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NERDC · 15 topics

Chemistry

G3N tutors you through the full NERDC Chemistry syllabus offline — from Theme 1: Introduction and Basic Concepts, Theme 2: Atomic Structure, Theme 3: Periodic Table and Elements and more — with adaptive lessons, instant quizzes, flashcards and exam-ready summaries.

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Syllabus

What you’ll cover in Chemistry.

The complete topic outline G3N teaches, mapped to the NERDC curriculum.

SSS 1

5 topics
Theme 1: Introduction and Basic Concepts
  • Fundamentals of Chemistry
    • Define chemistry as the science of matter, its properties, structure, and reactions with energy
    • Identify major branches: inorganic (non-carbon), organic (carbon), physical (energy and structure), analytical (composition)
    • Identify common laboratory apparatus: beaker, flask, burette, pipette, test tube, condenser, thermometer
    • Understand function of equipment: proper use ensures safe and accurate experiments
    • Apply safety rules: protective equipment (goggles, gloves, coat), proper ventilation, chemical storage
    • Understand hazard symbols: flammable, toxic, corrosive, oxidizing; indicates danger and handling precautions
    • Recognize matter: anything with mass and volume; exists in states based on particle arrangement
    • Distinguish properties of matter: intensive (independent of amount: density, boiling point) vs. extensive (depend on amount: mass, volume)
  • Structure of Matter
    • Define elements: pure substances of one type of atom; cannot be broken down by chemical means
    • Define compounds: pure substances of two or more elements in fixed ratio; can be broken down
    • Define mixtures: combinations of substances (elements or compounds) in any ratio; can be separated by physical means
    • Classify mixtures: homogeneous (uniform composition), heterogeneous (visibly different parts)
    • Understand filtration: separates solid from liquid using filter paper; residue remains, filtrate passes through
    • Understand evaporation: heating liquid to gas causes solvent to evaporate; solid solute remains
    • Understand distillation: evaporation + condensation; separates components by boiling points
    • Understand chromatography: separates components based on different rates of travel through medium
Theme 2: Atomic Structure
  • Atomic Theory
    • State Dalton's atomic theory: all matter is atoms; atoms of element are identical; compounds are atoms in fixed ratio
    • Identify subatomic particles: protons (positive charge, nucleus), neutrons (no charge, nucleus), electrons (negative charge, orbitals)
    • Understand relative mass: proton mass ≈ neutron mass ≈ 1840 × electron mass
    • Define atomic number (Z): number of protons; identifies element; determines electron count in neutral atom
    • Define mass number (A): total protons + neutrons; determines isotope
    • Understand nucleus: dense central region; contains protons and neutrons
    • Understand electron orbitals: regions where electrons likely found; described by quantum numbers
    • Recognize that electrons arranged in shells: K shell (n=1, max 2e⁻), L shell (n=2, max 8e⁻), M shell (n=3, max 18e⁻)
Theme 3: Periodic Table and Elements
  • Classification of Elements
    • Understand periodic table organization: elements arranged by atomic number in rows (periods) and columns (groups)
    • Identify periods: rows 1-7 represent electron shells filled; determine size and reactivity
    • Identify groups/families: columns represent valence electrons; determine chemical properties
    • Recognize Group 1 (alkali metals): very reactive, soft, low density, form +1 ions
    • Recognize Group 17 (halogens): very reactive nonmetals, form -1 ions, diatomic
    • Recognize Group 18 (noble gases): inert, full electron shells, rarely react
    • Define metallic character: metals (left), nonmetals (right), metalloids (staircase boundary); trends left→right
    • Understand atomic radius trend: increases down group (more shells), decreases left→right (more protons pulling electrons)
Theme 4: Chemical Bonding
  • Types of Bonding
    • Understand ionic bonding: transfer of electrons between metal (cation) and nonmetal (anion); electrostatic attraction
    • Identify ionic compound characteristics: high melting/boiling points, conduct when molten/dissolved, brittle, many soluble in water
    • Recognize common cations: H⁺, Li⁺, Na⁺, K⁺, Ca²⁺, Mg²⁺, Al³⁺, NH₄⁺
    • Recognize common anions: F⁻, Cl⁻, Br⁻, I⁻, O²⁻, S²⁻, OH⁻, NO₃⁻, SO₄²⁻, CO₃²⁻
    • Understand covalent bonding: sharing of electrons between nonmetals; creates strong directional bonds
    • Distinguish polar covalent (unequal sharing) from nonpolar (equal sharing) based on electronegativity difference
    • Identify covalent compound characteristics: low melting/boiling points, don't conduct electricity, volatile many
    • Understand metallic bonding: 'sea' of delocalized electrons around metal cations; explains properties
Theme 5: Chemical Reactions
  • Reaction Types and Equations
    • Write chemical equations: reactants → products; use formulas, coefficients to balance
    • Balance equations: ensure equal atoms on both sides; preserves conservation of mass
    • Classify combustion reactions: substance reacts with O₂; C,H compounds produce CO₂ + H₂O
    • Balance combustion equations: adjust O₂ last; common pattern (CₓHᵧ + (x+y/4)O₂ → xCO₂ + (y/2)H₂O)
    • Understand oxidation-reduction (redox): transfer of electrons; oxidation state changes
    • Define oxidation: loss of electrons or increase in oxidation state
    • Define reduction: gain of electrons or decrease in oxidation state
    • Apply oxidation state rules: elements = 0, compounds H = +1 (usually), O = -2 (usually), ionic charge

SSS 2

5 topics
Theme 1: Stoichiometry
  • Quantitative Chemistry
    • Define mole: amount of substance (Avogadro's number = 6.02 × 10²³ particles)
    • Calculate molar mass: sum of atomic masses (g/mol); numerically equal to relative formula mass
    • Convert between moles and grams: n = m/M where n is moles, m is mass, M is molar mass
    • Convert between moles and particles: n = N/Nₐ where N is number of particles
    • Apply molar ratios from equations: stoichiometric coefficients give mole ratios
    • Solve stoichiometric calculations: given mass of reactant, find mass of product using molar masses and coefficients
    • Identify limiting reactant: reactant that runs out first; determines maximum product
    • Calculate theoretical yield: maximum product possible if reaction goes to completion
Theme 2: Solutions and Concentration
  • Solutions
    • Define solubility: mass of solute dissolving in 100g solvent at given temperature
    • Distinguish saturated (maximum solute dissolved), unsaturated (could dissolve more), supersaturated (more than maximum)
    • Understand concentration as molarity: M = n/V = moles solute / liters solution
    • Calculate molarity: prepare solutions, dilute solutions (M₁V₁ = M₂V₂)
    • Understand other concentration units: molality (mol/kg solvent), percentage (mass or volume)
    • Understand dilution: adding solvent increases volume, decreases concentration; moles solute unchanged
    • Apply dilution equation: M₁V₁ = M₂V₂ to calculate new concentration or volume
    • Understand titration: adding standard solution until reaction complete; calculates concentration
Theme 3: Thermochemistry
  • Energy and Reactions
    • Distinguish endothermic (absorbs energy, ΔH > 0) from exothermic (releases energy, ΔH < 0) reactions
    • Define enthalpy (H): total heat content; ΔH = H_final - H_initial
    • Define heat of reaction: enthalpy change during reaction; measured in kJ/mol
    • Understand exothermic benefits: releases useful heat; spontaneous if ΔH negative and ΔS positive
    • Understand endothermic requirements: needs continuous energy input; requires very negative ΔS for spontaneity
    • Apply Hess's law: if reactions added to get target reaction, ΔH values add; independent of path
    • Calculate using Hess's law: manipulate equations (reverse = negate ΔH, multiply = multiply ΔH) to find target ΔH
    • Understand bond energy: energy to break bonds (endothermic), energy released forming bonds (exothermic)
Theme 4: Rates of Reaction and Equilibrium
  • Kinetics and Equilibrium
    • Understand factors affecting rate: temperature (higher = faster), concentration (higher = faster), surface area (greater = faster)
    • Define collision theory: reactions require particles collide with correct orientation and sufficient energy
    • Define activation energy (Eₐ): minimum energy for successful collision; lower Eₐ = faster reaction
    • Understand reaction rate: measure of change per unit time; depends on activation energy
    • Define catalyst: substance that lowers Eₐ without being consumed; speeds up reaction
    • Understand equilibrium: forward and reverse reactions occur at same rate; concentrations constant
    • Write equilibrium expressions: K = [products]/[reactants] with concentrations raised to stoichiometric coefficients
    • Interpret equilibrium constant: K >> 1 (products favored), K << 1 (reactants favored), K ≈ 1 (similar amounts)
Theme 5: Acids, Bases, and Salts
  • Acid-Base Chemistry
    • Define acids (Brønsted): H⁺ donors; common: HCl, H₂SO₄, HNO₃, CH₃COOH
    • Define bases (Brønsted): OH⁻ or H⁺ acceptors; common: NaOH, NH₃, Ca(OH)₂
    • Understand strong acids: completely dissociate (HCl, H₂SO₄, HNO₃); weak acids partially dissociate (CH₃COOH, HF)
    • Understand strong bases: completely dissociate (NaOH, KOH, Ca(OH)₂); weak bases partially dissociate (NH₃)
    • Define pH scale: pH = -log[H⁺]; neutral pH = 7, acidic < 7, basic > 7
    • Calculate pH: from [H⁺] concentration; use pH + pOH = 14
    • Understand neutralization: acid + base → salt + water; H⁺ + OH⁻ → H₂O
    • Apply neutralization equation: calculate concentrations after reaction

SSS 3

5 topics
Theme 1: Electrochemistry
  • Electrical and Chemical Processes
    • Assign oxidation states: number of electrons lost/gained; use rules to assign to each atom
    • Identify oxidizing agents (reduced, gains electrons) and reducing agents (oxidized, loses electrons)
    • Balance redox equations: balance atoms, balance charges using electron method
    • Understand electrochemical cells: spontaneous reactions produce electricity (galvanic) or electricity drives reactions (electrolytic)
    • Define electrode types: anode (oxidation), cathode (reduction); direction reverses in galvanic vs. electrolytic
    • Calculate electrode potentials: use standard potentials (E°); predict spontaneity (E°_cell > 0 = spontaneous)
    • Apply Nernst equation: E = E° - (0.0592/n)·log(Q) at 25°C; relates potential to concentrations
    • Understand Faraday's laws: moles produced ∝ charge transferred; Q = n·F where F = 96,485 C/mol
Theme 2: Organic Chemistry
  • Carbon Compounds
    • Understand alkanes (CₙH₂ₙ₊₂): single C-C bonds; saturated; nonpolar; inert; nomenclature -ane
    • Understand alkenes (CₙH₂ₙ): double C=C bonds; unsaturated; reactive; nomenclature -ene
    • Understand alkynes (CₙH₂ₙ₋₂): triple C≡C bonds; unsaturated; very reactive; nomenclature -yne
    • Recognize functional groups: determine reactivity and properties of organic molecules
    • Understand alcohols (-OH): hydroxyl group; polar; water soluble; oxidizable to aldehydes/ketones
    • Understand aldehydes (C=O at end): easily oxidized; give silver mirror test
    • Understand ketones (C=O in middle): less easily oxidized than aldehydes
    • Understand carboxylic acids (-COOH): acidic, form esters with alcohols
Theme 3: Nuclear Chemistry
  • Nuclear Processes
    • Understand radioactivity: unstable nuclei spontaneously decay; emit particles or radiation
    • Identify alpha decay: ⁴₂He emitted; A decreases by 4, Z decreases by 2
    • Identify beta decay: electron emitted; A unchanged, Z increases by 1
    • Identify gamma decay: high-energy photon; A and Z unchanged; just energy release
    • Balance nuclear equations: mass number and atomic number conserved
    • Define half-life: time for half of nuclei to decay; N(t) = N₀(1/2)^(t/t₁/₂)
    • Calculate remaining nuclei: use half-life formula for multiple half-lives
    • Apply radiocarbon dating: ¹⁴C half-life = 5,730 years; dates organic materials
Theme 4: Chemistry of Selected Elements
  • Group Chemistry
    • Understand halogens (Group 17): very reactive; forms -1 ions; F > Cl > Br > I in reactivity
    • Understand halogen reactions: displace less reactive halogens; Cl₂ + 2KBr → 2KCl + Br₂
    • Understand alkali metals (Group 1): very reactive; form +1 ions; reactivity increases down group
    • Understand alkaline earth metals (Group 2): reactive; form +2 ions; less reactive than alkali metals
    • Understand transition metals: variable oxidation states; colored ions; catalytic properties
    • Understand metal extraction: reduction processes (roasting, smelting, electrolysis) produce pure metals
    • Classify extraction methods: carbon reduction for less reactive, electrolysis for more reactive
    • Understand environmental chemistry: pollution, greenhouse effect, ozone depletion
Theme 5: Analytical Chemistry
  • Analysis and Testing
    • Identify qualitative analysis: determines what's present, not amounts
    • Test cations: use precipitating agents or flame tests to identify metal ions
    • Test anions: use specific tests (Cl⁻ → AgNO₃ → white ppt; SO₄²⁻ → BaCl₂ → white ppt)
    • Understand quantitative analysis: determines amount of substance present
    • Apply gravimetry: precipitate analyte, measure mass to find concentration
    • Apply titration: add standard solution to analyte until endpoint; calculate concentration
    • Understand spectroscopy: measures light absorption/emission at specific wavelengths
    • Apply UV-Vis spectroscopy: measures absorption in visible/UV range; relates to color and concentration
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