Syllabus

• Acid and Base (strong, weak, and polyatomic).
• Choice of indicators.
• Redox (Permanganate, Iodometric).

• Cations (NH₄ ⁺, Na⁺, K⁺, Mg²⁺, Zn ²⁺ , Cu²⁺, Fe²⁺, Fe³⁺, Ca ²⁺ , Ba²⁺, Pb²⁺, Ag⁺).

• Anions (NO₃ ^-, S^2-, SO₃ ^2-, SO₄ ^2-, Cl^-, Br^-, I^-, CO ₃ ^2-, PO₄ ^3-, OH^-).

• Flame colors (Na, Li, K, Ca, Sr, Cu, B).
• Amphoteric oxides (Zn, Sn, Pb, and Al).

• Alkene, halogenoalkane, alcohol, aldehydes, carboxylic acids.

• Dyes: colour vs structure (aromaticity and chromophore).
• Beer's Law.

• Counting of nucleons.
• Isotopes.
• Types of radioactivity.
• Radioactive decay (alpha, beta, and gamma).

• Nuclear reactions (alpha and beta decay, positron emission, electron capture, gamma emission, and spontaneous fission).

• Balancing equations.
• Stoichiometric calculations.
• Mass and volume relations (including density).
• Mass, volume, and mole percent.
• Empirical formula.
• Avogadro's number.
• Concentration calculations.

• Main group elements (electron configuration, Pauli exclusion principle, Hund's rule, electronegativity, electron affinity, first ionization energy, atomic size, ion size, highest oxidation number).

• Main group trends in physical properties (melting point, boiling point, metal character, magnetic properties, and electrical conductivity)

• Reactivity series (K, Na, Ca, Mg, Al, C, Zn, Fe, Sn, Pb, H, Cu, Hg, Ag, Au).

• Bond types (polar/nonpolar and covalent/ionic bonds).

• Electronegativity (determine type of bond: ionic, polar, and nonpolar).

• Lewis structures.
• Octet rule.
• Formal charges.

• VSEPR (no more than four electron pairs about the central atom with the central atom exceeding the "octet rule").

• Delocalization and resonance.

• Combination reactions
• Decomposition reactions.
• Precipitation, single and double-replacement reactions.
• Redox reaction (neutral, alkaline, and acidic).

• Main group and transition metal compounds.

• Trend in Reactivity of (heavy elements more reactive).
• Products of reaction (water, halogens, and oxygen).
• Basicity of oxides.

• Binary molecular compounds of hydrogen, formulas, and acid-base properties (CH₄, NH₃, H₂O, H ₂S).

• The oxidation state of boron and aluminium in their oxides and chlorides is +III.

• Si's oxidation state in its chloride and oxide is +IV.
• The +II and +IV oxidation states of carbon, tin, and lead.

• Oxides of nitrogen (Reaction of NO to form NO2, dimerization of NO ₂, Reaction of NO₂ with water).

• Redox properties of nitrogen (HNO₃ and nitrates).

• The +IV and +VI oxidation states of sulfur, reaction of their oxides with water, and properties of their acids.

• Reaction of thiosulfate anion with iodine.

• Reactivity and oxidant strength decrease from fluorine to iodine.

• Acid-base properties of the hydrogen halides.
• The oxidation state of fluorine in its compounds is -I
• The -I, +I, +III, +V, and +VII oxidation states of chlorine.
• Reactions of halogens with water.

• Common oxidation states of common transition metals: Cr(+II), Cr(+III) Mn(+II), Mn(+IV), Mn(+VII) Ag(+I) Fe(+II), Fe(+III), Co(+II), Zn(+I), Cu(+I), Cu(+II), Ni(+II).

• The insolubility of Ag, Hg, and Cu in HCl.

• M²⁺ arising from the dissolution of the other metals in HCl.

• Permanganate and Dichromate are strong oxidants in acid solution.

• Definition of coordination number.

• Writing equations for complexation reactions given all formulas.

• Formulas of common complex ions (Ag(NH₃)₂ ⁺, Ag(S₂O₃)₂ ^3-,FeSCN⁺, Cu(NH₃)₄ ²⁺).

• Drawing structures (Condensed Formula, Kekule & Skeletal Structures).

• DBE (double bond equivalent).
• Properties, isomerism (structural and stereoisomerism).

• Substance classes: hydrocarbons (alkane, alkene, alkyne, simple cycloalkane and alkadiene), alcohols, aldehydes, ketones, carboxylic acids, and esters, as well as structure and properties of the substance classes amines, phenols, amides, and amino acids.

• Types of organic reactions: complete combustion, oxidation, substitution, addition, elimination, condensation, hydrolysis and decarboxylation.

• Ideal gas law.
• Dalton's law.

• First Law (Concept of systems and surroundings, Energy, Heat, and Work).

• Enthalpy (Relationship between internal energy and enthalpy).
• Enthalpy is a state property (Hess's law).
• Reaction enthalpy (use of standard formation enthalpies).
• Reaction entropy and disorder.

• Reaction Gibbs energy and definition (ΔG = ΔH – TΔS).

• Using ΔG to predict the direction and spontaneity.
• Relationship between Gibbs and equilibrium constant K.

• Equilibrium constant (homogeneous and heterogeneous).
• Reaction quotient (Q/Y).

• Relating equilibrium constants of pressure (K_p) and concentration (K_c).

• Le Chatelier's principle.

• Solubility constant (product) definition (K_sp).

• Calculation of solubility in water from K_sp.

• Common-Ion Effect.

• Complex formation constant (K_K)

• Simple coupled equilibria.

• Arrhenius definitions of acids and bases.
• Bronsted-Lowry definitions.
• Conjugate acids and bases.

• pH, K_w definition and K_a or K_b as a measure of acid and base strength.

• Acidity or basicity of ions.
• Buffer system and capacity.

• Calculation of pH from pK_a (weak acid).

• Calculation of pH of a simple buffer solution.

• Simple knowledge of amphoterism and their pH (pH = ½(pK _S1+pK_S2)).

• Factors affecting reaction rate.
• Reaction coordinates and the basic idea of a transition state.
• Differential rate laws.
• Concept of reaction order.
• Rate constant definition.

• 0, 1, and 2 order reactions and their integrated rate laws (single reactant).

• Dependence of concentration on time.
• Concept of half-life.
• Relationship between half-life and rate constant.

• Determine reaction order (method of initial rates and graphs of integrated rate laws).

• Reaction mechanisms (concept of molecularity, rate-determining step).

• Basic concepts of collision theory.
• Arrhenius's law.

• Catalysts and how it affects activation energies (homogeneous, heterogeneous, and biocatalysts).

• Solving quadratic equations.
• Use of logarithms and exponentials.
• Solving simultaneous equations with 2 unknowns.
• Elementary geometry such as Pythagorean's theorem.
• Plotting graphs (normal, exponential, and logarithmic).

• Recognition of molecular ions.
• Recognition of fragments with the help of a table.
• Recognition of typical isotope distribution.

• Bragg's Law.

• Interpretation using a table of frequencies (N-H stretch, O-H stretch, C-H stretch (sp²), C-H stretch (sp³), C=O stretch and C=C stretch).

• Recognition of hydrogen bonds.

• General concepts (chemical shift, integration, spin-spin coupling, and coupling constants).

• Interpretation of a simple ¹H spectrum

• Identification of o- and p-disubstituted benzene.

• Interpretation of simple spectra of ¹³C (proton decoupled) and other ½ spin nuclei.

• Complexometric titrations (EDTA).

• Transition metal elements (electron configuration, Pauli exclusion principle, Hund's Rule, electronegativity, electron affinity, first ionization energy, atomic size, ion size, highest oxidation number).

• Shape, orientation, and Quantum numbers (n, l, m) of s, p, and d orbitals.

• Radial and angular nodes.

• Valence bond theory (σ-bonds, π-bonds, hybrid orbitals).

• Molecular orbital (MO) diagram (2 period).
• Bond orders.
• Para- and diamagnetism.

• Comproportionation and disproportionation reactions.
• Special bonding (3c-2e) using molecular orbital theory.

• Simple metal complexes.

• Properties of hydrides.
• Other compounds, properties, and oxidation states.

• Other properties.

• The acid-base properties of aluminum oxide/hydroxide.

• Reaction of boron(III) oxide and boron(III) chloride with water.

• Other compounds, properties, and oxidation states.

• The acid-base and redox properties of the oxides and chlorides.
• Other compounds, properties, and oxidation states.

• Phosphorus (+III, +V) oxide and chloride, and their reaction with water.

• Redox properties (HNO₂ and NH₂NH₂).

• Bi(+V) and Bi(+III).
• Other compounds, properties, and oxidation states.

• Other compounds, properties, and oxidation states.

• Mononuclear oxoanions of chlorine.

• Reaction of Cl₂O and Cl₂O₇ with water.

• Other compounds, properties, and oxidation states.

• Colors of ions in aqueous solution: : Cr(+II), Cr(+III) Mn(+II), Mn(+IV), Mn(+VII) Ag(+I) Fe(+II), Fe(+III), Co(+II), Zn(+II), Cu(+I), Cu(+II), Ni(+II).

• Chromium hydroxide and Zinc hydroxide are amphoteric and the other +2 oxides/hydroxides of the metals listed above are basic.

• pH dependence of products of permanganate acting as oxidants.
• Interconversion between chromate and dichromate.
• Other compounds, properties, and oxidation states.

• Formulas of other complex ions.

• Ligand field theory (e_g and t_2g terms, high/low spin, and color).

• Color of complex compounds (spectrochemical series).
• Para and diamagnetic.

• Isomerism (Structural, Coordination, Linkage, Geometric: cis/trans, planar, octahedra, enantiomers).

• Unit cell (cubic).
• Coordination number.
• Packing type (aba, abc, abcd).
• Solid structures (metals, NaCl, CsCl, ZnS).
• Density for metals and salts.

• IUPAC nomenclature, including E/Z and R/S stereoisomerism.

• Draw stereochemically unequivocal structures for organic molecules.

• Account for optical activity and the difference between enantiomers, diastereomers, and meso compounds.

• Differentiate between S_N1/S_N2 and E1/E2 reactions.

• Draw resonance forms for cations and anions.

• Predict reactivity of organic molecules based on structure, resonance, and inductive effects.

• Draw reaction mechanisms for simple and polar reactions.

• Suggest syntheses in one or more steps of simple, organic molecules.

• Design simple reactions with common functional groups.

• Apply inorganic reagents for oxidation, reduction, and substitution in synthetic planning.

• Account for structure and reactivity of carbohydrates, amino acids, lipids, and nucleic acids.

• Born-Haber cycle for ionic compounds.
• Bond enthalpies (definition and use).

• Electromotive force (definition).
• Galvanic Cells.
• Notation of cell diagrams.
• Standard electrode potential.
• Nernst equation.
• Relationship between ΔG and electromotive force.
• Electrolysis.
• Corrosion.

• Lewis acids and bases (hard and soft).
• MCB (not too complex).
• Bjerrum plot (reading).

• Steady-State approximations (maximum of 4 steps, where an equilibrium step counts as 2 steps).

• Use of math skills from the bronze tier to derive simple expressions.

• Single-variable Calculus (basic derivatives and integrals).
• Taylor series.

Mathematical equations may be provided for questions.