science_notes_day_1.pdf Che 101LLR
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This 3 page Class Notes was uploaded by Brittney Lillie on Monday September 19, 2016. The Class Notes belongs to Che 101LLR at University at Buffalo taught by Jim Atwood in Fall 2016. Since its upload, it has received 4 views. For similar materials see General Chemistry in Chemistry at University at Buffalo.
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Date Created: 09/19/16
Jim Atwood Office hours NSC 556 Tuesday 11:0011:59 Wednesday 10:0011:00 By appointment use email HW P1 8/30/16 A. Definitions B. Significant Figures C. Dimensional Analysis D. Classification 1. What is Chemistry? a. Synthesis of new materials i. Medicines ii. Fabrics iii. Food iv. Electronic Materials b. Control changes of matter i. Pollution Removal ii. Energy c. Identify and Concentration of substances i. Hg levels ii. PH of natural waters – Acidity iii. Physiologically active compounds Chemistry is the Study of Matter 2. Historical perspective a. Crafts i. Brewing ii. Tanning iii. Dyeing (Practical – Chapters 3,4,5,10) b. PhilosophyNature of Matter c. Greek Philosophers > Understand (Theoretical – Chapters 6,7,8,9) C. Scientific Method 1.Observation 2.Theory 3. New Observations 4. New Theory B. Significant Figures – Uncertainty in Measurements 1. Rules for a number a. All nonzero digits are significant 457 = 3 significant figures 0.25= 2 significant figures b. Zeros between nonzero digits are significant 1005= 4 significant figures 1.03= 3 significant figures c. Zeros to the left of the first nonzero digit are not significant 0.02 = 1 significant figure 0.0026= 2 significant figures d. Zeros at the end of the number to the right are significant 0.2200=4 significant figures 3.0 = 2 significant figures 2. Rules for Calculations a. In addition of subtraction one reports the result to same number of decimal places as the term with the fewest significant figures 20.41+1.322+83=104.732 Then rounds to 105 because of significant figures b. In multiplication and division one reports the result with no more significant figures then the measurement with fewest figures. Ex. 6.221∗5.2=32.3492 Then rounds to 32 because of significant figures C. Dimensional Analysis – Unit Convention Number X 1 = Numbers Ex. 1. I weigh 180lb, how many kilograms? 1.00kg=2.205lb 180lb×1kg÷2.05lb=81.6 kg 2. A sign says 40.km/h, how many mile/h? 40km miles h ×0.621mi÷1.00km=25 h D. Classification of Matter Gas, Liquid, Solid Heterogeneous – Not uniform throughout Homogeneous – Uniform throughout
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