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Significant Figures & Scientific Notation
Unit 1 Significant Figures & Scientific Notation
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Significant Figures – The accuracy of a measurement.
Rule # 1 All Non-zero numbers are significant. 235 mol mL kg (3 Sig figs) (2 Sig figs) (5 Sig figs)
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Captive zeros are significant – zeros between non-zero numbers.
Rule # 2 Captive zeros are significant – zeros between non-zero numbers. mm s g (6 sig figs) (5 sig figs) (3 sig figs)
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Rule # 3 Zeros after nonzero numbers with a decimal present are significant. 59.00 g kL m (4 Sig figs) (2 Sig figs) (5 Sig figs)
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Rule # 4 Zeros that act as place holders are not significant. -Zeros to the left of nonzero numbers or to the right of nonzero number when NO decimal is present. 100 L mL Pa (1 Sig figs) (2 Sig figs) (3 Sig figs)
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Multiplication and Division
Perform calculation Round the answer to the same number of significant figures as the least amount of sig figs in the problem. 1.) 3.2 x 11.0 = 35.2 = 35 2.) 7456 x 3.56 = = 26500
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Practice: 2.2 x 3.12 = x 3.10 = 3. 96 =
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Scientific Notation There are atoms in 12 grams of carbon. The mass of a proton is kg. Who wants to write all those #’s??? Scientific Notation is a short hand way to write very large or very small #s.
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How to write #’s in Scientific Notation
1- Move the decimal so that only one sig fig is to the left of it 2- Remove all non significant zeros 3- Multiply the rest of the # by 10, and raise it to the power equal to the # of times you moved the decimal (1.0 x 10x) 4- The way you move the decimal depends on whether it is a positive or negative power Decimal moves right = Negative power (the # was less than 1.0) Decimal moves left = Positive power (the # was greater than 1.0)
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Scientific Notation Practice
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