ch 1 - • • • • • • CHM-114 Spring 2007...

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Unformatted text preview: • • • • • • CHM-114 Spring 2007 Instructor: John Holloway Office: PS C-255 Office Hours: M: 1:40 - 3:30, Th: 1:45 - 3:00 Phone: 965-6907 E- Mail: Use Blackboard site EUse Learning Resource Center (H-137) CHM-114 Spring 2007 CHM 114 General Chemistry for Engineers. (4) Emphasis toward engineering Emphasis Students without high school chemistry or chemical engineering majors Students must enroll in the CHM 113, 116 sequence instead of CHM 114. must 3 hours lecture 1 hour discussion 2 hours lab. hours Prerequisites: MAT 106 (or 3 semesters of high school algebra) MAT 1 year of high school chemistry. Who I am: • Geologist, Geochemist, Environmental Chemist Who I am: • Geochemist, Environmental Chemist • CHM-114 Spring 2007 CHM-114 Spring 2007 Syllabus Syllabus - look at it! • lecture schedule • lab schedule lab • • Note that labs start this week !! Note Quiz and Lab Quiz & Lab All sections start in room PS H - 231 400 points 400 200 * Course Point Distribution • 4 One Hour Exams One • Final Exam • Labs 150 Course Grade Distribution Approximate Grades Grade average ≥ 88% A ≥ 76% B ≥ 64% C ≥ 52% D 52% or less E • Quizzes (12 or more) 150 • TOTAL POINTS 900 Your TA • • Is in charge of Quiz & Lab Your Teaching Assistant • Your biggest help in this class !! • Treat her/him with great respect • They can remove you from lab, hence this class • • Lab Manual - Bauer, Birk & Sawyer (2000) Required Materials Text Book: Brown, LeMay & Bursten Chemistry, The Central Text Chemistry, Science 10th Edition Science • • Laboratory Inquiry in Chemistry Need the lab manual this week. Goggles - Need by next week. Bound carbonless notebook for lab (one for each group member) Need by next week. Need Group Work • Lab/lecture group assignments to be made during the first lab meetings this week meetings • After groups are assigned, the group should sit together during lecture to facilitate discussions and participate in group quizes lecture Suggested Homework Problems • Chapter one: 1, 3, 5, 7, 11, 19, 21, 23, 35, 37, 39, 41, 43, 45, 47, 53, 58, 64 • Chapter two: 1, 3, 5, 13, 15, 17, 19, 23, 29, 33, 35, 37, 41, 42, 51, 53, 55, 57, 43, 45, 47, 49, 59, 83, 86 • Chapter three: 1, 3, 4, 5, 7, 11, 13, 15, 17, 21, 23, 27, 29, 31, 33, 35, 39, 43, 45, 55, 57, 59, 63, 65, 66, 67, 69, 71, 75, 77, 81, 83, 85, 89 67, • • Chapter four: 1,, 3, 5, 7, 8, 11, 13, 15, 17, 19, 21, 29, 33, 35, 37, 39, 41, 45, 47, 49, 53, 55, 57, 59, 65, Chapter 1 67, 69, 73, 91, 93 67, • 107 problems / 4 weeks = 27 per week CHM-114 Spring 2007 Chapter 1 Matter and Measurement • 1.1 The Study of Chemistry • Chemistry is the study of properties of matter and the changes it undergoes. undergoes. • What is matter ? What matter • Has mass; occupies space; made up of ~100 elements; elements combine to form molecules (compounds if they contain more than combine one element) one Chapter 1 Matter and Measurement Chemistry is about bonding between atoms! • Bonding is about electrons! • So chemistry is about electrons • The number of electrons is determined by the element element • Let’s look at elements Let’s • The Periodic Table Elements and compounds • • Compounds contain more than one element. They always have the Classifications of Matter Classify these as Classify same composition, regardless of source (law of constant same composition; law of definite proportions). composition; • Make a list of things (and their parts) found in the classroom. • solid, liquid, or gas • homogeneous or heterogeneous • pure substances and mixtures • elements or compounds • How do you place them into these classifications? Classifications of Matter • Matter can be placed in these classes both on the basis of macroscopic properties, and by considering their atomic/molecular macroscopic distributions. distributions. Classification of Matter Method to classify matter Classify • • • • mixtures pure substances elements compounds Physical and Chemical Changes Units of Measurement • Is this a physical or a chemical change? • Explain your reasoning. Manipulate numbers • Multiply and divide 5 x 103 and 2 x 10-4 (5 x 103) x (2 x 10-4) = 5 x 2 x 103 x 10-4 = 10 x 10-1 = 1 x 100 = 1 • • What is the size of an atom? of Earth? How do we express such numbers conveniently? • Place the following numbers in order of increasing value: Place (5 x 103) / (2 x 10-4) = 5/2 x 103/10-4 = 2.5 x 107 • • • • • Derived Units: Density Density: d = mass / Volume units of g/mL or g/cm3 What causes substances to have different densities? What Density is a fundamental property of matter ! Density Density • Carbon dioxide gas is more dense than helium gas. Why? • Water is more dense than ice. Why? Density • Why is the density of a solid usually greater than that of its liquid, which is greater than that of its gas? which 1.5 Uncertainty in Measurement Significant Figures The difference between precision and accuracy: • What are significant figures? Why are they important? When do you need to worry about them? worry Procedure for significant figures Procedure Count all non-zero digits. What about zeros? CHM-114 Spring 2006 • • • • • • • • Instructor: John Holloway Office: PS C-255 Office Hours: M: 1:40 - 3:30, Th: 1:45 - 3:00 Web Office hours: Tu 3:00 - 5:00, W: 2:00 - 3:00 Phone: 965-6907 E- Mail: [email protected] Class website: http://my.asu.edu Class Learning Resource Center (H-137) Learning ...
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This note was uploaded on 11/07/2009 for the course CHM 114 taught by Professor Aksyonov during the Spring '08 term at ASU.

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