Grade: 10-12
Credit: One
Prerequisite: One laboratory science course

Chemistry I is a laboratory-oriented course designed to enable all students to acquire an understanding of how chemical theory is developed and how a chemist thinks and works. Students investigate the composition, properties and reactions of matter. The approach is inductive and mathematical, as well as conceptual.

Laboratory experiments and the use of technology are integral parts of the course. Many of the experiments use computers, CBL’s (calculator based laboratory), and probeware for the collection and analysis of data. Simulation software and videodisks are also used. Students are given the opportunity to acquire, manipulate and present data using these technologies.

Indicators are notated with the Virginia Standards of Learning for Chemistry. All Virginia Standards of Learning for Chemistry are included in this course. The basic chemical principles are applied to organic chemistry, biochemistry, nuclear chemistry, and environmental chemistry.

Benchmarks and indicators are organized by the following strands:

1. Inquiry in Chemistry
2. The Structure of the Atom
3. Structures and Properties of Matter
4. Interactions of Matter

Benchmark
Students will recognize the contributions made by scientists throughout culture, and explain how scientific knowledge builds and changes over time. Students will participate in the scientific process.

Indicators: (SOL CH.1)

1. Consider how the world would be different without a specific discovery or advancement.
2. Participate both as an individual and as a team member on scientific investigations.
3. Create an experimental design diagram that identifies the various levels of the independent variable, dependent variable, the control, the constants, and the number of trials.
4. Organize a set of data in a logical and coherent manner using appropriate tables, diagrams, charts, or graphs.
5. Construct graphs and use the graph to determine trends and mathematical relationships.
6. Write a conclusion for a scientific investigation that includes a statement of results, the relationship of the results to the hypothesis, an explanation and a defense of the results, and an analysis of possible sources of error.
7. Follow appropriate laboratory techniques and use equipment and chemicals in a safe manner.

Benchmark
Students will explain the makeup of matter in terms of particles and forces.

Indicators: (SOL CH.2)

1. Identify the three basic particles of matter and their charges, relative masses, and location.
2. Describe the development of our concept of the atom through Dalton, Thomson, Rutherford, Bohr to our modern concept.
3. Define the terms: atomic number, mass number, and isotope.
4. Interpret the isotopic notation and use isotopic abundance data to calculate the average mass of the elements.
5. Write and balance nuclear equations using appropriate notation for nuclear particles and emissions.
6. Explain the concept of half-life and solve half-life problems.
7. Write electron configurations and orbital notations for any atom or ion.
8. Differentiate between core electrons and valence electrons.
9. Classify elements as metals, nonmetals, or metalloids based on their position on the periodic table.
10. Use the periodic table to predict and explain physical and chemical properties (including atomic size, electronegativity, shielding effect) based on the position of the element on the periodic table. Reference should be made to the period (series) and/or group (family) that the element is in on the periodic table.

Benchmark:
Students will understand that the structure and properties of matter are dependent upon the structure and properties of the atoms and compounds that make up matter. This is dependent upon the intramolecular and intermolecular bonding that takes place.

Indicators: (SOL CH.2, CH.3, CH.4, CH.5)

1. Differentiate between ionic and covalent bonding.
2. Classify matter in terms of elements, compounds, and mixtures.
3. Name and write formulas for covalent and ionic compounds.
4. Differentiate between and determine molecular and empirical formulas.
5. Draw Lewis structures for compounds.
6. Predict whether a compound is polar or nonpolar and use polarity to account for properties of the compound.
7. Use a solubility curve to determine the solubility of a solute at a given temperature and describe the effect of temperature on solubility for that substance.
8. Relate solution concentrations to colligative properties.
9. Describe with words and mathematical equations the interrelationships of temperature, volume and pressure.
10. Calculate the partial pressure and vapor pressure of gases in a mixture.
11. Interpret a diagram (heating curve) in terms of kinetic energy and potential energy.
12. Calculate the enthalpy change associated with a phase change, using molar heats of fusion and vaporization.
13. Use calorimetry to determine the specific heat capacity of a substance.

Benchmark:
Students will understand that chemical reactions happen all around us. Students will be able to classify the various types of chemical reactions and quantify aspects of the reaction process.

Indicators: (SOL CH.3, CH.4, CH.5)

1. Classify a reaction as synthesis, decomposition, single replacement, double replacement, neutralization, oxidation-reduction, or dissociation /ionization.
2. Compare exothermic and endothermic reactions in terms of bond making, bond breaking, and potential energy changes.
3. Differentiate between oxidation and reduction and assign oxidation number for each element in a compound.
4. Use collision theory to explain how the rate of a reaction is influenced by the nature of the reactants (activation energy), temperature, concentration, surface area, and catalysis.
5. Identify and interpret the components of a potential energy diagram, and explain how a catalyst affects it.
6. Describe chemical equilibria.
7. Define the term mole and Avogadro’s number.
8. Use the mole, molar mass, and Avogadro’s number in problems that require the calculation of the number of grams, molecules, atoms, of moles of a given substance.
9. Calculate solution concentrations.
10. Balance a chemical equation and interpret the equation in terms of moles, representative particles, masses and volumes of gases.
11. Determine the reactivity of a metal compared to other metals.
12. Determine the enthalpy change for various reactions using calorimetry and/or Hess’s Law.
13. Describe acid/base solutions be writing the appropriate dissociation (ionization) equations and calculate the pH and/or pOH of the solution.
14. Explain how the terms strong and weak are used to describe acids, bases, and other electrolytes.
15. Classify a solution as acidic, basic, or neutral, based on the pH of the solution.

All students will take the Virginia Standards of Learning Test for Chemistry.

Last update: August 21, 1998