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Senior High School Specialized Subject: General Chemistry 1 & 2



General Chemistry 1 & 2 is one of the specialized subjects under the Academic career track and the STEM learning strand. Some examples of the things that you will learn from taking this subject include:

  • Matter and its Properties
    • The particulate nature of matter
    • States of matter
      • the macroscopic
      • microscopic view
    • Physical and chemical properties
    • Extensive and intensive properties
    • Ways of classifying matter
      • pure substances and mixtures
      • elements and compounds
      • homogeneous and heterogeneous mixtures
    • Methods of separating mixtures into their component substances
  • Measurements
    • Accuracy and precision
    • Significant figures in calculations
    • Density measurement
  • Atoms, Molecules, and Ions
    • Dalton’s atomic theory
    • Basic laws of matter
    • Atomic structure
    • Subatomic particles (protons, electrons, neutrons)
    • Molecules and ions
    • Chemical formulas
    • Naming compounds
  • Stoichiometry
    • Atomic mass
    • Avogadro’s number
    • The mole concept
    • Percent composition and chemical formulas
    • Chemical reactions and chemical equations
    • Types of chemical reactions in aqueous solutions
  • Mass relationships in chemical reactions
  • Gases
    • Pressure of a gas
      • Units of pressure
    • The Gas Laws
      • Boyle’s law
      • Charles’ law
      • Avogadro’s law
    • Ideal Gas Equation
    • Dalton’s law of partial pressures
    • Gas stoichiometry
    • Kinetic molecular theory of gases
  • Electronic Structure of Atoms
    • Quantum mechanical description of the atom
    • Schrodinger’s model of the hydrogen atom and wave functions
    • Main energy levels, sublevels, and orbitals
    • Quantum numbers
    • Electron Configuration
      • Aufbau principle
      • Pauli exclusion principle
      • Hund’s rule
      • Diamagnetism and paramagnetism
      • Orbital diagrams
  • Electronic Structure and Periodicity
    • The electron configuration and the periodic table
    • Periodic variation in atomic properties
      • Atomic radius and effective nuclear charge; the shielding effect in many-electron atoms
      • Ionic radius
      • Ionization energy
      • Electron affinity
  • Chemical Bonding Ionic Bonds
    • The stability of noble gases
    • Forming ions
    • Ionic bonding
    • Ionic compounds
    • Formulas
    • Structure
    • Properties
  • Covalent Bonds
    • Formation of covalent bonds
    • Formulas of molecular compounds
    • Lewis structure of molecules
    • Molecules of elements
    • Molecules of compounds
    • Structure and properties of
    • molecular compounds
    • Strength of covalent bonds
    • Electronegativity and bond polarity
    • Geometry of molecules
    • Polarity of compounds
  • Organic compounds
    • The carbon atom
    • Bonding patterns in hydrocarbons
    • Properties and reactivities of common functional groups
    • Polymers
    • Biomolecules
  • Intermolecular Forces and Liquids and Solids
    • Kinetic molecular model of liquids and solids
    • Intermolecular forces
    • Dipole-dipole forces
    • Ion-dipole forces
    • Dispersion forces
    • Hydrogen bonds
    • Properties of liquids and IMF
    • Surface tension
    • Viscosity
    • Vapour pressure, boiling point
    • Molar heat of vaporization
    • Structure and properties of water
    • Types and properties of solids
    • Crystalline and amorphous solids
    • Types of crystals
    • Phase changes
  • Physical Properties of Solutions
    • Types of solutions
    • Energy of solution formation
    • Concentration Units and comparison of concentration units
      • percent by mass, by volume
      • mole fraction
      • molality
      • molarity
      • percent by volume, percent by mass, PPM
    • Solution stoichiometry
    • Factors affecting solubility
    • Colligative properties of nonelectrolyte and electrolyte solutions
  • Thermochemistry
    • Energy changes in chemical reactions: exothermic and endothermic processes
    • First law of thermodynamics
    • Enthalpy of a chemical reaction
    • Calorimetry
    • Standard enthalpy of formation and reaction Hess’ law
  • Chemical Kinetics
    • The rate of a reaction
    • Factors that influence reaction rate
    • The rate law and its components
    • Collision theory
    • Catalysis
  • Chemical Thermodynamics
    • Spontaneous processes
    • Entropy
    • The second law of thermodynamics
    • Gibbs free energy and chemical equilibrium
  • Chemical Equilibrium
    • The equilibrium condition
    • Writing the reaction quotient/equilibrium constant expression
    • Predicting the direction of a reaction
    • Significance of the equilibrium constant
    • Le Chatelier’s principle
  • Acid-Base Equilibria and Salt Equilibria
    • Bronsted acids and bases
    • The acid-base properties of water
    • pH- a measure of acidity
    • Strength of acids and bases
    • Weak acids/weak bases and ionization constants
    • Relationship between the ionization constants of acids and their conjugate bases
    • The common ion effect
    • Buffer solutions
    • Solubility equilibria
  • Electrochemistry
    • Redox reactions
    • Galvanic cells
    • Standard reduction potentials
    • Spontaneity of redox reactions
    • Batteries
    • Corrosion
    • Electrolysis

While studying, you will also be asked to demonstrate what you have learned by participating in class activities that may include the following:

  • Designing a representation or simulation of any of the following:
    • atomic structure
    • gas behavior
    • mass relationships
    • reactions
  • Illustrating the reactions at the molecular level in any of the following:
    • enzyme action
    • protein denaturation
    • separation of components in coconut milk
  • Designing a simple investigation to determine the effect on boiling point or freezing point when a solid is dissolved in water
  • Preparing a poster on a specific application of one of the following:
    • Acid-base equilibrium
    • Electrochemistry
  • Using properties of matter to identify substances and to separate them
  • Comparing consumer products on the basis of their components for use, safety, quality and cost
  • Determining the molar mass of elements and compounds
  • Calculating the mass of a given number of moles of an element or compound or vice versa
  • Calculating the percent composition of a compound from its formula
  • Writing equations for chemical reactions and balance the equations
  • Calculating reaction yield when a limiting reagent is present
  • Determining the polarity of a bond based on the electronegativities of the atoms forming the bond

These examples only cover the scope of the specialized subjects under the Academic track and STEM learning strand. For the scope of the core and contextualized subjects under the senior high school curriculum, please refer to their respective lists.

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