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Chem Syllabus

UNIT 12: This final unit will include selected objectives from Chapter 15 (Energy and Chemical Change), Chapter 16 (Reaction Rates), Chapter 17 (Chemical Equilibrium), and Chapter 19 (Redox Reactions.)

REDOX

Selected Chapter 19 objectives:

The student can

1. Assign oxidation numbers.

2. Identify which species is oxidized or reduced.

3. Identify the oxidizing agent and reducing agent.

4. Define, explain, and use in context: catalyst, inhibitor, rate-determining step,

oxidation, reduction, activated complex, transition state, etc.

5. Explain what an oxidation-reduction reaction is (transfer of electrons.)

EQUILIBRIUM

SELECTED CHAPTER 17 OBJECTIVES: The student can

1. Describe and predict equilibrium shifts in a chemical system caused by changing conditions (LeChatelier’s Principle.)

2. Use the equilibrium constant to predict the relative amount of products and reactants in a system.

3. Write an equilibrium expression based on a balanced equation.

4. Solve problems involving equilibrium.

5. Define and explain: reversible reaction, chemical equilibrium, dynamic equilibrium, equilibrium constant, homogeneous vs. heterogeneous equilibrium, LeChatelier’s Principle, solubility product constant, common ion effect.

KINETICS

SELECTED CHAPTER 16 OBJECTIVES: The student can

1. Define, explain, and apply these concepts: kinetics, activated complex, activation energy, collision theory, reaction rate, catalyst, (heterogeneous and homogeneous), inhibitor, rate law, reaction order, rate constant, rate-determining step, reaction mechanism, endothermic vs. exothermic.

2. Write the equation for average reaction rate and calculate average reaction rate, given data.

3. List and explain factors that affect reaction rates: concentration, surface area, temperature, catalysts and inhibitors,

4. Analyze activation energy diagrams and identify all components. Identify the reaction as endothermic or exothermic.

5. Write reaction rate laws, using chemical equations.

6. Determine reaction order from experimental data.

THERMODYNAMICS

SELECTED CHAPTER 15 OBJECTIVES:

The student can

1. Define, explain, and apply these concepts: energy, potential energy, chemical potential energy, kinetic energy, Law of Conservation of Energy, temperature, heat, endothermic, exothermic, activation energy, calorie, Calorie, joule, specific heat, calorimetry, enthalpy, thermochemical equation, state function, spontaneous combustion, entropy, second law of thermodynamics, free energy.

2. Perform calculations involving specific heat of specific substances.

3. Differentiate among enthalpy (heat) of combustion, molar enthalpy (heat) of fusion, molar enthalpy (heat) of vaporization, standard enthalpy (heat) of formation (bond enthalpy), heat of reaction.

4. Correctly use and explain the use of positive and negative signs and their significance.

5. Experimentally determine the energy required for a given quantity of water to change from ice at a given temperature to steam at a given temperature.

6. Determine the heat of formation for a reaction, given heat of formation values for all compounds.

7. Use Hess's Law to determine the overall enthalpy change for a given reaction/equation.

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UNIT 11: ACIDS/BASES UNIT OBJECTIVES: The student can

1. Define and explain: titration, buret, end point, acid, base, binary acid, oxyacid, amphoteric, pH, pOH, equilibrium, monoprotic, polyprotic, strong acid/base, weak acid/base, conjugate acid/base, buffer.

2. Explain the pH scale and identify substances by pH measurement.

3. List properties of acids and bases.

4. List common acids and bases.

5. Differentiate among 3 acid/base models: Arrhenius, Bronsted-Lowry, and Lewis.

6. Define “equilibrium constant” and tell how the acid and base ionization constants are similar to it.

7. Write the ion product constant for water and use it to solve problems.

8. Write equations for neutralization reactions and predict products.

9. Determine the concentration of an acid or base by performing a titration.

UNIT 10 OBJECTIVES: Solutions (Chapter 14 in text) The student can

1. Define and explain: mixture, solution, solute, soluble, solvent, heterogeneous, suspension, thixotropic, colloid, Brownian motion, Tyndall effect, homogeneous, solubility, miscible, insoluble, immiscible, concentration, solvation, colligative properties, equilibrium, vapor pressure lowering, boiling point elevation, freezing point depression, osmotic pressure, unsaturated, saturated, and supersaturated solutions.

2. List and demonstrate factors that affect the rate of solvation (agitation, surface area, temperature, concentration.)

3. Calculate concentration: percent by mass, percent by volume, molarity, molality, and mole fraction.

4. Explain the solubility of gases in terms of temperature and pressure.

5. Solve problems using Henry’s Law.

6. Prepare solutions of specific molarity or other units using concentration formulas and the dilution equation (M1V1 = M2V2).

7. Explain the process of dissolving at the microscopic level.

8. List colligative properties and explain each.

UNIT 9 OBJECTIVES: The Gas Laws

1. Analyze the relationship between microscopic and macroscopic models of matter.

2. Analyze the nature and behavior of gaseous, liquid, and solid substances using the kinetic molecular theory. (DOK 3)

3. Use the ideal gas laws to explain the relationships between volume, temperature, pressure, and quantity in moles. (DOK 2)

· Difference between ideal and real gas

· Assumptions made about an ideal gas

4. Convert among units of pressure and temperature.

5. Recite, use, and apply these gas laws: Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, Combined GL, Dalton’s Law, Henry’s Law, Avogadro’s Law, and Ideal Gas Law. (DOK 2)

6. Calculate molar volume and number of moles of a gas using experimental data.

7. Use stoichiometry to solve problems involving gases.

8. Find the density of a gas at STP.

9. Define, explain, and use in context: ideal gas, pressure, gas particle, molar volume, Kelvin/Celsius temperature.

10. Analyze and draw particle diagrams to explain the behavior of gas particles.

Unit 8: Stoichiometry (Chapter 11)

Objectives: The student can

1. Explain the mole-mass relationship in a balanced equation and in balanced formulas of ionic or covalent compounds.

2. Correctly balance a chemical equation and use molar ratios to solve problems.

3. Given mass or moles of a reactant, calculate the mass of a product, using a balanced equation and mole ratios.

4. Define: limiting reagent/reactant, excess reagent/reactant, theoretical yield, percent yield, molar mass, molar ratio, mole, stoichiometry.

5. Calculate: molar mass, percent composition, empirical formula, molecular formula, molar ratio, theoretical yield, actual yield, percent yield.

6. Find the limiting reagent and theoretical yield, given a sample problem.

Unit 7: The Mole

Objectives: The student can

Calculate/convert among moles, grams, and number of particles for elements and compounds by using dimensional analysis and writing appropriate conversion factors.
Identify particles for elements (atoms) and compounds (molecules or formula units.)
Identify number of moles or atoms of one element in a given quantity of a compound.
Determine molar mass for elements and compounds.
Determine percent composition for a given compound and use that information to find grams or moles of one element in sample of the compound.
Given grams or percentages, determine the empirical formula of a compound. Additionally, determine the molecular formula, given the molar mass of the actual compound.
Define, explain, and use in context: empirical formula, molecular formula, molar mass, formula weight, particle, mole, Avogadro’s number, hydrate, anhydrous/anhydrate.
Determine moles of water in a hydrate using experimental data, and write the formula for a given compound as well as name the compound.
Prior knowledge: Write balanced formulas, given names of compounds. Use Periodic Table to determine charges of ions. Name compounds using rules for ionic compounds, covalent compounds, and acids. Determine if a compound is ionic or covalent.

New 6: Equations & Reactions (Chapter 9)

Unit Objectives: The student can

1. List and explain five types of chemical reactions: single displacement, double displacement, synthesis, decomposition, and combustion.

2. Define: coefficient, reactants, products, yields, spectator ions, electrolyte.

3. Write and balance chemical equations, including those based on word/paragraph format.

4. Using a Solubility Table, determine whether compounds will be solid, gas, liquid, or aqueous in chemical equations, and predict whether a reaction will occur.

5. Using an activity series, determine whether a reaction will occur or not, along with products.

6. Explain the Law of Conservation of Mass.

7. Write ionic and net ionic equations, and predict whether a reaction will occur.

8. List indicators of chemical change.

Unit 5: Ionic, Metallic, and Covalent Bonding (Chapter 7 & 8 in text)

Objectives--- The student can:

1. Define: ion, cation, anion, oxyanion, monatomic ion, polyatomic ion, ionic bond, binary ionic compound, valence electrons, oxidation number, crystal lattice, electrolyte, lattice energy, formula unit, sea of electrons, delocalized electrons, metallic bond, alloy (substitutional and interstitial) malleability, ductility, durability, covalent bond, molecule, Lewis structure, sigma bond, pi bond, endothermic, exothermic, polar, nonpolar, metal, nonmetal, hybridization, coordinate covalent bond, resonance structure, VESPR model, electronegativity, intermolecular forces, covalent network solid.

2. Name ionic and covalent compounds, given the formula; write the formula if given the name.

3. Identify the number of atoms of each element in a compound.

4. List and explain properties of ionic compounds, metals, and covalent compounds.

5. Draw Lewis structures for simple ionic and covalent compounds.

6. Determine whether compounds are polar or nonpolar.

7. Determine the molecular shapes of molecules and make models : linear, trigonal planar, tetrahedral, trigonal pyramidal, or bent. Recognize trigonal bipyramidal and octahedral shapes.

8. Determine the bond character of polar covalent bonds.

9. Identify intermolecular forces: dispersion (London) forces, induced dipole, dipole-dipole, hydrogen bond.

10. Rank compounds by polarity, melting point, boiling point, viscosity, surface tension.

Unit 4 Electrons in Atoms

Objectives: The student can---

1. Define: electromagnetic radiation, wavelength, frequency, Hertz, amplitude, crest, trough, nanometer, electromagnetic spectrum, quantum, Planck’s constant, photoelectric effect, photon, atomic emission spectrum, ground state, excited state, quantum number, Heisenberg uncertainty principle, atomic orbital, principle quantum number, electron configuration, Aufbau principle, Pauli exclusion principle, Hund’s rule, quantum mechanical model of the atom.

2. Explain the relationship between wavelength and frequency.

3. Calculate wavelength or frequency of electromagnetic waves, given the speed, c, and one other variable.

4. Given the frequency, calculate energy of a quantum or photon.

5. Compare and contrast the Bohr Model and Quantum Mechanical Model of the atom.

6. Demonstrate and explain various colors of light which are emitted by various chemicals.

7. Write electron configurations and orbital diagrams for atoms of various elements, using the aufbau principle, the Pauli exclusion principle, and Hund’s rule.

8. Draw electron dot structures for individual atoms.

9. Name and explain all four quantum numbers and how these numbers differentiate one electron from another in an atom. Assign quantum numbers to the outermost electron in an atom. Know the symbols for each QN.

10. Explain Einstein’s work with the photoelectric effect and how it contributed to our understanding of the dual nature of light.

11. Correctly fill orbitals using the Pauli Exclusion Principle, Hund’s Rule and the Aufbau Principle. Identify violations of these rules.

12. List the types of radiation on the electromagnetic spectrum and rank by wavelength, frequency, and energy.

Unit 3 Atomic Structure (Ch. 4 & 6)

Objectives: The student can---

1. Define: atom, proton, neutron, electron, ion, isotope, period, group, metal, nonmetal, halogen, metalloid, transition elements, noble gas, valence electrons, energy shells, radioactivity, radiation, nuclear reaction, radioactive decay, transmutation, nucleon, alpha radiation, alpha particle, beta radiation, beta particle, gamma ray, half-life, positron emission, electron capture.

2. Identify scientists and their contributions to atomic theory: Democritus, Aristotle, John Dalton, J.J. Thomson, Rutherford, Niels Bohr, Heisenberg, Schrodinger, Mendeleev.

3. Identify periods and group on the Periodic Table.

4. Draw Bohr models of atoms.

5. Identify number of protons, neutrons, and electrons for atoms, ions, and isotopes.

6. Calculate average atomic mass of elements.

7. Identify symbols, given element name, and identify element, given symbol.

8. List the main points of atomic theory.

9. Identify elements by family name and give general characteristics of each family.

10. Identify periodic trends on the Periodic Table.

11. Write nuclear equations for simple reactions (alpha, beta, positron emission, electron capture) and identify final element in a series.

12. Predict products and write equations for nuclear reactions: alpha decay, beta decay, positron emission, electron capture, and bombardment reactions.

13. Recite the subatomic particles of an atom, along with masses and charges.

14. Solve half-life problems using the half-life equation or the long method.

Unit 2-Matter: Classifying Matter/Properties & Changes

Goals and Objectives. The student can...

1. Define, explain, provide examples, and use in context: matter, solid, liquid, gas, vapor, sublimation, deposition, thixotopic, homogeneous, heterogeneous, pure substance, mixture, extensive, intensive, atoms, compounds, freezing/solidification, melting, evaporation/vaporization, filtration, chromatography, distillation, extraction, crystallization, decanting, solution, solute, solvent, element, allotrope, miscibility, suspension, colloid, Tyndall effect.

2. Differentiate between chemical and physical change (and properties) and provide examples of each.

3. List indicators of chemical change.

4. Interpret a phase diagram.

5. Classify substances as pure substances (element or compound) or mixtures (how many types of element/compounds in the mixture.)

6. Identify the appropriate technique used to separate mixtures (use a magnet, evaporation, filtration, etc.)

7. Identify and explain the Law of Conservation of Mass/Matter.

8. Calculate the percent by mass/percent composition.

9. Know (define, explain, and use in context) all terms from prior unit(s) and perform calculations using equations from prior unit(s) (ex: percent loss, percent recovery, density, etc.)

10. Identify laboratory equipment by name and function.

11. Identify and use significant figures correctly in simple calculations.

12. Write a comprehensive lab report using format given by the teacher and identify all components used in the scientific method.

13. Choose a type of graph to use, and construct a quality graph using a data set.

Unit 1: Analyzing Data

Objectives. The student can..

Chapters 1 & 2 Objectives: The student can---

1. Identify metric prefixes and their abbreviations.

2. Convert between metric units.

3. Calculate percent loss or percent error.

4. Identify significant figures in numbers and measurements.

5. Add, subtract, multiply, and divide using the appropriate number of sig figs.

6. Add, subtract, multiply, and divide using scientific notation.

7. Convert between units using the dimensional analysis method.

8. Use the formula for density to calculate density, mass, or volume, or to identify an unknown.

9. State safety precautions that must be taken in a science lab/classroom.

10. Recite classroom procedures and policies.

11. Identify and explain safety rules and symbols.

12. Define and explain vocabulary: science, chemistry, matter, observation, qualitative, quantitative, extensive, intensive, precision, significant figures, accuracy, mass, weight, scientific method, independent/dependent variables, control, hypothesis, constants.

13. List several branches of chemistry and what topics they are concerned with.

14. Identify lab equipment, function, and whether it can be used over a flame.

15. Use measuring instruments and report measurements to correct degree of precision.

16. Graph data appropriately.

17. Calculate density and percent change.

18. Recite steps of the scientific method and identify components.

19. Use a calculator to solve problems and report answers rounded to the correct # of sig figs.