Chemistry flashcards

176 QCE Chemistry cards across 4 modules (53 definitions, 70 key facts, 12 fill-the-gap, 41 formulas). Each session gives you 20 cards, due cards first. Swipe right for easy, left for hard, down for again. Keyboard: Space to flip, 1 to 4 to rate.

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What this deck covers

Unit 1: Chemical fundamentals (structure, properties and reactions) (39 cards, 8 dot points)
Unit 2: Molecular interactions and reactions (29 cards, 7 dot points)
Unit 3: Equilibrium, acids and redox reactions (47 cards, 8 dot points)
Unit 4: Structure, synthesis and design (61 cards, 12 dot points)

Sample cards from this deck

Definition
Covalent bonding, Lewis structures, VSEPR and polarity (QCE Chemistry Unit 1)
Define CH_4
Four C-H bonds (very weak polarity). Tetrahedral, perfectly symmetric. Bond dipoles cancel. Non-polar overall.
Definition
The pH scale and introduction to acid-base chemistry (QCE Chemistry Unit 2)
Define Strong acid or base: ionises essentially completely in water
Written with a single arrow. The concentration of dissolved H+ (or OH-) equals the concentration of acid (or base) added.
Definition
Bronsted-Lowry acids and bases (QCE Chemistry Unit 3)
Define HCO3- (hydrogencarbonate)
Acid: donates H+ to give CO3^2-. Base: accepts H+ to give H2CO3.
Definition
Addition polymerisation and polymer properties (QCE Chemistry Unit 4)
Define HDPE (high-density polyethene)
Made by low-pressure Ziegler-Natta catalysis. Chains are essentially linear (few branches). Tight packing; density 0.94 to 0.97 g/cm^3; crystallinity around 60 to 80 percent. Stiff, opaque, higher softening point (about 130 to 135 degrees C). Used for milk crates, rigid pipes, fuel tanks.
Definition
Electron configuration and periodic trends (QCE Chemistry Unit 1)
Define Across a period
Z rises by one each step; S stays roughly constant (electrons added to the same shell shield each other poorly). So Z_eff rises strongly.
Definition
Solubility rules and precipitation reactions (QCE Chemistry Unit 2)
Define Complete ionic equation
All aqueous strong electrolytes (soluble ionic compounds and strong acids/bases) are written as separated ions. Insoluble solids, weak electrolytes, gases and molecular liquids stay together.
Definition
Buffer systems and resistance to pH change (QCE Chemistry Unit 3)
Define Weak acid plus its conjugate base
For example, ethanoic acid (CH3COOH) and sodium ethanoate (CH3COONa).
Definition
Chromatography techniques: TLC, GC and HPLC (QCE Chemistry Unit 4)
Define Mobile phase (eluent)
A liquid or gas that flows over or through the stationary phase, carrying the sample with it.
Definition
Exothermic and endothermic reactions, enthalpy and calorimetry (QCE Chemistry Unit 1)
Define Products
Products (ending energy, right; lower than reactants for exothermic, higher for endothermic).
Fill the gap
Stoichiometry of reactions involving gases (QCE Chemistry Unit 2)
Example: a reaction theoretically gives ___ of NH_3 from a fixed amount of N_2 and H_2 at 200 degrees C and 300 kPa; the actual yield collected is 4.50 L, measured at the same temperature and pressure.
Example: a reaction theoretically gives 0.500 mol of NH_3 from a fixed amount of N_2 and H_2 at 200 degrees C and 300 kPa; the actual yield collected is 4.50 L, measured at the same temperature and pressure.