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Curriculum Map for Organic Chemistry Course Understandings Students will understand: Chemistry is the study of matter and the changes it undergoes. Atomic theory is the foundation for the study of chemistry. The nature of science depends on the ability to conduct scientific experiments with reproducible results. Chemical bonding occurs as a result of attractive forces between particles. Essential Questions In what ways has the theory of the atom changed over time due to technological improvements? What are the differences between pure substances and mixtures? What factors determine the types of chemical bonds that form between particles? Assessments Formative Assessments – Students will be assessed using a weekly quiz to check understanding. Students will be informally assessed using in class assignments, homework, and class activities. A posttest will be given at the conclusion of each chapter to assess comprehension and analysis of concepts. How does the distribution of electrons in atoms affect the formation of a compound? First Quarter Diagnostic – Students’ prior knowledge will be assessed through teacher questioning. Students’ prior knowledge will be tested through homework problems. Summative Assessments – Quarterly Exam #1 will be given to assess student comprehension and analysis. Course Knowledge/Skills Standard: 3.2.C.A1 – Differentiate between physical properties and chemical properties Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.2 – Classify observations as qualitative and/or quantitative. Standard: 3.2.C.A1 – Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures Anchor: CHEM. A.1.2 – Compare the properties of mixtures Eligible Content CHEM.A.1.2.1 – Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.2.2 – Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated). CHEM.A.1.2.3 – Describe how factors (e.g., temperature, concentration, surface area) can affect solubility. Anchor: CHEM. A.2.1 – Explain how atomic theory serves as the basis for the study of matter Eligible Content CHEM.A.2.1.1 – Describe the evolution of the atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.1.2 – Differentiate between the mass number of an isotope and the average atomic mass of an element. Anchor: CHEM.B.1.2 – Apply the mole concept to the composition of matter Eligible Content CHEM.B.1.2.2 – Apply the law of definite proportions to the classification of elements and compounds as pure substances Standard: 3.2.C.A4 – Predict how combinations of substances can result in physical and/or chemical changes. Anchor: CHEM.B.1.1 – Explain how the mole is a fundamental unit of chemistry. Eligible Content CHEM.B.1.1.1 – Apply the mole concept to representative particles (e.g., counting, determining mass of atoms, ions, molecules, and/or formula units). Standard: 3.2.C.A5 – Models – Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of the atom) and understand how each discovery leads to modern theory. Anchor: CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.1 – Classify physical or chemical changes within a system in terms of matter and/or energy. Standard 3.2.C.A5 – Describe Rutherford’s “gold foil” experiment that lead to the discovery of the nuclear atom. Identify the major components (protons, neutrons, and electrons) of the nuclear atom and explain how they interact. Anchor: CHEM.A.2.1 – Explain how atomic theory serves s the basis for the study of matter. Eligible Content CHEM. A.2.1.1 – Describe the evolution of atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. Standard: 3.2.C.A1 – Explain the relationship of an elements position on the periodic table to its atomic number, ionization energy, electro-negativity, atomic size, and classification of elements. Anchor: CHEM.A.2.1 – Explain how atomic theory serves as the basis for the study of matter. Eligible Content CHEM.A.2.1.2 – Differentiate between the mass number of an isotope and the average atomic mass of an element. Anchor: CHEM.A.2.3 – Explain how periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. Eligible Content CHEM.A.2.3.2 – Explain how the periodicity of chemical properties led to the arrangement of elements on the periodic table. Standard: 3.2.C.A1 – Use electro-negativity to explain the difference between polar and non-polar covalent bonds. Anchor: CHEM.B.2.3 – Explain how atoms form chemical bonds. Eligible Content CHEM.B.1.3.2 – Classify a bond as being polar covalent, non-polar covalent, or ionic. Standard: 3.2.C.A2 – Compare the electron configurations for the first twenty elements of the periodic table. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.1 – Predict the ground state electronic configurations and/or orbital diagram for a given atom or ion. Standard: 3.2.C.A2 – Relate the position of an element on the periodic table to its electron configuration and compare its reactivity to the reactivity of other elements in the table. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.2 – Predict characteristics of an atom or an ion based on its location on the periodic table (e.g., number of valence electrons, potential types of bonds, reactivity. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.4 – Relate the existence of quantized energy levels to atomic emission spectra. Standard: 3.2.C.A2 – Explain how atoms combine to form compounds through both ionic and covalent bonding. Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.4 – Relate the physical properties of matter to its atomic or molecular structure. Anchor: CHEM.B.1.3 – Explain how atoms for chemical bonds. Eligible Content CHEM.B.1.3.1 – Explain how atoms combine to form compounds through ionic and covalent bonding. Standard: 3.2.C.A2 – Predict chemical formulas based on the number of valence electrons. Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.5 – Apply systematic set of rules (IUPAC) for naming compounds and writing chemical formulas (e.g., binary covalent binary ionic, ionic compounds containing polyatomic ions). Standard: 3.2.C.A2 – Draw Lewis dot structures for simple molecules and ionic compounds. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.3 – Explain the relationship between the electron configurations and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). Anchor: CHEM.B.1.3 – Explain how atoms form chemical bonds. Eligible Content CHEM.B.1.3.3 – Use illustrations to predict the polarity of a molecule. Anchor: CHEM.B.1.4 – Explain how models can be used to represent bonding. Eligible Content CHEM.B.1.4.1 – Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball-and-stick models, graphical models, solid-sphere models, structural formulas, skeletal formulas, Lewis dot structures). Eligible Content CHEM.B.1.4.2 – Utilize Lewis dot structures to predict the structure and bonding in simple compounds. Students will understand: Periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. What factors identify the types of chemical reactions? How can materials with the same chemical composition be so different? Chemical reactions are predictable. Formative Assessments – What is the role of carbon in the molecular diversity of life? Second Quarter Diagnostic – Students’ prior knowledge will be assessed through teacher questioning. Students’ will be assessed through homework problems. Students will be assessed using a weekly quiz to check understanding. Students will be informally assessed using in class assignments, homework, and class activities. Standard: 3.2.C.A1 – Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures Anchor: CHEM. A.1.2 – Compare the properties of mixtures Eligible Content CHEM.A.1.2.1 – Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.2.2 – Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated). CHEM.A.1.2.3 – Describe how factors (e.g., temperature, concentration, surface area) can affect solubility. Anchor: CHEM. A.2.1 – Explain how atomic theory serves as the basis for the study of matter Eligible Content A posttest will be given at the conclusion of each chapter to assess comprehension and analysis of concepts. Summative Assessments – Quarterly Exam #2 will be given to assess student comprehension and analysis. CHEM.A.2.1.1 – Describe the evolution of the atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.1.2 – Differentiate between the mass number of an isotope and the average atomic mass of an element. Standard: 3.2.C.A5 – Models – Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of the atom) and understand how each discovery leads to modern theory. Anchor: CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.1 – Classify physical or chemical changes within a system in terms of matter and/or energy. Standard: 3.2.C.A2 – Explain how atoms combine to form compounds through both ionic and covalent bonding. Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.4 – Relate the physical properties of matter to its atomic or molecular structure. Anchor: CHEM.B.1.3 – Explain how atoms for chemical bonds. Eligible Content CHEM.B.1.3.1 – Explain how atoms combine to form compounds through ionic and covalent bonding. Standard: 3.2.C.A2 – Draw Lewis dot structures for simple molecules and ionic compounds. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.3 – Explain the relationship between the electron configurations and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). Anchor: CHEM.B.1.3 – Explain how atoms form chemical bonds. Eligible Content CHEM.B.1.3.3 – Use illustrations to predict the polarity of a molecule. Anchor: CHEM.B.1.4 – Explain how models can be used to represent bonding. Eligible Content CHEM.B.1.4.1 – Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball-and-stick models, graphical models, solid-sphere models, structural formulas, skeletal formulas, Lewis dot structures). Eligible Content CHEM.B.1.4.2 – Utilize Lewis dot structures to predict the structure and bonding in simple compounds. Standard: 3.2.C.A4 – Interpret and apply the Laws of Conservation of Mass, Constant Composition (Definite Proportions), and Multiple Proportions. Anchor: CHEM.B.1.2 – Apply the mole concept to the composition of matter Eligible Content CHEM.B.1.2.2 – Apply the law of definite proportions to the classification of elements and compounds as pure substances Standard: 3.2.C.A4 – Classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement, and combustion. Anchor: CHEM.B.2.1 – Predict what happens during a chemical reaction. Eligible Content: What factors identify the types of chemical reactions? Students will understand: Chemical reactions are predictable. Periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. How can materials with the same chemical composition be so different? What is the role of carbon in the molecular diversity of life? Third Quarter Diagnostic – Students’ prior knowledge will be assessed through teacher questioning. Students’ prior knowledge will be tested through homework problems. Formative Assessments – Students will be assessed using a weekly quiz to check understanding. Students will be informally assessed using in class assignments, homework, and class activities. A posttest will be given at the conclusion of each chapter to assess comprehension and analysis of concepts. Summative Assessments – Quarterly Exam #3 will be given to assess student comprehension and analysis. CHEM.B.2.1.4 – Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.B.2.1.5 – Balance chemical equations by applying the law of conservation of matter. Standard: 3.2.C.A1 – Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures Anchor: CHEM. A.1.2 – Compare the properties of mixtures Eligible Content CHEM.A.1.2.1 – Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.2.2 – Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated). CHEM.A.1.2.3 – Describe how factors (e.g., temperature, concentration, surface area) can affect solubility. Anchor: CHEM. A.2.1 – Explain how atomic theory serves as the basis for the study of matter Eligible Content CHEM.A.2.1.1 – Describe the evolution of the atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.1.2 – Differentiate between the mass number of an isotope and the average atomic mass of an element. Standard: 3.2.C.A5 – Models – Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of the atom) and understand how each discovery leads to modern theory. Anchor: CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.1 – Classify physical or chemical changes within a system in terms of matter and/or energy. Standard: 3.2.C.A2 – Explain how atoms combine to form compounds through both ionic and covalent bonding. Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.4 – Relate the physical properties of matter to its atomic or molecular structure. Anchor: CHEM.B.1.3 – Explain how atoms for chemical bonds. Eligible Content CHEM.B.1.3.1 – Explain how atoms combine to form compounds through ionic and covalent bonding. Standard: 3.2.C.A2 – Draw Lewis dot structures for simple molecules and ionic compounds. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.3 – Explain the relationship between the electron configurations and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). Anchor: CHEM.B.1.3 – Explain how atoms form chemical bonds. Eligible Content CHEM.B.1.3.3 – Use illustrations to predict the polarity of a molecule. Anchor: CHEM.B.1.4 – Explain how models can be used to represent bonding. Eligible Content CHEM.B.1.4.1 – Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball-and-stick models, graphical models, solid-sphere models, structural formulas, skeletal formulas, Lewis dot structures). Eligible Content CHEM.B.1.4.2 – Utilize Lewis dot structures to predict the structure and bonding in simple compounds. Standard: 3.2.C.A4 – Interpret and apply the Laws of Conservation of Mass, Constant Composition (Definite Proportions), and Multiple Proportions. Anchor: CHEM.B.1.2 – Apply the mole concept to the composition of matter Eligible Content CHEM.B.1.2.2 – Apply the law of definite proportions to the classification of elements and compounds as pure substances Standard: 3.2.C.A4 – Classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement, and combustion. Anchor: CHEM.B.2.1 – Predict what happens during a chemical reaction. Eligible Content: CHEM.B.2.1.4 – Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.B.2.1.5 – Balance chemical equations by applying the law of conservation of matter. Students will understand: Chemical reactions are How are changes in matter accompanied by Fourth Quarter Diagnostic – Lab concepts will be assessed while applying content skills. Standard: 3.2.C.A1 – Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures predictable. changes in energy? What is the role of carbon in the molecular diversity of life? How do structures of biologically important molecules (e.g., carbohydrates, lipids, proteins, nucleic acids) account for their functions? How might advances in science and technology affect society? Students’ prior knowledge will be assessed through teacher questioning. Students’ prior knowledge will be tested through homework problems. Formative Assessments – Students will be assessed using a weekly quiz to check understanding. • Students will be informally assessed using in class assignments, homework, and class activities. • A posttest will be given at the conclusion of each chapter to assess comprehension and analysis of concepts. Summative Assessments – Quarterly Exam #4 will be given to assess student comprehension and analysis. Anchor: CHEM. A.1.2 – Compare the properties of mixtures Eligible Content CHEM.A.1.2.1 – Compare properties of solutions containing ionic or molecular solutes (e.g., dissolving, dissociating). CHEM.A.1.2.2 – Differentiate between homogeneous and heterogeneous mixtures (e.g., how such mixtures can be separated). CHEM.A.1.2.3 – Describe how factors (e.g., temperature, concentration, surface area) can affect solubility. Anchor: CHEM. A.2.1 – Explain how atomic theory serves as the basis for the study of matter Eligible Content CHEM.A.2.1.1 – Describe the evolution of the atomic theory leading to the current model of the atom based on the works of Dalton, Thomson, Rutherford, and Bohr. CHEM.A.2.1.2 – Differentiate between the mass number of an isotope and the average atomic mass of an element. Standard: 3.2.C.A5 – Models – Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of the atom) and understand how each discovery leads to modern theory. Anchor: CHEM.A.1.1 Identify and describe how observable and measurable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.1 – Classify physical or chemical changes within a system in terms of matter and/or energy. Standard: 3.2.C.A2 – Explain how atoms combine to form compounds through both ionic and covalent bonding. Anchor: CHEM.A.1.1 – Identify and describe how observable and measureable properties can be used to classify and describe matter and energy. Eligible Content CHEM.A.1.1.4 – Relate the physical properties of matter to its atomic or molecular structure. Anchor: CHEM.B.1.3 – Explain how atoms for chemical bonds. Eligible Content CHEM.B.1.3.1 – Explain how atoms combine to form compounds through ionic and covalent bonding. Standard: 3.2.C.A2 – Draw Lewis dot structures for simple molecules and ionic compounds. Anchor: CHEM.A.2.2 – Describe the behavior of electrons in atoms. Eligible Content CHEM.A.2.2.3 – Explain the relationship between the electron configurations and the atomic structure of a given atom or ion (e.g., energy levels and/or orbitals with electrons, distribution of electrons in orbitals, shapes of orbitals). Anchor: CHEM.B.1.3 – Explain how atoms form chemical bonds. Eligible Content CHEM.B.1.3.3 – Use illustrations to predict the polarity of a molecule. Anchor: CHEM.B.1.4 – Explain how models can be used to represent bonding. Eligible Content CHEM.B.1.4.1 – Recognize and describe different types of models that can be used to illustrate the bonds that hold atoms together in a compound (e.g., computer models, ball-and-stick models, graphical models, solid-sphere models, structural formulas, skeletal formulas, Lewis dot structures). Eligible Content CHEM.B.1.4.2 – Utilize Lewis dot structures to predict the structure and bonding in simple compounds. Standard: 3.2.C.A4 – Interpret and apply the Laws of Conservation of Mass, Constant Composition (Definite Proportions), and Multiple Proportions. Anchor: CHEM.B.1.2 – Apply the mole concept to the composition of matter Eligible Content CHEM.B.1.2.2 – Apply the law of definite proportions to the classification of elements and compounds as pure substances Standard: 3.2.C.A4 – Classify chemical reactions as synthesis (combination), decomposition, single displacement (replacement), double displacement, and combustion. Anchor: CHEM.B.2.1 – Predict what happens during a chemical reaction. Eligible Content: CHEM.B.2.1.4 – Predict products of simple chemical reactions (e.g., synthesis, decomposition, single replacement, double replacement, combustion). CHEM.B.2.1.5 – Balance chemical equations by applying the law of conservation of matter.