Chemistry Fundamentals
Chemistry Fundamentals covers the essential principles of matter and chemical change from atomic theory and periodic trends through chemical bonding, stoichiometry, thermochemistry, equilibrium, and introductory organic chemistry. The course provides a rigorous conceptual and quantitative foundation that connects macroscopic observations to atomic-level explanations.
Who Should Take This
This course is ideal for students preparing for introductory college chemistry, AP Chemistry, or any standardized exam with a chemistry component. It is also well-suited for professionals in engineering, biology, or environmental science who need a refresher on foundational chemical principles before tackling more advanced material.
What's Included in AccelaStudy® AI
Adaptive Knowledge Graph
Practice Questions
Lesson Modules
Console Simulator Labs
Exam Tips & Strategy
13 Activity Formats
Course Outline
1Atomic Structure 6 topics
Describe the structure of the atom including the nucleus containing protons and neutrons and the electron cloud, and define atomic number, mass number, and isotopes
Explain the quantum mechanical model of the atom including electron shells, subshells (s, p, d, f), orbitals, and write ground-state electron configurations using the Aufbau principle, Hund's rule, and the Pauli exclusion principle
Describe the Bohr model of the hydrogen atom including energy levels, electron transitions, and how photons are emitted or absorbed when electrons change energy levels
Apply the relationship between electron configuration and the position of an element in the periodic table to identify the block, period, and group of any element from its configuration
Calculate the average atomic mass of an element from the masses and natural abundances of its isotopes using the weighted average formula
Analyze the historical development of atomic models from Dalton through Thomson, Rutherford, Bohr, and the quantum mechanical model, evaluating the experimental evidence that required each revision
2Periodic Table and Trends 5 topics
Identify the organization of the periodic table including periods, groups, and the main classifications of metals, nonmetals, metalloids, representative elements, transition metals, and noble gases
Explain periodic trends in atomic radius, ionization energy, electron affinity, and electronegativity and predict how these properties change across periods and down groups
Apply periodic trends to predict the chemical reactivity of elements, identify likely oxidation states, and explain why noble gases are largely unreactive
Analyze how effective nuclear charge and electron shielding explain periodic trends, and compare the properties of isoelectronic species to illustrate the effect of nuclear charge on ionic radius
Describe the physical and chemical properties of representative element families including alkali metals, alkaline earth metals, halogens, and noble gases
3Chemical Bonding 7 topics
Describe ionic bonding including the transfer of electrons between metals and nonmetals, the formation of cations and anions, and the properties of ionic compounds such as high melting points and electrical conductivity in solution
Draw Lewis structures for covalent molecules and polyatomic ions including single, double, and triple bonds, lone pairs, and apply formal charge to identify the most stable resonance structure
Apply VSEPR theory to predict the electron geometry and molecular geometry of molecules with two through six electron domains, including tetrahedral, trigonal planar, bent, and linear shapes
Explain polarity of bonds and molecules using electronegativity differences and molecular geometry, and predict whether a molecule will have a net dipole moment
Describe metallic bonding using the electron sea model and relate the delocalized electron structure to the properties of metals including conductivity, malleability, and ductility
Explain intermolecular forces including London dispersion forces, dipole-dipole interactions, and hydrogen bonding, and relate force strength to physical properties such as boiling point and vapor pressure
Analyze how bond type and intermolecular forces determine the physical and chemical properties of ionic, covalent network, molecular, and metallic solids, using diamond, NaCl, ice, and copper as examples
4Stoichiometry 5 topics
Describe the mole concept including Avogadro's number, molar mass, and the interconversion between mass, moles, and number of particles for elements and compounds
Balance chemical equations and apply mole ratios from balanced equations to calculate theoretical yields in mole-to-mole, mass-to-mass, and limiting reagent stoichiometry problems
Calculate percent yield and percent composition by mass, and determine the empirical and molecular formula of a compound from combustion analysis or mass percent data
Analyze sources of error in stoichiometric calculations including impure reactants, side reactions, and incomplete reactions, and explain how percent yield quantifies the efficiency of a chemical process
Apply stoichiometry to solution chemistry problems including calculating molarity, dilution calculations using M1V1 = M2V2, and moles of solute in a given volume of solution
5Types of Chemical Reactions 5 topics
Identify and describe the five major categories of chemical reactions: synthesis, decomposition, single replacement, double replacement, and combustion, with representative examples of each
Apply activity series and solubility rules to predict whether single replacement and double replacement reactions will occur and write net ionic equations for precipitation reactions
Describe reaction rate and the factors that affect it including concentration, temperature, surface area, and catalysts, and explain how collision theory accounts for these effects
Analyze activation energy diagrams for exothermic and endothermic reactions, identify the transition state, and explain how catalysts lower the activation energy without changing the overall energy change
Apply net ionic equation writing to identify spectator ions in double replacement reactions and represent only the species that actually undergo change during precipitation, neutralization, and gas-forming reactions
6Thermochemistry 5 topics
Describe the concepts of system and surroundings, exothermic and endothermic reactions, enthalpy (H), and the sign conventions for heat flow in chemical and physical processes
Apply Hess's law and standard enthalpies of formation to calculate the enthalpy change of a reaction that cannot be directly measured
Calculate heat transfer using q = mcΔT and apply calorimetry principles to determine the enthalpy of reaction from measured temperature changes in a constant-pressure calorimeter
Describe entropy as a measure of disorder and explain how the second law of thermodynamics and the concept of Gibbs free energy (ΔG = ΔH − TΔS) determine whether a reaction is spontaneous
Analyze how temperature, enthalpy, and entropy interact to determine spontaneity, predict under what conditions an endothermic reaction can become spontaneous, and evaluate the four possible combinations of ΔH and ΔS signs
7Gas Laws 4 topics
Describe Boyle's law, Charles's law, Gay-Lussac's law, and Avogadro's law using both verbal statements and mathematical relationships between pressure, volume, temperature, and moles of gas
Apply the ideal gas law PV = nRT to solve problems involving any three of the four variables given the fourth, using appropriate units and the gas constant R
Apply Dalton's law of partial pressures and Graham's law of effusion to solve problems involving gas mixtures and the relative rates of diffusion of gases with different molar masses
Analyze the conditions under which real gases deviate significantly from ideal behavior using the van der Waals equation and explain why high pressure and low temperature cause deviations
8Solutions and Concentrations 4 topics
Describe the dissolution process including solvation, the role of intermolecular forces in determining miscibility and solubility, and the like-dissolves-like principle
Calculate solution concentration in units of molarity, molality, and mass percent, and apply Henry's law and the effect of temperature on gas and solid solubility in liquids
Apply colligative property calculations for boiling point elevation, freezing point depression, and osmotic pressure using the van't Hoff factor for electrolyte solutions
Analyze how colligative properties depend on solute particle concentration rather than identity, and compare the effect of ionic versus molecular solutes on boiling and freezing point changes
9Acids, Bases, and pH 5 topics
Describe the Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases and identify conjugate acid-base pairs in proton transfer reactions
Calculate pH, pOH, and hydrogen ion concentration using the relationships pH = -log[H+] and the water autoionization constant Kw, and determine whether a solution is acidic, basic, or neutral
Apply Ka and Kb expressions to calculate the pH of weak acid and weak base solutions, and explain the relationship between acid strength and the extent of dissociation
Explain buffer solutions including how a weak acid and its conjugate base resist changes in pH, apply the Henderson-Hasselbalch equation, and describe the biological importance of buffers
Analyze acid-base neutralization reactions and titration calculations to determine the concentration of an unknown acid or base using equivalence point data and indicator selection
10Chemical Equilibrium 5 topics
Describe dynamic chemical equilibrium including the condition where forward and reverse reaction rates are equal, and write equilibrium constant expressions (Kc and Kp) for homogeneous reactions
Apply Le Chatelier's principle to predict the direction an equilibrium will shift in response to changes in concentration, pressure, volume, and temperature
Calculate equilibrium concentrations using an ICE table approach for reactions given initial concentrations and the equilibrium constant, and interpret whether K > 1 or K < 1 favors products or reactants
Analyze how industrial processes such as the Haber process for ammonia synthesis exploit Le Chatelier's principle to maximize yield under practical temperature and pressure constraints
Apply the reaction quotient Q compared to K to predict the direction a reaction will proceed to reach equilibrium, and explain the relationship between K and Gibbs free energy ΔG° = -RT ln K
11Redox Reactions 4 topics
Describe oxidation-reduction reactions in terms of electron transfer, define oxidation number, and identify the oxidizing agent and reducing agent in a reaction
Apply the half-reaction method to balance redox equations in acidic and basic solutions, ensuring conservation of mass and charge
Analyze the activity series of metals to predict whether a single-replacement redox reaction will occur spontaneously and explain the driving force in terms of relative reduction potentials
Apply oxidation state rules to assign oxidation numbers to atoms in elements, ions, and compounds, and use changes in oxidation state to identify oxidation and reduction in complex reactions including those involving polyatomic ions
12Introduction to Organic Chemistry 5 topics
Describe the unique bonding properties of carbon including its tetravalence, ability to form single, double, and triple bonds, and capacity for forming long chains and rings as the basis of organic chemistry
Identify the major organic functional groups including alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, carboxylic acids, amines, and esters, and describe their characteristic physical and chemical properties
Apply IUPAC nomenclature rules to name and draw structural formulas for straight-chain and branched alkanes up to 10 carbons, and identify structural isomers
Explain the biological importance of organic macromolecules including carbohydrates, lipids, proteins, and nucleic acids by relating their functional groups and structures to their roles in living systems
Analyze how the polarity and intermolecular forces of organic functional groups explain the solubility, boiling points, and reactivity differences between compound classes such as alcohols versus alkanes of similar molecular weight
Scope
Included Topics
- Atomic structure and subatomic particles, periodic table trends and element properties, chemical bonding (ionic, covalent, metallic), VSEPR and molecular geometry, stoichiometry and molar calculations, types of chemical reactions, thermochemistry and enthalpy, gas laws (Boyle, Charles, Avogadro, ideal gas), solutions and concentration calculations, acids and bases including pH calculations, chemical equilibrium and Le Chatelier's principle, redox reactions and oxidation states, introduction to organic chemistry functional groups
Not Covered
- Advanced organic synthesis mechanisms and multi-step reaction planning
- Electrochemistry and electrochemical cells beyond introductory redox
- Nuclear chemistry and radioactive decay beyond conceptual overview
- Quantum mechanical calculations and orbital mathematics
- Industrial chemistry processes and reactor design
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