Significant Figures Honors Chem section 1.5. Accuracy vs. Precision Accuracy: how close a measured...
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Transcript of Significant Figures Honors Chem section 1.5. Accuracy vs. Precision Accuracy: how close a measured...
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SignificantFigures
Honors Chem section 1.5
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Accuracy vs. Precision
• Accuracy: how close a measured value is to the true value.
• Precision: the degree of reproducibility of a measurement. It depends on how well you make a measurement
These terms are often incorrectly used interchangeably
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Examples
• Your summer job is guessing people’s weights at the traveling carnival
• Imagine you have one person who keeps coming back and you guess their weights as:• 56 kg • 65 kg • 70 kg • 51 kg
• The average of these= 60.5kg• If their actual weight is 60kg, the avg
prediction turns out to be accurate, but not precise
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Examples
• If instead you had made guesses of:– 69kg -69kg -67kg -68kg
• Your guesses would be precise, but not accurate
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Precision
• Precision can also mean how detailed the number is– Two Scales:
• Scale #1 = 180lbs• Scale #2 = 180.49lbs
– Which one is more precise?– What is the difference in the scales?
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Does that matter?
• Mass of Obama
• Would it have been ok to report a time as 35 seconds instead of 35.14s?– Would have been OK, but not USEFUL for
Olympic competition
• Could you have timed him so precisely with an analog watch?
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exactly
• Exact #’s– # of people in the room (counting #)– 12 eggs/dz– 1g = 1000mg
• Inexact #’s– #’s obtained by measurement– Always have a level of uncertainty
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Measuring
• Measured quantities are reported in such a way that only the last digit is uncertain
• The number tells you what it was measured with
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measuring
• Always estimate one digit further than the measurement instrument gives (this is the uncertain digit)
• Uncertainties of equipment are given as +/-
+/- 0.01g +/- 0.1g
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Significant Figures
• The way we report numbers tells us how we measured them…hence Significant Figures
• All digits of a measured quantity, including the uncertain one, are called significant figures
• Not all #’s are significant, however – and we will learn to count how many there are
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Examples – How Many Sig Fig’s are In Each Number?
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The Rules• You’ll never find easier rules for significant figures than
these… trademarked at Tennent:
• 2 Conditions:– If there is a decimal point: Begin counting on
the right, and count numbers until there are no more left, or you have hit all zeroes
– If there is no decimal point: Begin counting on the left, and count numbers until there are no more left, or you have hit all zeroes
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?
• Which of the following is an inexact quantity?– A) the # of people in your math class– B) the mass of a penny– C) the # of grams in a kilogram
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?
• Which of the following is an inexact quantity?– A) the # of people in your math class– B) the mass of a penny– C) the # of grams in a kilogram
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Uncertainty
• Which measurement has more uncertainty? What are the uncertainties?
26.1g 26.10g
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Uncertainty
• Which measurement has more uncertainty? What are the uncertainties?
26.10g 26.100g
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Special Conditions• Scientific Notation
• When numbers are written in Scientific Notation, all of the numbers written are significant
• Counting Numbers
• Counting numbers are considered to have an infinite number of sig figs (you’ll see the importance of this in calculations)
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Calculations with sig figs
• Answers can only be as precise as the least precise measurement
• Addition/Subtraction– The answer must have as many digits past the
decimal point as the number with the fewest digits
• Multiplication/Division– The answer must have the same number of significant
figures as the number with the fewest sig figs
Use scientific notation when rounding is difficult
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+/-
– 43.2g + 51.0g + 48.7g = 142.9g
– 258.3kg + 257.11kg + 253kg = 768.41kg
– 0.0487m + 0.05834m + 0.00483m = 0.11187m
– 5.236cm – 3.14cm = 2.096cm
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X & /
– 24cm x 3.26cm = 78.24
– 120m x 0.10lm = 12
– 1.23m x 2.0m = 2.46
– 60.2g / 20.1ml = 2.995024876
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Sig fig calculations
• The result of adding 1.17 x 10-2 and 8 x 10-3 is, to the correct # of sig figs:– A) 1.9 x 10-2
– B) 1.97 x 10-2
– C) 2.0 x 10-2
– D) 0.02– E) none of the above
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Sig fig calculations
• The result of adding 1.17 x 10-2 and 8 x 10-3 is, to the correct # of sig figs:– A) 1.9 x 10-2
– B) 1.97 x 10-2
– C) 2.0 x 10-2
– D) 0.02– E) none of the above
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Sig fig calculations
• (107.36 – 99.2)(5.4033 x 105) = 4.4090928 x 106
• the above calculation, when expressed to the correct number of sig figs is:– A) 4.4 x 106
– B) 4.40 x 106
– C) 4.41 x 106
– D) 4.4090 x 106
– E) 4.091 x 106
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Sig fig calculations
• (107.36 – 99.2)(5.4033 x 105) = 4.4090928 x 106
• the above calculation, when expressed to the correct number of sig figs is:– A) 4.4 x 106
– B) 4.40 x 106
– C) 4.41 x 106
– D) 4.4090 x 106
– E) 4.091 x 106
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Density & Units
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