Numbers in Science Chemists deal with very large numbers 602000000000000000000000.

Slides:

Advertisements

Similar presentations

And Now, A Little Math Hooray!!. Measurements and Calculations Chapter 5.

Advertisements

Homework Answers m/s m g/L cm3

Zumdahl • Zumdahl • DeCoste

Uncertainty in Measurements

Measurements: Every measurement has UNITS.

Rules for Counting Significant Figures - Details Nonzero integers always count as significant figures has 4 sig figs.

Numbers in Science Chemists deal with very large numbers… (Do you recognize this number?)

SIGNIFICANT FIGURES AND METRIC CONVERSIONS To Round or not To Round????

IB Chem I Uncertainty in Measurement Significant Figures.

1. To show how very large or very small numbers can be expressed in scientific notation 2. To learn the English, metric, and SI systems of measurement.

MeasurementsandCalculations. Numbers Numbers in science are different than in math. Numbers in science always refer to something grams 12 eggs.

Uncertainty in Measurements: Using Significant Figures & Scientific Notation Unit 1 Scientific Processes Steinbrink.

What is Science Study of the physical universe An organized body of facts Experimentation –Observation Cannot be vague Avoid inference.

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,

Chemistry 3.1 Uncertainty in Measurements. I. Accuracy, Precision, & Error A. Accuracy – how close a measurement comes to the “true value”. 1. Ex: Throwing.

The Importance of measurement Scientific Notation.

SIGNIFICANT FIGURES Measured Data Counted & Defined Data (exact numbers) Calculated Data –Multiplication & Division –Addition & Subtraction.

Measures of Science.  Why do we use it?  Expresses decimal places as powers of 10  Written in the form M x 10 n  M (mantissa): numerical part of the.

Week.  Student will: scientific notation  Write in scientific notation.

Significant Figures and Scientific Notation The measuring device determines the number of significant figures a measurement has. Significant figures reflect.

1 Measurements. 2 Nature of Measurement Measurement - quantitative observation consisting of 2 parts Part 1 - number Part 2 - scale (unit) Part 2 - scale.

Section 5.1 Scientific Notation and Units 1.To show how very large or very small numbers can be expressed in scientific notation 2.To learn the English,

MEASUREMENTS. What is the difference between these two measurement rulers? Should we record the same number for each scale reading? The second scale gives.

Section 5: Significant Figures Cartoon courtesy of Lab-initio.com Unit 1: Matter & Measurement.

Measurement and Significant Figures. Precision and Accuracy What is the difference between precision and accuracy in chemical measurements? Accuracy refers.

Metric Base Units Meter (m) – length Kilogram (kg) – mass Kelvin (K) – temperature Second (s) – time Mole (mol) – amount of substance.

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.

Chemistry by the numbers Units of Measurement – The Metric System Length: Mass: Volume: Temperature: Pressure: milli-centi-deci-(unit)deka-hecta-kilo-

Measurements. What do we measure? Fundamental properties Fundamental properties mass (weight)kilogram mass (weight)kilogram lengthmeter lengthmeter timesecond.

V. Limits of Measurement 1. Accuracy and Precision.

Scientific Notation & Significant Figures in Measurement.

Uncertainty in Measurement A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty. Significant figures.

Welcome to the World of Chemistry Measurement, Scientific Notation, Significant Figures.

V. Limits of Measurement 1. Accuracy and Precision.

Uncertainty in Measurement A digit that must be estimated is called uncertain. A measurement always has some degree of uncertainty.

Click to add text Significant Figures Physical Science.

Significant Figures.

Significant Figures All the digits that can be known precisely in a measurement, plus a last estimated digit.

Chemistry I. Precision and Accuracy Accuracy refers to the agreement of a particular value with the true value. Precision refers to the degree of agreement.

Significant figures A significant figure represents an actual measurement A measurement of all the digits known with certainty, plus one that is estimated.

Section 5.2 Uncertainty in Measurement and Significant Figures 1.To learn how uncertainty in a measurement arises 2.To learn to indicate a measurement’s.

Numbers in Science Chemists deal with very large numbers… (Do you recognize this number?)

Chapter 2: Measurement & Problem Solving pg LO: I can use scientific notation with sig figs in mathematic calculations.

Sig Fig and Conversion Practice

Daily Review Tell the difference between accuracy and precision. Give an example. Record 56, in scientific notation. Record in scientific.

Uncertainty and Significant Figures

What is a significant figure?

Observing, Measuring, & Calculating

Objectives To show how very large or very small numbers can be expressed in scientific notation To learn the English, metric, and SI systems of measurement.

Chapter 2, Measurements and Calculations

Unit 3: Measurement and Calculations

Warm up: Mass of Object g Volume of Water 12.5 mL

PHYSICS 11 TODAY’s OBJECTIVE:

Pre-AP Chemistry Measurements and Calculations.

1.3 NOTES Scientific Measurement

Introduction: Matter and Measurement

Metric Systems and Significant Figures

Significant Figures and Scientific Notation

Analyzing Data Chemistry Chapter 2.

Basic Units Length meters Mass kilograms Time seconds.

The Scientific Method: A logical series of steps

Metric Base Units Meter (m) – length Kilogram (kg) – mass

Uncertainty and Significant Figures

Uncertainty and Significant Figures

Chemistry Measurement Notes

Chemistry Measurement Notes

Significant Figures (Sig figs)

Sig Fig and Conversion Practice

Chemistry Significant Figures.

Presentation transcript:

Numbers in Science Chemists deal with very large numbers

m/s

Scientific Notation Is a way of making these numbers easier to write.

To write these numbers in scientific notation, move the decimal so that it is expressed as: A number between 1 and 10 Times ten to a power

Practice problems 12300= 2.5 X 10 3 = 1.0 X = 2.05 X =

The importance of units Numbers are used in science for quantifying measurements. However, all numbers must be followed by a unit!! Naked numbers have no meaning in science!

Measurements in science Observations in science should be quantified whenever possible. For this reason, scientists must master the tools used for measuring and the units that are used to express them.

General rules for measurement All units will be metric. Memorize the units for: Length = meter (m) mass = gram (g) volume = liter (L)

Prefixes used with the basic units Kilo- Centi- Milli-

Practice 1 kg = g1 m = cm 1 km = m1 L = mL 1 cm = m1 cm = mm 1 mL = L

Significant figures (digits) Pay attention to the precision of your tools Record all of the numbers in a measurement that you are certain of, plus one more (an approximation) called “the uncertainty.” All of the measured numbers, plus the uncertain number are called significant figures.

Why are they important? 1. They communicate the precision of the measuring tools used by the chemist. 2. They determine how precise the answers to calculations (using the measuring tools) can be.

Precision of Tools? What do you mean?

Significant figures (digits) are 1. Non-zero integers 2. Captive zeros Ex: Trailing zeros with a decimal point

Significant figures are not 1. Leading zeros Trailing zeros without a decimal point Exact numbers—they have an unlimited # of Sig. figs. a) counts: 3 apples b) formula numbers:  r 2 c) definition: 1 inch = 2.54 cm

Significant figures in calculations 1. Multiplication and division rules Answer will have the same number of sig. figs. as the measurements with the smallest number of sig. figs. Ex: What is the density of an object with a mass of g and a volume of 3.3 ml?

2. Addition or Subtraction Answer will have the same number of decimal places as the measurement with the least number of decimal places. Ex: mm mm mm =

Do you and your calculator have a communication problem? Solve the problem below using your calculator. 3.0 x 10 5 = 1.5 x 10 2 * 2.0 x 10 3

Calculations (4 X 10 2 )(2X 10 3 )= (4X10 2 )/(2X )=