1. Contrast observations and conclusions.

2. Apply the steps of the scientific method

3. Explain the basic safety rules for working in a chemistry lab

4. Learn the names, functions, and location of all safety equipment

5. Demonstrate safe and accurate lab techniques LAB

6. Define terms used to describe controlled experiments and lab techniques

7. Design, implement, and evaluate a controlled experiment. LAB

8. Measure volume, mass and length using the instrument’s precision LAB

9. Identify the instruments, quantities, and metric units of measurement used in chemistry.

10. Perform metric conversions

11. Relate the uncertainty in measurements to significant figures.

12. Identify the number of significant figures in a measurement

13. Use significant figures to round scientific calculations

14. Write numbers in scientific notation and do calculations using scientific notation.

15. Define and calculate density

16. Determine the identity of unknown substances using density and other physical properties. LAB

17. Solve problems using the factor label method

18. Calculate percent of error

19. Contrast precision and accuracy

20. Identify direct and inverse relationships using graphs

21. Graph data and analyze the results LAB

1. Label the sections of the periodic table that contain metals, nonmetals, and metalloids.

2. Learn element names and symbols

3. Contrast matter and energy

4. Do percent composition problems

5. Trace energy transformations and apply to the Law of Conservation of Energy.

6. Define energy and recognize energy units

7. Classify physical and chemical changes

8. Review the four states of matter

9. Discuss energy changes that accompany changes of state

10. Review physical and chemical changes.

11. Sketch energy diagrams for both endothermic and exothermic reactions.

12. Indicate on energy  diagrams the effect of a catalyst on a chemical change.

13. Classify matter as homogeneous and heterogeneous

14. Classify endothermic and exothermic changes.

15. Interpret change of state graphs.

16. State the Law of Conservation of Matter. LAB

17. Contrast elements, compounds, and mixtures. LAB

18. Combine the Law of Conservation of Energy and Mass in terms of Einstein’s equation, E = mc².

19. Perform the Fe + S --> FeS reaction. LAB

20. Determine the percent of one component in a mixture using lab data.

21. Calculate molar masses

22. Find the percent composition given a compound’s formula.

23. Determine the Freezing Point of Vanillin using lab data. LAB

1. Describe the development of atomic model through history including the work of Dalton, Thomson, Rutherford, Bohr, and quantum mechanical theory.

2. Name and describe the three major subatomic particles in an atom.

3. Determine the number of protons, electrons, and neutrons in atoms or ions.

4. Define isotopes and calculate average atomic masses based on percent abundance data.

5. Explain radioactivity in terms of nuclear stability and describe the three most common types of radiation.

6. Complete nuclear equations for transmutation reactions.

7. Use half-life values to calculate amount decayed.

1. Define the mole.

2. Use Avogadro’s number to calculate the number of particles.

3. Calculate molar mass given the chemical formula.

4. Do calculations converting moles, mass, and number of particles.

5. Determine the number of copper atoms in a penny using lab data. LAB

1. Describe the relative energies of electrons using electron configuration.

2. Apply the Aufbau diagram, Pauli exclusion principle, and Hund’s rule in writing ground state electron configurations.

3. Quantize your periodic table.

4. Write ground state electron configurations for elements.

5. Do Flame Testing Lab to understand Bohr’s model of the atom. LAB

6. Explain how electrons become excited and how light is emitted.

7. Learn the shorthand notation for electron configurations.

1. Explain similar properties within a group using electron configurations.

2. Observe the Reactions of the Alkali metals with water. LAB

3. Determine pattern of properties for Group1 and 2 Metals LAB

4. Distinguish between groups (families) and periods.

5. Identify the sublevel blocks in relation to periodic table.

6. Explain the formation of cations and anions in terms of electron transfer.

7. Discover the pattern of ion charges using Lewis Dot Structures.

8. Describe and explain the periodic and group trends for atomic radius and ionization energy.

9. Define atomic radius, ionization energy, electron affinity & electronegativity.

10. Memorize the polyatomic ions: ammonium, nitrate, hydroxide, chlorate, acetate, sulfate, carbonate, chromate, phosphate

1. Contrast ionic compounds versus covalent compounds - LAB

2. Name ionic compounds.

3. Write formulas for ionic compounds.

4. Name binary covalent compounds.

5. Write formulas for binary covalent compounds.

6. Write formulas for ionic compounds using polyatomic ions.

7. Distinguish between ionic bonding, polar covalent bonding, and nonpolar covalent bonding.

8. Define oxidation and reduction

1. Classify reaction types as synthesis, decomposition, single replacement, double replacement, or combustion. LAB

2. Balance skeleton equations.

3. Write balanced equations from word descriptions.

4. Review nomenclature rules – name and write compound formulas.

5. Calculate percent composition.

6. Define empirical and molecular formulas.

7. Recognize the patterns in the periodic table with regards to oxidation numbers. 

8. Contrast oxidation and reduction.

9. Identify the seven diatomic elements and draw the corresponding Lewis doe structure for each these molecules.

10. Predict the products formed when given reactants.

11. Use lab data to determine the percent of water in a hydrated salt. LAB

1. Define stoichiometry.

2. Interpret balanced equations using coefficients as moles.

3. Write mole ratios from a balanced equation.

4. Solve mole – mole problems.

5. Use mole ratios to solve mass-mass problems.

6. Solve mass-mass problems using lab data. LAB

7. Write balanced equation for observed chemical reactions.

8. Define limiting reactant, excess reactant and theoretical yield.

9. Determine the limiting reactant using mole-mole calculations.

10. Calculate the amount of excess reactant left unused.

11. Calculate percent yield in the synthesis of a compound and explain the meaning of this value. LAB

12. Study the impact of a scientist’s discoveries and achievements. Project 13.11.06, 13.11.08

1. State the Kinetic Theory and use it to explain the properties of the gases.
2. State and use the Ideal Gas Law.
3. Explain why real gases deviate from the gas laws
4. Describe how any two of the following variables with respect to gases (pressure, volume, temperature, and moles) relates to one another.
5. Do calculations using the combined gas law.
6. Use Dalton’s law of partial pressure to determine the pressure of a gas collected over water
7. Experimentally determine the molar volume. LAB
8. Use the Ideal Gas Law and mass data to determine molar mass. LAB

1. Define reversible reactions and chemical equilibrium.

2. State and apply Le Chatelier’s principle.

3. Predict changes in equilibrium positions using Le Chatelier’s principle. LAB

4. Calculate solution concentration in Molarity

5. Solve Problems using Molarity

6. Write equilibrium constant expressions.

7. Use equilibrium constants to solve problems.

8. Discuss all stressors that would result in either minimizing or maximizing a particular substance in an equilibrium system.

1. Describe the properties of solutions and suspensions.

2. Identify the solute and the solvent in a solution.

3. Describe the relationship between the polarity of a solvent/solute mixture and solubility.

4. Use the solubility product constant K_sp to determine relative solubility. 

5. Describe the effects of temperature and pressure on solubility.

6. Explain the dissolving mechanism.

7. Use the enthalpy of solution to determine how energy changes affect the solubility of a substance. 

8. Interpret solubility curves and compare unsaturated, saturated and supersaturated solutions. LAB

9. Calculate the molarity of solutions; do any necessary calculations needed to prepare a solution of a particular molarity.

10. Solve solution stoichiometry problems using volumes and concentrations.

12.11.34, 12.11.63, 13.11.09

1. Distinguish between kinetic energy (KE) and potential energy (PE.)

2. Convert between energy units (J, cal, Cal, kJ, kcal.)

3. Define and identify endothermic and exothermic reactions.

4. Identify endothermic and exothermic reactions from PE diagrams.

5. Solve calorimetry problems.

6. Define specific heat.

7. Calculate heat lost or gained during a phase change using heats of phase changes.

8. Determine the identity of an unknown metal using calorimetry - LAB

1. Describe the properties of acids and bases.

2. Understand Arrhenius, Bronsted-Lowery, and Lewis acid/base theories.

3. Identify a substance as an acid or base using the pH of the solution.

4. Calculate pH, pOH, [H⁺], [OH^-]

5. Compare acid strengths using Ka values; compare base strengths using Kb values.

6. Write balanced equations for acid/base reactions: LAB

7. Discuss the environmental effects of acid anhydrides in the atmosphere. 

8. Explain buffer solution equilibria and identify the buffer region in a titration curve.  .

9. Calculate unknown concentrations using neutralization reactions and titration data. LAB