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Department: Science Course Number and Title: 523 (CP) and 518 (H) Chemistry 1 Course Description This course covers the most frequent theories of the nature of matter and its interaction. Major emphasis will be on chemical interactions from both a descriptive and mathematical approach. The student will derive conclusions from laboratory experiments and solving problems. MHS Learning Expectations: • Demonstrate the ability to problem solve effectively. Essential Questions: How does chemistry impact society? How can we use the properties of matter and elements to help us to understand the interactions of matter? How do matter and energy cycle in our world? Students will know: Students will be able to: • Physical and chemical properties • Classify and describe matter using reflect the nature of the interactions physical and chemical properties between molecules or atoms, and that reflect the nature of the can be used to classify and describe interactions between molecules or matter. atoms. • Atomic models are used to explain • Use atomic models to explain atoms and help us understand the atoms and describe the interaction interaction of elements and of elements and compounds. compounds observed on a • Write the electron configurations macroscopic scale. Nuclear for the first twenty elements of the chemistry deals with radioactivity, periodic table. nuclear processes, and nuclear • Describe the relationship between properties. Nuclear reactions nuclear reactions and energy. produce tremendous amounts of Relate the law of conservation of energy and lead to the formation of mass to nuclear reactions. elements. • Identify the three main types of • Repeating (periodic) patterns of radioactive decay (alpha, beta, and physical and chemical properties gamma) and compare their occur among elements that define properties (composition, mass, families with similar properties. The charge, and penetrating power). periodic table displays the repeating • Describe the process of radioactive patterns, which are related to the decay by using nuclear equations, atoms’ outermost electrons. and explain the concept of half-life • Atoms bond with each other by for an isotope transferring or sharing valence • Describe and explain the periodic electrons to form compounds. patterns of physical and chemical • • • • • In a chemical reaction, one or more reactants are transformed into one or more new products. Chemical equations represent the reaction and must be balanced. The conservation of atoms in a chemical reaction leads to the ability to calculate the amount of products formed and reactants used (stoichiometry). Gas particles move independently of each other and are far apart. The behavior of gas particles can be modeled by the kinetic molecular theory. In liquids and solids, unlike gases, particles are close to each other. The driving forces of chemical reactions are energy and entropy. The reorganization of atoms in chemical reactions results in the release or absorption of heat energy. Solids, liquids, and gases dissolve to form solutions. Rates of reaction and chemical equilibrium are dynamic processes that are significant in many systems (e.g., biological, ecological, geological). Acids and bases are important in numerous chemical processes that occur around us, from industrial procedures to biological ones, from the laboratory to the environment. Oxidation-reduction reactions occur when one substance transfers electrons to another substance, and constitute a major class of chemical reactions. • • • • • • • • • • • • properties that occur among elements. Describe the process of the bonding including ionic, polar covalent, nonpolar covalent, and hydrogen bonding. Use this knowledge to construct formulas and models of the compounds created. Understand the process of chemical reactions and relate the law of conservation of mass to balancing equations. Predict the products of chemical reactions and perform calculations that relate to these chemical reactions. Determine percent compositions, empirical formulas, and molecular formulas. Calculate the mass-to-mass stoichiometry for a chemical reaction. Calculate percent yield in a chemical reaction. Describe the different states of matter and use the Kinetic Molecular Theory to explain the behaviors of gases. Explain the importance of energy and entropy in chemical reactions. Describe the formation and components of solutions. Calculate concentration in terms of molarity. Use molarity to perform solution dilution and solution stoichiometry. Identify and explain the factors that affect the rate of dissolving (e.g., temperature, concentration, surface area, pressure, mixing). Compare and contrast qualitatively the properties of solutions and • • • • pure solvents (colligative properties such as boiling point and freezing point). Identify the factors that affect the rate of a chemical reaction (temperature, mixing, concentration, particle size, surface area, catalyst). Predict the shift in equilibrium when a system is subjected to a stress (LeChatelier’s principle) and identify the factors that can cause a shift in equilibrium (concentration, pressure, volume, temperature). Relate the rates of reaction and chemical equilibrium to biological, ecological, and geological systems. Identify and explain acid -base and oxidation-reduction reactions. Course Outline Semester One Semester Two Lab Techniques, Lab Safety, Measurements and Significant Figures Chemical Reactions continued Introduction to Matter and the Periodic Table of Elements Mole Conversions Atomic Structure Percent Composition by Mass and Empirical/Molecular Formula Nuclear Chemistry Stoichiometry Ionic Compounds Thermochemistry Covalent Compounds and VSEPR Kinetic Molecular Theory and Gas Laws Metals Mixtures, Solutions and Molarity Chemical Reactions Equilibrium and Acids/Bases Primary Course Materials Textbook: Matter and Change (2013) will be provided to each student. In addition, you will have access to an electronic textbook for your use online. You will be given a username and password to access the text online. Additional Materials: laboratory activities, computer simulations, scientific articles, teachercreated projects, and extensions to college level content Grade Determination: Quarterly grades will be based on: Tests Quizzes Projects and labs Homework and class work 50 % 20 20 10 Major Assignments: 4 Formal Lab Reports and 4 Core Assignments, Midyear and final exam, each containing an Open Response. These assignments are given in common for all students taking chemistry. Midyear and Final Exams Midyear and Final Exams will be given. These exams count as 10% of the respective semester grade. The average of the first and second quarter grades will count 90% in determining the first semester average. Similarly, the second semester average will include the average of third and fourth quarter grades at 90% and the final exam at 10%. The average for the entire year will be the average of both semesters. Q1 = 22.5% Q2 = 22.5% Midterm = 5% Q3 = 22.5% Q4 = 22.5% Final = 5%