REVIEW TOPICS FOR EXAM 2 (CHAPTERS 3 AND 4) BEST METHOD FOR STUDYING As you read Chapter 3.1, go to Chapter 3.1 in this Review Topics Packet along with your class notes. Repeat the process with the remaining chapters and sections. When you are through with reading/reviewing, go to the Review Problems Packet. TEST STRUCTURE: 1 HOUR, 30 MINUTES Part 1: Chemical Names/Symbols, Naming Covalent Compounds, Definitions, Memorized Materials Part 2: Everything else. You will a periodic table for Part 2 only. You will also get a list of relevant equations for Part 2 only. DEFINITIONS/VOCABULARY Like Exam 1, definitions are your responsibility. I can supply the definition, and you will have to supply the vocabulary word. I can give you the vocabulary word, and you will have to supply the definition. Sometimes I will give you examples of a vocabulary word that you need to identify. Sometimes I will ask you to supply examples for a vocabulary word I can ask matching, true/false, and fill-in-the-blank type questions. Chapter 3 You are responsible for all words in bold throughout Chapter 3. The Key Terms exercise on pp. 92 93 will be helpful in studying the Chapter 3 vocabulary. Chapter 4 You will be responsible for all words in bold throughout Chapter 3, except for... Chapter 4, Section 11: Heisenberg Uncertainty Principle The Key Terms exercise on p. 126 will be helpful in studying the Chapter 4 vocabulary. Special Terms (in your notes, but not in your textbook): A column on the periodic table is known as a group or family A row on the periodic table is known as a period Miscible/miscibility vs. immiscible/immiscibility (from lab): you are responsible for recognizing an example for this term, as well as the definition. You will not be expected to provide an example of miscible or immiscible liquids. Carryovers from Exam 1 All metric prefixes and metric relationships (1000 mg = 1 g, 1000 g = 1 kg, 1 dm 3 = 1 L, etc ) For calculations, the answers must have the correct number of significant digits. Density: you must know how to use density as a conversion factor. You must know the value for the density of water, including units. Page 1 of 7
CHAPTER 3, SECTION 1: PHYSICAL STATES OF MATTER Know the three physical states and their properties. Know the terms for all six changes of state. When given an example for a change in state, be able to supply the correct vocabulary word. Be able to provide an example of each of the six changes in state. CHAPTER 3, SECTION 2: ELEMENTS, COMPOUNDS, AND MIXTURES Heterogeneous mixtures: know the definition and be able to recognize/provide examples. Homogeneous mixtures: know the definition and be able to recognize/provide examples. Alloys: Know the definition and be able to recognize examples. You will not be asked to provide examples. Compare/contrast the properties of homogeneous mixtures and heterogeneous mixtures. Compare/contrast the terms mixture and substance. Compounds: know the definition and be able to recognize/provide examples. Elements: know the definition and be able to recognize/provide examples. Compare/contrast the properties of elements and compounds. CHAPTER 3, SECTION 3: NAMES AND SYMBOLS OF THE ELEMENTS Know the names and chemical symbols of the memorized elements list. For chemical symbols with two letters, make sure the first letter is capitalized and the second letter is lower- -case. Capitalized second letters will count as spelling errors. CHAPTER 3, SECTION 4: METALS, NONMETALS, AND METALLOIDS SEMIMETALS Know the location of the metals, metalloids, and nonmetals. You will be given a periodic table with a region shaded in. You must state whether the region indicates: metals, nonmetals, semimetals, transition metals, inner transition metals, post-transition metals, alkali metals, alkali earth metals, halogens, and noble gases. You are not responsible for actinides, lanthanides, or trans-uranium elements Know that the atomic number (the number of protons in an element) defines the element. Page 2 of 7
CHAPTER 3, SECTION 5: COMPOUNDS AND CHEMICAL FORMULAS Know the Law of Definite Composition You will be expected to know how to use percent-by-mass as conversion factors. Know the term molecule, even though we did not go over it in class. Be able to recognize examples of molecules when given chemical formulas. You will not be asked to supply definitions of molecules. Know the term chemical formula. When given a chemical formula, state the number of atoms of each element based upon the subscripts. CHAPTER 3, SECTION 6: PHYSICAL AND CHEMICAL PROPERTIES Know the term physical property. On a list of properties, be able to identify the physical properties on the list. Know the term chemical property. On a list of properties, be able to identify the chemical properties on the list. CHAPTER 3, SECTION 7: PHYSICAL AND CHEMICAL CHANGES Know the definition of a physical change and be able to provide three examples. Note: You may only list one phase change Sample Question: List three examples of physical changes: Student 1: crushing an aluminum can, evaporating water, and dissolving sugar in water Score: 6 points (full credit) Student 2: evaporating water, melting iron, and subliming dry ice Score: 2 points out of 6, (phase change only counts once, you listed three) Know the definition of a chemical change and be able to provide three examples. When given a list that contains physical changes and chemical changes, be able to identify/label them. Page 3 of 7
CHAPTER 3, SECTION 8: LAW OF CONSERVATION OF MASS Know the definition of the Law of Conservation of Mass (in word form and in chemical equation form. Word form: Mass can neither be created nor destroyed during a chemical reaction. Chemical Equation Form: total mass of reactants = total mass of products You will be given a chemical equation. The mass of all but one of the substances in the chemical equation will be given. You will be asked to determine the missing mass value. You will not be required to show your work for these problems. However, I do give partial credit for work shown (except in Multiple Choice questions). Caution: For multiple choice questions, I am notorious for including correct numerical answers with incorrect sigdigs and/or incorrect units. CHAPTER 3, SECTION 9: POTENTIAL AND KINETIC ENERGY You are not responsible for Potential or Kinetic Energy CHAPTER 3, SECTION 10: LAW OF CONSERVATION OF ENERGY You are not responsible for the Law of Conservation of Energy CHAPTER 4, SECTION 1: DALTON MODEL OF THE ATOM (DALTON S ATOMIC THEORY) You do not need to know Dalton s biographical information or his dates. Know the five parts of Dalton s Model of the Atom Know which ones are correct. Know which ones have been proven incorrect, and how they were proven incorrect. CHAPTER 4, SECTION 2: THOMSON MODEL OF THE ATOM (CRT EXPERIMENT/PLUM PUDDING MODEL) You do not need to know Thomson s biographical information or his dates. Know how the CRT Experiment led to the Plum Pudding Model of the Atom You might have to sketch part of the CRT Experiment under the following conditions: Empty CRT CRT with a small amount of any vapor in it. CRT with a small amount of any vapor in it AND an external electric field. The CRT tube itself, the cathode, anode, and power source will always be drawn/labeled for you. Know which part of Dalton s Atomic Theory this experiment disproved. Page 4 of 7
CHAPTER 4, SECTION 3: RUTHERFORD MODEL OF THE ATOM (GOLD FOIL EXPT/NUCLEAR MODEL) You do not need to know Rutherford s biographical information or his dates. Know how the Gold Foil Experiment led to the Nuclear Model of the Atom You might have to sketch part of the Gold Foil Experiment, assuming the Plum Pudding Model was correct. Gold Foil Experiment: what really happened. The parts of the Gold Foil Experiment will be drawn for you and labeled. You will only have to draw the paths of the alpha particles. Know which part of Dalton s Atomic Theory this experiment disproved. Know the symbols for proton (p + ), neutron (n o ), and electron (e ). Know the charges of the proton, neutron, and electron. Know the relative masses of the proton, neutron, and electron. CHAPTER 4, SECTION 4: ATOMIC NOTATION Know how the atomic number (Z) relates to an element. Know how the mass number (A) relates to the isotope. A Be able to interpret atomic notation: Z X Know the definition of isotopes. Be able to recognize examples of isotopes. You will not be expected to provide examples of isotopes. Be able to fill in information about the atomic notation, the isotope name, A, Z, #p +, #n o, and e. When given two out of three of the following (#protons, #neutrons, mass number), I will not make you show your work (simple addition or subtraction) for determining the unknown quantity. CHAPTER 4, SECTION 5: ATOMIC MASS When given the mass and the abundance of each isotope of an element, determine its atomic mass. Remember that regardless of the sigfig rules that I want your calculated answers to have a total of two significant digits after the decimal point. Remember that you will have to show all work as demonstrated in class including units through each step. Page 5 of 7
CHAPTER 4, SECTION 6: THE WAVE NATURE OF LIGHT Know the term electromagnetic spectrum. The textbook uses the terms radiant energy spectrum and continuous spectrum. Know the term and the variable for the wavelength of a wave (including units). From a diagram, be able to determine the value (including units) for the wavelength of a wave. Know the term and the variable for the frequency of a wave (including units). From a diagram, be able to determine the value (including units) for the frequency of a wave. Know the order of types of radiation: From lowest energy to highest energy (or vice versa) From longest wavelength to shortest wavelength (or vice versa) From lowest frequency to highest frequency (or vice versa) Know the term continuous spectrum You are not responsible for knowing that the visible spectrum is from 400 nm to 700 nm. CHAPTER 4, SECTION 7: THE QUANTUM CONCEPT OF THE ATOM Know the term photon Know the diagram and relevant definitions/keywords for Light by Emission We will not discuss this section in depth in any other way. You will only be tested on this in relation to the Bohr Model of the Atom (Chapter 4, Section 8). CHAPTER 4, SECTION 8: THE BOHR MODEL OF THE ATOM Explain how quantized energy led to the Bohr Model of the Atom. Explain the emission line spectrum in terms of the Bohr Model of the Atom. Lab Related: If given several sets of emission line spectrum samples and one unknown, be able to determine which substances are not present in the unknown sample. CHAPTER 4, SECTION 9: ENERGY LEVELS AND SUBLEVELS Know the types of levels and sublevels of the atom. (Do the reading!) Be able to recognize s-orbitals, p-orbitals, d-orbitals, and f-orbitals. You will not have to draw them. Be able to state the maximum number of electrons that can occupy any level or sublevel. CHAPTER 4, SECTION 10: ELECTRON CONFIGURATION You can read this section, but Appendix 6 and the Lecture Notes will be more helpful. For any atom, be able to write the full electron configuration. You may not write the abbreviated electron configuration. Page 6 of 7
CHAPTER 4, SECTION 11: QUANTUM MECHANICAL MODEL OF THE ATOM Aside from the definition of orbital, you will not be asked anything about this section. I will only teach this section in relation to where are these s, p, d, f orbitals coming from? I will not test you on this information...not even as extra credit questions. LEWIS STRUCTURES (LAB EXPERIMENT 11) You will be responsible for AXE Notation and names (tetrahedral, trigonal pyramidal, bent, and linear). You will be responsible for writing Lewis Dot Structures for atoms and for molecules. (I will not give you ions on this Exam except for Extra Credit maybe.) PERIODIC TRENDS You will NOT be responsible for periodic trends (atomic radius, electronegativity, ionization energy, electron affinity, or metallicity). SOLUTIONS: %(W/W) AND %(V/V) On Part 1 of the Exam (the memorization portion), you may be asked to write the equation for determining concentration %(w/w) or %(v/v) of a solution. For all other parts, you will be given the equation. NAMING COVALENT COMPOUNDS Will be on Exam 2 DEFINITIONS LIST Chapter 3: alloy, atom, atomic number, chemical change, chemical formula, chemical property, compound, deposition, ductile, element, heterogeneous mixture, homogeneous mixture, law of conservation of mass, malleable, metal, molecule, nonmetal, periodic table, physical change, physical property, physical state, semimetal, sublimation, substance, freezing, vaporization, melting, condensation You are not responsible for: law of conservation of energy, kinetic energy Chapter 4: atomic mass, atomic mass unit (amu), atomic notation, atomic nucleus, atomic number (Z), Bohr atom, continuous spectrum, electron (e ), electron configuration, emission line spectrum, energy level, energy sublevel, frequency, isotope, light, mass number (A), neutron (n 0 ), orbital, photon, proton (p + ), quantum mechanical atom, visible spectrum, wavelength. The radiant energy spectrum is what scientists call The electromagnetic spectrum. You are responsible for knowing all of the types of radiation in order. You are not responsible for uncertainty principle Page 7 of 7