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Standards of Learning - Science - Chemistry
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The Chemistry standards are designed to provide students with a detailed understanding of the interaction of matter and energy. This interaction is investigated through the use of laboratory techniques, manipulation of chemical quantities, and problem-solving applications. Scientific methodology will be employed in experimental and analytical investigations, and concepts will be illustrated with practical applications that should include examples from environmental, nuclear, organic, and biochemistry content areas.

Technology including graphing calculators, computers, and probeware will be employed where feasible. Students will understand and use safety precautions with chemicals and equipment. The standards emphasize qualitative and quantitative study of substances and the changes that occur in them. In meeting the chemistry standards, students will be encouraged to share their ideas, use the language of chemistry, discuss problem-solving techniques, and communicate effectively.

The Chemistry standards continue to focus on student growth in understanding the nature of science. This scientific view defines the idea that explanations of nature are developed and tested using observation, experimentation, models, evidence, and systematic processes. The nature of science includes the concepts that scientific explanations are based on logical thinking; are subject to rules of evidence; are consistent with observational, inferential, and experimental evidence; are open to rational critique; and are subject to refinement and change with the addition of new scientific evidence. The nature of science includes the concept that science can provide explanations about nature, can predict potential consequences of actions, but cannot be used to answer all questions.

CH.1 The student will investigate and understand that experiments in which variables are measured, analyzed, and evaluated, produce observations and verifiable data.  Key concepts include
  1. designated laboratory techniques;
  2. safe use of chemicals and equipment;
  3. proper response to emergency situations;
  4. manipulation of multiple variables with repeated trials;
  5. accurate recording, organizing, and analysis of data through repeated trials;
  6. mathematical and procedural error analysis;
  7. mathematical manipulations (SI units, scientific notation, linear equations, graphing, ratio and proportion, significant digits, dimensional analysis);
  8. the use of appropriate technology including computers, graphing calculators, and probeware for gathering data and communicating results; and
  9. construction and defense of a scientific viewpoint (the nature of science).
CH.2 The student will investigate and understand that the placement of elements on the periodic table is a function of their atomic structure.  The periodic table is a tool used for the investigations of
  1. average atomic mass, mass number, and atomic number;
  2. isotopes, half lives, and radioactive decay;
  3. characteristics of subatomic particles as to mass and charge;
  4. families or groups;
  5. series and periods;
  6. trends including atomic radii, electronegativity, shielding effect, and ionization energy;
  7. electron configurations, valence electrons, and oxidation numbers;
  8. chemical and physical properties; and
  9. historical and quantum models.
CH.3 The student will investigate and understand how conservation of energy and matter is expressed in chemical formulas and balanced equations.  Key concepts include
  1. nomenclature;
  2. balancing chemical equations;
  3. writing chemical formulas (molecular, structural, empirical, and Lewis diagrams);
  4. bonding types (ionic, covalent);
  5. reaction types (synthesis, decomposition, single and double replacement, oxidation-reduction, neutralization, exothermic and endothermic); and
  6. reaction rates and kinetics (activation energy, catalysis, degree of randomness).
CH.4 The student will investigate and understand that quantities in a chemical reaction are based on molar relationships.  Key concepts include
  1. Avogadro's principle and molar volume;
  2. stoichiometric relationships;
  3. partial pressure;
  4. gas laws;
  5. solution concentrations;
  6. chemical equilibrium; and
  7. acid/base theory: strong electrolytes, weak electrolytes, and nonelectrolytes; dissociation and ionization; pH and pOH; and the titration process.
CH.5 The student will investigate and understand that the phases of matter are explained by kinetic theory and forces of attraction between particles. Key concepts include
  1. pressure, temperature, and volume;
  2. vapor pressure;
  3. phase changes;
  4. molar heats of fusion and vaporization;
  5. specific heat capacity; and
  6. colligative properties.
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