Comprehensive Study Guide on Chemical Bonding, Physical Properties, and Organic Chemistry

Learning Intentions:
- Describe the formation of ionic bonds through the transfer of electrons between metal and non-metal atoms.
Success Criteria:
- Describe ionic bonding as the transfer of electrons from a metal atom to a non-metal atom.
- Use a model or diagram to describe the formation of a cation and an anion.
- Construct chemical formulas for simple ionic compounds.
- Investigate and describe a physical property of an ionic substance.

Key Vocabulary:
- Ionic bond: The strong electrostatic attraction between oppositely-charged ions.
- Cation: A positively charged ion formed when a metal atom loses valence electrons.
- Anion: A negatively charged ion formed when a non-metal atom gains valence electrons.
- Lattice: A regular, repeating three-dimensional arrangement of alternating oppositely charged ions held together by electrostatic forces.
Physical Properties of Ionic Solids:
- Hardness: Ionic solids are hard because of the strong electrostatic forces holding the lattice structure together.
- Brittleness: Ionic solids are brittle; when pressure is applied, like-charged ions align and repel each other, causing the crystal lattice to fracture.
- High Melting Point: Ionic solids have high melting points due to the extensive thermal energy required to overcome the strong electrostatic attractions throughout the ionic lattice.
Word Bank Reference (Alphabetical Order):
- brittle
- cation
- electrostatic
- hard
- ions
- lattice
- metal
- non-metal

Learning Intentions:
- Describe the formation of covalent bonds through electron sharing, and metallic bonds through delocalised electrons.
Success Criteria:
- Describe covalent bonding as non-metal atoms sharing pairs of valence electrons.
- Recognise that some elements exist as diatomic molecules.
- Describe metallic bonding as metal ions surrounded by a 'sea' of delocalised electrons.
- Construct chemical formulas for simple covalent molecules.

Key Vocabulary:
- Covalent bond: A bond in which two non-metal atoms share one or more pairs of valence electrons.
- Diatomic molecules: Molecules comprising two atoms of the same or different non-metal elements bonded covalently (e.g., $\text{H}_2$ , $\text{O}_2$ , $\text{N}_2$ , $\text{Cl}_2$ ).
- Metallic bonding: Electrostatic attraction between positive metal cations and a surrounding 'sea' of mobile, delocalised valence electrons.
- Delocalised electrons: Valence electrons that are free to move throughout the structure rather than being bound to a single atom.

Learning Intentions:
- Conduct an investigation to observe and compare the physical and chemical properties of ionic, covalent, and metallic substances, and explain how these relate to their uses.
Success Criteria:
- Safely conduct tests of melting behaviour, solid conductivity, and solubility/dissolved conductivity.
- Record results systematically in a table.
- Explain how each substance's properties relate to its bond type.
- Identify risks and apply safe practice throughout the investigation.
Key Vocabulary:
- Malleable: Able to be hammered or pressed into shape without breaking.
- Conductivity: The ability of a material to allow electricity (or heat) to pass through it.
Investigation Procedures and Safety Protocol:
- Melting Behaviour Test: Observe state changes and heat resistance to assess relative bonding strengths and melting point ranges across sample types.
- Solid Electrical Conductivity Test: Test raw solid samples in an electrical circuit to determine electron mobility.
- Solubility and Dissolved Conductivity Test: Attempt dissolution in liquid solvents ( $\text{H}_2\text{O}$ ) and test the conductivity of the resulting solutions to identify ion liberation.
- Risk Identification and Safe Practice: Follow mandatory laboratory protocols including wearing safety gear, handling heat sources cautiously, avoiding chemical skin contact, and mitigating electrical hazards.

Learning Intentions:
- Consolidate understanding of bonding by constructing a concept map and writing a scaffolded extended response.
Success Criteria:
- Summarise the key ideas of ionic, covalent, and metallic bonding in a concept map.
- Apply the six-level scaffold to plan and write an extended EVALUATE response.
- Analyse a set of investigation data to draw a conclusion.

Key Vocabulary:
- Directing verb: EVALUATE: Make a judgement about the merit, worth or value of something based on evidence, weighing up positives and negatives to reach an overall conclusion.
Extended Writing and Scaffold Application:
- Utilize a six-level scaffold framework to structure extended academic evaluation responses.
- Connect bonding concepts and experimental data to substantiate conclusions.
- Critically analyze positive and negative findings to arrive at an overall evidence-based judgment.
Word Bank Reference (Alphabetical Order):
- building
- concept
- connect
- Describe
- evidence
- Explain
- levels
- overall

Learning Intentions:
- Distinguish organic from inorganic compounds and describe how crude oil is separated into useful fractions by fractional distillation.
Success Criteria:
- Distinguish between organic and inorganic compounds.
- Define a hydrocarbon as a compound containing only carbon and hydrogen atoms.
- Describe how crude oil is separated into fractions using fractional distillation.
- Explain why different fractions come off the distillation column at different heights.
Key Vocabulary:
- Organic compound: A compound whose molecules are based on carbon, usually bonded with hydrogen (and often other elements).
- Inorganic compound: A compound that does not possess carbon-hydrogen ( $\text{C}-\text{H}$ ) structural frameworks.
- Hydrocarbon: A compound containing only carbon and hydrogen atoms.
Fractional Distillation Principles:
- Crude oil is heated to vaporize before entering the bottom of a fractionating column.
- The distillation column maintains a temperature gradient (hotter at the bottom, cooler at the top).
- Fraction Separation: Hydrocarbon fractions separate at different heights based on boiling points:
- Fractions with larger molecules and higher boiling points condense near the lower, hotter regions of the column.
- Fractions with smaller molecules and lower boiling points rise further up before condensing at cooler heights.