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Year 10 Science Extension Term 1: CHEMISTRY Text: Pearson Science 10 SB 2e Year 10 Chemical Sciences Content Descriptions The atomic structure and properties of elements are used to organise them in the Periodic Table (ACSSU186) • • • • recognising that elements in the same group of the periodic table have similar properties describing the structure of atoms in terms of electron shells explaining how the electronic structure of an atom determines its position in the periodic table and its properties investigating the chemical activity of metals Different types of chemical reactions are used to produce a range of products and can occur at different rates (ACSSU187) • • • • investigating how chemistry can be used to produce a range of useful substances such as fuels, metals and pharmaceuticals predicting the products of different types of simple chemical reactions using word or symbol equations to represent chemical reactions investigating the effect of a range of factors, such as temperature and catalysts, on the rate of chemical reactions Wk Topic Content Activities Resources and Experiments Assessment & Homework 1 Atomic Structure AB: 5.1 – Knowledge preview SB: p193 prac 1 – Investigating a metallic element Unit Review Questions SB: 5.1 p192 SB 5.1 2 Ionic Compounds Revise the structure of an atom. Explain that the existence of atoms has been shown using a scanning tunnelling microscope (STM). The existence of sub-atomic particles has been postulated using indirect evidence. All elements are basically structurally the same. They have protons and neutrons in the nucleus and the nucleus is orbited by electrons. The number of protons determines the type of element. The number of protons is known as the atomic number. The atomic mass is the number of protons plus the number of neutrons. Discuss how analogies and models can be used to help with the visualisation of abstract concepts. Explain that all atoms of the same element have the same number of protons in the nucleus but that the number of neutrons can vary. Understand that ionic bonding occurs between metals and non-metals. In ionic bonding atoms gain a full outer shell of electrons through metals give electrons to non-metals causing the formation of ions Know the properties of ionic compounds and describe them o Can conduct electricity when molten or aqueous but not solid o High melting and boiling points o Hard o Brittle Understand that in ionic solids the ions are organised in a lattice, but when ionic solids are placed in solution the ions separate. SB: p194 prac 2 – Investigating a nonmetallic element Chemical formula writing worksheet- polyatomic and simple plus Lewis structures Chemical bondingintroduction and properties of metallic and ionic worksheet Experiments- A rough diamond from page 124 using soft lollies to make diamond Wk Topic Content Metallic compound Covalent compound Understand that in metallic bonding metals lose their valence electrons to form positive ions. The lost valence electrons become delocalised and are shared amongst all the metal ions forming a sea of electrons Use the atomic structure of metallic compounds to explain the properties of metals o Good conductors of heat and electricity o Hard o High melting and boiling points o Malleable and ductile Understand that covalent bonding occurs between non-metals. The atoms share electron pairs to gain a full outer shell of electrons. Covalent substances can either be found as molecules or networks Use the structure of covalent compounds to explain their properties o Molecules Poor conductors of heat and electricity Brittle and soft when solid low melting and boiling points o Networks high melting and boiling points strong and hard Can sometimes conduct electricity Activities Resources and Experiments Assessment & Homework Wk Topic Content Activities 3 Arranging the elements AB: 5.2 – Periodic nature of the elements SB 5.2 Family groupings SB 5.3 How the periodic table is arranged. Use Figure 5.2.1 to assist. Define the terms period and group as related to the periodic table. Outline the two numbering systems for the groups. Explain why elements in the same group have similar properties. The concept of grouping in the periodic table means that certain elements within the same group will have similarities. However, there are also a lot of differences within the family groupings. Outline the importance of the groupings, but also remind students of their differences. The properties of the alkali metals. Explain where they can be found in the periodic table. The properties of the Group 14 elements. Where they can be found in the periodic table and compare their diversity to the other groups The properties of the halogens. Explain where they can be found in the periodic table. The noble gases and their unreactive nature. Explain where they can be found in the periodic table. The properties of the transition metals. Explain where they can be found in the periodic table. AB: 5.5 – Organic chemistry (Extension activity) AB: 5.6 – Hydrocarbons (Extension activity) SB: p208 SkillBuilder – Predicting chemical equations AB: 5.4 – Families of the periodic table Resources and Experiments SB: p204 prac 2 – Cardgame analogy Alkali metals and alkaline earths, the halogens, noble gases, transition gases. SB: p213 Prac 1 – The alkaline earths SB: p204 Prac 2 – Halogen precipitates Assessment & Homework Unit Review Questions SB:5.2 p202 Unit Review Questions SB: 5.3 p212 Wk Topic Content Activities 4 Electrons and the periodic table Discuss how the development of human SB: p216 SkillBuilder – Electron configuration SB: 5.4 understanding of atomic structure influenced the periodic table. Explain how scientists came to understand that the electrons were largely responsible for the chemical activity of elements. Explain how electrons do not orbit the nucleus in a completely random way. They are arranged in energy levels or shells. Define the term electron configuration. Explain that electrons can gain or lose energy. As electrons gain energy they gain kinetic energy and move into high orbits around the nucleus as they lose energy the kinetic energy is converted to light and heat. (Remind students that energy is never created or destroyed; it is changed from one form to another.) The amount of energy being lost as light determines the colour of the flame. Emphasise that all elements in the same group have the same number of outer shell electrons. Explain that each period has one more shell than the previous period. This means that although elements are in the same group their properties are a little different. Emphasise that all elements in the same group have the same number of outer shell electrons. Explain that each period has one more shell than the previous period. This means that although elements are in the same group their properties are a little different. Explain why elements in the same group have similar properties. Discuss why the properties of elements change down a group. AB: 5.7 – Electron configuration and shells SB: p222 Prac 1 – Firework colours SkillBuilder – Periods and groups SB: p218 Worked example – Periods and groups Resources and Experiments Assessment & Homework Unit Review Question SB: 5.4 p221 Wk Topic Content Activities Resources and Experiments 5 Chemical equations AB: 6.1 – Knowledge preview SB: p236 Prac 2 – Conservation of mass SB: 6.1 Explain that chemical equations are a simple method for giving a detailed description of the changes which take place during a chemical reaction. Chemical equations can be written in words but convey much more information if symbols are used. An even more informative equation uses symbols for the chemicals and also indicates the state of those chemicals. States can be solid, liquid or gas or aqueous. Explain aqueous is not a state of matter but means the substance is dissolved in water. Revise the terms product and reactant. Emphasize that matter is not gained or lost during chemical reactions so every atom must be accounted for on both sides of a chemical equation. When the number of atoms of each atom is the same in the products and reactants then the equation is balanced. SB: p235 Prac 1 – Reactions with modelling clay SB: p232 STEM4fun – Conserving mass in chemical reactions SB: p236 SkillBuilder – Balancing equations SB: p233 Worked example – Balancing equations AB: 6.8 – Balancing chemical equations Assessment & Homework Atomic Structure, Periodic table, Bonding, topic test Unit Review Questions SB: 6.1 p234 Wk Topic Content Activities Resources and Experiments Assessment & Homework 6 Energy in Chemical Reactions Revise the concept that the bonds between atoms in compounds store energy. SB: p237 science4fun – Acrobatic flame Unit Review Questions SB: 6.2 p242 Define the terms exothermic and endothermic. Explain that in endothermic reactions the products possess more energy than the reactants and that the reverse is true for exothermic reactions. SB: p243 Prac 1 – Exothermic and endothermic reactions AB: 6.2 – Combustion of magnesium SB: 6.2 7 8 Combustion Corrosion Respiration The atomic structure and properties of elements are used to organise them in the Periodic Table (ACSSU186) SB: 6.3 investigating the chemical activity of metals Different types of chemical reactions are used to produce a range of products and can occur at different rates (ACSSU187); investigating how chemistry can be used to SB: p245 Prac 3 – Rust prevention These reactions are all exothermic but combustion reactions are more vigorous and produce large amounts of heat and light quickly. Investigation Classifying Chemical Reactions SB: p241 SHE – Biofuels Reactions with oxygen include: SB: p244Prac 2 – Corrosion as an exothermic reaction produce a range of useful substances such as fuels, metals and pharmaceuticals using word or symbol equations to represent chemical reactions predicting the products of different types of simple chemical reactions SB: p246 science4fun – Raisin lava lamp SB: p251 SkillBuilder – predicting precipitation reactions SB: p251 Worked example – Predicting precipitation reactions. AB: 6.3 – Classifying chemical reactions AB: 6.4 – Classifying chemical reactions in context SB: p255 Prac 1 – Heating metal carbonates Investigation validation SB: p256 Prac 2 – Precipitation reactions Unit Review Questions SB: 6.3 p254 SB: p257 Prac 3 – Identifying unknown solutions Student design Wk Topic Content Activities Resources and Experiments Assessment & Homework 9 Rates of Chemical Reaction Explain that reactions can occur at different rates. Explain that the rates of chemicals reactions can SB: p258 science4fun – Jellied fruit SB: p266 Prac 1 – Temperature and reaction rate Unit Review Questions SB: 6.4 p265 be influenced by external factors. Discuss each of these factors and how they change the rate of SB: 6.4 reaction. These factors include: Temperature Concentration of the reactants Surface area of the reactants Agitation (stirring of the reactants) Use of catalysts (either chemical or enzymes) AB: 6.5 – Reaction rate and surface area of reactants AB: 6.6 – Fast and slow reactions AB: 6.7 – Rate of chemical reactions–particle diagrams SB: p263 Working with science – Molecular gastronomy chef SB: p267 Prac 2 – Concentration and reaction rate SB: p268 Prac 3 – Agitation and reaction rate SB: p269 Prac 4 – Surface area and reaction rate Student design SB: p264 SHE – Enzymes in medicine 10 Topic Test Equations, Reactions Topic Test Assessment Outline Assessment Type Title Weighting Test Topic test. 10% Practical Investigation and Validation Electrolysis 10%