Learning Objectives for Chemistry 173

Transcription

1 Learning Objectives for Chemistry 173 Glenbrook North High School Academic Year, This outline provides a comprehensive list of the topics and concepts you will learn in this course. For each topic I have given the relevant sections in your textbook (Modern Chemistry by Sarquis) as well as links to lecture notes that supplement the book. Be sure to cross reference this material with your lecture and experimental notes as well as any multimedia sources shared on the course website. Upon successful completion of the course the student should be able to: 1 Defining Chemistry and Matter Chapter 1 1. Explain what types of questions chemistry attempts to answer. 2. Describe the main branches of chemistry. 3. Distinguish between an atom, element, and compound. 4. Explain the differences between extensive and intensive properties. 5. Describe the three states of matter relevant to chemists. 6. Use particle diagrams to model matter and the particulate level. 7. Explain the difference between a physical and chemical property. 8. Explain the difference between a pure substance and a mixture. 9. Describe how the periodic table organizes the elements. 10. Identify an element as a metal, nonmetal, or metalloid. 11. Identify the major named groups (families) on the periodic table. 2 The Kinetic-Molecular Theory of Matter Chapter 10, Sections 1 and 4 1. Explain the five assumptions made in the kinetic-molecular theory of matter. 2. Use the kinetic-molecular theory to explain the physical properties of matter in the gas state. 1

2 3. Sketch a Maxwell distribution plot and explain how it relates to kinetic-molecular theory. 4. Describe, using particle diagrams, equilibrium changes for phase changes. 5. Explain the role of energy in phase changes. 6. Use the Maxwell distribution plot to explain phase changes. 7. Read a phase diagram to determine the state of matter for a compound at a given temperature and pressure. 8. Identify sections of a phase diagram that are at equilibrium. 9. Relate changes of state to a phase diagram and Maxwell distribution plot. 3 The Physical Behavior of Gases Chapter 11, Sections 1 and 2 1. Explain how gas particles generate pressure. 2. Draw particle diagrams to represent mixtures of gases. 3. Explain Dalton s law of partial pressure and use it to calculate pressures of gases in a mixture. 4. Explain, using kinetic-molecular theory, why gas volume and pressure are inversely proportional. 5. Use the Boyle s law equation to solve for changes in pressure or volume of a gas. 6. Use a plot of pressure and volume to predict the changes of a gas. 4 Measurements and Calculations. Chapter 2 1. Explain how modeling is crucial to forming scientific theories. 2. Explain the difference between mass and weight. 3. Use particle diagrams to explain the property, density. 4. Use the density equation to solve for mass, volume, or density. 5. Use dimensional analysis to convert between equivalent units. 6. Explain the difference between accuracy and precision. 7. Calculate percentage error for experimental values. 8. Explain why measurements need to be recorded with the proper number of significant figures. 9. Determine the number of significant figures in a measurement. 10. Perform calculations following the rules of significant figures. 11. Express measurements in scientific notation. 2

3 5 The Structure of Atoms. Chapter 3 1. Describe the three laws that explain how matter behaves in chemical reactions. 2. Describe how the cathode ray tube lead to the discovery of the electron. 3. Describe how the gold foil experiment lead to the discovery of the nucleus. 4. The describe the properties of the subatomic particles. 5. Sketch diagrams that show the types and locations of the subatomic particles in a given atom. 6. Explain why the average mass of most elements is a weighted value. 7. Sketch diagrams to show the differences between isotopes of an atom. 8. Write element symbols indicating the atomic number and mass number. 9. Define the quantity of a mole. 10. Explain how molar mass allows us to count by weighing. 11. Use dimensional analysis to convert between mass, moles, and number of particles. 6 Nuclear Chemistry Chapter 21, Section 1, 2 (only alpha, beta, and gamma and up to p. 649), 3, and 4 1. Explain what the plot known as the Band of Stability tells us about atoms and their isotopes. 2. Use the Band of Stability plot to determine if an isotope is stable. 3. Describe the process of radioactive decay. 4. Write nuclear equations for alpha, beta, and gamma decay. 5. Draw particle diagrams for alpha, beta, and gamma decay. 6. Describe half life in regards to radioactive elements. 7. Sketch and interpret a plot of half life for a radioactive element. 8. Describe the general effects of ionizing radiation on living tissue. 9. Explain the challenges of storage and disposal of nuclear waste. 10. Use particle diagrams to explain the process of nuclear fission. 3

4 7 The Arrangement of Electrons in Atoms Chapter 4 1. Describe the properties of electromagnetic radiation. 2. Calculate the wavelength and frequency for electromagnetic radiation. 3. Describe what it means for humans to see light. 4. Define a quantum. 5. Define a photon. 6. Calculate the energy of a photon. 7. Explain the difference between a ground state and an an excited state. 8. Diagram and explain how the Bohr model of the atom explains the emission spectrum of hydrogen. 9. Explain the bizarre conclusion of the two-slit experiment. 10. Describe the uncertainty principle. 11. Explain how modern quantum theory differs from the Bohr model of the atom. 12. Sketch the shapes of s and p orbitals. 13. Explain what an Aufau diagram represents. 14. Create an Aufbau diagram following the exclusion principle and Hund s rule. 15. Write electron configurations for the first twenty elements. 16. Relate orbital sketches to electron configurations and Aufbau diagrams. 8 Periodicity Chapter 5 1. Describe how the general layout of the periodic table relates to electron configurations. 2. Identify the s block, p block, and main group elements. 3. Explain and diagram the periodic trend in atomic radii. 4. Explain and diagram the periodic trend in ionization energy. 5. Explain and diagram the periodic trend in electron affinity. 6. Explain and diagram the periodic trend in ion radii as compared to their neutral atom. 7. Explain and diagram the periodic trend in electronegativity. 8. Define valence electrons and explain why they are important for the stability of atoms. 4

5 9 Chemical Bonding Chapter 7, Sections 1, 2 (up to p. 178), 3, 4, and 5 (skip p ). 1. Describe the general approach by which atoms form compounds. 2. Explain graphically how bond formation is a lower energy state for the system of atoms. 9.1 Ionic Bonds 1. Describe the formation of an ionic bond. 2. Use electron configurations to show the transfer of electrons between a metal and nonmetal to form an ionic bond. 3. Define a formula unit. 4. Sketch the three dimensional structure of an ionic lattice. 5. Describe a polyatomic ion such as hydroxide. 6. Describe the properties of ionic compounds. 9.2 Metallic Bonds 1. Describe and diagram the sea of electron model for the bonding in metals. 2. Describe the properties of metals. 10 Chemical Names and Formulas Chapter 7, Sections 1 and 3 1. Explain why a standardized nomenclature system is necessary. 2. Relate a formula unit of an ionic compound to its composition. 3. Write formulas for ionic compounds given the compound s name. 4. Write names for ionic compounds given the formula. 5. Write formulas for covalent compounds given the compound s name. 6. Write names for covalent compounds given the formula. End of Fall Term 5

6 10.1 Covalent Bonding and Molecular Compounds 1. Explain how non metals share electrons to form covalent bonds. 2. Describe the relationship between bond length and energy. 3. Use electron configurations and Aufbau diagrams to show the formation of simple covalent bonds. 4. Write electron dot diagrams for main group elements. 5. Use electron dot diagrams to write Lewis structures and structural formulas for simple molecules with single, double, and triple covalent bonds Molecular Geometry 1. Explain how electron pairs around a central atom influence the shape of a molecule. 2. Use VSEPR theory to predict the shape of simple molecules. 3. Describe the approximate bond angles in simple molecules. 4. Identify chiral carbons in a molecule. 5. Explain how a chiral carbon leads to stereoisomers. 6. Explain how stereoisomers can have different physiological properties Intermolecular Forces 1. Use electronegativity to describe the dipole in a covalent bond. 2. Explain and diagram dipole-dipole forces. 3. Predict the polarity of simple molecules. 4. Describe and diagram the similarities and differences between dipole interactions, hydrogen bonding, and dispersion forces. 5. Use the types of intermolecular forces present in molecules to explain their relative melting and boiling points. 11 Chemical Reactions 1. Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred. 2. Describe a chemical reaction at the macroscopic level. 3. Describe a chemical reaction at the particulate level. 6

7 4. Draw particle diagrams by hand or using a computer to represent a chemical reaction. 5. Describe a chemical reaction at the symbolic level of a chemical equation. 6. Write balanced chemical equations. 12 Qualitative Analysis 1. Describe aqueous solutions. 2. Draw particle diagrams of aqueous solutions. 3. Write complete and net ionic equations for chemical reactions in aqueous solution. 4. Using solubility trends, predict whether a precipitate will form when two aqueous solutions are combined. 5. Given experimental evidence, deduce the identity of unknown aqueous solutions. 13 Stoichiometry 1. Describe the types of relationships indicated by a balanced chemical equation. 2. State the mole ratios from a balanced chemical equation. 3. Draw particle diagrams reflecting the particle ratios in a balanced chemical equation. 4. Describe the steps used in solving stoichiometric problems. 5. Solve stoichiometric problems. 6. Identify the limiting reactant in a chemical reaction. 7. Identify the excess reactant in a chemical reaction and calculate the amount remaining after the reaction has come to completion. 8. Calculate the masses of reactants and products for a chemical reaction. 9. Explain the difference between theoretical and empirical yield. 10. Calculate the theoretical yield for a chemical equation. 11. Determine the percent yield for a chemical reaction. 7