DepED Chemistry 3 Curriculum Guide Notes

Course Overview and Administrative Framework

  • Issuing Department: Department of Education (DepED), Republic of the Philippines (BAGONG PILIPINAS)
  • Course Title: Chemistry 3
  • Target Audience / Grade Level: Grade 11 / Grade 12
  • Curriculum Track: Academic Track (Elective)
  • Prerequisite Courses: Chemistry 1, Chemistry 2
  • Time Allotment: 80 hours total for one academic term

Course Description and Foundational Concepts

  • Core Focus: Building upon foundational chemical concepts developed in Chemistry 1 and Chemistry 2, specifically enabling learners to examine acid-base systems and chemical equilibria in aqueous solutions.
  • Acid-Base Systems:
    • Exploration of acid-base behavior utilizing three fundamental theoretical frameworks: Arrhenius, Brønsted-Lowry, and Lewis.
    • Analysis of quantitative acid and base concentrations.
    • Execution of titration experiments and interpretation of corresponding titration curves to analyze how the strengths of reactants influence pH at the equivalence point.
  • Buffer Systems: Investigation into the specific mechanics of buffer systems and their essential role in maintaining stable pH across biological, environmental, and chemical systems.
  • Chemical Equilibrium:
    • Investigation of dynamic chemical equilibrium operating within closed systems.
    • Application of mathematical equilibrium constants and Le Chatelier’s principle to predict the extent and direction of chemical reactions.
  • Instrumental Analysis & Separation Techniques:
    • Overview and implementation of physical separation techniques.
    • Application of colorimetry to determine solution concentrations through light absorption data and experimental interpretation.
  • Electrochemistry:
    • Explanation of fundamental oxidation-reduction (redox) processes.
    • Execution of simple electrolysis laboratory experiments.
    • Analysis of practical redox applications in electrochemical cells, battery technologies, corrosion prevention, and sustainable energy technologies.
  • Cross-Disciplinary Integration:
    • Utilization of graphical data, experimental metrics, and mathematical models to construct and communicate formal scientific explanations.
    • Promotion of systems thinking to connect chemical applications with environmental science, health sciences, and industrial processes.
    • Direct alignment with Green Chemistry principles and the Sustainable Development Goals (SDGs).

Unit 1: Acid-Base and Chemical Equilibrium

  • Module 1: Strength and Concentration of Acids and Bases

    • Content Standards:
      • Acids and bases found in everyday life and environmental systems play important roles in maintaining chemical balance in natural environments and human activities.
      • Different acid-base theories explain the behavior of acids and bases.
      • The pH of solutions describes the concentration of hydrogen ions, and the strength and concentration of acids and bases determine their behavior in chemical reactions.
    • Learning Standards:
      • Differentiate Arrhenius, Brønsted-Lowry, and Lewis' acid-base theories.
      • Calculate the pH of acids and bases commonly found at home and in the environment.
      • Conduct pH measurements to identify differences in the strengths of acids and bases.
      • Describe the dissociation of acids and bases in water, conjugate acid-base pairs in solution, and the amphiprotic nature of certain substances.
      • Explain the difference between strong and weak acids and bases and distinguish these from concentrated and dilute solutions.

  • Module 2: Acid-Base Titrations

    • Content Standards:
      • Titration curves provide graphical representations of acid-base reactions.
    • Learning Standards:
      • Conduct simple titration experiments and perform titrimetric calculations.

  • Module 3: Buffer Systems

    • Content Standards:
      • Buffer systems maintain relatively constant pH in natural, biological, and chemical systems.
    • Learning Standards:
      • Explain the role of buffer systems in maintaining stability in natural environments and biological systems.

  • Module 4: Chemical Equilibrium

    • Content Standards:
      • Chemical systems reach dynamic equilibrium in closed systems and the extent and direction of reactions can be predicted using equilibrium constants and Le Chatelier’s principle.
    • Learning Standards:
      • Differentiate static and dynamic equilibrium and relate equilibrium to closed chemical systems.
      • Explain the reversibility of chemical reactions using real-life examples, including:
        • Dissolution and release of carbon dioxide (CO2CO_2) in water.
        • Formation and decomposition of calcium carbonate (CaCO3CaCO_3) in limestone.
        • The Haber-Bosch process for ammonia synthesis.
      • Use equilibrium constant expressions (KcK_c) to calculate the concentrations of reactants and products at chemical equilibrium and determine the extent and direction of a chemical reaction.
      • Conduct investigations on the effects of temperature, concentration, volume, or pressure on a chemical system at equilibrium.
      • Analyze how reaction rates and chemical equilibrium are applied in environmental processes and industrial practices to optimize processes, reduce waste, and design sustainable solutions using Green Chemistry and systems thinking.

Unit 1 Performance Standards and Suggested Tasks

  • Performance Standards:
    • Design and conduct investigations to analyze the properties and behavior of acids, bases, and buffer systems.
    • Interpret pH values and titration curves using mathematical and graphical models.
    • Communicate scientific explanations using chemical equations and experimental evidence.
    • Explain chemical equilibrium and Le Chatelier’s principle, conduct investigations to observe changes in equilibrium systems, and apply these concepts to explain industrial and environmental processes using Green Chemistry principles.
  • Suggested Performance Tasks:
    • Task 1: Conduct an acid-base titration investigation to determine the concentration and strength of an unknown acid or base commonly found in household or environmental samples; explain the results using acid-base theories and neutralization concepts.
    • Task 2: Conduct an investigation on chemical equilibrium by changing temperature, concentration, or pressure in a reversible reaction system using Le Chatelier’s principle.

Unit 2: Instrumental Analysis and Electrochemistry

  • Module 5: Separation of Mixtures

    • Content Standards:
      • Mixtures can be separated based on differences in physical properties using appropriate techniques.
    • Learning Standards:
      • Differentiate common separation techniques, such as filtration, recrystallization, distillation, and chromatography based on their principles.
      • Conduct a laboratory activity using a separation technique and explain the results based on physical properties.

  • Module 6: Instrumental Analysis (Colorimetry)

    • Content Standards:
      • Instrumental analytical techniques use measurable signals such as light absorption to determine the concentration of substances.
    • Learning Standards:
      • Explain the principles of colorimetry based on light absorption by substances.
      • Describe the relationship between absorbance and concentration using calibration curves.
      • Conduct a colorimetry-based investigation to determine the concentration of an unknown solution.

  • Module 7: Redox Reactions

    • Content Standards:
      • Oxidation-reduction reactions involve electron transfer and changes in oxidation numbers.
    • Learning Standards:
      • Use the concepts of oxidation and reduction in terms of electron transfer and oxidation numbers to analyze redox reactions.
      • Write half-reactions and balance overall equations to represent redox reactions.

  • Module 8: Galvanic Cells

    • Content Standards:
      • Electrochemical cells convert chemical energy into electrical energy through redox processes.
    • Learning Standards:
      • Create diagrams of galvanic cells to identify the anode, cathode, and direction of electron flow.

  • Module 9: Electrochemical Potentials

    • Content Standards:
      • Standard electrode potentials and cell potentials can be used to predict the direction and spontaneity of redox reactions.
    • Learning Standards:
      • Use table of standard reduction potentials to identify and compare the reduction potentials of galvanic half-cells and the reactivity of metals in aqueous solutions.
      • Use cell potential values to predict the spontaneity of redox reactions.

  • Module 10: Electrolysis

    • Content Standards:
      • Electrolysis drives nonspontaneous redox reactions using electrical energy.
    • Learning Standards:
      • Conduct experiments on electrolysis processes.

  • Module 11: Applications of Electrochemistry

    • Content Standards:
      • Electrochemical principles are applied in technologies such as batteries, corrosion control, and sustainable energy systems.
    • Learning Standards:
      • Explain electrochemistry applications in batteries, sustainable energy technologies, and corrosion control.

Unit 2 Performance Standards and Suggested Tasks

  • Performance Standards:
    • Explain different separation techniques, interpret colorimetric data to determine concentrations, and conduct investigations using appropriate techniques.
    • Analyze redox reactions and use standard reduction potentials and cell potential values to predict reactivity and spontaneity.
    • Explain electrolysis processes and apply electrochemical principles to real-world systems such as batteries, corrosion control, and sustainable energy technologies.
  • Suggested Performance Tasks:
    • Task 1: Perform laboratory activity using either a separation technique (e.g., filtration or chromatography).
    • Task 2: Conduct a colorimetry investigation to determine the concentration of an unknown solution using a calibration curve and interpret the results.
    • Task 3: Construct and analyze a simple galvanic cell using two different metal electrodes and electrolyte solutions and explain the electron flow and spontaneity of the reaction using redox concepts.
    • Task 4: Investigate electrochemical applications by analyzing a real-world system (e.g., battery technology, corrosion prevention, or metal electroplating) and explain how electrochemical principles are used to improve energy efficiency, prevent corrosion, or support sustainable technologies.