S3 Chemistry Atomic Structure, Bonding & Properties

Transcription

1 S3 Chemistry Atomic Structure, Bonding & Properties REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

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3 S3 Chemistry Atomic Structure, Bonding & Properties Lessons 1 & 2 History of the Atom REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

4 Learning Objectives & Success Criteria Today we will learn About the scientific history of the discovery of the atom. We will do this by Researching the different scientists involved in atomic science and presenting a poster based on their work. Using each other s posters as a learning tool and peer assessing. We will have succeeded if All members of the class can complete a summary table on the key scientists involved in the scientific history of the discovery of the atom using the information extracted from classmates posters.

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6 Atomic Theory Scientists Your scientist will be one of the following: Ernest Rutherford Neils Bohr John Dalton JJ Thomson Werner Heisenberg You will team up with the classmates who have part of the same photo as you.

7 Sources of Information

8 Poster Key Features Your poster must include the following: 1.Name of scientist 2.Date of proposed theory 3.What did they think an atom looked like? Include a picture if available. 4.Were they correct (or did other scientists improve upon their model)? If you want to add more information you can but be sure to include the above first of all!

9 Learning Objectives & Success Criteria Today we will learn About the scientific history of the discovery of the atom. We will do this by Researching the different scientists involved in atomic science and presenting a poster based on their work. Using each other s posters as a learning tool and peer assessing. We will have succeeded if All members of the class can complete a summary table on the key scientists involved in the scientific history of the discovery of the atom using the information extracted from classmates posters.

10 Lesson 1 - Exit Task 3 Things Tell me three things One thing you have done well 2. One thing you would like to find out more about 3. One thing you know now that you didn t know 50 minutes ago

11 Lesson 2 Starter What were the 4 key features you were asked to include on your poster? Name of scientist, date of proposed theory, what they think an atom looked like (picture if available) & if they were correct? Tick each of the features you have already finished on your poster. You now have only 20 minutes to complete the rest of your poster. We will then be placing our posters up for classmates to learn from. Do your best for each other!

12 S3 Chemistry Atomic Structure, Bonding & Properties Lessons 1 & 2 History of the Atom REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

13 Learning Objectives & Success Criteria Today we will learn About the scientific history of the discovery of the atom. We will do this by Researching the different scientists involved in atomic science and presenting a poster based on their work. Using each other s posters as a learning tool and peer assessing. We will have succeeded if All members of the class can complete a summary table on the key scientists involved in the scientific history of the discovery of the atom using the information extracted from classmates posters.

14 Lesson 2 - Exit Task Match Up Match the atomic theory model to the scientist. Rutherford Solid sphere model Thomson Planetary model - electrons in specific energy levels Dalton Planetary model discovered the nucleus Bohr Plum pudding model

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16 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 3 Structure of the Atom REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

17 Learning Objectives & Success Criteria Today we will learn to Identify the properties and locations of protons, electrons and neutrons in an atom. We will do this by Hearing about what an atom is made of and drawing our own atoms. We will have succeeded if We can state the mass, charge and location of the 3 subatomic particles. We can draw atom diagrams which include the correct electron arrangement.

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19 + + The electrons are always found outside the nucleus in electron shells.

20 Most of the atom is empty space! Imagine a Helium atom the size of Wembley stadium. The nucleus would be the size of a football on the centre spot. The electrons would be the size of two peas flying around the whole stadium. The rest of it is emptiness!

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23 Copy & complete the following table to summarise the key features about the 3 subatomic particles.

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25 Write the electron arrangement for the following atoms:

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28 Learning Objectives & Success Criteria Today we will learn to Identify the properties and locations of protons, electrons and neutrons in an atom. We will do this by Hearing about what an atom is made of and drawing our own atoms. We will have succeeded if We can state the mass, charge and location of the 3 subatomic particles. We can draw atom diagrams which include the correct electron arrangement.

29 Rate your understanding of today s lesson using your fingers. Fist to Five

30 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 4 Nuclide Notation REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

31 Learning Objectives & Success Criteria Today we will learn What is meant by the terms Atomic Number and Mass Number and how to use these two numbers to work out the numbers of each subatomic particle in an atom. We will do this by Carrying out simple calculations using Atomic number and Mass Number. Using the periodic table and data book to help find these two numbers. We will have succeeded if We can work out the number of protons, electrons and neutrons from the nuclide notation or when given the Atomic and Mass numbers.

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44 Learning Objectives & Success Criteria Today we will learn What is meant by the terms Atomic Number and Mass Number and how to use these two numbers to work out the numbers of each subatomic particle in an atom. We will do this by Carrying out simple calculations using Atomic number and Mass Number. Using the periodic table and data book to help find these two numbers. We will have succeeded if We can work out the number of protons, electrons and neutrons from the nuclide notation or when given the Atomic and Mass numbers.

45 What? How? Explain what you have learnt today and how you have learnt it?

46 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 5 The Properties of Elements REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

47 Lesson Starter 1. What do you think we mean when we say a property of an element? A property is any characteristic of an element. 2. Give some examples of properties of elements. Physical properties (what they are like: colour, size, density, melting point, boiling point, odour). Chemical properties (what they can react with).

48 Learning Objectives & Success Criteria Today we will learn About the properties of elements and how electron arrangement links to properties of elements. We will do this by Carrying out conductivity tests on elements. Watching video clips about certain groups of elements and using the data book to learn about the electron arrangements within groups. We will have succeeded if We can use the position of an element in the periodic table to predict it s properties.

49 **REMINDER**

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55 All metals conduct electricity. All non-metals except carbon (graphite) are non-conductors (insulators). Mercury, the only metal which is a liquid at room temperature, can conduct electricity. All metals in the liquid state can conduct electricity.

56 1 2 Non-Metals /0 Metals _

57 Periodic Table - Important Areas Summary Group 1 Alkali Metals - very reactive metals (stored in oil). React violently with water to produce an alkali and hydrogen gas. Soft and can be cut with a knife. Members become more reactive as you move down the group. Group 7 - Halogens - very reactive non-metals. All coloured elements. Members become less reactive as you move down the group. Group 8/0 - Noble Gases - extremely unreactive gases. They do not readily combine with other elements to form compounds. Transition Metals middle block elements Form brightly coloured compounds. Variable valency. Several are used as catalysts to speed up chemical reactions.

58 Same group, ends in same number Crossing a period group by group, the last number increases by 1 each time. 0/8

59 Outer Electrons & Chemical Properties Elements in the same group have similar chemical properties. This is because elements in the same group have the same number of outer electrons. The number of outer electrons an element has is responsible for how it reacts. When an element has an incomplete outer shell of electrons it is unstable and it reacts with (forms bonds with) other elements to achieve stability.

60 Elements in group 8 (0) each have a full outer electron shell giving the noble gases a special stability. This means noble gases do not need to form bonds with other elements i.e. do not form compounds.

61 Learning Objectives & Success Criteria Today we will learn About the properties of elements and how electron arrangement links to properties of elements. We will do this by Carrying out conductivity tests on elements. Watching video clips about certain groups of elements and using the data book to learn about the electron arrangements within groups. We will have succeeded if We can use the position of an element in the periodic table to predict it s properties.

62 Mind Map Produce a mind map to summarise the lesson today.

63 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 6 Lose, Gain, Share: Making Compounds REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

64 Lesson Starter Name all the elements present in the following 5 compounds. 1.Aluminium bromide 2.Hydrogen oxide 3.Sodium hydroxide 4.Nitrogen hydride 5.Nickel sulfate Aluminium & bromine Hydrogen & oxygen Sodium & hydrogen & oxygen Nitrogen & hydrogen Nickel & sulfur & oxygen

65 Learning Objectives & Success Criteria Today we will learn About the types of bonding which exist. We will do this by Considering which types of elements are joining together in compounds and learning the rules about when atoms LOSE, GAIN or SHARE electrons. We will have succeeded if We can use the name of a compound to predict the type of bonding within it. We will also use the name to predict whether the bond is formed by loss & gain of electrons or by sharing electrons.

66 **REMINDER** A compound is a substance made up of two or more types of atom joined. A mixture is a substance made up of two or more types of substances (atoms/elements/compounds) NOT JOINED

67 **REMINDER** Naming Compounds Compound names are recognisable because they have 2 parts e.g. sodium chloride (sodium & chlorine). If a compound name ends in -IDE that compound only contains the 2 elements obvious from it s name. e.g. Except where the second part of the compound name is hydroxide or cyanide. sodium hydroxide = sodium, hydrogen and oxygen sodium cyanide = sodium, carbon and nitrogen If a compound name ends in -ATE or -ITE that compound contains the 2 elements obvious from it s name PLUS OXYGEN e.g. sodium carbonate (sodium, carbon & oxygen).

68 We learned in the last lesson that all elements except the noble gases have an incomplete outer electron shell and must form bonds to achieve stability. Achieving A Noble Gas Arrangement When elements bond they are able to achieve a full outer shell of electrons like a noble gas by LOSING, GAINING or SHARING electrons.

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70 Achieving A Noble Gas Arrangement Lithium Electron Arrangement = 2,1 Closest Noble Gas electron arrangement = 2 (He) Change to electrons = Lose 1

71 Achieving A Noble Gas Arrangement Fluorine Electron Arrangement = 2,7 Closest Noble Gas electron arrangement = 2, 8 (Ne) Change to electrons = Gain 1

72 Achieving A Noble Gas Arrangement Oxygen Electron Arrangement = 2,6 Closest Noble Gas electron arrangement = 2, 8 (Ne) Change to electrons = Gain 2

73 Achieving A Noble Gas Arrangement Aluminium Electron Arrangement = 2,8,3 Closest Noble Gas electron arrangement = 2,8 (Ne) Change to electrons = Lose 3

74 Achieving A Noble Gas Arrangement Calcium Electron Arrangement = 2, 8, 8, 2 Closest Noble Gas electron arrangement = 2, 8, 8 (Ar) Change to electrons = Lose 2

75 HINT Use the data book p4 to help you decide (remember the zig-zag line)

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78 Lose, Gain, Share Ionic compounds form by a metal atom losing electrons and a non-metal atom gaining electrons to form ions. Covalent compounds form by two or more non-metal atoms sharing electrons Now reconsider the compounds from the last 2 slides & state whether they would LOSE/GAIN or SHARE electrons.

79 Lose, Gain, Share Lose/Gain Share Lose/Gain Lose/Gain Share

80 Lose, Gain, Share Share Lose/Gain Share Lose/Gain Share

81 Exit Task Mr Wrong Explain why this student statement is wrong Sodium chloride, like other covalent compounds, bonds by sharing electrons

82 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 7 Covalent Bonding REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

83 Lesson Starter 1. Name the type of bonding in the following compounds: A Phosphorus chloride B Copper chloride covalent ionic 2. What would happen to the electrons in the above compounds as they bond (i.e. lose/gain OR share)?: A B Share Lose/Gain

84 Learning Objectives & Success Criteria Today we will learn How non-metal atoms join together via covalent bonds to form covalent compounds. We will do this by Hearing about what a covalent bond is. Drawing covalent molecules and building them using molecular model kits. We will have succeeded if We can state the definitions of the terms covalent bond, covalent molecule and diatomic. We can use our periodic table to find and name the 7 diatomic elements.

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86 Covalent Elements element). chlorine chlorine

87 Covalent Compounds atoms of different elements (forming a compound). compound). hydrogen chlorine hydrogen chloride

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90 Using Molecular Models Building Molecules oxygen hydrogen Using the molecular model kits (molymods) and the colour key shown opposite build a diatomic molecule of the 4 elements shown in the key. Remember diatomic means 2 atoms. chlorine nitrogen How many bonds does each molecule have joining the 2 atoms? Remember that where there is a hole in the model atom a bond must be inserted and all bonds must be joined to something (except with Nitrogen).

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92 Covalent Networks Covalent networks are giant structures with no fixed number of atoms. In covalent network structures all atoms are non-metals Brief slide/note and are on joined covalent by network? covalent bonds. Covalent network substances can be elements or compounds. Covalent Network Element Diamond Covalent Network Compound Silicon Dioxide (sand)

93 Learning Objectives & Success Criteria Today we will learn How non-metal atoms join together via covalent bonds to form covalent compounds. We will do this by Hearing about what a covalent bond is. Drawing covalent molecules and building them using molecular model kits. We will have succeeded if We can state the definitions of the terms covalent bond, covalent molecule and diatomic. We can use our periodic table to find and name the 7 diatomic elements.

94 Definition Choose three new words you have learnt today and write dictionary definitions.

95 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 8 Ionic Bonding REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

96 Lesson Starter 1. What is a covalent bond? A shared pair of electrons between 2 non-metal atoms. 2. Why do the atoms of some elements form bonds? To achieve stability by obtaining a full outer electron shell like a noble gas. 3. What are the 7 diatomic elements (hint use your periodic table to help)? Hydrogen, Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, Iodine (remember HON 7).

97 Learning Objectives & Success Criteria Today we will learn How metal and non-metal atoms are altered to become ions and how they subsequently join together via ionic bonding to form ionic compounds. We will do this by Reflecting on what we learned in our lose, gain, share lesson. Learning about the changes which arise in electron arrangement when electrons are transferred and how these changes link with the exact charge of the ion formed. We will have succeeded if We can use the electron arrangement of an element to predict the charge on the ion it forms to achieve stability like a noble gas.

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100 Li Li + Cl Cl -

101 Ionic Lattice

102 More Ionic Bonding Mg -> Mg 2+ 2 F -> 2 F -

103 Writing Ion Symbols Using the electron arrangement information from the data booklet we can work out the symbol for an ion of an element which has achieved stability by electron transfer (i.e. has a full outer electron shell like a noble gas). We do this by the following steps: 1. Write the symbol for an atom of the element. 2. Write the electron arrangement for that atom. 3. Consider what change to electron numbers would result in a full outer shell. 4. Consider what this change to electron numbers would mean in terms of ion charge and add the charge as a superscript.

104 Ion Name Aluminium Chloride Oxygen Lithium Calcium Nitride Phosphide Sodium Writing Ion Symbols Atom electron arrangement 2,8,3 2,8,7 2,6 2,1 2,8,8,2 2,5 2,8,5 2,8,1 Closest Noble Gas electron arrangement 2,8 (Ne) 2,8,8 (Ar) 2,8 (Ne) 2 (He) 2,8,8 (Ar) 2,8 (Ne) 2,8,8 (Ar) 2,8 (Ne) Change to electrons Lose 3 Gain 1 Gain 2 Lose 1 Lose 2 Gain 3 Gain 3 Lose 1 Ion symbol Al 3+ Cl - O 2- Li + Ca 2+ N 3- P 3- Na +

105 Learning Objectives & Success Criteria Today we will learn How metal and non-metal atoms are altered to become ions and how they subsequently join together via ionic bonding to form ionic compounds. We will do this by Reflecting on what we learned in our lose, gain, share lesson. Learning about the changes which arise in electron arrangement when electrons are transferred and how these changes link with the exact charge of the ion formed. We will have succeeded if We can use the electron arrangement of an element to predict the charge on the ion it forms to achieve stability like a noble gas.

106 Exit Task Summary Table Copy & complete the summary table. It outlines the key differences between ionic and covalent bonding. Element types involved in this bonding. What happens to the electrons during this bonding? Named example Covalent Bonding Non-metals only. Electrons are shared. Carbon dioxide. Ionic Bonding One metal and one non-metal. Electrons are lost by the metal and gained by the nonmetal. Sodium chloride.

107 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 9 Writing Formulae (Prefixes & Diagrams) REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

108 Lesson Starter For the following elements write the symbol of the ion which would be formed when that element achieves a full outer electron shell like a noble gas: 1 Magnesium atom : Mg Electron arrangement: 2, 8, 2 2 Fluorine atom: F Electron arrangement: 2, 7 3 Aluminium atom: Al Electron arrangement: 2, 8, 3 Mg 2+ F - Al 3+

109 Learning Objectives & Success Criteria Today we will learn How to write simple chemical formulae. We will do this by Using diagrams to work out formulae. Using prefixes to work out formulae. Using valency rules / visual aids to work out formulae. We will have succeeded if We can select the most appropriate method of writing formulae for a compound and apply it in order to write down the formula correctly.

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111 Using Models/Diagrams carbon H SiH 4 or oxygen O O Si H 4 Si hydrogen O 2 H H H chlorine nitrogen H H H H C C C H H H H C 3 H 8 or H 8 C 3

112 Hydrogen oxide - water H O H H 2 O or OH 2 Hydrogen chloride H Cl HCl or ClH H Carbon hydride H C H H CH 4 or H 4 C Chlorine Cl Cl Cl 2

113 Hydrogen H H H 2 Cl Carbon chloride Cl C Cl Cl CCl 4 or Cl 4 C Nitrogen hydride H N H NH 3 or H 3 N H

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115 Chemical Formula From Prefixes Sometimes the name of a compound contains a prefix which allows us to write the formula. Prefixes when present before the name of an element tell you how many atoms of that element are present in the formula of that compound. e.g. sulfur dioxide Contains 1 sulfur and 2 oxygens e.g. SO 2

116 Glue in the handout then complete the table on the right.

117 Selecting the Best Method of Writing Formulae 1. If given a diagram or model simply count the atoms. 2. If given a name including a prefix write down formula using prefix(es) to guide how many of each atom in the formula. 3. IF AND ONLY IF there is no diagram and no prefix present in the compound name then we have to use something called valency.

118 Valency Valency is the combining power of an element i.e. how many bonds it can form. It is linked to the group number in the periodic table. Note that the Noble gases do not have a valency because they are unreactive and do not form compounds.

119 Valency & Group Number Use your data book and/or the table above to find out the valency of the following elements:

120 **Optional activity** Valency Method Using Visual Aids Step 1 Use your data book (or the table copied from the last slide) to find the valency of each element in the compound. Hint: Add this number of pegs to the plate with the relevant symbol. Step 2 Combine as many copies of each peg plate as required in order to connect ALL peg bonds between the elements. Step 3 Use the picture created to write down your formula. potassium bromide KBr

121 Formulae & Bonding Type The formula does not always represent the exact number of particles of each type in a compound. It can sometimes represent the ratio of different particles. In covalent molecules the formula is the exact number of atoms in the compound. In covalent network and ionic substances the formula is the ratio of particles (ions in an ionic lattice and atoms in a covalent network).

122 Learning Objectives & Success Criteria Today we will learn How to write simple chemical formulae. We will do this by Using diagrams to work out formulae. Using prefixes to work out formulae. Using valency rules / visual aids to work out formulae. We will have succeeded if We can select the most appropriate method of writing formulae for a compound and apply it in order to write down the formula correctly.

123 Reach For The Stars - Rating Exercise Rate your understanding of the 3 Key Areas covered today: A Writing Formulae from diagrams/models B Writing Formulae from names with a prefix C Writing Formulae from valency with visual aids

124 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 10 Writing Formulae (SVSDF) REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

125 Lesson Starter 1. Write the formula for the following molecule: CCl 4 or Cl 4 C 2. Write the formula for nitrogen trifluoride. Hint Does the name have a prefix? 3. Write the formula for sulfur bromide. Hint Would working out the valency help? NF 3 S Br S Br Br SBr 2

126 Learning Objectives & Success Criteria Today we will Practise writing simple chemical formulae for elements in the numbered groups of the periodic table as well as the transition metal block. We will do this by Using a method called SVSDF, involving the valency of elements. We will also find out how valency is indicated for transition metals. We will have succeeded if We can write the chemical formula for simple two element compounds including those containing transition metals.

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131 Learning Objectives & Success Criteria Today we will Practise writing simple chemical formulae for elements in the numbered groups of the periodic table as well as the transition metal block. We will do this by Using a method called SVSDF, involving the valency of elements. We will also find out how valency is indicated for transition metals. We will have succeeded if We can write the chemical formula for simple two element compounds including those containing transition metals.

132 Objective Traffic Lights How do you feel about the lesson objectives? Red = don t think I have grasped this Amber = feeling OK about this, have just about got there Green = Confident I have achieved this

133 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 11 Word Equations REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

134 Lesson Starter SO 2 CaF 2 CuO Mn 3 N 2

135 Learning Objectives & Success Criteria Today we will learn How to write equations which summarise the chemicals involved and how they change in a chemical reaction. We will do this by Learning about what must be and what must not be included in word equations. Practising writing word equations from descriptions of chemical reactions. We will have succeeded if We can write a word equation for any chemical reaction which is described for us.

136 Word Equations A word equation describes what we start with (reactants) during a chemical reaction and what we end up with (products). It is similar to a recipe with reactants being like the ingredients and the product(s) being what we have made using those ingredients. The ingredients or reactants appear on the left of the equation while the products appear on the right.

137 plus Changes into OR Reacts to produce Reactants appear on the left of the arrow and products appear on the right.

138 Example 1 Word Equations When you are given a sentence telling you how a chemical reaction has taken place, you should be able to write a word equation from that. Sodium reacts with chlorine to produce sodium chloride reactants products Sodium + chlorine sodium chloride

139 reactants products Example 2 Acid reacts with alkali to produce salt and water. Acid + Alkali Salt + Water

140 Example 3 reactants products Nitrogen and hydrogen combine to form nitrogen hydride. nitrogen + hydrogen nitrogen hydride

141 Example 4 Mercury oxide decomposes on heating to form mercury and oxygen. reactants products mercury oxide mercury + oxygen

142 Example 5 reactants products Calcium carbonate fizzes up when it is added to nitric acid. This is because carbon dioxide gas is being made. Calcium nitrate and water are left in the beaker at the end of the reaction. calcium carbonate + nitric calcium + acid nitrate water

143 Example 6 reactants products Your body uses food and oxygen to make carbon dioxide and water in a process called respiration. food + oxygen carbon dioxide + water

144 Example 7 Rusting happens when iron reacts with the oxygen in air to form iron oxide reactants products iron + oxygen iron oxide

145 Word Equation Extension Task Try the 2 sheets of examples on writing word equations. The examples in the first sheet have been partially done for you. DO NOT WRITE ON THE SHEETS Copy and complete the word equations into your jotter for both exercises.

146 Learning Objectives & Success Criteria Today we will learn How to write equations which summarise the chemicals involved and how they change in a chemical reaction. We will do this by Learning about what must be and what must not be included in word equations. Practising writing word equations from descriptions of chemical reactions. We will have succeeded if We can write a word equation for any chemical reaction which is described for us.

147 Exit Task Spot the Blooper! State what is wrong with each of the following word equations. 1.carbon + oxygen gas carbon dioxide 2.zinc + hydrochloric acid = zinc chloride + hydrogen 3.Lead iodide and potassium nitrate are produced when lead nitrate and potassium iodide are reacted together Reactants on products side (RHS) and vice versa Lead iodide + potassium nitrate lead nitrate + potassium iodide

148 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 12 Equations Using Symbols & Formulae REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

149 Lesson Starter Write word equations for the following 3 chemical reactions: 1 2 3

150 Learning Objectives & Success Criteria Today we will learn How to write equations using symbols and formulae (including symbols which indicate the state of substances). We will do this by Learning the different state symbols. Applying our knowledge of elements to write the appropriate symbol/formula for them. Using the prefix or valency method (as appropriate) to work out the formulae for compounds. We will have succeeded if We can write an equation, including symbols and formulae for a chemical reaction which is described for us.

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152 (l) (g) (aq) (s) (s) (l) (g) (g) (s) (aq)

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154 NOTE -State symbols can be worked out for the elements using the melting point/boiling point information on NAT 5 data book p5

155 NOTE - State symbols can be worked out for the elements using the melting point/boiling point information on NAT 5 data book p5 boron boron B (s) + F 2 (g) BF 3

156 NOTE - State symbols can be worked out for the elements using the melting point/boiling point information on NAT 5 data book p5 Si (s) + Br 2 (g) SiBr 4

157 Extra Examples 1. Hot magnesium ribbon reacts vigorously with steam. It glows very brightly and the products are magnesium oxide and hydrogen gas. a. Write a word equation for the reaction. magnesium + steam magnesium oxide + hydrogen b. Write an equation using symbols and formulae for the reaction. Mg (s) + H 2 O (g) MgO (s) + H 2 (g)

158 Extra Examples 2. C 4 H 10 + O 2 CO 2 + H 2 O

159 Symbol & Formulae Equation Extension Task Try the sheet of examples on writing equations using symbols and formulae. DO NOT WRITE ON THE SHEETS Copy and complete the equations into your jotter.

160 Learning Objectives & Success Criteria Today we will learn How to write equations using symbols and formulae (including symbols which indicate the state of substances). We will do this by Learning the different state symbols. Applying our knowledge of elements to write the appropriate symbol/formula for them. Using the prefix or valency method (as appropriate) to work out the formulae for compounds. We will have succeeded if We can write an equation, including symbols and formulae for a chemical reaction which is described for us.

161 Exit Task Flow-Chart Can you draw a flowchart like the one we used in today s lesson to help us write equations using symbols and formulae.

162 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 13 Properties of Compounds: Physical State & Solubility REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

163 HINT Write word equation first to help you!!! Na (s) + Cl 2 (g) NaCl (s) CuO (s) + C (s) Cu (s) + CO 2 (g)

164 Learning Objectives & Success Criteria Today we will learn About the properties of compounds and how they link to the type of bonding in that compound. We will do this by Examining the state of different compounds at room temperature. Testing the solubility of various compounds. Spotting any patterns based on the type of bonding. We will have succeeded if We can state how the physical state and solubility of compounds varies based on their type of bonding.

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167 Water, H 2 O Physical State & Bonding Type The physical state of a compound at room temperature is an indication of the bonding type in that compound. View the compound display then complete the table indicating the state of each compound and the bonding type (ionic or covalent). Compound Solid/liquid/gas Type of Bonding Sucrose, C 12 H 22 O 11 Sodium chloride, NaCl Methane, CH 4 Paraffin Wax, C 12 H 52 Calcium oxide, CaO Silicon dioxide (sand), SiO 2 Carbon dioxide, CO 2 Acetone, C 2 H 6 O Potassium iodide, KI liquid solid solid gas solid solid solid gas liquid solid covalent covalent ionic covalent covalent ionic covalent covalent covalent ionic

168 Physical State & Bonding Type

169 Physical State & Bonding Type Conclusions All ionic substances are in the solid state at room temperature. Covalent substances can be, solid liquid or gas at room temperatures.

170 Solubility & Bonding Type Test the solubility of each of the substances listed below and try to spot any patterns based on bonding type. Remember only to use a tiny quantity of each sample. Compound Type of Bonding Soluble / Insoluble Copper Chloride, CuCl 2 Sucrose, C 12 H 22 O 11 Sodium chloride, NaCl Starch, (C 6 H 10 O 5 )n Paraffin Wax, C 12 H 52 Sodium thiosulfate, Na 2 S 2 O 3 Silicon dioxide (sand), SiO 2 ionic covalent ionic covalent covalent ionic covalent soluble soluble soluble insoluble insoluble soluble insoluble

171 Solubility & Bonding Type Conclusions Ionic substances are usually soluble in water. Covalent substances can vary in their solubility. Some are soluble in water (they do dissolve). and others are insoluble in water (they do not dissolve). Sometimes covalent compounds which do not dissolve in water do dissolve in other solvents.

172 Learning Objectives & Success Criteria Today we will learn About the properties of compounds and how they link to the type of bonding in that compound. We will do this by Examining the state of different compounds at room temperature. Testing the solubility of various compounds. Spotting any patterns based on the type of bonding. We will have succeeded if We can state how the physical state and solubility of compounds varies based on their type of bonding.

173 Exit Task Question you have about the lesson Pyramid Things you have been reminded of today Things you have learned today

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175 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 14 Properties of Compounds: Electrical Conductivity REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

176 Learning Objectives & Success Criteria Today we will learn About the properties of compounds and how they link to the type of bonding in that compound. We will do this by Testing the conductivity of various compounds. Spotting any patterns based on the type of bonding. We will have succeeded if We can state how the conductivity of compounds varies based on their type of bonding.

177 Electrical Conductivity Electricity is a flow of charged particles. Elements and compounds that conduct electricity are called. conductors Elements and compounds that do not conduct electricity are called non-conductors (or insulators ).

178 Testing Electrical Conductivity What happens when a substance is included as part of an electrical circuit gives us information about the particles in the substance and the way they are held together. The terminals through which the electrical current enters and leaves the substance under test are called the electrodes.

179 Testing the Conductivity of Compounds Compound Type of Bonding Conductor / Non-conductor Copper chloride (s), CuCl 2 Copper chloride (aq), CuCl 2 Sucrose (s), C 12 H 22 O 11 Sucrose (aq), C 12 H 22 O 11 Sodium chloride (s), NaCl Sodium chloride (aq), NaCl Sodium thiosulfate (s), Na 2 S 2 O 3 Sodium thiosulfate (aq), Na 2 S 2 O 3 Starch (s), (C 6 H 10 O 5 ) n Paraffin Wax (s), C 12 H 52 Silicon dioxide (s), SiO 2 ionic ionic covalent covalent ionic ionic ionic ionic covalent covalent covalent non-conductor conductor non-conductor non-conductor non-conductor conductor non-conductor conductor non-conductor non-conductor non-conductor

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181 Conductivity & Bonding Type

182 Conductivity & Bonding Type Conclusions Covalent compounds never conduct electricity, no matter what the physical state. The conductivity of ionic compounds varies dependent on the physical state. Solid ionic compounds conduct never electricity but molten (liquid) and dissolved (aqueous) ionic compounds always do.

183 Learning Objectives & Success Criteria Today we will learn About the properties of compounds and how they link to the type of bonding in that compound. We will do this by Testing the conductivity of various compounds. Spotting any patterns based on the type of bonding. We will have succeeded if We can state how the conductivity of compounds varies based on their type of bonding.

184 Show Me Board - Exit Task State whether each numbered label should say conductor or non-conductor on the diagram below

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186 Lesson Starter Sort the list of substance names under the appropriate heading. Metal Element Non-metal Element Ionic Compound Covalent compound

187 Lesson Starter Sort the list of substance names under the appropriate heading. Metal Element Non-metal Element Ionic Compound Covalent compound solid iron solid carbon (graphite) solid copper chloride molten wax (C 12 H 52 ) liquid bromine Liquid potassium sulphide glucose solution (C 6 H 12 O 6 ) Sodium bromide solution

188 S3 Chemistry Atomic Structure, Bonding & Properties Lesson 15 Properties of Substances Summarised & Explained REVISION I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relative to their positions SCN 3-15a NEW LEARNING Through gaining an Understanding of the structure of atoms and how they join, I can begin to connect the properties of substances with their possible structures SCN 4-15a Atomic structure and bonding related to properties of materials National 4

189 Learning Objectives & Success Criteria Today we will Summarise the key properties of different types of substances and explain conductivity and physical state at room temperature. We will do this by Practice using the name of a substance to decide what TYPE of substance it is, what type of BONDING it will have and what PROPERTIES it is likely to have from our experiments. Hearing about why only certain substances conduct. Using diagrams to understand state at room temperature. We will have succeeded if We can state the key properties of different substance types and explain some of them.

190 Elements: Conductors or Non-Conductors? Sort the list of elements under the appropriate heading. Conductor Non-conductor solid copper Liquid nitrogen molten magnesium solid iodine molten iron argon gas chlorine gas solid graphite liquid mercury solid sodium liquid bromine

191 Elements: Conductors or Non-Conductors? Sort the list of elements under the appropriate heading. Conductor Non-conductor solid copper molten magnesium molten iron solid graphite liquid mercury Liquid nitrogen solid iodine argon gas chlorine gas liquid bromine solid sodium

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194 Compounds: Conductors or Non-Conductors? Sort the list of compounds under the appropriate heading. Conductor Non-conductor liquid hexane (C 6 H 12 ) barium nitrate solution solid carbon tetrachloride solid magnesium chloride sodium sulfate solution molten sodium chloride molten aluminium fluoride solid silver bromide liquid ethanol (C 2 H 5 OH) liquid selenium chloride

195 Compounds: Conductors or Non-Conductors? Sort the list of compounds under the appropriate heading. Conductor Non-conductor molten sodium chloride liquid hexane (C 6 H 12 ) barium nitrate solution solid carbon tetrachloride molten aluminium fluoride solid silver bromide sodium sulfate solution solid magnesium chloride liquid ethanol (C 2 H 5 OH) liquid selenium chloride

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198 Conductivity of Substances - Explained In order for a substance to conduct electricity it must contain charged particles which can. flow Non-metal elements and covalent compounds do not contain any charged particles so do not conduct electricity. Metal elements and carbon in the form of graphite do conduct because they contain delocalised electrons (charged particles which can flow). Ionic compounds contain ions (charged particles) but they are only free to flow when ionic compounds are molten or in solution. So ionic compounds only conduct electricity in these states, not when. solid

199 Ionic Substances Physical State- Explained Ionic compounds are all solid at room temperature because lots of very strong ionic bonds hold together the ions in giant ionic lattices. Very high temperature would be needed in order to have enough energy to break those bonds (melt the substance).

200 Covalent Substances Physical State- Explained Remember there are two types of covalent substance: Covalent Networks are all solid at room temperature because lots of very strong covalent bonds hold together the atoms in giant networks. Very high temperature would be needed in order to have enough energy to break those bonds (melt the substance).

201 Covalent Substances Physical State- Explained Remember there are two types of covalent substance: Covalent Molecules are all liquid or gas at room temperature because only very weak attractive forces must be broken between molecules to make them melt/boil. We are not breaking the strong covalent bonds within the molecule. So only a very low temperature would be needed to have enough energy to do this.

202 Properties of Compounds OVERALL SUMMARY Complete the table below using the information you have learned over the last few lessons: Property Ionic Compounds Covalent Compounds State(s) at room temperature. Relative melting & boiling points Solubility in water Electrical conductivity when solid Electrical conductivity when molten (liquid) Electrical conductivity when in solution (aqueous) solid high soluble non-conductor conductor conductor solid, liquid or gas high or low soluble or insoluble non-conductor non-conductor non-conductor

203 Learning Objectives & Success Criteria Today we will Summarise the key properties of different types of substances and explain conductivity and physical state at room temperature. We will do this by Practice using the name of a substance to decide what TYPE of substance it is, what type of BONDING it will have and what PROPERTIES it is likely to have from our experiments. Hearing about why only certain substances conduct. Using diagrams to understand state at room temperature. We will have succeeded if We can state the key properties of different substance types and explain some of them.

204 Exit Task Consider the work you have done in this whole topic. Select two things you have done/understood well and one thing you still don t understand/have to work on. Two Stars & A Wish