Chapter 2 - Section 3 Suggested Reading Pages 44 - 57 Using Scientific Measurements.

Slides:



Advertisements
Similar presentations
Chapter 2 – Scientific Measurement
Advertisements

SECTION 2-3. Objectives 1. Distinguish between accuracy and precision 2. Determine the number of significant figures in measurements 3. Perform mathematical.
Chapter 2 Section 3.
I. Scientific Method. The Scientific Method A logical approach to solving problems or answering questions. Starts with observation- noting and recording.
Chapter 2: Measurement and Calculations… Section 2-1: Scientific Method (pg29-31) will not be explicitly covered but used throughout this entire class…
Lesson Starter Look at the specifications for electronic balances. How do the instruments vary in precision? Discuss using a beaker to measure volume versus.
Scientific Notation Converting into Sci. Notation: –Move decimal until there’s 1 digit to its left. Places moved = exponent. –Large # (>1)  positive.
I II III I. Using Measurements CH. 2 - MEASUREMENT.
Unit 2. Measurement This lesson is 8 days long.
Chapter 2 Lesson Starter
C. What are Significant Figures The places in the numbers that are important. They tell you how precise a measurement is. The places in the numbers that.
I II III I. Using Measurements CH. 2 - MEASUREMENT.
Homework: Due Friday 9/4 Do 1-10 on a separate sheet of paper, include units. Do all problems on slide 25 as well.
I. Using Measurements (p )
Unit 1- Units and Measurement Chemistry. Scientific Notation, Measurement, Accuracy, Precision, Error.
Chapter 2: Measurement and Calculations… Section 2-1: Scientific Method (pg29-31) will not be explicitly covered but used throughout this entire class…
Objectives Distinguish between accuracy and precision. Determine the number of significant figures in measurements. Perform mathematical operations involving.
Measuring. What are Significant Figures Any digit of a number that is known with certainty. They tell you how precise a measurement is. Any digit of a.
I II III I. Using Measurements CH. 2 - MEASUREMENT.
Chapter 2: analyzing data
Significant Figures and Scientific Notations Examples and Problems.
CH. 1 - MEASUREMENT I. Units of Measurement. Scientific Method.
I. Using Measurements MEASUREMENT IN SCIENCE. A. Accuracy vs. Precision Accuracy - how close a measurement is to the accepted value Precision - how close.
Ch. 3, Scientific Measurement. Measurement Measurement: A quantity that has a number and a unit. Like 52 meters.
I II III I. Using Measurements MEASUREMENT. A. Accuracy vs. Precision  Accuracy - how close a measurement is to the accepted value  Precision - how.
I. Using Measurements (p )
Preview Lesson Starter Objectives Accuracy and Precision Significant Figures Scientific Notation Using Sample Problems Direct Proportions Inverse Proportions.
I II III I. Using Measurements (p. 8-15) CH MEASUREMENT.
Uncertainty in measurement  Every measurement has error associated with it.  The more precise the measurement the less error.  Error in a measurement.
Units of Measure & Conversions. Number vs. Quantity  Quantity - number + unit UNITS MATTER!!
I II III I. Using Measurements MEASUREMENT. A. Accuracy vs. Precision  Accuracy - how close a measurement is to the accepted value  Precision - how.
Accuracy & Precision & Significant Digits. Accuracy & Precision What’s difference? Accuracy – The closeness of the average of a set of measurements to.
I II III Using Measurements MEASUREMENT. Accuracy vs. Precision  Accuracy - how close a measurement is to the accepted value  Precision - how close.
CHEMISTRY CHAPTER 2, SECTION 3. USING SCIENTIFIC MEASUREMENTS Accuracy and Precision Accuracy refers to the closeness of measurements to the correct or.
Chapter 2 © Houghton Mifflin Harcourt Publishing Company Accuracy and Precision Accuracy refers to the closeness of measurements to the correct or accepted.
Measuring and Calculating Chapter 2. n Scientific method- a logical approach to solving problems n -Observation often involves making measurements and.
Scientific Notation and Significant Figures A. Accuracy vs. Precision Accuracy - how close a measurement is to the accepted value Precision - how close.
I II III III. Using Measurements (p ) CH. 2 - MEASUREMENT.
CH. 2 - MEASUREMENT. Observing and Collecting Data Data may be Qualitative (descriptive) Flower is red Quantitative (numerical) 100 flowers.
WHAT WE HAVE LEARNED. SCIENTIFIC NOTATION 1. Move the decimal to the right of the first non-zero number. 2. Count how many places the decimal had to.
I. Using Measurements (p )
Course Outline Math Review Measurement Using Measurements.
I II III Welcome to Chemistry 116!.  Work to be turned in will only be accepted during the first 10 minutes of lab, or will be considered late  Work.
I. Using Measurements (p )
III. Using Measurements (p )
Measurement.
CH. 2 - MEASUREMENT I. Using Measurements.
CH. 1 - MEASUREMENT I. Units of Measurement.
Measurement Accuracy vs Precision Percent Error Significant Figures
Unit 2- Measurements- Significant Figures & Scientific Notation
I. Using Measurements (p )
Measurement Accuracy vs Precision SI Units Dimensional Analysis
CH. 2 - MEASUREMENT.
-Accuracy & Precision - Significant Digits -Scientific Notation
Lesson 2 – Sci. Notation, Accuracy, and Significant Figures
MEASUREMENT I. Units of Measurement.
Dimensional Analysis.
Accuracy and Precision
Chapter 2 Section 3-A.
Dimensional Analysis, Significant Figures, & the Metric System
I. Using Measurements (p )
Section 2-3 Using Measurements
CH. 2 - MEASUREMENT I. Using Measurements.
CH. 2 - MEASUREMENT I. Using Measurements.
MEASUREMENT Using Measurements C. Johannesson.
CH. 1- MEASUREMENT II. Using Measurements.
CH. 2 - MEASUREMENT I. Using Measurements.
I. Using Measurements (p )
Scientific Measurements
I. Using Measurements (pp )
Presentation transcript:

Chapter 2 - Section 3 Suggested Reading Pages Using Scientific Measurements

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

Neither

Precision

Accuracy & Precision

Percent Error  Indicates accuracy of a measurement experimental value – accepted value accepted value X 100 % Error =

Making Measurements  Write down all certain or exact digits you can read off the instrument, AND one more estimated digit.  Measuring always involves some estimation.

*Uncertainty  Estimate the last digit  Uncertainty is plus-or-minus based on the estimated digits place.  The ratio of the estimated uncertainty to the smallest scale division depends on the separation between the markings.

 Left: 1.5 ± 0.5 inches  Right: 1.48 ± 0.01 inches

 30.0 ± 0.1 degrees C

 Read at the bottom of the meniscus  4.86 ± 0.01 ml

 Try to read these and estimate uncertainty correctly.

 Left: 5.75 ± 0.01 mL

 Middle: 3.0 ± 0.5 mL

 Right: 0.35 ± 0.05 mL

*Mercury Meniscus is inverted

Significant Figures  Indicate precision of a measurement.  Recording Significant Figures  Significant figures in a measurement include the known digits plus a final estimated digit 2.32 cm

Counting Significant Figures  Count all numbers EXCEPT:  Leading zeros  Trailing zeros without a decimal point -- 2,500

, Significant Figures Significant Figures Examples: , sig figs 3 sig figs 2 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 Sig Fig Rules

 Add/Subtract - The # with the fewest digits to the right of the decimal place determines the place of the last sig fig in the answer mL mL 7.85 mL  7.9 mL 3.75 mL mL 7.85 mL

Significant Figures  Add/Subtract – working with whole numbers, round so the final sig fig is in the same place as the leftmost uncertain digit. 224 g g 354 g  350 g 224 g g 354 g

Significant Digits  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

Significant Digits 5. (15.30 g) ÷ (6.4 mL) Practice Problems = g/mL  18.1 g g g g 4 SD2 SD  2.4 g/mL 2 SD

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 significant digits. 65,000 kg  6.5 × 10 4 kg

Practice Problems 7. 2,400,000  g kg 9.7  km  10 4 mm 2.4  10 6  g 2.56  kg km 62,000 mm = = = =

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:

Proportions  Direct Proportion  Inverse Proportion y x y x

Percent  A fraction can be written as a percent by converting it to a decimal and then multiplying by 100.  Ex: 900 million kilograms of plastic soda bottles are produced each year. 180 million kilograms of them are recycled. 900 million kg = 0.2 x 100% = 20% 180 million kg