I II III III. Using Measurements (p ) CH. 2 - MEASUREMENT
A. Accuracy vs. Precision Accuracy - how close a measurement is to the accepted value Precision - how close a series of measurements are to each other ACCURATE = CORRECT PRECISE = CONSISTENT
Let’s use a golf analogy
Accurate?No Precise?Yes
Accurate?Yes Precise?Yes
Precise?No Accurate? No
Accurate?Yes Precise?We can’t say!
Dart Example
B. Percent Error Indicates accuracy of a measurement your value accepted value
B. Percent Error A student determines the density of a substance to be 1.40 g/mL. Find the % error if the accepted value of the density is 1.36 g/mL. % error = 2.9 %
Your Turn What is the percent error for a mass measurement of 17.7 g, if the correct value is 21.2 g? A volume is measured experimentally as 4.26 mL. What is the percent error, given the correct value is 4.15 mL?
Error in Measurement Some error or uncertainty always exists in any measurement. skill of the measurer conditions of measurement measuring instruments
C. Significant Figures Indicate precision of a measurement. Recording Sig Figs Sig figs in a measurement include the known digits plus a final estimated digit 2.35 cm
C. Significant Figures Counting Sig Figs (Table 2-5, p.47) Count all numbers EXCEPT: Leading zeros Trailing zeros without a decimal point -- 2,500
, C. Significant Figures Counting Sig Fig Examples , sig figs 3 sig figs 2 sig figs
C. Significant Figures Calculating with Sig Figs Multiply/Divide - The # with the fewest sig figs determines the # of sig figs in the answer. (13.91g/cm 3 )(23.3cm 3 ) = g 324 g 4 SF3 SF
C. Significant Figures Calculating with Sig Figs (con’t) Add/Subtract - The # with the lowest decimal value determines the place of the last sig fig in the answer mL mL 7.85 mL 224 g g 354 g 7.9 mL 350 g 3.75 mL mL 7.85 mL 224 g g 354 g
C. Significant Figures Calculating with Sig Figs (con’t) Exact Numbers do not limit the # of sig figs in the answer. Counting numbers: 12 students Exact conversions: 1 m = 100 cm “1” in any conversion: 1 in = 2.54 cm
C. Significant Figures 5. (15.30 g) ÷ (6.4 mL) Practice Problems = g/mL 18.1 g g g g 4 SF2 SF 2.4 g/mL 2 SF
D. Scientific Notation Converting into Sci. Notation: Move decimal until there’s 1 digit to its left. Places moved = exponent. Large # (>1) positive exponent Small # (<1) negative exponent Only include sig figs. 65,000 kg 6.5 × 10 4 kg
D. Scientific Notation 7. 2,400,000 g kg 9.7 km 10 4 mm Practice Problems 2.4 10 6 g 2.56 kg km 62,000 mm
D. Scientific Notation Calculating with Sci. Notation (5.44 × 10 7 g) ÷ (8.1 × 10 4 mol) = 5.44 EXP EE ÷ ÷ EXP EE ENTER EXE = = 670 g/mol= 6.7 × 10 2 g/mol Type on your calculator: