility increases with temperature, except for gases (e.g. NH 3 ) whose solubility decreases as temperature increases.
77 A suspension is a mixture in which very small particles of a solid or a liquid are suspended in either a liquid or a gas. Examples of suspensions include chalk dust suspended in water and mud suspended in water. Small droplets of one liquid suspended in another liquid is called an emulsion. Small droplets of a solid or a liquid suspended in a gas is called an aerosol.
78 A magnified view of an oil in water emulsion.
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80 Clouds are aerosols very small droplets of water suspended in air.
81 Smoke is an aerosol very small solid particles suspended in air.
82 A suspension is a heterogeneous mixture because it does not have a consistent / uniform composition throughout. Colour, density and other properties may vary throughout the suspension. The insoluble particles in a suspension are large enough to prevent light passing through. Suspensions are therefore translucent or opaque.
83 Over a period of time, the particles in a suspension my settle to the bottom of the container due to the effect of gravity.
84 Double check your definitions and understanding by classifying the following substances as either elements, compounds or mixtures.
85 This is an example of A pure compound. C 2 H 5 OH = Ethanol
86 This is an example of A pure chemical element. O 2 = Oxygen (Group VI)
87 This is an example of A pure compound. C 6 H 6 = Benzene
88 This is an example of A mixture of three compounds. CH 4 = Methane, C 2 H 2 = Ethyne C 2 H 6 = Ethane
89 This is an example of A pure chemical element. N 2 = Nitrogen (Group V)
90 Okay, so what exactly is an atom?
91 The reaction of the element sodium with water. Time: 11 seconds. sodium + water sodium hydroxide + hydrogen 2Na (s) + 2H 2 O (l) 2NaOH (aq) + H 2 (g)
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93 How small could you cut the piece of sodium and still get the same reaction to occur?
94 The smallest piece of sodium that would react with water in the same way as a lump of sodium is a sodium atom. An atom is the smallest part of an element that demonstrates all of the typical properties of that element.
95 What is a molecule?
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97 A molecule is a group of two or more non-metallic elements that are held together by covalent bonds. Examples of simple molecules include: The element nitrogen, N 2. The element oxygen, O 2. The compound ammonia, NH 3. The compound methane, CH 4.
98 A single atom is said to be monatomic, e.g. the noble gases, He and Ne. Molecules that contain two atoms bonded together are said to be diatomic, e.g. nitrogen N 2. Molecules that contain three atoms bonded together are said to be triatomic, e.g. water H 2 O. Molecules that contain more than three atoms bonded together are said to be polyatomic, e.g. methane CH 4.
99 A diatomic molecule of the element nitrogen N 2 Note: This is described as a homonuclear molecule because the atoms are all of the same element. A triatomic molecule of the compound water H 2 O Note: This is described as a heteronuclear molecule because the atoms are of different chemical elements.
100 A polyatomic molecule of methane CH 4 Note: Molecules that are composed of more than three atoms covalently bonded together are usually described as polyatomic, which literally means many atoms.
101 Higher Order Thinking Skills Compare and contrast the properties of elements, compounds and mixtures. You can use a graphic organiser, like the following Venn Diagram, to help organise your thoughts and ideas.
102 Higher Order Thinking Skills
103 Higher Order Thinking Skills In what ways are elements, compounds and mixtures all similar to each other? e.g. They are all composed of atoms, ions or molecules. e.g. Compounds and mixtures are composed of different chemical elements which may or may not be chemically bonded together.
104 Higher Order Thinking Skills In what ways are the pairs similar to each other? e.g. A simple mixture is composed only of only two chemical elements. e.g. They are both pure substances. e.g. They are both composed of more that one chemical element.
105 Higher Order Thinking Skills In what ways are elements, compounds and mixtures different from each other? e.g. Elements are composed of only one type of atom. e.g. The components of a mixture can be separated by a physical process. e.g. The ratio of elements in a compound is fixed.
106 Flow diagram! Design a flow diagram that will allow you to logically and systematically classify a substance as either an element, compound, mixture of elements, mixture of compounds or a mixture of an element and an compound.
107 Example Flow Diagram to Classify Elements, Compounds and Mixtures
108 Example Flow Diagram to Classify Elements, Compounds and Mixtures
109 Example Flow Diagram to Classify Elements, Compounds and Mixtures
110 Example Flow Diagram to Classify Elements, Compounds and Mixtures
111 Example Flow Diagram to Classify Elements, Compounds and Mixtures
112 Example Flow Diagram to Classify Elements, Compounds and Mixtures
113 Example Flow Diagram to Classify Elements, Compounds and Mixtures
114 Example Flow Diagram to Classify Elements, Compounds and Mixtures
115 Example Flow Diagram to Classify Elements, Compounds and Mixtures
116 Example Flow Diagram to Classify Elements, Compounds and Mixtures
117 Example Flow Diagram to Classify Elements, Compounds and Mixtures
118 Example Flow Diagram to Classify Elements, Compounds and Mixtures
119 Example Flow Diagram to Classify Elements, Compounds and Mixtures
120 Could I have some questions to check my understanding?
121 Question One: Which one of the following is a list of elements? A) Air, carbon dioxide, hydrogen and silver. B) Calcium oxide, petrol, pure water and zinc. C) Copper, iron, oxygen and sulfur. D) Mercury, nitrogen, salt water and steel.
122 Question One: Which one of the following is a list of elements? A) Air, carbon dioxide, hydrogen and silver. B) Calcium oxide, petrol, pure water and zinc. C) Copper, iron, oxygen and sulfur. D) Mercury, nitrogen, salt water and steel.
123 Question Two: Which one of the following is a list of compounds? A) Aluminium, carbon dioxide, pure water and zinc. B) Copper(II) oxide, pure water, sodium chloride and sugar. C) Brass, carbon, iron(ii) sulphide and salt water. D) Gold, polluted air, steel and sulfur.
124 Question Two: Which one of the following is a list of compounds? A) Aluminium, carbon dioxide, pure water and zinc. B) Copper(II) oxide, pure water, sodium chloride and sugar. C) Brass, carbon, iron(ii) sulphide and salt water. D) Gold, polluted air, steel and sulfur.
125 Question Three: Which one of the following is a list of mixtures? A) Air, bronze, steel and tap water. B) Copper, gold, platinum and silver. C) Iron, pewter, sodium chloride and sulfur. D) Oxygen, stainless steel, sugar and zinc oxide.
126 Question Three: Which one of the following is a list of mixtures? A) Air, bronze, steel and tap water. B) Copper, gold, platinum and silver. C) Iron, pewter, sodium chloride and sulfur. D) Oxygen, stainless steel, sugar and zinc oxide.
127 Presentation on Elements, Compounds and Mixtures by Dr. Chris Slatter Nanyang Girls High School 2 Linden Drive Singapore Based on a publication by the Royal Society of Chemistry, London, England 1 st February 2016
128 Answers to the Card Sorting Activity Elements Cards Compounds Cards Mixtures Cards
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