Chemistry flashcards

What this deck covers

• Unit 1: How can the diversity of materials be explained? (50 cards, 12 dot points)

  • Allotropes of carbon and covalent network solids: VCE Chemistry Unit 1 (5)
  • Atoms, isotopes and mass spectrometry: VCE Chemistry Unit 1 (3)
  • Chemical nomenclature and formulae (VCE Chemistry Unit 1) (5)
  • Covalent bonding, Lewis structures, VSEPR and polarity: VCE Chemistry Unit 1 (4)
  • Electron configurations and periodic trends: VCE Chemistry Unit 1 (5)
  • Empirical and molecular formulae (VCE Chemistry Unit 1) (4)
  • Intermolecular forces and covalent substances: VCE Chemistry Unit 1 (5)
  • Mass spectrometry as an analytical technique: VCE Chemistry Unit 1 (6)
  • Metallic and ionic bonding: VCE Chemistry Unit 1 (3)
  • Mole concept and stoichiometry (VCE Chemistry Unit 1) (3)
  • Organic functional groups (introduction) (VCE Chemistry Unit 1) (2)
  • Solubility, aqueous solutions and like dissolves like: VCE Chemistry Unit 1 (5)
• Unit 2: How do chemical reactions shape the natural world? (59 cards, 13 dot points)

  • Choosing analytical techniques for water quality: VCE Chemistry Unit 2 (5)
  • Colorimetry, UV-visible spectroscopy and AAS: VCE Chemistry Unit 2 (5)
  • Concentration units, acids and bases, and pH: VCE Chemistry Unit 2 (3)
  • Gravimetric analysis: VCE Chemistry Unit 2 (4)
  • Metal reactivity series and displacement reactions: VCE Chemistry Unit 2 (5)
  • Polarity and intermolecular forces in aqueous solutions: VCE Chemistry Unit 2 (3)
  • Properties of water, dissolving and precipitation: VCE Chemistry Unit 2 (5)
  • Reactions of acids with metals, oxides, hydroxides and carbonates: VCE Chemistry Unit 2 (5)
  • Redox reactions and oxidation numbers in water: VCE Chemistry Unit 2 (5)
  • Stoichiometry of aqueous reactions: VCE Chemistry Unit 2 (5)
  • Strong vs weak acids and bases, Ka and Kb: VCE Chemistry Unit 2 (5)
  • Volumetric analysis and titration: VCE Chemistry Unit 2 (3)
  • Writing ionic and net ionic equations for aqueous reactions: VCE Chemistry Unit 2 (6)
• Unit 3: How can design and innovation help to optimise chemical processes? (34 cards, 8 dot points)

  • Calorimetry and q = mcΔT: VCE Chemistry Unit 3 (4)
  • Dynamic equilibrium, Kc and Le Chatelier's principle: VCE Chemistry Unit 3 (3)
  • Electrolytic cells and Faraday's laws: VCE Chemistry Unit 3 (5)
  • Fuels, energy content and energy density: VCE Chemistry Unit 3 (5)
  • Galvanic cells, fuel cells and cell EMF: VCE Chemistry Unit 3 (5)
  • Rate of reaction and collision theory: VCE Chemistry Unit 3 (5)
  • Redox reactions and the electrochemical series: VCE Chemistry Unit 3 (4)
  • Thermochemical equations and enthalpy changes: VCE Chemistry Unit 3 (3)
• Unit 4: How are carbon-based compounds designed for purpose? (43 cards, 9 dot points)

  • Food chemistry: biomolecules, enzymes and energy content: VCE Chemistry Unit 4 (5)
  • Mass spectrometry and infrared spectroscopy: VCE Chemistry Unit 4 (3)
  • Medicinal chemistry and sustainable chemistry: VCE Chemistry Unit 4 (6)
  • Medicinal chemistry: drug action and structure-activity relationships (VCE Chemistry Unit 4) (5)
  • NMR spectroscopy and HPLC: VCE Chemistry Unit 4 (5)
  • Organic nomenclature and functional groups: VCE Chemistry Unit 4 (5)
  • Organic reactions and reaction pathways: VCE Chemistry Unit 4 (3)
  • Sustainable chemistry: 12 principles and atom economy (VCE Chemistry Unit 4) (6)
  • Unit 4 AoS 3 student-designed practical investigation: VCE Chemistry (5)

Sample cards from this deck

1. Definition

   Allotropes of carbon and covalent network solids: VCE Chemistry Unit 1

   Define Allotropes

   Allotropes are different structural forms of the same element in the same physical state. Carbon is the textbook example: the atoms are identical, but the way they bond to one another produces wildly different materials.

2. Definition

   Gravimetric analysis: VCE Chemistry Unit 2

   Define Quantitative precipitation

   Add the precipitating reagent in excess so essentially every analyte ion is captured in the solid phase.

3. Definition

   Calorimetry and q = mcΔT: VCE Chemistry Unit 3

   Define Bomb calorimetry

   A sample is burned in pure oxygen inside a sealed steel "bomb" surrounded by water. Because heat goes into multiple components (the steel bomb, the water jacket, the stirrer, the thermometer), the whole apparatus is calibrated with a known electrical input first. The calibration factor (CF, in J °C^-1) converts the measured ΔT directly into energy released.

4. Definition

   Food chemistry: biomolecules, enzymes and energy content: VCE Chemistry Unit 4

   Define Amino acids

   Amino acids are the monomers. Each has an alpha-carbon bonded to an NH2 (amine), a COOH (carboxylic acid), an H, and an R side chain. The 20 standard amino acids differ only in R. R groups can be non-polar (hydrophobic), polar (hydrophilic), acidic, or basic.

5. Definition

   Mass spectrometry as an analytical technique: VCE Chemistry Unit 1

   Define Acceleration

   A high voltage accelerates the cations to a common kinetic energy.

6. Definition

   Colorimetry, UV-visible spectroscopy and AAS: VCE Chemistry Unit 2

   Define Atomiser

   Atomiser (a flame, typically air/acetylene): aspirates the sample, evaporates the solvent, breaks compounds into atoms, and reduces ions to ground-state atoms.

7. Definition

   Electrolytic cells and Faraday's laws: VCE Chemistry Unit 3

   Define Cathode

   Cathode (reduction) is connected to the negative terminal of the power supply. Cations migrate to the cathode and gain electrons.

8. Definition

   Medicinal chemistry and sustainable chemistry: VCE Chemistry Unit 4

   Define Drug action

   Medicines are chemicals that modify biochemical processes (e.g. enzyme inhibition, receptor binding). Drugs typically interact with biological targets (enzymes, receptors, ion channels) using intermolecular forces: hydrogen bonding, ionic interactions, dispersion forces, dipole-dipole, hydrophobic interactions.

9. Definition

   Chemical nomenclature and formulae (VCE Chemistry Unit 1)

   Define Balance charges

   Total positive charge equals total negative charge.

10. Definition

    Writing ionic and net ionic equations for aqueous reactions: VCE Chemistry Unit 2

    Define Cancel spectator ions

    Cancel spectator ions (ions that appear identically on both sides). Check both mass and charge balance.