Chem LectureChapter One- Introduction to ChemistryStates of Matter- GLS, properties..etcTypes of Energy- PE KE, equations, what are they, how they changePhysical vs Chemical ChangesBasic data analysis- accuracy and precision (difference between the two)UNITS, uncertainty( difference in accuracy of measurements) 10.24, four is the uncertain number( an estimation)Significant Figures-Any non-zero digit, 1-9= significant alwaysZeros- trailing zero with a decimal point= 4.30 mL(0 is significant)Sandwiched = 307 g Examples- 7.543, 4 sig figures 0.52, 2 0.9087, 4 34.0, 3 1.2x106 , 2 10, 1 -----10. =2 0.000004, 1Adding and Subtracting- SF is determined by the number of decimal places 13.4+0.066+1.02= 14.486----14.5(4.35-0.137)g/10.83mL----4.213/10.83—4.21g/10.83mL=0.388374g/mL=0.389g/mLMultiplying and Dividing- SF is determined by the lowest number of significant figures that you are using 0.235x450x1.367=144.56025----140 Conversions K H D (base unite)d c m (king henry drank _____ during class Monday)Dimensional Analysis—watch SF and always make sure that units
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