Month September October November December Essential What are the physical and Question(s) chemical properties of matter? Skills/ Objectives How do scientists use tools of measurements in scientific investigations? A. Chemistry, nature of science, measurement, solving problems, derived units. B. Matter: Physical and chemical properties, Mixtures. A. 1. Identify qualitative and quantitative observations. 2. Describe the nature of science. 3. Identify metric prefixes and know how they change a base unit. 4. Use conversion factors. 5. Give examples and use derived units. B. 6. Distinguish between and give examples of physical and chemical properties and changes. 7. Define a chemical reaction. 8.Distinguish between mixtures and substances. A. Atoms, elements and the periodic table, Compounds and chemical formulas. B. Atomic theories. Atomic Number, Mass Number and Atomic Mass. A. 1. Identify particles in an atom 2. Recognize elements and symbols. 3. Locate metals and nonmetals on a periodic table 4. Explain symbols and subscripts in a chemical symbol and chemical formula. 5. Compare elements and compounds. B. 6. Describe different models, theories and experiments by Dalton, Thomson, Rutherford, Bohr. 7. Find, write and explain an elements atomic number, symbol for an ion or atom, mass number and its relation to atom s mass. 8. Explain how isotopes of same element are different. C. Explain and calculate the average atomic mass of an element. What are compounds? What are their names and formulas for compounds? Molecular compounds and formulas, Ions, polyatomic ions and ionic compounds. A. 1. Define a molecular compound. 2. Write formula, understand prefixes for molecular compound names. 3. Determine formula units from simple ratios. 4. Write formulas and recognize common polyatomic ions and acids. 5. Name molecular compounds and ions. B. 1. Explain what a mole is and convert between moles and number of particles 2. Define and find molar mass and mass of element and compound using periodic table. 3. Convert between molar mass, mass, and moles. 4. Find percent composition of a compound 5. Find molecular formula and empirical formula of a compound and hydrate. How do scientists describe large quantities of atoms and molecules? What are chemical reactions and how are they represented? A. Measuring matter. Molar mass, molar volume. Percent composition. Empirical and molecular formulas and hydrates. B. Chemical reactions. Balancing chemical equations. A. 1. Define STP and standard molar volume. 2. Convert between gas volume, moles, mass, and number of particles. B. 1. Identify reactants and products in a chemical equation and understand symbols used. 2. Explain the need for balanced equations and use coefficients to balance a chemical equation. 3. Describe combination, decomposition and combustion reactions and identify examples using reactants. 4. Describe and identify single replacement reactions and double replacement reactions.
Month September cont d October cont d November cont d December cont d Standards/ NJCCCS 1 : 5.1.12.A.1-3, Benchmarks Assessment/ Resources 5.1.12.D.2+3 Textbook: Packard, K.A., Jacobs, D.H., & Marshall, R.H. (2007). Chemistry Pearson AGS Globe, MN. Chapter 1,2 Lab: 1. Making observations Quantity or Quality. 2. Accuracy & Precision 3. Reading equipment accurately. 5.1.12.D.2+3, 5.2.12.A.1-4 Chapter 2, 8 Lab: 1. Determining % of water of hydration in a crystalline salt. 2. What % of a U.S. penny is zinc? 5.1.12.D.2+3, 5.2.12.A.1-4 Chapter 3 Lab: 1. Determining the empirical formula of copper sulfide from % composition. 2. Determining % of oxygen in Potassium Chlorate. 5.1.12.D.2+3, 5.2.12.B.1+3 Chapter 4, 5 Lab: 1. Decomposition of sodium chlorate. & discussion, quizzes, unit tests, 1 NJCCCS 2009 New Jersey Core Curriculum Standards retrieved on September 1, 2013 from New Jersey Department of Education Website. http://www.state.nj.us/education/cccs/standards/5/5.pdf
Month January February March April Essential Question(s) Skills/Objectives Why do specific amounts of substances react? How is a chemical reaction similar to a recipe? Stoichiometry and moles, mass, particles, volume. A. 1. Explain use of coefficients to a balanced equation to create mole rations. 2. Solve molemole conversion problems. 3. Convert between mass-mole, mass-mass problems. 4. Solve stoichiometry problems using avogadro s number of particles. 5. Solve stoichiometry problems using gas volume at STP. 6. Distinguish between percent yield, actual yield and theoretical yield. What are the types of chemical bonds and how are they formed? Electronegativity and bond type. Dot diagrams of molecules and molecular geometry. Polar and nonpolar molecules. A. 1. Explain how electrons are involved in chemical bonds. 2. Define electronegativity and describe the types of chemical bonds. 3. Predict bond type using electronegativity values. 4. Draw dot diagrams for compounds and polyatomic ions. 5. Describe single, double, and triples bonds. 6. Name and give examples of molecular shapes. 7. Explain the effects of lone pairs on, and identify molecular geometry using dot diagrams. 8. Distinguish between polar and nonpolar molecules, and describe asymmetric geometry. 9. Distinguish between different interparticle forces. How are electrons arranged in an atom? What are the patterns among elements of a periodic table? A. Energy levels and orbitals. Electron configuration. B. Development of periodic table. Patterns in valence electrons and atomic size. A. 1. Describe the contributions of Planck, Einstein, Bohr. 2. Explain movement of electrons between energy levels. 3. Explain the four types of orbitals and some of their shapes. 4. Use emission spectrum to identify elements. 5. Explain, use rules for and write electron configuration of atoms and ions using diagonal chart. 6. Identify valence electrons and explain the similarity between elements in the same row and column. 7. Describe noble gas using valence electrons. 8 Write abbreviated electron configuration using periodic table. 9. Historical development and patterns in periodic table. How does matter change from one state to another? What is heat and how is it transferred? A. Condensed states of matter. Heating and cooling processes. B. Measuring heat. Enthalpy. A. 1. Define condensation, sublimation, boiling, freezing and melting. 2. Explain change of state of substances in terms of particle forces. 3. Tell what kind of physical change each H describes. 4. Read and interpret heating or cooling graphs and calculate H for a heating or cooling process. B. 1. Distinguish between endothermic and exothermic reactions. 2. Describe transfer of heat. 3. Use heat equation to solve calorimetry problems. 4. Define enthalpy and heat of reaction. 5. Explain what entropy is.
Month January con d February cont d March cont d April cont d Standards/ Benchmarks Assessments/ Resources 5.1.12.B.1-4, 5.1.12.C.1-2, 5.1.12.D.2+3, 5.2.12.A.1, 5.2.12.B.3 Chapter 6 5.1.12.D.2+3, 5.2.12.B.1-3, 5.2.12.D.2 Chapter 12 5.1.12.D.2+3, 5.2.12.A.1+2+4, 5.2.12.B.1 Chapter 10, 11 5.1.12.D.2+3, 5.2.12.A.2, 5.2.12.B.1, 5.2.12.C.1+2, 5.2.12.D.2, 5.2.12.D.5 Chapter 14, 13 Lab: 1. Actual yield versus theoretical yield of copper sulfide. 2. Synthesis of zinc chloride, actual yield versus theoretical yield. & discussion, quizzes, unit tests, class participation. Lab: 1. Investigation: Chromatography and polarity. 2. Individual student presentation on assigned element. Lab: 1. Colored flames and electrons. 2. Investigation: Valence electrons of metals. Group presentations on assigned topic. & discussion, quizzes, unit tests,
Month May June Essential Question(s) What are the properties and behavior of gases? What are the properties and behavior of water? Properties of gases. Measuring pressure and temperature. Dalton s law of partial pressure. A. Water: Physical properties of water. Phase diagram of water. Enthalpy changes. B. Final Review Skills/Objectives A. 1. Compare the behavior of particles in solids, liquids, and gases 2. State how temperature and pressure are related. 3. Convert between pressure units. 4. Describe absolute temperature scale and convert between Kelvin and degrees Celsius. 5. Define partial pressure and Dalton s law of partial pressure. 6. Calculate pressure of a mixture of gases or of one gas. 7 Explain the relationships between changes in gas volume, pressure, or temperature. 8 Write equation for combined gas law. 9. Use law to calculate pressure, volume, or temperature of a gas. A. 1. Describe unique properties of water. 2. Relate properties of water to hydrogen bonding. 3. Use phase diagram to identify state of a substance at a specific temperature and pressure. B. Review for final exam Standards/Benchmarks 5.1.12.D.2+3, 5.2.12.B.3, 5.2.12.C.1, 5.2.12.D.2 Assessments/Resources, Chapter 7 5.1.12.D.2+3, 5.2.12.A.5+6, 5.2.12.B.3, 5.2.12.C.2, 5.2.12.D.2, Chapter 14 Labs: 1. The density of a gas experimental value versus theoretical value. discussion, quizzes, unit tests, Lab: 1. Preparation and properties of oxygen 2. Comparing the concentration of saturated solutions.