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Chemistry Notes Significant Figures & Scientific Notation
Describing Numbers We can describe and use numbers in several different ways. These include scientific notation and significant figures.
Scientific Notation In scientific notation, a number is written as the product of two numbers: a coefficient and 10 raised to a power.
Examples: Convert to or from Scientific Notation: 2.41 x 102 241 =662 .0034 241 = 6015 = = = 6.62 x 102 = 3.4 x 10-3 =
Significant Figures Significant figures are the numbers in a measurement that “matter”.
Rules for determining Significant Figures 1Rules for determining Significant Figures 1. All non-zero digits are significant. 1, 2, 3, 4, 5, 6, 7, 8, 9
2. Zeros between non-zero digits are significant2. Zeros between non-zero digits are significant. (AKA captive or trapped zeros) 102 7002 3 sig figs 4 sig figs
3. Leading zeros (zeros at the beginning of a measurement) are NEVER significant.00542 0.0152 3 sig figs 3 sig figs
4. Trailing zeros (zeros after last integer) are significant only if the number contains a decimal point. 210.0 4 5240 3 3 0.860 5240. 4 3 5240.0 5 524000
5. All digits in the coefficient are significant in scientific notation.2.1 x 10-5 6.02 x 1023 2 3
6. Exact numbers have unlimited Significant FiguresExamples: 1 dozen = exactly 12
Examples: How many significant digits do each of the following numbers contain:a) d) b) e) c) f) x 1023 2 2 2 5 3 4
Rounding: 5 round up < 5 round down (don’t change) Examples:Round to 1 significant digit = Round to 3 sig. digs. = Round to 2 = Round 65,002 to 2 sig. digs. = 40 61.6 0.016 65,000 or 6.5 x104
Addition and Subtraction– The measurement with the fewest decimal places to the right of the decimal point determines the number of decimal places in the answer.
Examples: Solve using correct significant figures 45.756 m + 62.1 m =
Multiplying and Dividing Measurements- The measurement with the fewest total significant figures determines the number of significant figures in the answer.
Examples: Solve using correct significant figures:3.43 m X m = m X m = 45.01 m / m = 22.0 m2 m2 55 m2 m2 20. m2
Chapter 2 – Scientific Measurement
Uncertainty in Measurements
Calculations with Significant Figures
Rules For Significant Digits
Aim: How can we perform mathematical calculations with significant digits? Do Now: State how many sig. figs. are in each of the following: x 10.
Uncertainty in Measurements: Using Significant Figures & Scientific Notation Unit 1 Scientific Processes Steinbrink.
The Scientific Method 1. Using and Expressing Measurements Scientific notation is written as a number between 1 and 10 multiplied by 10 raised to a power.
Counting Significant Figures:
Uncertainty in Measurements and Significant Figures Group 4 Period 1.
The Importance of measurement Scientific Notation.
Significant Figures and Scientific Notation Significant Figures:Digits that are the result of careful measurement. 1.All non-zero digits are considered.
measured certain digits. last digit is estimated, but IS significant. do not overstate the precision 5.23 cm cm Significant Figures (Sig Figs) (uncertain)
Significant Figures. Rules 1.All nonzeroes are significant 2.Zeroes in-between are significant 3.Zeroes to the left are not significant 4.Zeroes to the.
Week. Student will: scientific notation Write in scientific notation.
Significant Figures & Rounding Chemistry A. Introduction Precision is sometimes limited to the tools we use to measure. For example, some digital clocks.
Significant figures are the figures that are known with a degree of certainty.
SIGNIFICANT FIGURES AMOLE WHAT & WHY? Refer to them as “Sig Figs” for short Used to communicate the degree of precision measured Example -
Significant Figures Wednesday, August 12 th. Do Now 1. Place the following numbers in scientific notation or standard Notation x
SIGNIFICANT FIGURES. What are they? It is important to be honest when reporting a measurement, so that it does not appear to be more accurate than the.
Math Outline Math Concepts Important to Chemistry A.Significant Figures and Rounding B.Scientific Notation C.Unit Conversions & Conversion Factors.
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