Significant Figures and Percent Error

Slides:



Advertisements
Similar presentations
Physics Rules for using Significant Figures. Rules for Averaging Trials Determine the average of the trials using a calculator Determine the uncertainty.
Advertisements

Significant Figures. 1.All nonzero digits are significant. Example: 145 (3 sig figs) 2.Zeroes between two significant figures are themselves significant.
DIFFERENTIATE: ACCURACY AND PRECISION Three targets with three arrows each to shoot. Can you hit the bull's-eye? Both accurate and precise Precise but.
Uncertainty in Measurements
Significant Figures.  All measurements are inaccurate  Precision of measuring device  Human error  Faulty technique.
Accuracy, Precision, Signficant Digits and Scientific Notation.
Rules For Significant Digits
Section 2.3 Measurement Reliability. Accuracy Term used with uncertainties Measure of how closely individual measurements agree with the correct or true.
IN THE CHEMISTRY SECTION OF YOUR NOTEBOOK, TAKE CORNELL STYLE NOTES OVER THE INFORMATION PRESENTED IN THE FOLLOWING SLIDES. Measurements in Chemistry Aug.
Measurement book reference p Accuracy  The accuracy of the measurement refers to how close the measured value is to the true or accepted value.
Significant Figure Notes With scientific notation too.
The Importance of measurement Scientific Notation.
Significant Figures What do you write?
Significant Figures and Scientific Notation Significant Figures:Digits that are the result of careful measurement. 1.All non-zero digits are considered.
Week.  Student will: scientific notation  Write in scientific notation.
Significant Figures Rules and Applications. Rules for Determining Significant Figures 1.) All Non-Zero digits are Significant. 1.) All Non-Zero digits.
Significant Figures 1.All non-zero digits are significant (2.45 has 3 SF) 2.Zeros between (sandwiched)non- zero digits are significant (303 has 3 SF)
SIGNIFICANT FIGURES AMOLE WHAT & WHY?  Refer to them as “Sig Figs” for short  Used to communicate the degree of precision measured  Example -
Chemistry 100 Significant Figures. Rules for Significant Figures  Zeros used to locate decimal points are NOT significant. e.g., 0.5 kg = 5. X 10 2 g.
Significant Figures in Calculations. A calculated answer cannot be more precise than the least precise measurement from which it was calculated. The answer.
Percent Composition. Molar Mass Calculate the Molar Mass of H 2 O 1 mole of H 2 O contains 2 mols H and 1 mol O. The mass of 2 moles H = 2 mol(1.008 g/mol)=
Significant Figures.
Measurements in Chemistry Aug 6, 2014 In the chemistry section of your notebook, Take Cornell style notes over the information presented in the following.
Drill – 9/14/09 How many significant figures: Now complete the back of the measurement worksheet from last week (the graduated.
Mastery of Significant Figures, Scientific Notation and Calculations Goal: Students will demonstrate success in identifying the number of significant figures.
Significant Figures. Rule 1: Digits other than zero are significant 96 g = 2 Sig Figs 152 g = __________ Sig Figs 61.4 g = 3 Sig Figs g = __________.
Significant Digits or Significant Figures. WHY??? The number of significant figures in a measurement is equal to the number of digits that are known with.
Significant Figures.
Mathematical Operations with Significant Figures Ms. McGrath Science 10.
Significant Figures. Rule 1: Nonzero numbers are always significant. Ex.) 72.3 has 3 sig figs.
1-2 Significant Figures: Rules and Calculations (Section 2.5, p )
SIG FIGURE’S RULE SUMMARY COUNTING #’S and Conversion factors – INFINITE NONZERO DIGIT’S: ALWAYS ZERO’S: LEADING : NEVER CAPTIVE: ALWAYS TRAILING :SOMETIMES.
UNIT 2: Scientific Measurement Honors Chemistry GHS.
Significant Figures SIGNIFICANT FIGURES You weigh something and the dial falls between 2.4 lb and 2.5 lb, so you estimate it to be 2.46 lb. The first.
Rules for Significant Figures
Unit 3 lec 2: Significant Figures
Learning Targets I can use correct numbers of significant figures and units in both measurements and calculations. I can accurately measure mass and volume.
Significant Figure Rules
Significant Figures Sig Figs.
Significant Figures.
Measurement: Significant Figures
Warm –up #2 What is chemistry? Write what you recall about the definition and name 2 areas of study of chemistry.
Significant Figures.
Aim: Why are Significant Figures Important?
SIG FIGURE’S RULE SUMMARY
Significant Figures.
Unit 2- Measurements- Significant Figures & Scientific Notation
Significant Digits or Significant Figures
IV. Significant figures
Warm up: Mass of Object g Volume of Water 12.5 mL
Notes Significant Figures!.
DETERMINING SIGNIFICANT FIGURES
Significant Figures All non-zero digits are significant (2.45 has 3 SF) Zeros between (sandwiched)non-zero digits are significant (303 has 3 SF)
Unit 1 lec 3: Significant Figures
Exact and Inexact Numbers
Section 3-2 Uncertainty in Measurements
Significant digits.
Significant Figures Be able to identify the number of significant figures that an number has.
Significant Figures or Digits
Measurement book reference p
Section 2.3 Uncertainty in Data
Significant Figures.
5. Significant Figures- = represent the valid digits of a measurement and tells us how good your instrument is.
Accuracy vs. Precision & Significant Figures
How do you determine where to round off your answers?
The Mathematics of Chemistry
Significant Figures & Scientific Notation
Aim: How do we determine the number of significant figures in a measurement? Warm Up What is the difference between the values of 3, 3.0, and 3.00.
Uncertainty in Measurement
Significant Figures (Sig figs)
Presentation transcript:

Significant Figures and Percent Error

Rules for Significant Figures Nonzero numbers are ALWAYS significant. 1287 g 78,483 cm 58 mL 638 mol = 4 Sig Figs = 5 Sig Figs = 2 Sig Figs = 3 Sig Figs

Rules for Significant Figures Zeros in-between nonzero numbers are ALL significant. 101 mol 20,375 cd 1001 J 908 s = 3 Sig Figs = 5 Sig Figs = 4 Sig Figs = 3 Sig Figs

Rules for Significant Figures Zeros after nonzero numbers (trailing zeros) WITH A DECIMAL PRESENT are significant 6.0 mg 678.10 Kg 80.0 m 12.00 mL = 2 Sig Figs = 5 Sig Figs = 3 Sig Figs = 4 Sig Figs

Rules for Significant Figures Zeros in front of nonzero digits (preceding zeros) are not significant. They are called place holders. 0.78 Kg 0.0309 cd 290 amp 300 s = 2 Sig Figs = 3 Sig Figs = 2 Sig Figs = 1 Sig Figs

Zeros that are significant. = 3 Sig Figs 202 cm 510002 L 144.0 kg 670.00 cd = 6 Sig Figs = 4 Sig Figs = 5 Sig Figs

Zeros that are NOT significant, PLACE HOLDERS. = 1 Sig Figs 50 g 0.0072 m 0.0321 J 9000 L = 2 Sig Figs = 3 Sig Figs = 1 Sig Figs

= 4 Sig Figs = 3 Sig Figs = 4 Sig Figs = 4 Sig Figs Zeros that are significant (called Trailing) and zeros that are not significant (call Place Holder). = 4 Sig Figs 80020 s 0.00401 kg 0.03020 Amp 10230 L = 3 Sig Figs = 4 Sig Figs = 4 Sig Figs

Making Calculations with Significant Digits Multiplying and Dividing The final answer is rounded to have the same number of significant figures as the measurement with the least number of significant figures. 755 cm x 33 cm = 24915 92 m x 20 m = 1840 25000 cm2 2000 m2

0.894 g / 2.0 g = 0.447 g 40.0 x 3.8 = 152 203 x 4589 = 931567 10259 / 789 = 13.00253485 96.0 / 75.0 = 1.25 101 x 0.020 = 2.02 0.45g 1.50 932000 13.0 1.25 2.0

Making Calculations with Significant Digits Adding and Subtracting The final answer is rounded so that it has the same number of digits past the decimal as the measurement with the least number of digits past the decimal 120.60 89.001 6.3 215.901 + 215.9

756.05 23.02 733.03 − 733.03 9.002 2.32 45.659 56.981 + 56.98

45 32.5 12.5 − 13

|Approximate Value − Exact Value| PERCENT ERROR   |Approximate Value − Exact Value|   × 100% |Exact Value| Step 1: Calculate the error (subtract one value form the other) ignore any minus sign. Step 2: Divide the error by the exact value (you will get a decimal number) Step 3: Convert that to a percentage (by multiplying by 100 and adding a "%" sign)

GOOD MORNING!!  PICK UP: Calculator GET OUT: Notebook, pencil, TURN IN: Pennies if you brought them!! ‘ WARM UP: 1. How many significant figures are in these numbers? a. 803800 b. 803800.0 c. 0000000.3 d. .0000021 e. 84 2. In your own words, what is the definition of accuracy and precision? 3. In the lab, Sandy and Danny produced 8.5 grams of their product. According to their calculations, they should have produced 9.5 grams. What was their percent error? (about 10%)