Download Common Curriculum Map Discipline: Science Course: Chemistry

Common Curriculum Map
Discipline: Science
Course: Chemistry
August/September:
Standard:
Chapters 1, 2 and 3
11.A.5a Formulate hypotheses referencing prior research and knowledge.
11.A.5b Design procedures to test the selected hypotheses.
11.A.4c Collect, organize and analyze data accurately and precisely.
12.C.4a Use kinetic theory, wave theory, quantum theory and the laws of thermo-dynamics to explain
energy transformations.
12.C.4b Analyze and explain the atomic and nuclear structure of matter.
13.A.4b Assess the validity of scientific data by analyzing the results, sample set, sample size, similar
previous experimentation, possible misrepresentation of data presented and potential sources of error.
Essential Questions:
Chapter 1:
-What is Chemistry?
-What is the Scientific Method?
-How do you practice safety in the laboratory?
-What units are used in science for measurement?
-What are metric prefixes and how are they used?
-What causes uncertainty in measurements?
-What is the difference between accuracy and precision?
-What information is needed to calculate the density of an object?
-How can density be used to determine the mass or volume of an object?
-How do you convert from one scientific unit to another?
Chapter 2:
- What is energy and how is energy measured?
-What is the law of conservation of energy?
-How is temperature measured?
-What is absolute zero?
- What is matter?
-What is the law of conservation of matter?
What is an element?
-What is the difference between an element and a compound?
-What are the types of mixtures?
Chapter 3:
- What are atoms?
- What are the postulates of Dalton's atomic theory?
- How is atomic structure related to electricity?
- What did cathode rays indicate about atoms?
- What did Rutherford conclude from his alpha scattering experiment?
- What are the names and properties of the three subatomic particles?
- How can you determine the number of protons, neutrons, and electrons in an atom or ion?
- What is an isotope?
- What is atomic mass?
- What changes accompany nuclear reactions?
- What is radioactivity?
Content:
Chapter 1:
-Steps of the Scientific Method
-Laboratory safety rules.
-Lab on making observations.
- Differences between hypotheses, laws, and theories
- Common SI units used in chemistry
-Lab on measurement.
- Uncertainty in measurement
- Unit conversions using dimensional analysis
Chapter 2:
- Forms of energy (Kinetic, Potential, Radiant)
- Units for measuring energy (calories, joules, Calories)
- Law of Conservation of Energy
- Converting from one unit to another using dimensional analysis
- The Kelvin temperature scale
- Matter: States of matter, conservation of matter
- Differences between chemical & physical changes and chemical and physical properties
- Differences between elements, compounds, and mixtures
- Homogeneous and heterogeneous mixtures
- Three methods to separate mixtures (filtration, distillation, chromatography)
Chapter 3:
- Definition of an atom
- Three parts of an atom, and their charges and properties (proton, neutron, electron)
- Atomic number and mass number
- Definition of an ion and how to write it symbolically
- Definition of an isotope and how to write it symbolically
- Writing a complete chemical symbol based on the number of protons, neutrons, and electrons
- Calculating a weighted average atomic mass
Skills:
Chapter 1:
1. Formulate a hypothesis using available information.
2. Design an experiment to test their hypothesis.
3. Follow instructions while in the laboratory.
4. Analyze the results of an experiment and form a conclusion.
5. Identify possible sources of error.
6. Distinguish between a law and a theory.
7. Explain how a theory may change over time with new information.
8. Identify SI units commonly used in chemistry.
9. Indicate the degree of uncertainty in a measurement.
10. Identify the number of significant digits in a measurement.
11. Perform calculations and round the answers to the appropriate number of significant digits.
12. Convert measurements from one unit to another.
Chapter 2:
1. List the 3 forms of energy.
2. Differentiate between kinetic and potential energy.
3. Calculate the amount of energy needed to perform a given process.
4. Explain the law of conservation of energy.
5. List the two main sources of energy used in the United States.
6. Use the relationship between Celsius and Kelvin to convert a Celsius temperature to a Kelvin
temperature.
7. Discuss the meaning of absolute zero.
8. Follow laboratory safety rules.
9. Accurately measure chemicals using a graduated cylinder.
10. Collect and record data.
11. Analyze data to draw conclusions.
12. Explain that in any reaction, mass is neither created nor destroyed.
13. Define matter.
14. List and describe the 3 main states of matter.
15. Distinguish between chemical and physical changes.
16. Explain the law of conservation of matter/mass.
17. Define a compound, an element, and a mixture.
18. Use their knowledge of elements, compounds, and mixtures to classify a given substance as a
compound, element, or mixture.
19. Distinguish between heterogeneous mixtures and homogeneous mixtures.
20. Briefly discuss three ways to separate the components of a mixture.
Chapter 3:
1. Define atom.
2. List the 4 postulates of the atomic theory of matter.
3. List the three main parts of an atom, along with each part’s electrical charge.
4. Discuss the relative size and mass of protons, electrons, and neutrons.
5. Use the periodic table to determine the atomic number of a given element.
6. Explain what an atomic number means.
7. Define an ion and accurately represent an ion symbolically.
8. Define an isotope.
9. Write a complete chemical symbol using available information.
10. Calculate a weighted average atomic mass.
Assessment:
Chapter 1:
- Uncertainty & Significant Digits Worksheet
- Unit Conversions Practice
- Chapter 1 Quiz
Chapter 2:
- Worksheets 2.1 & 2.2
- Conservation of Mass Lab
- Mixture Separation Lab
- ChemThink Particulate Nature of Matter Question Set
- Chapter 2 Test
Chapter 3:
- ChemThink Atomic Structure, Ions, and Isotopes Question Sets
- Various in-class exercises
- Atomic Mass of Candium Lab
October:
Standard:
Chapter 3
13.A.4c Describe how scientific knowledge, explanations and technological designs may change with
new information over time (e.g., the understanding of DNA, the design of computers)
Chapter 4:
11.A.4c Collect, organize and analyze data accurately and precisely.
12.C.4a Use kinetic theory, wave theory, quantum theory and the laws of thermo-dynamics to explain
energy transformations.
12.C.4b Analyze and explain the atomic and nuclear structure of matter.
CRISS: KWL
Chapter 5:
11.A.5a Formulate hypotheses referencing prior research and knowledge.
11.A.4c Collect, organize and analyze data accurately and precisely.
12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in relation
to their physical and/or chemical structures.
CRISS: KWL
Essential Questions:
Chapter 3:
- What is an atom and why is it important?
- How can we accurately represent an atom's composition?
Chapter 4:
- What are the four characteristics of an electromagnetic wave?
- What are the major regions of the electromagnetic spectrum?
- What is meant by energy quantization?
- How is the energy of radiation related to its wavelength?
- How does the idea of photons of light explain the photoelectric effect?
- What makes an atom give off light?
-What is a line spectrum?
- How does the Bohr model explain the line spectrum of hydrogen?
- What is an atomic orbital?
- How do the s, p, d and f orbitals compare in size, shape and energy?
- How are the electrons arranged within an atom?
Chapter 5:
- How is the periodic table arranged?
- What trends are visible in the periodic table and why?
- What is the periodic law?
- Who were the important contributors to the modern periodic table?
Content:
Chapter 3:
- Practice problems to review the chapter
Chapter 4:
- Quantum nature of matter
- Heisenberg's uncertainty principle
- Elecromagnetic radiation
- Bohr's model of an atom
- Ground and excited states
- Electron energy levels and orbital shapes
- Electron configurations
- The diagonal rule
- Orbital diagrams
Chapter 5:
- Scientists who contributed to the creation of the periodic table
- The periodic law
- Families/groups and periods on the periodic table
- Valence electrons
- Abbreviated electron configurations
- Periodic trends (atomic radius, ionic size, ionization energy, successive ionization energies)
Skills:
Chapter 3:
1. Define atom.
2. List the 4 postulates of the atomic theory of matter.
3. List the three main parts of an atom, along with each part’s electrical charge.
4. Discuss the relative size and mass of protons, electrons, and neutrons.
5. Use the periodic table to determine the atomic number of a given element.
6. Explain what an atomic number means.
7. Define an ion and accurately represent an ion symbolically.
8. Define an isotope.
9. Write a complete chemical symbol using available information.
10. Calculate a weighted average atomic mass.
Chapter 4:
1. Explain that objects emit or absorb energy only in certain fixed amounts called quanta.
2. Discuss how light behaves as both a particle and a wave.
3. Define the photoelectric effect and explain why it happens.
4. Arrange various types of electromagnetic radiation (X-rays, UV light, visible light, infrared light, radio
waves) in order of increasing energy.
5. Explain how and why atoms give off light.
6. Explain why each element has a unique line emission spectra.
7. Explain that an electron is never found in the nucleus of an atom.
8. Draw Bohr’s model of an atom.
9. Distinguish between the ground state and excited states.
10. Explain that energy level are quantized, and what quantized means.
11. Discuss Heisenberg’s uncertainty principle and why it applies to electrons.
12. Define an atomic orbital and explain how one is drawn.
13. Differentiate between principal energy levels (1, 2, 3, …) & energy sublevels (s, p, d, …).
14. Draw s and p electron orbitals.
15. List the two types of electron spin, and what types of spins will pair together.
16. Fill in an electron orbital diagram for a given element.
17. Use the diagonal rule to write an electron configuration for a given element.
18. Place electron orbitals in order from lowest to highest energy.
Chapter 5:
1. Find patterns and organize a series of objects into a table according to those patterns.
2. Use their organized table to predict the properties of a new object placed in the table.
3. List three people who contributed to the creation of the periodic table.
4. State the periodic law.
5. Differentiate between groups and periods on the periodic table.
6. List the family names of groups 1A, 2A, 7A, & 8A.
7. Explain how to refer to a group with no common family name.
8. Define a valence electron.
9. Draw an atom, showing the locations of all energy levels and electrons.
10. Explain the importance of valence electrons.
11. Use the periodic table to determine the number of valence electrons a given element has.
12. Write an abbreviated electron configuration for a given element.
13. Define ionization energy, successive ionization energies, electron affinity, and electronegativity.
14. List the trends in atomic radius, ionization energy, and electronegativity as you move down a group in
the periodic table.
15. List the trends in atomic radius, ionization energy, and electronegativity as you move across a period
in the periodic table.
16. Explain why the various trends exist.
17. Use their knowledge about family similarities to place elements into the periodic table.
Assessment:
Chapter 3:
- Practice Problems
- Review Jeopardy
- Chapter 3 Test
Chapter 4:
- Flame Test Lab
- Electron Configurations Worksheet
November:
Standard:
Chapter 5:
Ž 11.A.5a Formulate hypotheses referencing prior research and knowledge.
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 11.A.5d Apply statistical methods to make predictions and to test the accuracy of results.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Ž 13.A.4b Assess the validity of scientific data by analyzing the results, sample set, sample size, similar
previous experimentation, possible misrepresentation of data presented and potential sources of error.
Chapter 7:
Ž 12.C.5a Analyze reactions (e.g., nuclear reactions, burning of fuel, decomposition of waste) in natural
and man-made energy systems.
Ž 12.C.4b Analyze and explain the atomic and nuclear structure of matter.
CRISS:
- KWL
Essential Questions:
Chapter 5:
- Why do the elements in a group have similar properties?
- How is the periodic table arranged?
- What are the four blocks of the periodic table?
- What trends are visible in the periodic table and why?
Chapter 7:
- What is an ionic bond?
- What is the octet rule?
- How can we explain the reactivity of certain elements?
- How are compounds and molecules formed?
- What is a covalent bond?
- What is the difference between a polar and a nonpolar covalent bond?
- How do chemists name compounds?
- How are ionic, compounds, molecular compounds, and acids named?
Content:
Chapter 5:
- Applying knowledge of periodic trends to complete a series of activities.
- Electron affinity and electronegativity.
Chapter 6:
- Properties of various elements.
Chapter 7:
- Ionic Bonds
- Cations vs Anions
- The octet rule
- Lewis Dot structures
- Lewis dot diagrams to show the creation of molecules
- Monatomic vs polyatmoic ions
- The criss-cross method to determine chemical formulas
- Covalent bonds (single, double, and triple)
- Polar vs nonpolar covalent bonds
- Using electronegativities to determine the type of bond (ionic, polar covalent, or nonpolar covalent)
- Naming ionic and covalent compounds
Skills:
Chapter 5:
18. Accurately measure mass and volume or an element sample using an electronic balance and a
graduated cylinder.
19. Create a line graph to represent data.
20. Interpret the graph to draw conclusions about elements that were not measured.
21. Identify sources of error in their experiment.
22. Use their knowledge of trends in atomic radius to organize a collection of nuts, bolts, and screws into a
table.
23. Use their knowledge of the periodic table and data collected to organize a group of elements from
another planet into a table.
24. Use their table to make predictions about the properties of undiscovered elements.
Chapter 6:
1. Draw important detail from the textbook to create organized notes.
Chapter 7:
1. Explain what an ionic bond is.
2. Differentiate between cations and anions.
3. List some common properties of ionic compounds.
4. State the octet rule.
5. Apply the octet rule to determine the type of ion each element is most likely to form.
6. Draw a Lewis Dot structure for a given atom.
7. Draw a Lewis Dot diagram to show the exchange of electrons between atoms forming an ionic bond.
8. Differentiate between monatomic and polyatomic ions.
9. Use the crisscross method to write an empirical formula for a given ionic compound.
10. Differentiate between ionic and covalent bonds.
11. Differentiate between single, double, and triple covalent bonds.
12. Write a structural formula for a given molecule, indicating unshared electron pairs.
13. Explain the difference between a polar and nonpolar covalent bond.
14. Use proper notation to indicate the presence of a polar bond.
15. Use electronegativity values to determine whether two atoms will form a nonpolar covalent, polar
covalent, or ionic bond.
16. Correctly name an ionic or covalent compound.
Assessment:
Chapter 5:
- Family Density Lab sheet
- Periodic Trends Worksheet
- Chapter 5 Test
Chapter 6:
- Chapter 6 Quiz
December:
Standard:
Chapter 7:
Ž 12.C.5a Analyze reactions (e.g., nuclear reactions, burning of fuel, decomposition of waste) in natural
and man-made energy systems.
Ž 12.C.4b Analyze and explain the atomic and nuclear structure of matter.
Chapter 9:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5a Analyze reactions (e.g., nuclear reactions, burning of fuel, decomposition of waste) in natural
and man-made energy systems.
Ž 12.C.4b Analyze and explain the atomic and nuclear structure of matter.
Essential Questions:
Chapter 7:
- How can we explain the reactivity of certain elements?
- How are compounds and molecules formed?
- Chapter 9
- What are chemical reactions?
- Why do they occur?
- How can a chemical reaction be represented?
- How does a balanced chemical equation demonstrate the law of conservation of matter?
- What are the four general types of chemical reactions?
- What characteristics identify each type of chemical reaction?
Content:
Chapter 7:
- Ionic Bonds
- Cations vs Anions
- The octet rule
- Lewis Dot structures
- Lewis dot diagrams to show the creation of molecules
- Monatomic vs polyatmoic ions
- The criss-cross method to determine chemical formulas
- Covalent bonds (single, double, and triple)
- Polar vs nonpolar covalent bonds
- Using electronegativities to determine the type of bond (ionic, polar covalent, or nonpolar covalent)
- Naming ionic and covalent compounds
Chapter 9
- Definition and examples of chemical reactions
- Vocabulary of reactions - reactants and products
- Reasons substances react with each other.
- Ways to write equations - word equations vs. symbols
- Balancing chemical equations
- Four classifications of chemical reactions
Synthesis
Decomposition
Single replacement
Double replacement
Skills:
Chapter 7:
1. Explain what an ionic bond is.
2. Differentiate between cations and anions.
3. List some common properties of ionic compounds.
4. State the octet rule.
5. Apply the octet rule to determine the type of ion each element is most likely to form.
6. Draw a Lewis Dot structure for a given atom.
7. Draw a Lewis Dot diagram to show the exchange of electrons between atoms forming an ionic bond.
8. Differentiate between monatomic and polyatomic ions.
9. Use the crisscross method to write an empirical formula for a given ionic compound.
10. Differentiate between ionic and covalent bonds.
11. Differentiate between single, double, and triple covalent bonds.
12. Write a structural formula for a given molecule, indicating unshared electron pairs.
13. Explain the difference between a polar and nonpolar covalent bond.
14. Use proper notation to indicate the presence of a polar bond.
15. Use electronegativity values to determine whether two atoms will form a nonpolar covalent, polar
covalent, or ionic bond.
16. Correctly name an ionic or covalent compound.
Chapter 9:
1. Students will be able to describe the characteristics of a chemical reaction
2. Students will be able to write balanced equations
3. Classify chemical reactions into the major types.
Assessment:
Chapter 7:
- Chapter 7 Test
Chapter 9
- Chemical equation worksheet
- Chapter 9 review / quiz
January:
Standard:
Chapter 9:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5a Analyze reactions (e.g., nuclear reactions, burning of fuel, decomposition of waste) in natural
and man-made energy systems.
Ž 12.C.4b Analyze and explain the atomic and nuclear structure of matter.
Chapter 10:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Essential Questions:
Chapter 9:
- What happens during a chemical reaction?
- How much of each material is consumed or produced during a chemical reaction?
Chapter 10:
- How do scientists weigh atoms using a useful unit--the gram?
- How can we convert between different ways of measuring chemical substances?
Content:
Chapter 9:
- Chemical Reactions
- Definitions: reactant and product
- Balancing Equations
- 4 types of chemical reactions (composition, decomposition, single-replacement, and double-replacement)
Chapter 10:
- Atomic and formula mass
- The Mole and Avogadro's number
- Molar mass
- Mole conversions (mass<-->moles, particles<-->moles, and volume<-->moles)
Skills:
Chapter 9:
1. Differentiate between a reactant and a product in a chemical equation.
2. Define a chemical reaction.
3. Balance chemical equations.
4. List and describe the 4 simple types of chemical reactions.
5. Examine an equation and determine what type of chemical reaction it represents.
6. Accurately record observations.
Chapter 10:
1. Explain what a mole is.
2. State Avogadro’s number.
3. Calculate formula and molar masses.
4. Accurately record and interpret data.
5. Calculate the number of atoms present in a given number of moles.
6. Use the relationships between masses, moles, particles and volumes to convert between masses, moles,
particles, and volumes.
7. State the molar volume of gases at STP.
8. Convert between mass and moles.
9. Calculate the number of molecules present in a given number of moles.
10. Design an experiment to measure the number of chalk atoms used to write their name on a chalkboard.
Assessment:
Chapter 9:
- 9-1 Apply worksheet
- Balancing Equations worksheet
- Chemical Reaction Types worksheet
- Chemical Reactions Lab worksheet
- Chapter 9 Practice Problems
- Chapter 9 Quiz
February:
Standard:
Chapter 10:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Ž 13.A.4b Assess the validity of scientific data by analyzing the results, sample set, sample size, similar
previous experimentation, possible misrepresentation of data presented and potential sources of error.
Chapter 11:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Ž 13.A.4b Assess the validity of scientific data by analyzing the results, sample set, sample size, similar
previous experimentation, possible misrepresentation of data presented and potential sources of error.
Essential Questions:
Chapter 10:
- How can we accurately represent the composition of a substance?
- What is a mole and how does it relate to Avogadro's number?
- What is molar mass?
-How can you convert among the numbers of moles, the number of particles and the mass of a sample?
-What is the relationship between 1 mole of a gas and its volume at standard temperature and pressure?
-What is percentage composition of a substance?
-How are empirical formulas calculated?
-What is a molecular formula and how is it found?
Chapter 11:
- How can we used balanced chemical equations to determine the amounts of reactants used and products
produced in a chemical reaction?
- What is stoichiometry?
- How are molar relationships represented in a balanced chemical equation?
- What are the main types of stoichiometry problems?
- What determines the amount of products formed in a chemical reaction?
- How is the percent yield of a chemical reaction determined?
Content:
Chapter 10:
- Empirical formulas
- Molecular formulas
- Percent composition
Chapter 11:
- Stoichiometry
- Mole-Mole, Mass-Mass, Mass-Volume, & Volume-Volume conversions
- Limiting reactants
Skills:
Chapter 10:
1. Calculate percentage composition.
2. Define empirical formula and molecular formula.
3. Use percentage compositions to determine empirical formulas.
4. Use percentage compositions and molar masses to determine molecular formulas.
5. Accurately record and interpret data.
6. Analyze lab results to determine possible sources of error.
Chapter 11:
1. Accurately record and interpret data.
2. Define stoichiometry.
3. Perform mole-mole conversions.
4. Perform mass-mass, mass-volume, and volume-volume conversions.
5. Perform mass-mass calculations using lab data.
6. Analyze lab results to determine possible sources of error.
7. Explain what a limiting reactant is.
8. Determine the limiting reactant in a reaction when given a balanced chemical equation and the mass of
the reactants.
Assessment:
Chapter 10:
- Empirical & Molecular Formulas worksheet
- Washer Percent Composition lab worksheet
- Percent composition of gum lab worksheet
- Chapter 10 practice problems
- Chapter 10 test
Chapter 11:
- Mole-Mole Problems
- Stoichiometric Problems
- Atomin Accounting worksheet
- Mole & Mass Relationships lab worksheet
- Limiting Reactants
March:
Standard:
Chapter 11:
Ž 11.A.4c Collect, organize and analyze data accurately and precisely.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Chapter 12/14:
12.C.4a Use kinetic theory, wave theory, quantum theory and the laws of thermo-dynamics to explain
energy transformations.
Ž 12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in
relation to their physical and/or chemical structures.
Essential Questions:
Chapter 11:
- How can we used balanced chemical equations to determine the amounts of reactants used and products
produced in a chemical reaction?
- What is stoichiometry?
- How are molar relationships represented in a balanced chemical equation?
- What are the main types of stoichiometry problems?
- What determines the amount of products formed in a chemical reaction?
- How is the percent yield of a chemical reaction determined?
Chapter 12/14:
- What is heat?
- What happens when matter changes states?
- What are exothermic and ndothermic reactions?
- What is the significance of the enthalpy change of a reaction?
-How is a calorimeter used to determine enthalpy changes of reactions?
- How does the kinetic molecular theory account for the physical properties of the condensed states?
- What are the 3 types of intermolecular forces of attraction?
- Why do liquids have viscosity and surface tension?
- What are some of the unique properties of water?
- How are the properties of solids related to their bonding?
- How do crystalline solids differ from amorphous solids?
- What is involved in a change of state?
- What information is provided by heating curves and phase diagrams?
Content:
Chapter 11:
- Percent Yield
Chapter 12/14:
- Heat
- Exothermic and endothermic reactions
- Calorimetry
- Phase changes (evaporation/condensation, freezing/melting)
- Heating Curves
- Intermolecular forces (dispersion forces, dipole-dipole forces, hydorgen bonds)
- Properties of liquids (viscosity & surface tension)
Skills:
Chapter 11:
1. Explain the differences between expected yield and actual yield.
2. Calculate percent yield.
Chapter 12/14
1. Define heat.
2. Explain the difference between exothermic and endothermic reactions.
3. Collect and display data by creating a graph.
4. Interpret a graph to draw conclusions.
5. Define heat capacity and specific heat.
6. Use data collected from a calorimeter to determine the amount of heat released or absorbed.
7. Construct and use a calorimeter to calculate the number of Calories in a piece of snack food.
8. Explain why liquids evaporate.
9. Explain what happens at the boiling point.
10. Interpret the heating curve for water.
11. List and describe the three types of intermolecular forces.
12. Define viscosity and surface tension.
13. Use intermolecular forces to explain liquid properties such as viscosity, surface tension, and boiling
points.
14. List and explain the reason behind water’s unique properties.
15. Define heat of vaporization and heat of fusion.
16. Calculate heat exchanges as water moves between states of matter.
Assessment:
Chapter 11:
- Chapter 11 Quiz
- Percent Yield Worksheet
- Chapter 11 Test
Chapter 12/14:
- Hot Pack Lab
- Calorimetry Problems
- Chapter 12 and 14 test
- Food Calorimetry Lab
- Melting Ice Lab
- Boiling Point Lab
- Chapter 12/14 Quiz Review
- Chapter 12/14 Quiz
- Intermolecular Forces Worksheet
- Surface Tension lab
- Chapter 12/14 Test Review
- Chapter 12/14 Test
April:
Standard:
Chapter 13:
12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in relation
to their physical and/or chemical structures.
11.A.4b Conduct controlled experiments or simulations to test hypotheses.
Chapter 15:
12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in relation
to their physical and/or chemical structures.
Essential Questions:
Chapter 13:
- How can we explain the behavior of gases?
- What is the kinetic molecular theory or gases?
- What are some distinctive properties of gases?
-What are the 4 gas variables and how are they expressed?
- How is gas pressure measured?
- How do the gas laws relate the variables P, V, n and T?
- What is the ideal gas equation and how is it applied?
- What is a real gas?
- Upon which variables does gas density depend?
Chapter 15:
- What is a solution, and what factors affect its formation?
- How is the concentration of a solution described?
- How does a saturated solution differ from a supersaturated solution?
- What is solubility?
- What factors affect the rate of dissolving?
- What are four colligative properties of solutions?
Content:
Chapter 13:
- Properties of gases
- The four variables that fully describe a gas (temperature, pressure, volume, and amount)
- Base units of volume, temperature, and pressure
- How barometers and monometers work
- The combined gas law
- Dalton's law of partial pressures
- The ideal gas law
- Gases have lifting power
Chapter 15:
- Properties of solutions
- Definitions: solute, solvent, soluble, insoluble, electrolyte, aqueous
- Three types of solutions (solid, liquid, gaseous)
- Special type of liquid solution: aqueous
- Solution concentration measurements (molarity, molality, and mole fractions)
- Unsaturated, saturated, and supersaturated solutions
Skills:
Chapter 13:
1. List the six properties of gases.
2. Explain, using the kinetic-molecular theory of gases, why gases exhibit each of the 6 properties.
3. List the four variables used to fully describe a gas, along with their base units.
4. Convert between different units of pressure.
5. Explain how a barometer works.
6. Interpret changes in a barometer to predict weather changes.
7. Calculate pressures from manometer readings.
8. Create a working barometer.
9. Use what they know about pressure to explain various phenomena.
10. State the combined gas law.
11. Use the combined gas law to solve problems.
12. Draw generic graphs to show the relationships between pressure-volume, pressure-temperature,
pressure-amount, and volume-temperature.
13. Explain and use the Law of Partial Pressures.
14. Build a Cartesian diver and explain how/why it works.
15. Use the gas laws to explain various surprising phenomena.
16. State and use the ideal gas law.
17. Explain why gases have lifting power.
Chapter 15:
1. List the three properties of solutions.
2. Define solute, solvent, soluble, insoluble, aqueous, electrolyte.
3. Differentiate between solid, gaseous, and liquid solutions.
4. Explain the difference between liquid and aqueous solutions.
5. Calculate molarity, molality, and mole fractions.
6. Explain what saturated and supersaturated solutions are.
7. Create a supersaturated solution.
Assessment:
Chapter 13:
- Create a barometer lab
- Measuring Gases worksheet
- ChemThink Behavior of Gases Tutorial and Question Set
- Gas Law Thinking Skills worksheet
- 13-3 Practice Problems
- Build a Cartesian Diver lab
- 13-4 Practice Problems
- Ch. 13 Review Problems
- Ch. 13 Test
Chapter 15
- Nature of Solutions worksheet
- Supersaturation lab
- Molarity, Molality, and Mole Fractions worksheet
May/June:
Standard:
Chapter 15:
11.A.5a Formulate hypotheses referencing prior research and knowledge.
11.A.4b Conduct controlled experiments or simulations to test hypotheses.
12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in relation
to their physical and/or chemical structures.
Chapter 18:
11.A.5a Formulate hypotheses referencing prior research and knowledge.
12.C.5b Analyze the properties of materials (e.g., mass, boiling point, melting point, hardness) in relation
to their physical and/or chemical structures.
Essential Questions:
Chaper 15:
- What is a solution, and what factors affect its formation?
- How is the concentration of a solution described?
- How does a saturated solution differ from a supersaturated solution?
- What is solubility?
- What factors affect the rate of dissolving?
- What are four colligative properties of solutions?
Chapter 18:
- What is the difference between acids and bases?
- What are common properties of acids and bases?
Content:
Chapter 15:
- Solution formation & solubility
- Factors influencing solubility (nature of solute and solvent, temperature, & pressure)
- Factors affecting the rate of dissolving (surface area, stirring, dissolving)
- Colligative properties (vapor pressure reduction, boiling point elevation, and freezing point depression)
- Determining molar mass using colligative properties.
Chapter 18:
- Properties of acids and bases
- Arrhenius definition of acids and bases
- Bronsted-Lowry definition of acids and bases
- The hydronium ion
- Strength of acids and bases
Skills:
Chapter 15:
1. Define solubility.
2. List and describe the three factors influencing solubility.
3. List and describe three things that affect the rate of dissolving.
4. Use knowledge of molarity and molality to prepare solutions of given concentrations.
5. Explain what a colligative property is.
6. Explain why the addition of a solute will result in boiling point elevation of the solution.
7. Predict a solute’s affect on boiling or freezing points of the solution.
8. Use the molal boiling point constant to calculate boiling point elevations.
9. Use the molal freezing point constant to calculate freezing point depressions.
10. Use colligative properties to determine the molar mass of an unknown compound.
Chapter 18:
1. List and describe 6 properties of acids and bases.
2. Differentiate between the Arrhenius and Bronsted-Lowry definitions of acids and bases.
3. Explain why the Bronsted-Lowry definition is broader.
4. Explain what ion is produced when an acid dissociates in water.
5. Use simple tests to determine whether and unknown substance is an acid or a base.
6. Explain what determines the strength of an acid.
7. Explain what determines the strength of a base.
Assessment:
Chapter 15:
- Solubility & Dissolving
- Concentration Lab
- Colligative Properties
- Freezing Point Depression Lab
- Determining Molar Mass
- Magic Sand Lab
- Ch. 15 Review
- Ch. 15 Test
Chapter 18:
- Defining Acids & Bases
- Exploring Acids & Bases Lab
- Ch. 18 Quiz