Unit 1 Into to Measurement

Slides:



Advertisements
Similar presentations
Base Units of the SI System Quantity Base Unit Abbreviation Second s
Advertisements

SECTION 2-3. Objectives 1. Distinguish between accuracy and precision 2. Determine the number of significant figures in measurements 3. Perform mathematical.
Chapter 1: Measurements
Base Units Metric System -standard, used internationally(easy to communicate through language barriers -makes conversions simpler -based on the number.
Unit Conversion SI units: The International System of Units (abbreviated SI from the French Système international d'unités]) is the modern form of the.
Unit 1 Part 2: Measurement
Measurements: Every measurement has UNITS.
Scientific Measurement
Scientific Measurement and Significant Figures
Measurement & Conversions
Using and Expressing Measurements
CHAPTER 1 : MEASUREMENTS
Uncertainty In Measurement
Using and Expressing Measurements
Chapter 1.5 Uncertainty in Measurement. Exact Numbers Values that are known exactly Numbers obtained from counting The number 1 in conversions Exactly.
Section 2.3 Measurement Reliability. Accuracy Term used with uncertainties Measure of how closely individual measurements agree with the correct or true.
Unit 2. Measurement This lesson is 8 days long.
Accurate measurements are needed for a valid experiment.
Warm Up 1. How many miles is 870,655 in? (Hint: There are 5,280 ft in 1 mile). 2. Do you weigh yourself? Which scale would you use? Why? How do you know.
SIG FIGS Section 2-3 Significant Figures Often, precision is limited by the tools available. Significant figures include all known digits plus one estimated.
Measuring and Units.
Do Now: 1.How many significant figures are in the following: a) b) c) d) Convert the following to scientific notation: a)67000.
Measurement and Significant Figures. Precision and Accuracy What is the difference between precision and accuracy in chemical measurements? Accuracy refers.
Measurements and Calculations 1. To show how very large or very small numbers can be expressed in scientific notation 2. To learn the English, metric,
The Importance of measurement Scientific Notation.
Chapter 2 Standards of Measurement Objectives:  Understand Mass and Weight (2.1)  Identify the metric units of measurement (2.6)  Explain what causes.
I II III Units of Measurement Scientific Measurement.
3.1 Measurement and Uncertainty How do you think scientists ensure measurements are accurate and precise?
Section 2.1 Units and Measurements
Unit 1: Introduction to Chemistry Measurement and Significant Figures.
Measurement and Significant Figures. Precision and Accuracy What is the difference between precision and accuracy in chemical measurements? Accuracy refers.
Chapter 3. Measurement Measurement-A quantity that has both a number and a unit. EX: 12.0 feet In Chemistry the use of very large or very small numbers.
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.
Ch. 3, Scientific Measurement. Measurement : A quantity that has a and a. Like 52 meters.
Scientific Notation & Significant Figures in Measurement.
“Scientific Measurement”. Measurements and Their Uncertainty OBJECTIVES: Convert measurements to scientific notation.
Measurement Unit Unit Description: In this unit we will focus on the mathematical tools we use in science, especially chemistry – the metric system and.
Dimensional Analysis  What happens when you divide a number by itself?  What happens when you divide a unit by itself?  In both cases, you get the.
Measurement & Calculations Overview of the Scientific Method OBSERVE FORMULATE HYPOTHESIS TEST THEORIZE PUBLISH RESULTS.
Chapter 2 - Section 3 Suggested Reading Pages Using Scientific Measurements.
Accuracy & Precision & Significant Digits. Accuracy & Precision What’s difference? Accuracy – The closeness of the average of a set of measurements to.
Significant Figures… Bluefield High School 1. What is a significant digit? Significant digits is a set of internationally accepted rules for measurement.
Math Concepts How can a chemist achieve exactness in measurements? Significant Digits/figures. Significant Digits/figures. Sig figs = the reliable numbers.
UNITS Science makes all measurements using the metric system LengthMeter (m) MassGram (g) VolumeLiter(L) ( = inches) ( = ounces) ( =
Measurements and their Uncertainty
Chapter 2 Data Analysis. Units of Measurement Metric System The system of measurement used by Scientists Base unit modified by factor of 10 English System.
Measurements and Calculations Scientific Method Units of Measurement Using Scientific Measurements.
Measurement Vocab. Measurement: a quantity that has both a number and a unit Measuring: a description of your observation.
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.
Course Outline Math Review Measurement Using Measurements.
Significant Figures. Rule 1: Nonzero numbers are always significant. Ex.) 72.3 has 3 sig figs.
1 Scientific Measurement Objectives: Section 2.1 List common SI units of measurement and common prefixes used in the SI system. Distinguish mass, volume,
Significant Figures. Who cares? Sig Figs measure the degree of precision of a measurement.
Chemistry Math in Chemistry Unit. How wide is our universe? 210,000,000,000,000,000,000,000 miles (22 zeros) How would you use this number in a calculator?
Measurements and Calculations Scientific Method Units of Measurement Using Scientific Measurements.
Chapter 3 “Scientific Measurement”
Observing, Measuring, & Calculating
Scientific Notation Significant Figures Conversion Factors
Measurement.
Measurement Accuracy vs Precision Percent Error Significant Figures
Measurement I. Units of Measurement (p.34-45) Number vs. Quantity
Section 2.1 Units and Measurements
Measurement Accuracy vs Precision SI Units Dimensional Analysis
Analyzing Data Chemistry Chapter 2.
Section 3-2 Uncertainty in Measurements
Dimensional Analysis.
Chemistry Measurement Notes
Presentation transcript:

Unit 1 Into to Measurement

Uncertainty in Data Precision: A reliable measurement will give about the same results time and time again under the same conditions. Precision refers to the reproducibility of a measurement. Accuracy: A measurement that is accurate is the correct answer or the accepted value for the measurement. High accuracy = close to accepted value. http://www.youtube.com/watch?v=HmY4YiLCCaU

Examples: More Examples: True Value = 34.0 mL Measurements = 34.2 mL, 34.1 mL, 34.2 mL Accurate and/or Precise? True Value = 29.3 cm Measurements = 32.3 cm, 32.5 cm, 32.4 cm Accurate and/or Precise? True Value = 27.3 s Measurements = 27.9s, 30.2s, 26.9s Accurate and/or Precise?

Significant Figures You are often asked to combine measurements mathematically. When measurements are combined mathematically, the uncertainty of the separate measurements must be correctly be reflected in the final answer. A set of rules exists to keep track of the significant figures in each measurement. The significant figures (SIG FIGS) in a measurement include the certain digits and the estimated digit of a measurement.

SIG FIG RULES !! Nonzero numbers are always significant. 14 = 523= Zeros between nonzero numbers are always significant. Sandwich Zeros 101 = 2005 = Zeros after significant figures are significant only if they are followed by a decimal point. (All final zeros to the right of the decimal are significant). 100.0 = 2030.0 = Place holder zeros are NOT significant. To remove placeholder zeros, rewrite the number in scientific notation. 0.001 = 0.0000034 =

How many sig figs in these measurements? 3.4567 = _____ 3.00047 = _____ 0.00003409 = _____ 2.05 X 105 = _____ 0.100 = _____ 3000 = _____

Sig Figs in Calculations For multiplication and division: The least number of sig figs in the measurements determines how many sig figs in the final answer. Ex: 6.15 m x 4.026 m = 24.7599 m2 What is the fewest # of sig figs? (3) so the answer is rounded to 24.8 m2 If a calculation involves several steps, ONLY ROUND FINAL ANSWER, carry extra sig figs in intermediate steps. If the digit to be rounded is less than 5, round down; if 5 or more, round up.

Ex. 24 cm X 32.8 cm = 763.2 cm2 Ex. 8.40 g 4.2 g/mL = 2 g/mL   Round 763.2 cm2 to ____________ Ex. 8.40 g 4.2 g/mL = 2 g/mL 2 g/mL must be rounded to ____________

For addition and subtraction: The sum or difference has the same number of decimal places as the measurement with the least number of decimal places. EX: 951.0g + 1407 g + 23.911 g + 158.18 g = 2540.091 g But the measurement with the fewest places past decimal is 1407 g ( It has no digits past decimal) SO the final answer must be rounded to 2540. g

Ex. 49.1 g + 8.001 g = 57.101 g   Round the answer to ___________ Ex. 81.350 m – 7.35 m = 74 m Round the answer to ____________

Percent Error Percent error compares a measurement with its accepted value. A percent error can be either positive or negative. % ERROR = measured - accepted x 100 accepted % ERROR = what you got – what is correct x 100 what is correct

Scientific Notation Some measurements that you will encounter in physics can be very large or small. Using these numbers in calculations is cumbersome. You can work with these numbers more easily by writing them in scientific notation. A number written in scientific notation is written in the form  M X 10n Where M is a number between 1 and 10 (known as the coefficient) and 10 is raised to the power of n (known as the exponent). Circle the numbers that are in correct scientific notation:   1 X 104 12 X 1012 0.9 X 103 2.54 X 10-3 9.99 X 102

Step 1: Determine M by moving the decimal point in the original number to the left or right so that only one nonzero digit is to the left of the decimal….do it!!! 27508.   Step 2: Determine “n” , the exponent of 10, by counting the number of decimal places the decimal point has moved. If moved to the left, n is positive. If moved to the right, n is negative. 2.7508 4 places to the left, n = 4 Answer = 2.7508 X 104

Write the following quantities in scientific notation…do it!!! 0.0050 = 235.4 = 18,903 = 0.0000101 = Write the following quantities in arithmetic notation…do it!!! 1.45 X 104 = 2.34 X 10-3 6.02 X 1023 =

Units and Measurements The International System of measurement or “metric” system is the preferred system. Make sure you are familiar with the basic units that we will be using many times throughout the year. Quantity Unit Abbreviations Time Second s Length Meter m Mass Gram g Temperature Kelvin K

Make sure to be familiar with the common prefixes that make the base unit larger (kilo- for example) and prefixes that make the unit smaller ( examples milli - and centi-) You should know how to quickly change between the units, for example, from liter to milliliter or kilograms to grams. Prefix Symbol Kilo k. Hecta h. Deca da Base Unit Deci d Centi c Milli m

Factor Label/ Dimensional Analysis Dimensional Analysis: A technique of converting between units. Dimensional analysis use conversion factors. A conversion factor is always equal to 1. For example: 1000m or 60 minute 1 km 1 hour Conversion factors can be flipped to allow for cancellation of units. Choosing the correct conversion factors requires looking carefully at the problem.

Step 1: Show what you are given on the left, and what units you want on the right.   Step 2: Insert the required conversion factor(s) to change between units. In this case we need only one conversion factor, and we show it as a fraction, 1 hr/60 min. We put units of minutes on the bottom so they will cancel out with the minutes on the top of the given. Step 3: Cancel units where you can, and solve the math.

For example let’s look at the following question: Example 1: Given that there are 5280feet in a mile, How many feet are in 2.78 miles? Example 2: Convert 89 km into inches

Example 3: How many gallons are in 146 Liters. 1 Gal= 4 quarts 1 L = 1 Example 3: How many gallons are in 146 Liters? 1 Gal= 4 quarts 1 L = 1.057 quarts 1 L=1000ml Example 4: How many seconds in 5.00 days?