Chem 1010 Week 2 notes.
Chem 1010 Week 2 notes. CHEM 1010
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This 4 page Class Notes was uploaded by Chase Bobier on Thursday February 4, 2016. The Class Notes belongs to CHEM 1010 at Middle Tennessee State University taught by Tammy J Melton in Fall 2015. Since its upload, it has received 54 views. For similar materials see Introductory General Chemistry I in Chemistry at Middle Tennessee State University.
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Date Created: 02/04/16
Chemistry 1010 notes Chase Bobier 1-26-16, Week 2 Notes Important Terms Things You Need to Know The WONDERFUL Metric System! The metric system is the system of measurements used in the scientific community. The neat thing about the metric system is that all measurements are easily relatable to each other due to the fact that all metric measurements are based on multiples of ten. Here are some relations that will really help with metric conversions! 1mL = 1g 2 1cm = 1g Remember this for later in this course, they really are important. Base Metric Units The metric unit of weight is the gram, abbreviated as a lowercase g The metric unit of volume is the liter, abbreviated as an uppercase L The metric unit of length is the meter, abbreviated as a lowercase m As these base units change in size, prefixes are used to make it easier to recognize the size of the measurement. These are detailed in the following table. Prefix Abbreviation Meaning Decimal Equivalent Kilo k 103 1,000 deka da 101 10 -1 deci d 10-2 0.1 centi c 10 0.01 milli m 10-3 0.001 micro μ 10-6 0.000001 -9 nano n 10 0.000000001 Density Density is the amount of matter contained in a given space. Density is found by dividing the mass of a sample by the volume of the sample. (The equation looks like this: Mass g D= Volume ) and is shown as mL . The definition of weight is: the force of Earths gravity on and object. The definition of Mass is: the amount of matter in a sample; its resistance to acceleration due to gravity. Significant Digits Significant digits are essentially just the digits in a result that matter. Numbers 1 through 9 are always significant Trailing zeroes (zeroes at the back of a number) are significant Buried zeroes (zeroes in between actual numbers) are significant Leading zeroes (zeroes in front of a number) are not significant. Example: 0.00470030 Rules of significant digits in Addition and Subtraction The number of significant digits in the answers decimal is equal to the least amount of significant figures in the data Example: 7.939+6.26=14.20 If you did this on your Ti-30Xa, you would have gotten 14.199, but that is incorrect. Look at 6.26, it only has two sig. digits after the decimal, making it the limiting piece of data. Rules of significant digits in Multiplication and Division The number of sig.digits in the answer is equal to the least number of sig.digits in the data. Example: 2.44 cm/8.321cm=0.293cm When you do this problem on the Ti-30Xa, you get an answer of 0.293233986, but look at 2.44: it only has three total sig.digits, making it the limiting piece of data.
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