GENERAL CHEMISTRY · FREE STUDY HUB

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Study the official General Chemistry scope through unit-safe worked examples, focused lessons, randomized practice, and free supporting references.

Build a 30-question form →Study Laboratory ↗Build a Laboratory mix ↗Map Laboratory ↗Read scientific visuals ↗
30official questions
13official domains
66leaf-level topics
0invented domain weights

SHARED SCIENTIFIC VISUALS

Read every model in one language.

Structured inputs, text or data equivalents, no color-only meaning, and a visible evidence boundary now govern five reusable scientific visual systems.

  1. 01

    Notation

    Magnitude, exponent, unit, formula grammar, and significant figures remain distinct.

  2. 02

    Equations

    Coefficients, species, states, conditions, and reaction relationships stay attached.

  3. 03

    Molecules

    Named atoms, explicit bonds, charges, hydrogens, and stereochemical marks define connectivity.

  4. 04

    Graphs

    Axes, units, ranges, markers, line patterns, and complete source-value tables travel together.

  5. 05

    Mechanisms

    Electron sources and destinations are explicit; the drawing never outruns its evidence.

Open the scientific visual-language guide →

GASES

Match each law to its conditions.

15 study objectives across five official topics, with 5 guided lessons and 20 original questions. Fixed variables, kelvin and absolute-pressure requirements, mixture logic, and ideal-model limits stay explicit.

A

Kinetic molecular theory of gases

  1. 01Ideal-gas particle model and pressure
  2. 02Temperature, kinetic energy, and molecular speed
  3. 03Ideal behavior and model limits
B

Dalton’s gas law

  1. 01Total and partial pressure
  2. 02Mole fraction and partial pressure
  3. 03Gas collected over water
C

Boyle’s gas law

  1. 01Boyle conditions and inverse change
  2. 02Two-state Boyle calculations
  3. 03Boyle graphs and experimental evidence
D

Charles’s gas law

  1. 01Charles conditions and direct change
  2. 02Two-state Charles calculations
  3. 03Charles graphs and absolute zero
E

Ideal gas law

  1. 01Unit-safe ideal gas law
  2. 02Gas amount, molar mass, and density
  3. 03Model selection and reasonableness
Open the complete Gases map →Open all five lessons and twenty problems →Build a balanced five-topic set →

LIQUIDS AND SOLIDS

Move from particles to properties.

18 study objectives across six official topics, with 6 guided lessons and 24 original questions. The route separates bonding from intermolecular attraction and keeps every phase and property claim evidence-bounded.

A

Intermolecular forces

  1. 01Interparticle versus intraparticle forces
  2. 02Dispersion, dipole, hydrogen-bond, and ion–dipole recognition
  3. 03Relative attraction and polarizability
B

Phase changes

  1. 01Six phase changes and energy direction
  2. 02Heating curves and latent heat
  3. 03Phase diagrams and special points
C

Vapor pressure

  1. 01Evaporation and dynamic vapor equilibrium
  2. 02Temperature, attraction, and volatility
  3. 03Boiling point and external pressure
D

Structures

  1. 01Crystalline and amorphous solids
  2. 02Four major crystalline-solid types
  3. 03Unit-cell counting and packing
E

Polarity

  1. 01Bond dipoles and net molecular polarity
  2. 02Polarity and available attractions
  3. 03Evidence-controlled polarity comparisons
F

Properties

  1. 01Viscosity and molecular motion
  2. 02Cohesion, adhesion, and surface behavior
  3. 03Structure–property patterns in solids
Open the complete Liquids and Solids map →Open all six lessons and twenty-four problems →Build a balanced six-topic set →

SOLUTIONS

Separate particle count from particle identity.

15 study objectives across five official topics, with 5 guided lessons and 20 original questions. The route protects polarity and force comparisons, colligative versus non-colligative boundaries, saturation and gas-solubility conditions, and the denominator behind every concentration unit.

A

Polarity

  1. 01Solvent, solute, and molecular polarity
  2. 02Polarity matching and qualitative solubility
  3. 03Mixed functionality and evidence-controlled miscibility
B.1

Properties — colligative

  1. 01Colligative particle-count principle
  2. 02Vapor-pressure, boiling-point, and freezing-point shifts
  3. 03Osmosis and osmotic pressure
B.2

Properties — non-colligative

  1. 01Unsaturated, saturated, and supersaturated states
  2. 02Temperature, pressure, and solubility evidence
  3. 03Electrolytes, conductivity, and identity-dependent properties
C

Forces

  1. 01Three interaction sets in dissolution
  2. 02Solvation-force inventory
  3. 03Energetic evidence and solution-formation limits
D

Concentration calculations

  1. 01Molarity from amount and solution volume
  2. 02Dilution and solution preparation
  3. 03Choosing and converting concentration units
Open the complete Solutions map →Open all five lessons and twenty problems →Build a balanced five-topic set →

ACIDS AND BASES

Track the proton. Choose the regime.

12 study objectives across four official topics, with 4 guided lessons and 16 original questions. The route separates strength from concentration, protects logarithmic and temperature boundaries, and sequences neutralization, weak equilibrium, buffers, and titration regions.

A

pH

  1. 01Hydronium, hydroxide, and water autoionization
  2. 02pH and pOH logarithmic conversions
  3. 03Reading a logarithmic acidity scale
B

Strength

  1. 01Strength versus concentration
  2. 02Ka, Kb, pKa, and conjugate strength
  3. 03Structural evidence and percent ionization
C

Brønsted–Lowry reactions

  1. 01Reaction-specific proton donors and acceptors
  2. 02Conjugate pairs and amphiprotic species
  3. 03Direction of proton-transfer equilibrium
D

Calculations

  1. 01Strong acid–base mixing and excess reagent
  2. 02Weak-acid, weak-base, and salt equilibria
  3. 03Buffer and titration regime selection
Open the complete Acids and Bases map →Open all four lessons and sixteen problems →Build a balanced four-topic set →

CHEMICAL EQUILIBRIA

Compare Q with K. Then justify the response.

15 study objectives across five official topics, with 5 guided lessons and 20 original questions. The route separates equilibrium composition from reaction rate, generalizes acid-base constants, protects precipitation thresholds and ICE-table logic, and makes every Le Chatelier condition explicit.

A

Molecular

  1. 01Dynamic equilibrium at the molecular scale
  2. 02Reaction quotients and equilibrium expressions
  3. 03Composition, direction, and the meaning of K
B

Acid/base

  1. 01Acid and base constants in the general K framework
  2. 02Coupled proton-transfer equilibria
  3. 03Common-ion response and acid-base speciation
C

Precipitation

  1. 01Solubility-product expressions and molar solubility
  2. 02Precipitation thresholds after mixing
  3. 03Common ions and selective precipitation
D

Calculations

  1. 01Evaluate K and Q from chemical data
  2. 02Transform reactions and equilibrium constants
  3. 03ICE-table solutions and physical verification
E

Le Chatelier’s principle

  1. 01Concentration stresses through Q and K
  2. 02Gas volume, pressure, and inert-gas boundaries
  3. 03Temperature, catalysts, and equilibrium position
Open the complete Chemical Equilibria map →Open all five lessons and twenty problems →Build a balanced five-topic set →

THERMODYNAMICS AND THERMOCHEMISTRY

Track the boundary. Preserve the sign.

15 study objectives across five official topics, with 5 guided lessons and 20 original questions. The route separates state from path, system from surroundings, spontaneity from speed, and sensible heat from phase-change energy.

A

Laws of thermodynamics

  1. 01System boundaries and the first law
  2. 02State functions and path functions
  3. 03Second and third laws
B

Hess’s law

  1. 01Transform thermochemical equations
  2. 02Hess cycle construction
  3. 03Standard enthalpies of formation
C

Spontaneity

  1. 01Spontaneity is not speed
  2. 02Gibbs-energy direction criterion
  3. 03Temperature and Gibbs energy
D

Enthalpies and entropies

  1. 01Enthalpy signs and constant-pressure heat
  2. 02Entropy and multiplicity trends
  3. 03Standard reaction enthalpy and entropy
E

Heat transfer

  1. 01Sensible heat and thermal capacity
  2. 02Calorimeter energy balance
  3. 03Multistep heating and phase change
Open the complete Thermodynamics and Thermochemistry map →Open all five lessons and twenty problems →Build a balanced five-topic set →

CHEMICAL KINETICS

Measure the slope. Identify the law.

9 source-mapped study objectives across three official topics, with 3 guided lessons and 12 original questions. The route separates species rate from reaction rate, empirical order from coefficients, activation barriers from thermodynamic endpoints, and first-order half-life from zero- and second-order models.

A

Rate laws

  1. 01Reaction rate from concentration change
  2. 02Empirical rate laws and initial rates
  3. 03Integrated laws and linear plots
B

Activation energy

  1. 01Effective collisions and rate factors
  2. 02Arrhenius temperature dependence
  3. 03Energy profiles and catalytic paths
C

Half-life

  1. 01Half-life definition and data reading
  2. 02Order-dependent half-life relationships
  3. 03Repeated halves and kinetic-model selection
Open the complete Chemical Kinetics map →Open all three lessons and twelve problems →Build a balanced three-topic set →

OXIDATION–REDUCTION REACTIONS

Count the electrons. Close the circuit.

12 source-mapped study objectives across four official topics, with 4 guided lessons and 16 original questions. The route protects acidic versus basic balancing, oxidation-number rules and exceptions, electron and charge conservation, cell-potential signs, standard versus nonstandard conditions, thermodynamic and equilibrium links, electrolysis stoichiometry, electrode roles, and electron-versus-ion pathways.

A

Balancing equations

  1. 01Half-reaction electron ledger
  2. 02Acidic-solution half-reaction method
  3. 03Basic-solution conversion and verification
B

Determination of oxidation numbers

  1. 01Oxidation-number sum rules
  2. 02Rule priority and common exceptions
  3. 03Redox changes and agent labels
C

Electrochemical calculations

  1. 01Standard cell potential and direction
  2. 02Potential, free energy, equilibrium, and Q
  3. 03Current, charge, and electrolysis stoichiometry
D

Electrochemical concepts and terminology

  1. 01Electrode roles and charge pathways
  2. 02Galvanic versus electrolytic cells
  3. 03Cell notation and phase boundaries
Open the complete Oxidation–Reduction Reactions map →Open all four lessons and sixteen problems →Build a balanced four-topic set →

ATOMIC AND MOLECULAR STRUCTURE

Build from particles to shape.

24 study objectives across eight official topics. 8 lessons and 32 questions provide complete guided coverage.

A

Electron configuration

  1. 01Ground-state electron configurations
  2. 02Electron configurations of ions
  3. 03Valence and unpaired-electron inference
B

Orbital types

  1. 01Orbital types and qualitative shapes
  2. 02Subshell orbital counts and capacities
  3. 03Allowed quantum-number sets
C

Lewis-dot diagrams

  1. 01Valence-electron budgets
  2. 02Lewis structures and formal charge
  3. 03Resonance and octet exceptions
D

Atomic theory

  1. 01Evidence and atomic models
  2. 02Atomic number, mass number, and isotopes
  3. 03Average atomic mass
E

Quantum theory

  1. 01Photon wavelength, frequency, and energy
  2. 02Quantized energy and line spectra
  3. 03Quantum description and probability
F

Molecular geometry

  1. 01Electron-group and molecular geometry
  2. 02Lone pairs and bond-angle trends
  3. 03Bond dipoles and molecular polarity
G

Bond types

  1. 01Ionic, covalent, and metallic bonding
  2. 02Bond order, length, strength, and multiplicity
  3. 03Orbital overlap and hybridization
H

Sub-atomic particles

  1. 01Subatomic charge, mass, and location
  2. 02Particle inventory from nuclide notation
  3. 03Isotope, ion, and element identity
Open the complete Atomic/Molecular map →Open Lewis, Bonding, and Geometry lessons →Build a balanced eight-topic set →

PERIODIC PROPERTIES

Turn position into chemical evidence.

12 study objectives across four official topics, with 4 lessons and 16 original questions.

A

Representative elements

  1. 01Group, block, and valence pattern
  2. 02Common main-group ions
  3. 03Representative-element family behavior
B

Transition elements

  1. 01d-block position and ion configuration
  2. 02Variable oxidation states and formulas
  3. 03Characteristic transition-metal evidence
C

Periodic trends

  1. 01Atomic, ionic, and isoelectronic radius
  2. 02Ionization energy and shell evidence
  3. 03Electron attraction and metallic character
D

Descriptive chemistry

  1. 01Family-based reaction patterns
  2. 02Oxide character across a period
  3. 03Identification from chemical evidence
Open the complete Periodic Properties map →Open all four lessons and sixteen problems →Build a balanced four-topic set →

NUCLEAR REACTIONS

Conserve the nucleus. Name the change.

15 source-mapped study objectives across five official topics, with 5 guided lessons and 20 original questions. The route protects independent A/Z conservation, mass conventions, binding-energy units and basis, parent–daughter changes, decay mathematics, radiation quantities, activity-versus-dose boundaries, and precise fission, fusion, and chain-reaction terminology.

A

Balancing equations

  1. 01Nuclide notation and particle inventory
  2. 02Mass-number and atomic-number conservation
  3. 03Decay and bombardment equations
B

Binding energy

  1. 01Mass defect from supplied masses
  2. 02Binding energy and energy units
  3. 03Binding energy per nucleon and stability
C

Decay processes

  1. 01Parent–daughter changes by decay mode
  2. 02Decay constant and half-life
  3. 03Remaining fraction, age, and activity
D

Particles

  1. 01Nuclear-particle notation and identity
  2. 02Ionization, penetration, and shielding
  3. 03Particle inference from nuclear change
E

Terminology

  1. 01Nuclide and decay vocabulary
  2. 02Fission, fusion, and transmutation
  3. 03Activity, exposure, dose, and isotope use
Open the complete Nuclear Reactions map →Open all five lessons and twenty problems →Build a balanced five-topic set →

LABORATORY

Measure with intent. Conclude within evidence.

15 source-mapped study objectives across five official topics, with 5 guided lessons and 20 original questions. The complete bank protects apparatus purpose and reading, meniscus and transfer technique, calibration, accuracy and precision, random and systematic error, uncertainty and significant figures, hazard controls, PPE, waste handling, tables, graphs, anomalies, and supplied-protocol boundaries.

A

Basic techniques

  1. 01Reading and recording measurements
  2. 02Transfer, mixing, heating, and separation technique
  3. 03Procedure sequence and observation integrity
B

Equipment

  1. 01Volumetric glassware by purpose
  2. 02Measuring, heating, and support equipment
  3. 03Setup, calibration, and delivered readings
C

Error analysis

  1. 01Accuracy, precision, and percent error
  2. 02Random scatter and systematic bias
  3. 03Uncertainty, significant figures, and calibration evidence
D

Safety

  1. 01Hazard identification and control selection
  2. 02PPE and emergency response
  3. 03Chemical handling, storage, and waste
E

Data analysis

  1. 01Tables, variables, and units
  2. 02Graph choice, slope, intercept, and trend
  3. 03Replicates, anomalies, and bounded conclusions
Open the complete Laboratory map →Open all five lessons and twenty problems →Build a balanced five-topic set →

STOICHIOMETRY

21 focused objectives

Three assessable outcomes under each official topic. These are study units—not official topic weights.

A

Percent composition

  1. 01Formula mass and mass percent
  2. 02Composition from measured masses
  3. 03Composition comparison and purity
B

Empirical formulae

  1. 01Mass-to-mole ratio conversion
  2. 02Non-integer ratio resolution
  3. 03Empirical-to-molecular formula
C

Balancing equations

  1. 01Conservation and coefficient selection
  2. 02Formula identity versus coefficients
  3. 03Equation verification and simplest ratio
D

Moles and molecular formulas

  1. 01Mole, entities, and Avogadro’s constant
  2. 02Formula units and atom inventories
  3. 03Molecular and empirical identity
E

Molar mass

  1. 01Molar mass from a formula
  2. 02Mass–mole conversion
  3. 03Molar mass as an identification constraint
F

Density

  1. 01Density relationship and units
  2. 02Volume by displacement
  3. 03Density, identity, and measurement limits
G

Calculations from balanced equations

  1. 01Mole ratios from equations
  2. 02Limiting reactant and excess
  3. 03Theoretical, actual, and percent yield
Open the complete Stoichiometry learning lab →Build a balanced Stoichiometry set →

Transparent by design

The ADA publishes scope—not domain quotas.

The official manual lists 30 General Chemistry questions and the hierarchy below. It does not publish a question count for each domain, so DAT TRAIN will not present guessed percentages as official.

The 66 count is DAT TRAIN’s transparent leaf-level representation of the published hierarchy, including separate colligative and non-colligative solution properties. It is a curriculum index, not an exam weighting.

Figure 2 · PDF page 34

Official General Chemistry map

ADA DAT User’s Manual 2026

I

Stoichiometry and General Concepts

7 topics

  1. APercent composition
  2. BEmpirical formulae
  3. CBalancing equations
  4. DMoles and molecular formulas
  5. EMolar mass
  6. FDensity
  7. GCalculations from balanced equations
II

Gases

5 topics

  1. AKinetic molecular theory of gases
  2. BDalton’s gas law
  3. CBoyle’s gas law
  4. DCharles’s gas law
  5. EIdeal gas law
III

Liquids and Solids

6 topics

  1. AIntermolecular forces
  2. BPhase changes
  3. CVapor pressure
  4. DStructures
  5. EPolarity
  6. FProperties
IV

Solutions

5 topics

  1. APolarity
  2. B.1Properties — colligative
  3. B.2Properties — non-colligative
  4. CForces
  5. DConcentration calculations
V

Acids and Bases

4 topics

  1. ApH
  2. BStrength
  3. CBrønsted–Lowry reactions
  4. DCalculations
VI

Chemical Equilibria

5 topics

  1. AMolecular
  2. BAcid/base
  3. CPrecipitation
  4. DCalculations
  5. ELe Chatelier’s principle
VII

Thermodynamics and Thermochemistry

5 topics

  1. ALaws of thermodynamics
  2. BHess’s law
  3. CSpontaneity
  4. DEnthalpies and entropies
  5. EHeat transfer
VIII

Chemical Kinetics

3 topics

  1. ARate laws
  2. BActivation energy
  3. CHalf-life
IX

Oxidation–Reduction Reactions

4 topics

  1. ABalancing equations
  2. BDetermination of oxidation numbers
  3. CElectrochemical calculations
  4. DElectrochemical concepts and terminology
X

Atomic and Molecular Structure

8 topics

  1. AElectron configuration
  2. BOrbital types
  3. CLewis-dot diagrams
  4. DAtomic theory
  5. EQuantum theory
  6. FMolecular geometry
  7. GBond types
  8. HSub-atomic particles
XI

Periodic Properties

4 topics

  1. ARepresentative elements
  2. BTransition elements
  3. CPeriodic trends
  4. DDescriptive chemistry
XII

Nuclear Reactions

5 topics

  1. ABalancing equations
  2. BBinding energy
  3. CDecay processes
  4. DParticles
  5. ETerminology
XIII

Laboratory

5 topics

  1. ABasic techniques
  2. BEquipment
  3. CError analysis
  4. DSafety
  5. EData analysis

CALCULATION CHECKS

A chemistry answer needs more than arithmetic.

UNITS

Compatible conversions

Track the dimension of every quantity, and treat Celsius conversions differently from simple scale factors.

NUMBERS

Reasonable precision

Keep enough working digits, then round the result according to the information supplied.

NOTATION

Significant figures

Read decimal and scientific notation carefully so the reported precision matches the calculation.

EQUATIONS

Atoms and charge

Confirm that every element and the net charge are conserved, then reduce coefficients to the simplest whole-number ratio.

Free remediation

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Stoichiometry, Atomic and Molecular Structure, Periodic Properties, Gases, Liquids and Solids, Solutions, Acids and Bases, Chemical Equilibria, Thermodynamics and Thermochemistry, Chemical Kinetics, Oxidation–Reduction Reactions, Nuclear Reactions, and Laboratory objectives link to precise free sources. These broader references remain available for the rest of General Chemistry.

OpenStax Chemistry 2eFree full general-chemistry textbookOpen ↗Khan Academy ChemistryFree lessons and worked practiceOpen ↗Khan Academy AP/College ChemistryDeeper college-level concept reviewOpen ↗
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