# NSW HSC & Victoria VCE Chemistry & Physics: Equilibrium, Acid/Base Reactions, Organic Synthesis, Electromagnetism & Quantum/Light

> High-yield NESA NSW HSC and VCAA Victoria VCE Chemistry and Physics formulas, Le Chatelier's principle, Ksp, Brønsted-Lowry acids/bases, organic reaction pathways, spectroscopy (NMR, IR, MS), electromagnetism, and special relativity/quantum physics.

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- **Total Cards:** 32

## Flashcards (32 Cards)

| # | Front (Term / Prompt) | Back (Definition / Answer) | Example | Multiple-Choice Options |
| :--- | :--- | :--- | :--- | :--- |
| 1 | In HSC Chemistry (Module 5), how is the Solubility Product (Ksp) calculated for PbI2(s) ⇌ Pb2+(aq) + 2I-(aq) if its molar solubility s is 1.3 × 10^-3 mol/L, and what is the Common Ion Effect? | Ksp = [Pb2+][I-]^2 = (s)(2s)^2 = 4s^3 = 4 × (1.3 × 10^-3)^3 = 8.8 × 10^-9. Common Ion Effect: Adding a soluble salt containing a common ion (e.g., NaI adds I-) shifts the dissolution equilibrium to the left (by Le Chatelier's principle), markedly decreasing the molar solubility of PbI2 without changing Ksp. |  |  |
| 2 | In VCE Chemistry (Units 3–4), compare Galvanic (Voltaic) Cells, Electrolytic Cells, and Hydrogen Fuel Cells. | In ALL electrochemical cells: Oxidation occurs at the Anode and Reduction occurs at the Cathode ('AN OIL RIG CAT'). Galvanic Cell: spontaneous redox reaction (ΔG < 0, E°cell > 0) converting chemical energy to electrical energy; Anode is NEGATIVE, Cathode is POSITIVE. Electrolytic Cell: non-spontaneous reaction driven by external DC power supply; Anode is POSITIVE (connected to + terminal), Cathode is NEGATIVE. Fuel Cell: Galvanic cell with a continuous external supply of reactants (e.g., H2 at anode, O2 at cathode) that never goes flat as long as fuel is supplied. |  |  |
| 3 | In HSC & VCE Physics (Advanced Mechanics), what are the equations for Projectile Motion, Banked Circular Tracks (no friction), and Kepler's Third Law / Orbital Velocity? | Projectile Motion: Horizontal velocity vx = u·cosθ (constant, ax = 0); Vertical velocity vy = u·sinθ - gt; Time of flight (level ground) T = 2u·sinθ / g; Max height H = (u·sinθ)^2 / 2g. Banked Track (design speed v with zero sideways friction): tanθ = v^2 / (r·g). Orbital Velocity: Centripetal force = Gravitational force → v = √(GM / r); Escape velocity v_esc = √(2GM / r) = √2 · v_orbital; Kepler's 3rd Law: r^3 / T^2 = GM / (4π^2). |  |  |
| 4 | In HSC & VCE Chemistry, state Le Chatelier's Principle and predict how an exothermic equilibrium [N2(g) + 3H2(g) ⇌ 2NH3(g), ΔH = -92 kJ/mol] responds to: 1) Increased pressure (decreased volume), 2) Increased temperature, and 3) Addition of an iron catalyst. | Le Chatelier's Principle: If a system at dynamic equilibrium is subjected to a disturbance, the system shifts partially to counteract the disturbance. 1) Increased pressure shifts toward the side with FEWER gas moles (right → more NH3, 4 moles to 2 moles; Keq unchanged). 2) Increased temperature shifts in the ENDOTHERMIC direction (left → less NH3, and Keq DECREASES). 3) A catalyst lowers activation energy (Ea) of both forward and reverse reactions equally—reaches equilibrium faster, NO change in yield or Keq. |  |  |
| 5 | In HSC & VCE Physics (Electromagnetism), compare the magnetic force on a current-carrying wire (F = BIL·sinθ) with the Lorentz force on a moving charge (F = qvB·sinθ), and calculate the radius of the circular path of a charge in a uniform magnetic field. | When a charge q enters a magnetic field B perpendicular to its velocity v (θ = 90°), the magnetic force F = qvB acts purely perpendicular to v, doing ZERO work (kinetic energy and speed remain constant) and providing centripetal force: qvB = mv^2 / r → Radius r = mv / (qB). |  |  |
| 6 | On the Hertzsprung-Russell (H-R) Diagram (HSC Module 8), list the 4 main stellar regions, the nuclear fusion processes in Main Sequence vs. Red Giant stars, and the final stellar remnants by core mass. | Regions: Main Sequence (diagonal band from hot luminous O/B blue giants to cool dim M red dwarfs), Red Giants, Supergiants, and White Dwarfs (hot but very dim/small in lower-left). Main Sequence stars fuse H → He via the Proton-Proton chain (<1.3 solar masses) or CNO cycle (>1.3 solar masses). Red Giants fuse He → C and O via the Triple-Alpha process. Final remnants: <1.4 solar masses (Chandrasekhar limit) → White Dwarf (electron degeneracy pressure); 1.4–3 solar masses → Neutron Star; >3 solar masses → Black Hole. |  |  |
| 7 | In HSC & VCE Organic Chemistry, explain why the boiling points of homologous series for a given carbon chain length increase in the order: Alkane < Alkene < Haloalkane/Aldehyde/Ketone/Ester < Amine < Alcohol < Carboxylic Acid < Amide. | Determined by strength of Intermolecular Forces (IMFs): Alkanes/Alkenes are non-polar and have only weak dispersion forces (increasing with molar mass/chain length and decreasing with branching). Aldehydes, ketones, esters, and haloalkanes are polar and add dipole-dipole forces. Amines and Alcohols form strong intermolecular Hydrogen Bonds (O-H is more polar than N-H). Carboxylic acids form stable hydrogen-bonded dimers (2 H-bonds per pair), and primary Amides form extensive multi-site hydrogen bonding networks. |  |  |
| 8 | What is the relationship between pH, pOH, [H3O+], [OH-], Ka, Kb, and Kw at 25°C, and how does water's pH change when heated to 50°C? | At 25°C: Kw = [H3O+][OH-] = Ka × Kb = 1.0 × 10^-14; pH = -log10[H3O+]; pH + pOH = pKa + pKb = 14.00. Auto-ionization of water [2H2O(l) ⇌ H3O+(aq) + OH-(aq), ΔH > 0] is ENDOTHERMIC: heating water to 50°C shifts equilibrium right, increasing [H3O+] and [OH-] equally, so Kw increases and pH drops below 7.00, yet the water remains strictly NEUTRAL because [H3O+] = [OH-]. |  |  |
| 9 | In VCE Chemistry (Unit 4), how is a Calorimeter calibrated electrically or chemically (Calibration Factor CF), and how do you calculate the molar enthalpy of combustion ΔHc? | Electrical calibration: CF = E / ΔT = (V × I × t) / ΔT (in J/°C or J/K). When a fuel of mass m (or moles n) is burned causing temperature rise ΔTfuel: Energy released q = CF × ΔTfuel; Molar Enthalpy ΔHc = -q / n(fuel). Heat loss to surroundings increases the measured Calibration Factor if occurring during calibration, or decreases measured ΔT if occurring only during fuel combustion. |  |  |
| 10 | In HSC Physics (Module 8: From the Universe to the Atom), what are the 3 pillars of observational evidence supporting the Big Bang Theory? | 1) Hubble's Law of cosmological expansion (recessional velocity v = H0·d, measured via cosmological redshift of galactic absorption spectra), 2) Cosmic Microwave Background (CMB) radiation (uniform 2.7 K blackbody glow discovered by Penzias & Wilson—redshifted relic radiation from recombination 380,000 years after the Big Bang), and 3) Primordial Nucleosynthesis abundance ratio (~75% Hydrogen to ~25% Helium by mass). |  |  |
| 11 | In Nuclear Physics, compare Alpha (α), Beta-minus (β-), Beta-plus (β+ / Positron), and Gamma (γ) radioactive decay, and define Mass Defect and Binding Energy per Nucleon. | α (4/2 He nucleus): high ionizing power, low penetration (stopped by paper), A decreases by 4, Z by 2. β- (n → p + e- + anti-neutrino): moderate penetration (stopped by 5 mm Al), A unchanged, Z increases by 1. β+ (p → n + e+ + neutrino): Z decreases by 1. γ (high-energy photon): low ionizing, high penetration (thick lead). Mass Defect Δm = (Z·mp + N·mn) - m_nucleus; Binding Energy EB = Δm·c^2 (or Δm in u × 931.5 MeV). Iron-56 / Nickel-62 sits at the peak of the Binding Energy per Nucleon curve (~8.8 MeV/nucleon); Fission splits heavy nuclei (U-235) and Fusion combines light nuclei (H-2 + H-3) toward Iron-56. |  |  |
| 12 | How do you compare the Reaction Quotient (Q) with the Equilibrium Constant (Keq) to predict the direction of net reaction? | For aA + bB ⇌ cC + dD, Q = ([C]^c[D]^d) / ([A]^a[B]^b) excluding pure solids and pure liquids. If Q < Keq: forward reaction is favoured (shifts right to produce more products). If Q = Keq: system is at dynamic equilibrium. If Q > Keq: reverse reaction is favoured (shifts left to produce more reactants). Temperature is the ONLY factor that changes the numerical value of Keq. |  |  |
| 13 | Contrast the Classical Wave Model predictions with Einstein's Photon Model for the Photoelectric Effect (K_max = hf - φ). | Classical wave theory falsely predicted that light of ANY frequency would eject photoelectrons if intensity was high enough (after a time delay), and that higher intensity would increase maximum kinetic energy. Experiment showed: 1) Below a metal-specific Threshold Frequency f0 (where Work Function φ = hf0), ZERO electrons are emitted regardless of intensity; 2) Above f0, emission is instantaneous; 3) K_max = e·V_stop = hf - φ depends ONLY on frequency f (gradient of K_max vs. f graph is always Planck's constant h), while higher Intensity increases photocurrent (number of photons/sec) without changing K_max. |  |  |
| 14 | Compare the operation of a DC Motor (split-ring commutator) vs. an AC Induction Motor (squirrel-cage rotor) vs. an AC Alternator (slip rings). | DC Motor: Split-ring commutator reverses the current direction in the rotor coil every half-turn (180°) when the coil is perpendicular to the magnetic field so torque τ = nBIA·cosθ remains unidirectional. AC Alternator: Uses continuous Slip Rings to output sinusoidal AC EMF. AC Induction Motor: Stator windings fed by out-of-phase AC create a rotating magnetic field that induces eddy currents in the squirrel-cage rotor bars; by Lenz's law, the rotor chases the rotating magnetic field without any brushes or commutator. |  |  |
| 15 | In HSC & VCE Instrumental Analysis, match the key absorption/signal features for Infrared (IR) Spectroscopy, Mass Spectrometry (MS), 13C NMR, and 1H NMR. | IR Spectroscopy (bond vibrations): Broad O-H alcohol peak at 3200–3600 cm^-1; very broad 'bearded' O-H carboxylic acid peak at 2500–3300 cm^-1; sharp strong C=O carbonyl peak at ~1680–1750 cm^-1. Mass Spec: Molecular ion peak (M+) gives Molar Mass; base peak is the tallest (most stable/abundant) fragment cation. 13C NMR: Number of peaks = number of unique carbon environments; chemical shift δ identifies functional groups (C=O at 160–220 ppm). 1H NMR: Number of signals = unique proton environments; Peak Area integration = ratio of protons; Splitting (n+1 rule) = number of non-equivalent protons (n) on adjacent carbons. |  |  |
| 16 | How does Cosmic Ray Muon Decay provide experimental evidence for Special Relativity (Time Dilation and Length Contraction)? | Muons created in the upper atmosphere (~10 km up) travelling at 0.995c have a proper half-life t0 = 2.2 µs (classically decaying in ~660 m before reaching Earth). In Earth's frame, the muon's half-life is time-dilated by γ ≈ 10 to 22 µs, allowing it to travel >6.6 km. In the muon's rest frame, its half-life is still 2.2 µs, but the atmosphere's thickness is length-contracted by γ ≈ 10 from 10 km to 1 km. |  |  |
| 17 | Compare the Oxidation products of Primary (1°), Secondary (2°), and Tertiary (3°) Alcohols when heated with acidified Potassium Dichromate (Cr2O7^2-/H+) or Permanganate (MnO4^-/H+). | Primary (1°) Alcohol: gentle heating + distillation yields an Aldehyde; prolonged heating under Reflux with excess oxidant yields a Carboxylic Acid. Secondary (2°) Alcohol: oxidation under reflux yields a Ketone (cannot be oxidized further). Tertiary (3°) Alcohol: NO reaction with acidified dichromate/permanganate (no C-H bond on the hydroxyl-bearing carbon). Color changes: orange Cr2O7^2- turns green Cr3+; purple MnO4^- turns colourless Mn2+. |  |  |
| 18 | In Einstein's Special Theory of Relativity (HSC & VCE Physics), state the Two Postulates and write the formulas for Time Dilation, Length Contraction, Relativistic Momentum, and Mass-Energy Equivalence. | Postulate 1: The laws of physics are identical in all inertial (non-accelerating) frames of reference. Postulate 2: The speed of light in a vacuum c is constant (3.00 × 10^8 m/s) for all inertial observers regardless of motion of source or observer. Lorentz factor γ = 1 / √(1 - v^2/c^2) ≥ 1. Time Dilation: t = γ·t0 (moving clocks tick slower). Length Contraction: L = L0 / γ (contracted ONLY parallel to direction of motion). Relativistic momentum: p = γ·m0·v; Total energy E = γ·m0·c^2; Kinetic energy Ek = (γ - 1)m0·c^2. |  |  |
| 19 | In the Standard Model of Particle Physics (HSC Module 8), classify the 6 Quarks, 6 Leptons, and 4 Gauge Bosons, and state the quark composition of a Proton and a Neutron. | Matter fermions (12): 6 Quarks (Up, Down, Charm, Strange, Top, Bottom) which feel the Strong Nuclear Force and combine into Hadrons (Baryons = 3 quarks; Mesons = quark + antiquark); 6 Leptons (Electron, Muon, Tau, and their 3 corresponding Neutrinos) which do NOT feel the strong force. Proton = uud (+2/3 + 2/3 - 1/3 = +1); Neutron = udd (+2/3 - 1/3 - 1/3 = 0). Gauge Bosons (force carriers): Photon (electromagnetic), Gluon (strong nuclear), W+/W-/Z0 bosons (weak nuclear), plus the Higgs Boson (gives mass via the Higgs field). |  |  |
| 20 | What are the reagents, catalyst, and reflux conditions for Fischer Esterification, and how do you name the ester formed from Propanoic Acid and Butan-1-ol? | Heat the carboxylic acid and alcohol under Reflux with a concentrated Sulfuric Acid (H2SO4) catalyst (which acts as both a protonating catalyst to increase rate and a dehydrating agent to shift equilibrium toward the ester). Propanoic acid + Butan-1-ol ⇌ Butyl propanoate + H2O (the alcohol gives the '-yl' prefix; the carboxylic acid gives the '-oate' suffix). |  |  |
| 21 | State Faraday's Law of Electromagnetic Induction and Lenz's Law, and explain why Lenz's Law is a direct consequence of the Law of Conservation of Energy. | Faraday's Law: The magnitude of induced EMF in a circuit is directly proportional to the rate of change of magnetic flux linkage: ε = -N · (ΔΦB / Δt), where ΦB = B·A·cosθ. Lenz's Law (the minus sign): An induced current always flows in a direction such that its own magnetic field OPPOSES the change in magnetic flux that produced it. If it aided the flux change, it would create a self-accelerating runaway current, violating Conservation of Energy. |  |  |
| 22 | Compare the Arrhenius, Brønsted-Lowry, and Lewis definitions of Acids and Bases (HSC Module 6). | Arrhenius: Acid produces H+ in aqueous solution; Base produces OH- in aqueous solution (limited to aqueous solutions). Brønsted-Lowry: Acid is a proton (H+) donor; Base is a proton (H+) acceptor (explains gas-phase reactions like NH3(g) + HCl(g) → NH4Cl(s) and conjugate acid-base pairs). Lewis: Acid is an electron-pair acceptor (electrophile, e.g., BF3, AlCl3); Base is an electron-pair donor (nucleophile, e.g., :NH3). |  |  |
| 23 | In HSC & VCE Physics, explain the Transformer Equations, why Transformers require AC (not steady DC), and the two main causes of energy loss in a real transformer core. | Ideal Transformer: Vp / Vs = Np / Ns = Is / Ip (since Pp = Ps → Vp·Ip = Vs·Is). Steady DC produces a constant magnetic flux (ΔΦB / Δt = 0), so no EMF is induced in the secondary coil (except briefly at switch-on/off). Energy losses in real iron cores: 1) Eddy currents (minimized by using thin insulated laminated iron sheets perpendicular to flux), 2) Hysteresis loss (minimized using soft iron core), and 3) Flux leakage / Copper I^2R heating (minimized by high-voltage transmission: Ploss = I^2·R). |  |  |
| 24 | State Wien's Displacement Law and Planck's Quantum Hypothesis for Blackbody Radiation (the 'Ultraviolet Catastrophe'). | Wien's Law: λ_max · T = b (where b = 2.898 × 10^-3 m·K)—as a blackbody's absolute temperature T increases, its peak emission wavelength λ_max shifts to shorter (bluer) wavelengths and total radiated power increases at all wavelengths (P ∝ T^4). Classical Rayleigh-Jeans law predicted infinite UV energy at short wavelengths ('UV catastrophe'); Planck resolved this by postulating that electromagnetic energy is quantized in discrete packets E = nhf. |  |  |
| 25 | How did Indigenous Australians use solubility equilibria and leaching to detoxify Cycad seeds (Macrozamia) for food (HSC Module 5)? | Cycad seeds contain the water-soluble neurotoxin/carcinogen cycasin: cycasin(s) ⇌ cycasin(aq). By crushing the seeds (increasing surface area/reaction rate) and placing them in woven bags in running streams (open system), dissolved cycasin(aq) is continuously washed away, driving the equilibrium to the right until all solid toxin is leached out. |  |  |
| 26 | In HSC Chemistry (Module 7: Polymers), contrast Addition Polymerisation (LDPE vs. HDPE, PVC, Polystyrene, PTFE) with Condensation Polymerisation (Nylon-6,6 and PET Polyester). | Addition Polymerisation: unsaturated alkene monomers join via C=C double-bond opening with NO by-product (100% atom economy); LDPE (high pressure/temp free-radical peroxide initiator → highly branched, amorphous, low density/melting point flexible film) vs. HDPE (low pressure Ziegler-Natta catalyst → linear unbranched chains pack tightly, crystalline, rigid). Condensation Polymerisation: bifunctional monomers (e.g., diacid + diol → Polyester + H2O; hexanedioic acid + hexane-1,6-diamine → Nylon-6,6 polyamide + H2O) join with elimination of a small molecule like water. |  |  |
| 27 | In VCE Chemistry (Unit 4), compare the structure of Proteins (Primary, Secondary, Tertiary, Quaternary) and explain how Enzymes behave under pH/temperature denaturation vs. Competitive and Non-Competitive Inhibition. | Primary: covalent peptide bond sequence of amino acids. Secondary: α-helices and β-pleated sheets stabilized by hydrogen bonds between backbone C=O and N-H groups. Tertiary: 3D folding stabilized by R-group interactions (disulfide bridges -S-S-, ionic salt bridges, H-bonds, hydrophobic dispersion forces). Quaternary: multiple polypeptide subunits (e.g., haemoglobin). High temperature or extreme pH disrupts weak R-group/secondary bonds (Denaturation—primary peptide bonds stay intact unless hydrolyzed). Competitive inhibitors bind the Active Site (overcome by increasing [Substrate], Vmax unchanged, Km increases); Non-competitive inhibitors bind an Allosteric Site (alters active site shape, CANNOT be overcome by increasing [Substrate], Vmax decreases). |  |  |
| 28 | In Acid-Base Titrations, match the 3 acid-base combinations to the pH at the Equivalence Point and the best Indicator (Methyl Orange pH 3.1–4.4 vs. Bromothymol Blue 6.0–7.6 vs. Phenolphthalein 8.3–10.0). | 1) Strong Acid + Strong Base (HCl + NaOH): neutral salt (NaCl), Equivalence pH = 7.0 (Bromothymol Blue or Phenolphthalein). 2) Weak Acid + Strong Base (CH3COOH + NaOH): conjugate base CH3COO- hydrolyzes water to produce OH-, Equivalence pH > 7 (~8.7) → use Phenolphthalein. 3) Strong Acid + Weak Base (HCl + NH3): conjugate acid NH4+ donates H+ to water, Equivalence pH < 7 (~5.3) → use Methyl Orange. |  |  |
| 29 | State de Broglie's Matter-Wave Equation (λ = h / p) and explain how the Davisson-Germer electron diffraction experiment confirmed wave-particle duality and Bohr's quantized electron orbits. | de Broglie wavelength: λ = h / (mv). Davisson and Germer scattered electrons off a nickel crystal and observed constructive/destructive diffraction peaks matching X-ray Bragg diffraction. In Bohr's atom, stable electron orbits correspond to standing circular matter waves where the circumference equals an integer number of de Broglie wavelengths: 2πr = nλ = nh / (mv) → mvr = nh / (2π). |  |  |
| 30 | State Faraday's First and Second Laws of Electrolysis (VCE Chemistry Unit 3) and calculate the mass of Copper (M = 63.5 g/mol) deposited at the cathode from CuSO4(aq) by a current of 5.00 A for 30.0 minutes. | Charge Q = I × t = 5.00 A × (30.0 × 60 s) = 9,000 C. Moles of electrons n(e-) = Q / F = 9,000 C / 96,500 C/mol = 0.09326 mol. Half-equation: Cu2+(aq) + 2e- → Cu(s), so n(Cu) = n(e-) / 2 = 0.04663 mol. Mass m(Cu) = 0.04663 mol × 63.5 g/mol = 2.96 g. |  |  |
| 31 | In HSC & VCE Physics (Light & Waves), state Malus's Law for Plane-Polarised Light, Young's Double-Slit Interference formula, and what Polarisation proves about the nature of light. | Only TRANSVERSE waves can be polarised (proving light is a transverse wave). Malus's Law: I = I_max · cos^2(θ), where θ is the angle between the light's polarisation plane and the analyser's transmission axis. Young's Double Slit: Constructive interference (bright fringes) when path difference d·sinθ = mλ (m = 0, 1, 2...); Fringe spacing Δy = λL / d. |  |  |
| 32 | What is a Buffer Solution, how does the H2CO3 / HCO3- blood buffer respond to added acid (H+) or base (OH-), and where does the buffer region appear on a weak-acid titration curve? | A buffer contains comparable amounts of a weak acid and its conjugate base (or weak base + conjugate acid). In blood [H2CO3(aq) + H2O(l) ⇌ HCO3-(aq) + H3O+(aq)]: added H3O+ reacts with HCO3- to form H2O + H2CO3; added OH- reacts with H2CO3 to form HCO3- + H2O, resisting pH change. Maximum buffering capacity occurs at the Half-Equivalence Point where [HA] = [A-] and pH = pKa. |  |  |

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