Course Details

Chemistry Grade 11-12

This course emphasizes the mathematical, theoretical, and experimental basis of modern chemistry. Emphasis is placed on the use of theoretical and mathematical concepts to explain and predict chemical behavior. We

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Why Choose Online Chemistry Grade 11-12 Classes?

Board-aligned tutors - we match the tutor to your child's curriculum (US Common Core, Ontario, Australian, CBSE, ICSE, IGCSE, Cambridge or Singapore MOE).

Live, interactive 1:1 or small-group classes - the tutor sees your child's work in real time.

Customised practice worksheets - graded, reviewed and explained class by class.

Weekly homework support - assignments and concept revision before the next class.

Periodic class tests aligned to the board's exam pattern.

Detailed progress reports for parents every month.

Flexible scheduling - pick time slots that fit school and after-school activities.

Free demo class so you can meet the tutor before you commit.

Globally available - USA, UK, Canada, Australia, Singapore, UAE, GCC and India.

Recorded sessions provided for missed classes (group format) - no concept is left behind.

Overview

Chemistry Grade 11-12 is senior-secondary Chemistry for the PCB / PCM / JEE / NEET / AP / IB / A-level stream. WinQuest delivers it 1:1 or in small groups aligned to your board - CBSE Class 11/12, ICSE ISC, Cambridge AS/A-level (9701), AP Chemistry, Australian v9.0 Senior Chemistry, or Singapore H2 Chemistry.

What You'll Learn

Live interactive sessions
1st one-on-one session
Comprehensive curriculum
No long-term commitment
Personalized learning plan

Grade 11

Age 16+ 90 hrs

Atomic Structure & Periodic Properties

Quantum mechanical model of the atom - orbitals (s, p, d, f); quantum numbers (n, l, ml, ms); electron configuration.
Periodic trends - atomic radius (decreases across period, increases down group), ionisation energy, electronegativity (Pauling scale).
Photoelectron spectroscopy (PES) - measures binding energies of electrons; reveals shell structure and orbital energies.

Bonding & Molecular Structure

Ionic (metal + non-metal, electron transfer), covalent (electron sharing), and metallic bonding (sea of delocalised electrons).
Lewis structures (electron dots), VSEPR (predict geometry: tetrahedral, trigonal, linear), hybridisation (sp, sp2, sp3).
Intermolecular forces - London dispersion (weakest), dipole-dipole, hydrogen bonding (strongest non-bonded); affect MP, BP, solubility.

Stoichiometry & Reactions

Mole concept (1 mole = 6.022 x 10^23 particles; molar mass), empirical formula (simplest whole-number ratio) and molecular formula.
Limiting reagents (reactant that runs out first; determines product amount) and percent yield (actual / theoretical x 100).
Aqueous solutions (solute + solvent; molarity M = mol / L) and net ionic equations (showing only ions actually reacting).

Thermodynamics & Kinetics

Enthalpy (H, heat content), entropy (S, disorder), Gibbs free energy (G = H - TS; spontaneous if dG < 0).
Reaction rate laws (rate = k[A]^m[B]^n; order; rate constant k) and mechanisms (elementary steps; rate-determining step).
Activation energy (Ea; energy barrier) and catalysts (lower Ea by alternative pathway; not consumed).

Matter, Chemical Trends & Bonding

Atomic theory (Dalton, Thomson, Rutherford, Bohr, Schrödinger) and the periodic table (groups + periods; modern arrangement by atomic number).
Periodic trends - atomic radius (decreases across period, increases down group), ionisation energy, electronegativity, electron affinity.
Ionic bonding (metal + non-metal, complete electron transfer; ions, lattice) and covalent bonding (non-metals share electrons; sigma + pi bonds).

Chemical Reactions

Types of reactions - synthesis (A + B -> AB), decomposition (AB -> A + B), single displacement, double displacement, combustion, redox.
Balancing equations (atoms conserved) and stoichiometry (mole ratios; mass-mass, mass-volume problems).
Acids (donate H+; HCl, H2SO4), bases (accept H+ or release OH-; NaOH), and pH (-log[H+]; 0-14 scale; neutralisation).

Quantities in Chemical Reactions

Mole concept (1 mole = 6.022 x 10^23 particles; n = m/M) and calculations (mass-mole, mole-mole, mass-mass).
Limiting reagents (which runs out first; calculated via mole ratios) and percent yield (actual / theoretical x 100).
Solution chemistry - molarity (M = mol / L), dilution (M1V1 = M2V2), parts per million (ppm).

Solutions & Solubility

Concentrations (molarity, molality, mass %, mole fraction) and solubility (factors: temperature, pressure, polar / non-polar).
Acid-base equilibria (Ka, Kb; weak acid / base dissociation; conjugate pairs); pH (-log[H+]) and pOH (-log[OH-]); pH + pOH = 14 at 25C.
Titration calculations - moles acid = moles base at equivalence point; using known concentration to find unknown.

Properties & Structure of Matter

Atomic structure (nucleus with protons + neutrons; electrons in shells / orbitals) and the periodic table (groups, periods, blocks).
Ions (positive: cations; negative: anions), ionic bonding (electron transfer; lattice), ionic compounds (NaCl, MgO).
Covalent bonding (electron sharing between non-metals) and molecular shapes (VSEPR theory: linear, bent, trigonal, tetrahedral).

Reactions & Stoichiometry

Mole concept (1 mole = Avogadro number 6.022 x 10^23 particles) and chemical equations (balanced; conservation of mass).
Stoichiometric calculations - mass-mole, mole-mass, mass-mass; mole ratios from balanced equations.
Limiting reagents (reactant that runs out first; determines product amount) and yield (theoretical, actual, percent).

Acidic & Basic Solutions

Acids (sour, donate H+; HCl, citric), bases (bitter, accept H+; NaOH), and the pH scale (0-14; -log[H+]).
Acid-base reactions (neutralisation: acid + base -> salt + water) and titration (find unknown concentration using known).
Brønsted-Lowry theory - acids = proton (H+) donors; bases = proton acceptors; conjugate acid-base pairs.

Energy Transformations

Enthalpy (H, heat at constant pressure) and energy diagrams (reactants -> activated complex -> products; exo vs endo).
Bond enthalpies (energy to break a bond; average values) and Hess's law (enthalpy change is path-independent; sum of steps).
Calorimetry (measuring heat: q = mcdeltaT) using a calorimeter; specific heat capacity (J / g / C).

Some Basic Concepts & Atomic Structure

Mole concept (1 mole = 6.022 x 10^23 particles), molar mass (g/mol), atomic and molecular masses (in amu).
Atomic models - Bohr (electrons in fixed orbits), Schrödinger (quantum mechanical; orbitals; probability clouds).
Periodic table (18 groups, 7 periods, s/p/d/f blocks) and trends (atomic radius, ionisation energy, electronegativity).

Chemical Bonding & States of Matter

Ionic bonds (metal + non-metal), covalent bonds (electron sharing), coordinate bonds (both electrons from one atom).
VSEPR (electron pair repulsion predicts shape), hybridisation (sp, sp2, sp3; mixing orbitals), molecular orbital theory (bonding, antibonding).
Gas laws - Boyle's (PV = const), Charles's (V/T = const), Avogadro's (V/n = const); kinetic molecular theory.

Thermodynamics & Equilibrium

First law of thermodynamics (dU = q + w; energy conserved); enthalpy (H; dH = q at constant P).
Chemical equilibrium - Kc (concentrations), Kp (partial pressures), Le Chatelier's principle (system opposes change).
Ionic equilibrium - acids (Ka), bases (Kb), pH (-log[H+]); common ion effect; buffer solutions.

Organic Chemistry & Hydrocarbons

General principles (purification, qualitative + quantitative analysis) and techniques (distillation, recrystallisation, chromatography).
Hydrocarbons - alkanes (CnH2n+2; saturated), alkenes (CnH2n; double bond), alkynes (CnH2n-2; triple bond), aromatics (benzene).
Environmental chemistry (air, water, soil pollution; greenhouse effect; ozone depletion); redox reactions (oxidation: lose e-, reduction: gain e-).

Atomic Structure & Periodic Table

Atomic models - Dalton, Thomson, Rutherford, Bohr, Schrödinger (quantum mechanical with orbitals); quantum numbers.
Electronic configuration - filling of orbitals (Aufbau principle, Pauli exclusion, Hund's rule); e.g., Na: 1s^2 2s^2 2p^6 3s^1.
Periodic properties - atomic / ionic radius, ionisation energy, electron affinity, electronegativity; trends across period and group.

Bonding & States of Matter

Chemical bonding - ionic (electron transfer), covalent (sharing; sigma + pi), metallic (delocalised electron sea).
Gas laws (Boyle's, Charles's, Avogadro's) and ideal gas equation (PV = nRT; R = 8.314 J / mol / K).
Liquids (viscosity, surface tension, vapour pressure) and solids (crystalline vs amorphous; types of crystals).

Thermodynamics & Equilibrium

Thermochemistry - enthalpy (H), entropy (S, disorder), Gibbs free energy (G = H - TS; predicts spontaneity).
Chemical equilibrium - dynamic state; Kc, Kp expressions; Le Chatelier's principle (system opposes change).
Acid-base equilibria (Ka, Kb, pH, pOH; buffer solutions) and ionic equilibria (common ion effect, solubility product Ksp).

Organic & Environmental Chemistry

Organic chemistry - basics (carbon's tetravalency, catenation) and IUPAC nomenclature (root + suffix + prefix).
Hydrocarbons - alkanes (CnH2n+2), alkenes (CnH2n with C=C), alkynes (CnH2n-2 with triple bond); reactions and uses.
Environmental chemistry (atmospheric, water, soil pollution; greenhouse gases); redox (oxidation: lose e-, reduction: gain e-).

Atomic Structure & Bonding

Atomic structure (protons, neutrons, electrons; isotopes; mass spectrometry) and electron configuration (s, p, d, f orbitals).
Periodic patterns and trends - atomic radius (decreases across period; increases down group), ionisation energy, electronegativity.
Chemical bonding - covalent (electron sharing), ionic (transfer), metallic (sea); intermolecular forces (London, dipole, H-bond).

Stoichiometry & Energetics

Mole concept (1 mole = 6.022 x 10^23 particles) and chemical calculations (mass-mole, percent yield, limiting reagent).
Energetics - enthalpy (dH for reactions), Hess's law (path-independent; calculate dH via known steps).
Equilibria - Kc (concentrations) and Kp (partial pressures); position depends on conditions (Le Chatelier).

Organic Chemistry

Functional groups (-OH, -COOH, -CHO, -NH2, -X) and isomerism (structural: chain, position, functional; stereoisomerism).
Hydrocarbons - alkanes (saturated; combustion, substitution) and alkenes (double bond; addition reactions).
Halogenoalkanes (R-X; nucleophilic substitution: SN1, SN2; elimination), alcohols (-OH), and carbonyl compounds (-C=O).

Practical Skills

Quantitative experiments (precise measurements; significant figures; error analysis) and titration (acid-base; redox; complexometric).
Qualitative analysis - tests for cations (flame tests, precipitation) and anions (chloride: AgNO3; sulphate: BaCl2; carbonate: HCl).
AS Paper 3 practical exam practice - 2 hours; quantitative + qualitative tasks; lab safety; observations and conclusions.

Note

IGCSE 0620 Chemistry is sat at the end of Grade 10 / Year 11 in Cambridge schools.
Cambridge AS-level (9701) Chemistry is taken in Grade 11 / Year 12 - half of full A-level qualification.
See the Cambridge AS-level column above for the Grade 11 syllabus and exam structure.

Physical Chemistry I

Atomic structure (subatomic particles, isotopes, electronic configuration) and periodic table (s/p/d/f blocks, trends).
Bonding (covalent, ionic, metallic) and intermolecular forces (van der Waals, hydrogen bonding; affect MP, BP, solubility).
States of matter (solid, liquid, gas; phase diagrams); ideal gas equation (PV = nRT) and real gas deviations.

Inorganic Chemistry I

Periodicity - period 3 elements (Na to Ar); trends in properties (atomic radius, MP, BP, reactivity).
Group 2 elements (Be, Mg, Ca, Sr, Ba; alkaline earth metals) and their compounds (oxides, hydroxides, carbonates).
Group 17 halogens (F, Cl, Br, I; reactivity decreases down group; oxidising power; displacement reactions).

Organic Chemistry I

Isomerism (structural: chain, position, functional; stereoisomerism: cis/trans, optical) and reaction mechanisms (SN1, SN2, E1, E2).
Hydrocarbons - alkanes (saturated; CnH2n+2), alkenes (C=C; CnH2n), arenes (benzene; delocalised pi electrons).
Halogen derivatives (R-X) and alcohols (R-OH; primary, secondary, tertiary; oxidation reactions).

Practical Skills

Quantitative analysis - titration techniques (acid-base, redox, complexometric; using burette, pipette, conical flask).
Qualitative analysis - cation tests (flame tests, NaOH, NH3) and anion tests (chloride, sulphate, carbonate).
H2 Paper 4 practical exam practice - 2h30m; planning, analysis, evaluation; full lab skills assessment.

Grade 12

Age 17+ 90 hrs

Equilibrium & Acid-Base

Acid-base equilibria - Ka (acid dissociation), Kb (base dissociation), Kw (water = 10^-14 at 25C; Ka x Kb = Kw).
Buffer solutions (weak acid + conjugate base; resist pH change; Henderson-Hasselbalch: pH = pKa + log[A-]/[HA]) and titration curves (S-shape, equivalence point).
Solubility product Ksp - equilibrium constant for sparingly soluble salts (AgCl, BaSO4); predicting precipitation.

Thermodynamics & Electrochem

Spontaneity (dG < 0; dG = dH - TdS); Gibbs free energy and its sign determines reaction direction.
Electrochemical cells - voltaic (galvanic; spontaneous; chemical -> electrical; batteries) and electrolytic (non-spontaneous; electrical -> chemical).
Nernst equation (E = E0 - (RT/nF) ln Q; cell potential at non-standard conditions) and electrolysis (Faraday's laws; calculating mass deposited).

Kinetics in Depth

Rate laws - differential (rate = k[A]^m[B]^n) and integrated forms (zero, first, second order; half-life t1/2).
Reaction mechanisms (sequence of elementary steps) and intermediates (formed and consumed; not in overall equation); rate-determining step.
Catalysis - homogeneous (same phase as reactants; H+ for ester hydrolysis) and heterogeneous (different phase; Pt for H2 / O2).

Applications - Organic

Organic functional groups (-OH, -COOH, -CHO, -CO-, -NH2, esters, amides) and their characteristic reactions.
Polymerisation - addition (free radical; monomers add without loss; polyethene, PVC) and condensation (loss of small molecule; nylon, polyester).
Biochemistry - amino acids (20 in proteins; zwitterions), proteins (peptide bonds; 4 levels of structure), carbohydrates (glucose, sucrose, starch).

Organic Chemistry

Hydrocarbons (alkanes, alkenes, alkynes, aromatics), alcohols (-OH), aldehydes (-CHO), ketones (R-CO-R'), carboxylic acids (-COOH).
Esters (R-COO-R'; fragrances, fats), amines (R-NH2; basic), amides (R-CO-NH-R'; proteins), polymers (addition + condensation).
Organic mechanisms - substitution (SN1, SN2), elimination (E1, E2), addition (electrophilic, nucleophilic); synthesis (multi-step routes).

Structure & Properties of Matter

Atomic orbitals (s, p, d, f shapes) and molecular orbital theory (bonding, antibonding; sigma, pi MOs; bond order).
Intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding) and properties (MP, BP, viscosity, surface tension).
VSEPR (predicts geometry from electron pairs) and hybridisation in depth (sp, sp2, sp3, sp3d, sp3d2).

Energy Changes & Rates of Reaction

Thermochemistry (dH for reactions; standard enthalpy of formation, combustion, neutralisation) and Hess's law (path-independent).
Reaction kinetics - rate equations (zero, first, second order); rate constant k; Arrhenius equation (k = Ae^(-Ea/RT)).
Catalysis (lowers Ea via alternative pathway; not consumed; specific) and activation energy (Ea; minimum energy for reaction).

Equilibrium & Electrochemistry

Le Chatelier's principle (equilibrium shifts to oppose change) and Kc (equilibrium constant in concentrations); reaction quotient Q.
Acid-base equilibria (Ka, Kb, Kw); pH calculations (strong acid / base; weak acid: pH = 1/2(pKa - log C)); buffer pH.
Electrochemistry - voltaic cells (galvanic; chemical -> electrical; salt bridge; batteries) and electrolytic cells (electrical -> chemical; electroplating).

Equilibrium, Acids & Redox

Equilibrium - Le Chatelier (system opposes change) and Kc / Kp (constants for concentrations / partial pressures).
Acid-base equilibrium (Ka for weak acids; Kb for weak bases) and pH (-log[H+]; buffer pH via Henderson-Hasselbalch).
Redox reactions (oxidation: lose e-; reduction: gain) and electrochemistry (galvanic and electrolytic cells; Nernst equation).

Organic Chemistry & Polymers

Functional groups (-OH, -COOH, -NH2, -CHO, esters, amides) and their characteristic reactions (substitution, addition, oxidation).
Polymerisation - addition (radical; polyethene, polystyrene) and condensation (loss of H2O; nylon, polyester, proteins).
Biochemistry - proteins (peptide bonds; enzymes), carbohydrates (mono / di / polysaccharides), lipids (triglycerides, phospholipids).

Energy Storage & Conversion

Galvanic cells (spontaneous; chemical -> electrical) and electrolytic cells (non-spontaneous; electrical -> chemical; electroplating, refining).
Fuel cells (continuous reactants; e.g., H2 + O2 -> H2O + electricity) and batteries (primary: alkaline; secondary: Li-ion).
Reaction enthalpies - exothermic (dH < 0), endothermic (dH > 0); enthalpy of formation, combustion, neutralisation.

Analytical Methods

Spectroscopic methods - IR (functional group identification), NMR (1H, 13C: structure elucidation), MS (mass / charge ratio; molecular formula).
Chromatographic methods - GC (gas-liquid; volatile compounds), HPLC (high-performance liquid; non-volatile, sensitive).
Quantitative analysis (titration, gravimetric, instrumental) and qualitative analysis (tests for cations, anions, functional groups).

Solid State & Solutions

Solid state - types of crystals (ionic, covalent network, molecular, metallic), defects (Frenkel, Schottky), unit cells.
Solutions - concentrations (M, m, x), colligative properties (vapour pressure, BP elevation, FP depression, osmotic pressure).
Electrochemistry - cells (galvanic, electrolytic; EMF), Nernst equation (E = E0 - (RT/nF) ln Q), Kohlrausch (molar conductivity).

Chemical Kinetics & Surface Chem

Chemical kinetics - rate laws (rate = k[A]^m[B]^n), order of reaction (sum of exponents), half-life (t1/2; depends on order).
Surface chemistry - adsorption (physisorption, chemisorption), catalysis (heterogeneous, homogeneous, enzymes), colloids (Tyndall effect).
General principles of metallurgy - extraction (concentration, reduction, refining); thermodynamic + electrochemical principles.

p, d, f-block & Coord. Compounds

p-block elements - Group 13 (B, Al), Group 14 (C, Si), Group 15 (N, P), Group 16 (O, S), Group 17 (halogens), Group 18 (noble gases).
d-block elements (transition metals; variable oxidation states; coloured ions; catalytic activity) and f-block (lanthanides, actinides).
Coordination compounds - Werner's theory (primary + secondary valence; central metal + ligands), isomerism (geometric, optical).

Organic Chemistry - All

Haloalkanes (R-X; SN1, SN2 mechanisms) and haloarenes (Ar-X; resonance stabilised; less reactive than haloalkanes).
Alcohols (R-OH; primary, secondary, tertiary), phenols (Ar-OH; acidic), ethers (R-O-R'); aldehydes (-CHO), ketones (R-CO-R'), carboxylic acids (-COOH).
Amines (R-NH2; primary, secondary, tertiary; basic); biomolecules - carbohydrates (glucose, sucrose), proteins (peptide bonds), nucleic acids (DNA, RNA).

Physical Chemistry

Solid state (types of crystals, defects, unit cells), solutions (colligative properties), electrochemistry (Nernst, electrolysis).
Chemical kinetics (rate laws, order, Arrhenius) and surface chemistry (adsorption, catalysis, colloids).
General principles of metallurgy - extraction (concentration, reduction, refining); thermodynamics of extraction.

Inorganic Chemistry

p-block elements (Groups 13-18; properties, compounds, uses); d-block (transition metals) and f-block (lanthanides, actinides).
Coordination compounds - central metal + ligands; nomenclature, isomerism, bonding (VBT, CFT, MOT).
Qualitative analysis of inorganic salts - identifying cations (Pb2+, Cu2+, Fe3+ etc.) and anions (Cl-, SO4^2-, NO3-).

Organic Chemistry

Haloalkanes (R-X; nucleophilic substitution SN1, SN2; elimination) and haloarenes (Ar-X; less reactive due to resonance).
Alcohols (R-OH), phenols (Ar-OH; acidic), ethers (R-O-R'); aldehydes (-CHO), ketones (R-CO-R'), carboxylic acids (-COOH).
Amines (R-NH2; basicity) and biomolecules (carbohydrates: mono/di/poly; proteins: peptide bonds; nucleic acids: DNA/RNA).

Practical

Volumetric analysis (using burette, pipette, conical flask) and titrations (acid-base, redox, complexometric).
Qualitative analysis of inorganic salts - cation tests (flame, NaOH, NH3) and anion tests (Cl-, SO4^2-, CO3^2-).
ISC practical exam preparation - 3 hours; volumetric + qualitative analysis; lab safety; observations and conclusions.

Physical Chemistry

Chemical energetics - lattice enthalpy (energy to break ionic lattice into gas-phase ions), Born-Haber cycle (calculate lattice enthalpy).
Equilibria - acids (Ka), bases (Kb), buffers (Henderson-Hasselbalch; pH = pKa + log[A-]/[HA]), Ksp (solubility product).
Reaction kinetics - mechanisms (sequence of elementary steps) and orders (zero, first, second; rate equations).

Inorganic Chemistry

Periodicity - period 3 elements (Na to Ar); oxides (basic vs acidic; trend down the period).
Group 2 elements (Be, Mg, Ca, Sr, Ba; reactivity increases down group) and Group 17 (halogens; reactivity decreases down group).
Transition elements - chemistry of complexes (d-block; variable oxidation states; ligands; coloured ions; catalysts).

Organic Chemistry

Hydrocarbons (alkanes, alkenes, arenes; benzene resonance) and halogen derivatives (R-X; SN1, SN2, E1, E2 mechanisms).
Hydroxy compounds (alcohols R-OH, phenols Ar-OH), carbonyl compounds (aldehydes RCHO, ketones R-CO-R'), carboxylic acids (R-COOH).
Nitrogen compounds (amines, amides, nitriles), polymers (addition, condensation), spectroscopy (IR, NMR, MS for structure elucidation).

Past Paper Practice

4 Paper 4 (theory; 2 hours; 100 marks) and Paper 5 (planning + analysis + evaluation; 1h15m; 30 marks) mocks.
A* targeting (>= 90%); time management (90 min / paper); precise answers with units, sig figs, balanced equations.
May / October session preparation - past papers from 5+ years; examiner reports; common mistakes.

Note

IGCSE 0620 Chemistry is sat at the end of Grade 10 / Year 11 in Cambridge schools.
Cambridge A-level (9701) Chemistry is taken in Grade 12 / Year 13 - full A-level qualification (AS + A2 papers).
See the Cambridge A-level column above for the Grade 12 syllabus and exam structure.

Physical Chemistry II

Chemical energetics II - lattice energy, Born-Haber
Reaction kinetics - mechanisms and rate orders
Equilibria - ionic equilibria, buffers, Ksp

Inorganic Chemistry II

Periodicity - chemistry of period 3
Transition elements and complexes
Group 2 and Group 17 chemistry

Organic Chemistry II

Carbonyl compounds, carboxylic acids and derivatives
Nitrogen-containing compounds
Polymerisation and biochemistry

Exam Preparation

TYS past papers
Paper 1 (MCQ), Paper 2 (structured), Paper 3 (essay), Paper 4 (practical)
A-grade target writing

Requirements

A laptop or desktop with stable internet
Scientific calculator
Notebook for equations, mechanisms, lab reports
School Chemistry textbook + past papers

Reviews

4.84 / 5 ★ · 300+ students enrolled

Parents consistently rate our mentors for personalised attention, clear concepts and steady progress. Book a free demo to experience a class first-hand.

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Tutors give written feedback on every homework assignment, run a short formative quiz every 4-6 classes, and a longer chapter test at the end of each topic. Parents receive a monthly progress report covering concept mastery, homework completion and test scores.

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