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It also links molecular shape to polarity and distinguishes polar versus non-polar character.",{"name":70,"@type":61,"acceptedAnswer":71},"What is taught about reactions of metals and ionic compounds?",{"text":72,"@type":64},"For metals, it includes metallic bonding properties, determining a reactivity series via oxidation with water, acids and oxygen, and metal recycling as a circular economy example. 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Elements and the periodic table |\n| --- | --- |\n| 1.1.1.1. the definitions of elements, isotopes and ions, including appropriate notation: atomic number; mass number; and number of protons, neutrons and electrons\u003Cbr>1.1.1.2. the periodic table as an organisational tool to identify patterns and trends in, and relationships between, the structures (including shell and subshell electronic configurations and atomic radii) and properties (including electronegativity, first ionisation energy, metallic and non-metallic character and reactivity) of elements\u003Cbr>1.1.1.3. critical elements (for example, helium, phosphorus, rare-earth elements and post-transition metals and metalloids) and the importance of recycling processes for element recovery | ●  What are Atoms, Elements and Compounds?\u003Cbr>●  Classification of Matter\u003Cbr>●  Rutherford-Bohr Model\u003Cbr>●  Introduction to Bonding\u003Cbr>● Atomic Number\u003Cbr>●  What are Isotopes?\u003Cbr>●  Isotope Properties\u003Cbr>●  Periodic Trends: Electronegativity\u003Cbr>●  Periodic Trends: Ionisation Energy\u003Cbr>●  Periodic Trends: Metallic Character\u003Cbr>●  Periodic Trends: Atomic Radius\u003Cbr>●  Group 15 and 16\u003Cbr>●  History of the Atomic Model\u003Cbr>● The Structure of an Atom\u003Cbr>● Atomic Symbols\u003Cbr>●  Electron Configuration Revision\u003Cbr>●  Electron Configuration of Atoms\u003Cbr>●  Electron Configuration of Ions |\n| Content Descriptor | EP Lessons in 1.1.2. Covalent substances |\n| 1.1.2.1. the use of Lewis (electron dot) structures, structural formulas and molecular formulas to model the following molecules: hydrogen, oxygen, chlorine, nitrogen, hydrogen chloride, carbon dioxide, water, ammonia, methane, ethane and ethene\u003Cbr>1.1.2.2. shapes of molecules (linear, bent, pyramidal, and tetrahedral, excluding bond angles) as determined by the repulsion of electron pairs according to valence shell electron pair repulsion (VSEPR) theory\u003Cbr>1.1.2.3. polar and non-polar character with reference to the shape of the molecule | ●  Covalent Bonding |\n|  | ●  Electron Dot Diagrams of Atoms\u003Cbr>●  Lewis Structures of Molecules and Ions\u003Cbr>●  Development of the VSEPR Theory |\n|  | ●  Introduction to Shapes of Molecules |\n|  | ●  Shapes of Molecules-Extended |\n|  | ● The Ionic-Covalent Continuum |\n\n\n| 1.1.2.4. the relative strengths of intramolecular bonding (covalent bonding) and intermolecular forces (dispersion forces, dipole-dipole attraction and hydrogen bonding)\u003Cbr>1.1.2.5. physical properties of molecular substances (including melting points and boiling points and non-conduction of electricity) with reference to their structure and bonding\u003Cbr>1.1.2.6. the structure and bonding of diamond and graphite that explain their properties (including heat conductivity and electrical conductivity and hardness) and their suitability for diverse applications | ●  Polarity of Molecules\u003Cbr>● Types of Intermolecular Forces\u003Cbr>●  Physical Properties of Molecular Substances\u003Cbr>●  Carbon Chemistry\u003Cbr>●  Covalent Network Substances\u003Cbr>●  Physical Properties of Covalent Network Substances\u003Cbr>● Allotropes of Carbon\u003Cbr>●  Nanomaterials |\n| --- | --- |\n| Content Descriptor | EP Lessons in 1.1.3. Reactions of metals |\n| 1.1.3.1. the common properties of metals (lustre, malleability, ductility, melting point, heat conductivity and electrical conductivity) with reference to the nature of metallic bonding and the existence of metallic crystals\u003Cbr>1.1.3.2. experimental determination of a reactivity series of metals based on their relative ability to undergo oxidation with water, acids and oxygen\u003Cbr>1.1.3.3. metal recycling as an example of a circular economy where metal is mined, refined, made into a product, used, disposed of via recycling and then reprocessed asthe same original product or repurposed as a new product | ●  Metals in the Periodic Table\u003Cbr>●  Metals, No","cbCaiixEJatNHBVC","https://ap.wps.com/l/cbCaiixEJatNHBVC","pdf",231396,"English","# Area of Study 1: How do the chemical structures of materials explain their properties and reactions?\n## EP Lessons 1.1.1: Elements and the periodic table\n## EP Lessons 1.1.2: Covalent substances\n## EP Lessons 1.1.3: Reactions of metals\n## EP Lessons 1.1.4: Reactions of ionic compounds\n# Area of Study 2: How are materials quantified and classified?\n## EP Lessons 1.2.1: Quantifying atoms and compounds","[{\"question\":\"What topics are included in EP Lessons 1.1.1 (Elements and the periodic table)?\",\"answer\":\"It covers definitions of elements, isotopes and ions, atomic and mass numbers, atomic structure relationships, periodic table patterns and trends (including shell/subshell configuration, electronegativity, ionisation energy, metallic/non-metallic character, reactivity, and atomic radii), as well as key elements and recycling for element recovery.\"},{\"question\":\"How does the curriculum model covalent substances and molecular shapes?\",\"answer\":\"It uses Lewis electron dot structures, structural and molecular formulas to model specified molecules, and explains molecular shapes using VSEPR theory. It also links molecular shape to polarity and distinguishes polar versus non-polar character.\"},{\"question\":\"What is taught about reactions of metals and ionic compounds?\",\"answer\":\"For metals, it includes metallic bonding properties, determining a reactivity series via oxidation with water, acids and oxygen, and metal recycling as a circular economy example. For ionic compounds, it covers properties related to ionic bonding and crystal structure, naming and formula deduction from component ions (including polyatomic ions), formation via electron transfer, and precipitation prediction using solubility tables and balanced full/ionic equations with state symbols.\"}]","2023 VCE Chemistry EP Curriculum Map Unit 1 - Diverse Materials - (Area of Study 1) | PDF",35]