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General Chemistry Review plan for Midterm/Week of January 16, 2012 Please note that all page references refer to the course textbook. Dr. L. O’Reilly The midterm exam will consist of multiple choice questions, numeric responses, short answer questions and problems. The format will be the same as all of the in-class chapter tests given to date. The questions will include some chapter test questions already given and new questions. The material that will be tested includes information contained in the textbook and given in class from chapters 1 and 2, & 4 through and including any material covered in chapter 9. Please bring a #2 pencil to the test. To study for the midterm, YOU SHOULD: Review all past assignments, including in-class worksheets. Review your notes. Review past quizzes and chapter tests. Review all class handouts (Vocabulary; how-to guidelines; Aufbau principle & energy levels) Review the vocabulary (highlighted words) in each chapter. Review the concepts and questions noted below. Do the suggested practice problems (if noted below). Chapter 1 Topics by section Section 1.1 What are the traditional areas of study in chemistry? Why is the area of chemistry important to study? Section 1.2 What are some of the technologies that have resulted from the study of chemistry? Section 1.3 What are the steps involved in the scientific method? Section 1.4 What is an effective approach to solving a problem? Suggested Problems: pg #/Q# Pg. 5: Q6 Pg. 28: Q46, 47, & 48 Pg. 26: Q29; Pg. 28: Q51 Chapter 2 Vocabulary words (in bold throughout chapter) and: Topics by section 2.1 Identification of Extensive vs. Intensive Properties The three different states of matter Characteristics of each state of matter 2.2 Mixtures & the two types of mixtures 2.3 Distinction between an element and a compound Distinction between a substance and a mixture 2.4 Distinction between a chemical property and a physical property Distinction between a chemical change and a physical change Law of conservation of mass Suggested Problems: pg #/Q# Pg. 55/Q39 Pg. 55/Q43, 44 Pg. 37/Q6 Pg. 55/Q50; Pg. 56/Q72 Pg. 56/Q75 Pg. 56/Q73 Pg. 56/Q73; pg. 57/Q76,77,78 Pg. 57/Q80 Chapter 4 Vocabulary Words (in bold throughout chapter) and: Topics by section Suggested Problems: pg #/Q# 4.1 Contributions of Democritus & Dalton Pg. 104/Q1, Q2; Pg. 122/Q37 toward the model of the atom Pg. 104/Q6 Relative size of an atom Instrument used to observe an atom 4.2 Pg. 109/Q11; Pg. 122/Q41 What are the three types of subatomic particles? What are their properties? Pg. 109/Q12;Pg. 122/Q43 Roles that Thompson, Millikan, Goldstein, & Chadwick played in identifying the three types of subatomic particles Pg. 109/Q13 to 15 Rutherford Atomic Model Topics by section 4.3 What does the atomic number of an element represent? What subatomic particles are taken into account in an element’s atomic mass? What is an isotope? Calculate the atomic mass of an element using a weighted average Suggested Problems: pg #/Q# Pg. 113/Q16 & 17; Pg. 122/Q49 Pg. 114/Q18 & 19; Pg. 122/Q50 Pg. 122/Q52 Pg. 122/Q53; Pg. 119/Q25 Chapter 5 Vocabulary words (in bold throughout chapter) and: Topics by section 5.1 Bohr’s model of the atom; how it compares to Rutherford’s Model Principle energy levels and sublevels; shapes of sublevels Quantum mechanical Model 5.2 Rules for writing electron configurations (Aufbau Principle, Pauli Exclusion, Hund’s rule) Elements that are the exception to the rules when filling sublevels 5.3 Characteristics of Light as a wave (amplitude, wavelength, frequency) Electromagnetic Spectrum & relationship between wavelengths and energy, frequency Energy associated with light (Planck’s constant problems) Photons & the photoelectric effect (light as a particle) Suggested Problems: pg #/Q# Pg. 132/Q1 Pg. 132/Q4; Pg. 155/Q34 Pg. 152/Q36-38; 40; Pg. 153/Q56 Pg. 152/Q45; Pg. 154/Q68 Pg. 152//Q47 Pg. 153/Q64; 66 Pg. 154/Q70 Chapter 6 Vocabulary Words (handout & Word activity); Periodic Table Activities done in class; Name Origins of Elements (by people, place, Latin/Greek origin) and: Topics by section 6.1 Organizing principles of the periodic table: past and present Three classes of elements; location on periodic table; properties of each type 6.2 Groups/Family names Horizontal rows = periods Representative elements 1A -8A Why members of a family are chemically the same S, p, d & f blocks in periodic table 6.3 Trends in atomic size Trends in ionization energy Trends in ionic size Trends in Electronegativity Formation of ions Suggested Problems: pg #/Q# Pg. 166/Q2, 3 Pg. 166/Q4,5,6,7 Pg. 173/Q14,15,16,17 Pg. 182/Q18 Pg. 182/Q20 Pg. 182/Q21 Pg. 182//Q22; Pg. 186/Q45 Chapter 7 Vocabulary Words (Handout & Word Activity); How to Write a Winning Ionic Formula and: Topics by section 7.1 How to determine the number of valence electrons: Representative elements Electron Dot (Lewis)Structures Octet Rule & Ion Formation: Loss or Gain of Electrons (or How do I become Noble?Let me count the ways!) Suggested Problems: pg #/Q# Pg. 214/Q27, 28 Pg. 214/Q29 Pg. 214/Q32, 33, 34, 36 Topics by section 7.2 Ionic Compounds are Electrically Neutral: Writing Formula Units Properties of Ionic Compounds: high melting point, good conductor of electricity, held together by ionic bonds, metal & nonmetal components Suggested Problems: pg #/Q# Pg. 214/Q35, 43, 44 LAB (Covalent vs. Ionic); Pg. 214/Q46 7.3 Crystalline Structure of Metals Alloys you may be familiar with Pg. 216/Q73 Pg. 216/Q75 Chapter 8 Vocabulary; How to write Electron Dot (Lewis) Structures for Compounds; and Topics by section 8.1 Molecules & Molecular Formulas Nobility now means sharing electrons (covalent bonds) Suggested Problems: pg #/Q# Pg. 256/Q40,41 Pg. 256/Q45 8.2 Once again, the Octet Rule rules! Different representations of molecules & the information they tell you Electron Dot Structures (Lewis Structures) Single to triple covalent bonds Polyatomic atoms Coordinate covalent bonds Bond dissociation energy Pg. 173/Q14,15,16,17; Pg. 256/Q57 Pg. 256/Q49,58 Pg. 256/Q47 Pg. 256/Q56 Topics by section 8.3 VSEPR Theory Shapes of molecules/bond angles/example molecules Suggested Problems: pg #/Q# 8.4 Electronegativity & types of bonding Intermolecular forces: Hydrogen bond, van der Waals Forces Properties of a Molecular Compound: low melting point, sharing of electrons, poor conductor of electricity, weak intermolecular forces Pg. 257/Q64, 65 Pg. 257/Q66,67,68 LAB (Covalent vs. Ionic)