CHEM1B TTU K12
Composed course package for TTU K-12 CHEM 1B (Chemistry I, Semester B): chemical reactions, stoichiometry, gas laws, solutions, acids & bases, thermochemistry, and nuclear chemistry, filtered from the Chemistry Fundamentals corpus with syllabus-emphasis weighting.
180
Minutes
50
Questions
70/100
Passing Score
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 Covered
1Atomic Structure
2Periodic Table and Trends
3Chemical Bonding
4Stoichiometry
5Types of Chemical Reactions
6Thermochemistry
7Gas Laws
8Solutions and Concentrations
9Acids, Bases, and pH
10Chemical Equilibrium
11Redox Reactions
12Introduction to Organic Chemistry
13Nuclear Chemistry
What's Included in AccelaStudy® AI
Adaptive Knowledge Graph
Practice Questions
Lesson Modules
Console Simulator Labs
Exam Tips & Strategy
13 Activity Formats
Course Outline
1Stoichiometry 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
2Types 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
3Thermochemistry 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
4Gas Laws 5 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
Describe the kinetic molecular theory of gases, including the assumptions that gas particles are in constant random motion, have negligible volume relative to their container, and experience no intermolecular attractive forces, and explain how these assumptions account for the empirical gas laws
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
5Solutions and Concentrations 6 topics
Describe the dissolution process including solvation, the role of intermolecular forces in determining miscibility and solubility, and the like-dissolves-like principle
Classify a solute as a strong electrolyte, weak electrolyte, or nonelectrolyte based on its extent of dissociation into ions in aqueous solution, and relate electrolyte strength to the electrical conductivity of the resulting solution
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
Interpret a solubility-versus-temperature graph to determine the mass of solute that will dissolve in a given mass of solvent at a specified temperature, and classify a solution as unsaturated, saturated, or supersaturated by comparing its solute concentration to the graphed solubility curve
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
6Acids, Bases, and pH 6 topics
Describe the Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases and identify conjugate acid-base pairs in proton transfer reactions
Apply nomenclature rules to name and write formulas for binary acids and oxyacids (including the hydro-/-ic and -ic/-ous naming conventions) and for common bases, given either the chemical formula or the name
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
7Nuclear Chemistry 5 topics
Describe standard isotope notation (mass number and atomic number), define radioactivity, and distinguish alpha, beta, and gamma emissions by their particle identity, charge, mass, and relative penetrating power
Apply conservation of mass number and atomic number to write and balance nuclear equations for alpha decay, beta decay, and gamma emission, identifying the resulting daughter nuclide
Describe the differences between nuclear fission and nuclear fusion, compare their relative energy release, and identify real-world applications including nuclear power reactors and stellar fusion
Apply the concept of half-life to calculate the fraction or amount of a radioactive sample remaining after a given number of half-lives has elapsed
Analyze the practical benefits and risks of nuclear fission power generation versus nuclear fusion research, evaluating factors such as waste products, safety, and current technological feasibility
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, and introductory nuclear chemistry including isotope notation, nuclear equations, alpha/beta/gamma decay, half-life calculations, and nuclear fission and fusion
Not Covered
- Advanced organic synthesis mechanisms and multi-step reaction planning
- Electrochemistry and electrochemical cells beyond introductory redox
- Quantum mechanical calculations and orbital mathematics
- Industrial chemistry processes and reactor design
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