Chem 1211 1st Edition Lecture 3 Outline of Last Lecture I. States of MatterII. DefinitionsIII. Phase ChangesIV. PropertiesOutline of Current Lecture I. SubstancesII. MixtureIII. SI UnitsIV. NumbersV. Arithmetic FunctionsVI. Unit ConversionsCurrent LectureI. Substancesa. Pure substance- matter with both definite and constant composition with distinct chemical propertiesi. Element- cannot be chemically interconverted or broken down into simpler substancesII. Mixturea. Compound- a thing that is composed of two or more separate elements; a mixturei. Homogeneous mixture- uniform in composition; can’t tell that it’s a mixtureThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.ii. Heterogeneous mixture- made up by two or more different substance which are (mixed) together but are not combined chemicallyIII. SI UnitsQuantity Unit Symbola. Length b. Meters c. Md. Mass e. Kilograms f. Kgg. Time h. Seconds i. Sj. Current k. Ampere l. Am. Temperature n. Degrees Kelvin o. Kp. Amount substance q. Mole r. molIV. Numbersa. Mega- 1,000,000b. Kilo- 1,000c. Deka- 10d. Deci- 0.1e. Centi- .01f. Milli- .001g. Micro- .000001h. Nano- 1x10^-9i. Pico- 1x10^-12V. Arithmetic Functionsa. Use numbers with all significant figuresb. Do the mathc. Apply rulei. When multiplying/dividing, the final answer should have the smaller # of significant figuresii. When adding/subtracting, the answer should have the least number of digits behind the decimal IV. Unit Conversiona. 13.37 cm= ? inchesb. We know 2.54 cm = 1 inch (EXACTLY)c. 13.37 cm x (1 inch/2.54 cm) = 5.26
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