CH. 2 - MEASUREMENT I. Using Measurements

Activity – Significant figures & measurement With a partner, read all the instructions for the activity! Go to one of the lab stations in the back of the room and, using materials provided, complete the procedure and answer the questions that follow…on your own paper!! Return to your seats to read the passage on the back and complete the questions.

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

B. Percent Error your value accepted value Indicates accuracy of a measurement your value accepted value

% error = ____ % 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 = ____ %

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

Trailing zeros without a decimal point -- 2,500 C. Significant Figures Counting Sig Figs Count all numbers EXCEPT: Leading zeros -- 0.0025 Trailing zeros without a decimal point -- 2,500

Counting Sig Fig Examples C. Significant Figures Counting Sig Fig Examples 1. 23.50 1. 23.50 sig figs 2. 402 2. 402 sig figs 3. 5,280 3. 5,280 sig figs 4. 0.080 4. 0.080 sig figs

(13.91g/cm3)(23.3cm3) = 324.103g 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/cm3)(23.3cm3) = 324.103g

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 224 g + 130 g 354 g 224 g + 130 g 354 g 3.75 mL + 4.1 mL 7.85 mL 3.75 mL + 4.1 mL 7.85 mL  ___ mL  ___ 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 Practice Problems 5. (15.30 g ) ÷ (6.4 mL) = 2.390625 g/mL 6. 18.9 g - 0.84 g  _____g 18.06 g

D. Scientific Notation 65,000 kg  6.5 × 104 kg 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

Practice Problems 7. 2,400,000 g 8. 0.00256 kg 9. 7  10-5 km D. Scientific Notation Practice Problems 7. 2,400,000 g 8. 0.00256 kg 9. 7  10-5 km 10. 6.2  104 mm

D. Scientific Notation (5.44 × 107 g) ÷ (8.1 × 104 mol) = Calculating with Sci. Notation (5.44 × 107 g) ÷ (8.1 × 104 mol) = Type on your calculator: EXP EE EXP EE ENTER EXE 5.44 7 8.1 ÷ 4