Grace Joint School District 148 Science Chemistry District Course # Course Description Open 12 One year course Prerequisite Biology Content: Recommended for the college-bound student. Students will study matter and the changes it undergoes, learning the structure of atoms and molecules, elements, compounds, and mixtures. Also included will be why chemical reactions occur and how to control them. The instructional approach emphasizes the concepts of chemistry. This course is strongly recommended for the college-bound student. Adopted Materials Course Title Chemistry Use the periodic table to predict physical and chemical properties NO. Performance Objective Resource d 1 Define atomic radii 2 Define electronegativity 3 Identify extent of properties based on location on the periodic table. 4 Compare and contrast the properties of two elements. Describe the historical development of the periodic table. NO. Performance Objective Resource d 1 Explain Mendeleev's and Mosely's contribution to the development of the periodic table. Create and interpret graphs of data NO. Resource d 1 Collect data to create graphs. 2 Distinguish between different graphs. 3 Interpret graphs. s Explain and interpret the key concepts of the kinetic molecular theory. NO. Resource d 1 Predict particle activity associated with temperature District 11-12.C.1.1.1 11-12.C.1.2.1 11-12.C.1.2.2 11-12.C.1.2.3 Page 1 of 9
change. s Distinguish the common theories defining acids and bases. Resource d 1 Compare and contrast the different theories of acids and bases (e.g., Arrhenius Acids and Bases, Lewis Acids and Bases, Bronsted-Lowry Acids and Bases). 2 Classify compounds as acids or bases using the different theories. s Identify, compare and contrast physical and chemical properties and changes and appropriate computations. Resource d 1 Explain physical properties of certain substances 2 Explain chemical properties of certain substances. 3 Distinguish between a chemical and physical change. 4 Compare and contrast chemical and physical changes. s Perform computations using scientific notation, the metric system and dimensional analysis. 1 Identify a number in scientific notation. Resource d 2 Convert between standard and scientific notation by hand and with a calculator. 3 Perform mathematical operations using scientific notation 4 Measure and record using the metric system. 5 Convert measurements within the metric system. 6 Define dimensional analysis. 7 Convert units using dimensional analysis. 8 Defend the usefulness of dimensional analysis. s Compute measurement uncertainty to include precision, accuracy and the rules for significant digits. Resource d 1 Define precision. 2 Define accuracy. 3 Recognize precise and accurate measurements. 4 Compare and contrast precision and accuracy. 5 Recognize significant digits in a number. 6 Express measurements using the correct number of significant digits. 7 Use correct significant digits in calculations. s Perform calculations related to the conversion of grams to moles to particles, atoms, 11-12.C.1.2.4 11-12.C.1.3.1 11-12.C.1.3.2 11-12.C.1.3.3 Page 2 of 9
molecules and volume. 1 Define moles. 2 Explain the usefulness of moles. 3 Calculate molar mass. 4 Memorize Avogadro's number. 5 Determine the number of atoms, molecules, or particles in a certain number of moles. 6 Calculate the number of atoms in a certain number of grams in a specific substance and vice versa. 7 Know the standard molar volume 8 Calculate between moles and liters using the standard molar volume. Analyze and solve reaction stoichiometry problems. 1 Balance an equation. 2 Understand mole ratios of molecules in a chemical equation. 3 Convert moles to grams and grams to moles. 4 Solve stoichiometry problems. Express concentrations of solutions in various ways including molarity. Resource d Resource d Resource d 1 Define molarity. 2 Calculate molarity values of solutions. Interpret how the presence of solute particles affect the properties of a solution and be able to do calculations involving colligative properties. Resource d 1 Define colligative properties. 2 Use calculations to solve boiling point elevation and freezing point depression. s Analyze quantitative relationships involved in acid/base chemistry including ph. 1 Memorize the ph scale. 2 Determine whether a solution is acidic or basic based on the ph scale. 3 Predict the ph of a variety of substances 4 Calculate the ph from [H+] and [OH-]. Resource d in scope/sequence 11-12.C.1.3.4 11-12.C.1.3.5 11-12.C.1.3.6 11-12.C.1.3.7 11-12.C.1.3.8 Page 3 of 9
s Demonstrate an understanding of the scientific method. Evaluate the hypotheses, data, analysis, and conclusions in a science or technical text, verifying the data when possible and corroborating or challenging conclusions with other sources of information. Resource d 1 Memorize the components of the scientific method. 2 Validate the usefulness of the scientific method. 3 Analyze how certain experiments follow the scientific method. CCSSW Identify the parts of the scientific method within a journal abstract. CCSSW Summarize the parts of the scientific method within a journal abstract. s Select and use appropriate scientific equipment, materials and techniques. Follow precisely a complex multistep procedure when carrying out experiments, taking measurements, or performing technical tasks; analyze the specific results based on explanations in the text. Resource d 1 Recognize the basic laboratory equipment/materials. 2 Demonstrate proper usage of laboratory equipment/materials. 3 Select the appropriate equipment/materials to use to perform specific tasks. CCSSW Write a procedure for someone else to follow WHST 11-12.2 CCSSW Read and follow a procedure written by a Classmate. s Explain how a series of historically related and documented experiments led to the current model and structure of the atom. Write informative/explanatory texts, including the narration of historical events, scientific procedures/ experiments, or technical processes. Resource d 1 Describe the major contributions of specific scientists to the atomic theory. CCSSW Compare and contrast the theories leading up to the current model of the atomic structure. s Correctly write symbols, formulas and names for common elements, ions and compounds. Resource d 11-12.C.1.6.1. RST 11-12.6 RST. 11-12.8 WHST 11-12.2 WHST11-12.4 11-12.C.1.6.2 RST 11-12.3 WHST 11-12.2 11-12.C.1.7.1 WHST 11-12.2 RST 11-12.1 RST 11-12.9 11-12.C.1.8.1 RST 11-12.4 Page 4 of 9
1 Find elements on the periodic table. 2 Recognize the symbols for common elements. 3 Recognize the symbol for an ion. 4 Construct formulas for compounds. CCSSW Construct a paragraph describing a chemical reaction from a balanced chemical equation. CCSSW Construct a balanced chemical equation from a written description of a chemical reaction. Communicate scientific investigations and information clearly. Analyze the author's purpose in providing an explanation, describing a procedure, or discussing an experiment in a text, identifying important issues that remain unresolved. Synthesize information from a range of sources (e.g., texts, experiments, simulations) into a coherent understanding of a process, phenomenon, or concept, resolving conflicting information when possible. Resource d 1 Recognize and read a formal lab report 2 Compose a lab report. 3 Evaluate a lab report CCSSW Compose a lab notebook throughout the course. CCSSW Identify the purpose of the investigation. CCSSW Read and follow a procedure CCSSW Analyze data and write a summary of findings. CCSSW Evaluate whether findings relate to the purpose of investigation in a conclusion written in paragraph form. CCSSW Revise a lab report to better communicate scientific findings. s Explain and understand how electrons are involved in the formation of chemical bonds using the octet rule and Lewis dot diagrams. Resource d 1 Define valence electrons. 2 Determine the number of valence electrons using the periodic table. 3 Draw Lewis dot diagrams for various elements. 4 Explain the octet rule. 5 Define ionic bonds. 6 Define covalent bonds 7 Demonstrate how covalent bonds form using Lewis dot diagrams. 8 Demonstrate how ionic bonds form using Lewis dot diagrams. s Predict the polarity of chemical bonds using electronegativity. 11-12.C.1.8.2 RST 11-12.6 RST 11-12.9 WHST 11-12.10 RST 11-12.2 RST 11-12.3 WHST11-12.2 WHST 11-12.5 11-12.C.2.1.1 11-12.C.2.1.2 Page 5 of 9
Resource d 1 Understand the concept of electronegativity. 2 Use the trends for electronegativity on the periodic table to predict polarity. Predict physical properties of compounds based upon the attractive forces between atoms and molecules. Resource d 1 Use Lewis dot structures to predict attraction between molecules 2 Predict intermolecular physical properties (e.g., capillary action, surface tension, polarity). Distinguish and classify all matter into appropriate categories. 1 Define atom, element, compound, molecule, pure substance, heterogeneous mixture, and homogeneous mixture. 2 Classify different examples of matter. Explain the relationship and reactions of acids, bases, and salts. Resource d Resource d 1 Identify a neutralization reaction. 2 Predict the products of a neutralization reaction. Explain the role of dissociation and ionization in producing strong, weak, and nonelectrolytes. 1 Define strong and weak electrolytes, and nonelectrolytes 2 Explain how dissociation and ionization produce electrolytes. s Describe the Kinetic Molecular Theory as it applies to phases of matter. Resource d Resource d 1 Explain the kinetic molecular theory 2 Compare and contrast the molecular arrangement for each state of matter. 3 Explain how heat changes the molecular arrangement of matter. s Explain and calculate the changes in heat energy that occur during chemical reactions and 11-12.C.2.1.3 11-12.C.2.1.4 11-12.C.2.1.5 11-12.C.2.1.6 11-12.C.2.2.1 Page 6 of 9
phase changes. Resource d 1 Read and record temperature and mass measurements. 2 Identify the different types of phase changes. 3 Calculate the change in heat energy. 4 Explain the reasons for temperature change of a system. s Demonstrate the conservation of matter by balancing chemical equations. Resource d 1 Define the law of conservation of matter. 2 Use coefficients to balance chemical equations. 3 Defend how balancing equations is in accordance with the law of conservation of matter. s Differentiate between exothermic and endothermic chemical reactions during chemical or physical changes. Resource d 1 Define exothermic and endothermic reactions. 2 Identify chemical reactions and phase changes as endothermic and exothermic. s Interpret the classic historical experiments that were used to identify the components of an atom and its structure. Resource d in scope/sequence 1 Describe the experimental designs and conclusions of specific experiments to the development of the modern theory and model of the atom. 2 Interpret the data of these experiments to justify the conclusions. s Deduce the number of protons, neutrons and electrons for an atom or ion. Resource d in scope/sequence 1 Use the atomic number on the periodic table to find the number of protons of an atom or ion. 2 Use the atomic number and charge to determine the number of electrons for an atom or ion. 3 Use the atomic number and mass number to determine the number of neutrons in an atom or ion. s Describe the relationship between the structure of atoms and light absorption and emission. 11-12.C.2.3.1 11-12.C.2.3.2 11-12.C.2.3.3 11-12.C.2.4.1 11-12.C.2.4.2 11-12.C.2.4.3 Page 7 of 9
Resource d 1 Explain how the wavelengths of light emitted by an atom provide information about electron energy levels. s Determine and illustrate electron arrangements of elements using electron configurations and orbital energy diagrams. Resource d 1 Know that there are seven energy levels where electrons can be found. 2 List which sublevels (s, p, d, f) are in each energy level. 3 Show the number of orbitals and maximum number of electrons in each sublevel. 4 Illustrate the location of electrons of specific atoms using electron configuration and orbital energy diagrams. s Illustrate the Law of Conservation of Mass and the Law of Definite Proportions. Resource d 1 Define the Law of Conservation of Mass and the Law of Definite Proportions. 2 Perform an activity using a chemical equation and examine if the equation follows the Law of Conservation of Mass and the Law of Definite Proportions. s Classify, write and balance chemical equations for common types of chemical reactions and predict the products. Resource d 1 Label the parts of a chemical equation. 2 Translate word equations into chemical equations and vice versa. 3 Balance chemical equations by counting the total number of each type of atom for both reactants and products, then inserting coefficients. 4 Recognize the different types of chemical reactions. 5 Predict the products from various reactants for the different types of chemical reactions. s Describe the factors that influence the rates of chemical reactions. Resource d in scope/sequence 1 Discuss the factors that influence the rates of chemical reactions. s Demonstrate the ability to work safely and effectively in a chemistry laboratory. 11-12.C.2.4.4 11-12.C.2.5.1 11-12.C.2.5.2 11-12.C.2.5.3 Page 8 of 9
1 List the safety rules. 2 Discuss the importance of safety rules. 3 Identify the location of safety equipment. 4 Explain how and when to use the safety equipment. 5 Demonstrate how to work safely in the laboratory. CCSSW Write a procedure for someone else to follow. CCSSW Read and follow a procedure written by a classmate. s Assess the role of chemistry in enabling technological advances 1 List technology that was developed by chemists. 2 State career fields that use chemistry. 3 Explore the role of chemistry in the development of specific technology. CCSSW Read and summarize article relating to new chemical technology. CCSSW Evaluate the impact of the new technology. Evaluate the role of chemistry in energy and environmental issues. 1 List various forms of energy production. 2 Relate how chemistry is involved in energy production. 3 Evaluate how energy production affects the environment. 4 Discuss how chemistry can be used to help or harm the environment. CCSSW Research a local environmental issue. CCSSW Assess sources for strengths and limitations. CCSSW Write a one page paper on how chemistry is involved in a local environmental issue. Resource d Resource d Resource d 11-12.C.5.1.1 WHST 11-12.2 RST 11-12.3 11-12.C.5.2.1 RST 11-12.2 WHST 11-12.9 11-12.C.5.3.1 RST 11-12.7 WHST 11-12.7 WHST 11-12.8 WHST 11-12.1 Page 9 of 9