1 / 19

Scientific Notation and Significant Figures

Scientific Notation and Significant Figures. Why do we use Scientific Notation?. Why do we use Scientific Notation?. Chemists often use very LARGE and very SMALL numbers Examples: Mass of H atom: 0.000 000 000 000 000 000 000 001 67 g Mole of atoms: 602 000 000 000 000 000 000 000.

lotta
Download Presentation

Scientific Notation and Significant Figures

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Scientific Notation and Significant Figures

  2. Why do we use Scientific Notation?

  3. Why do we use Scientific Notation? Chemists often use very LARGE and very SMALL numbers Examples: Mass of H atom: 0.000 000 000 000 000 000 000 001 67 g Mole of atoms: 602 000 000 000 000 000 000 000

  4. Scientific Notation • Written as a COEFFICIENT and a POWER OF 10 • Example 1: 2300 = 2.3 x 103 Number of times coefficient must be multiplied by ten to get original number Coefficient ≥ 1 AND <10

  5. Example 2: 0.0052 =

  6. Example 2: 0.0052 = 5.2 x 10-3

  7. Convert to Scientific Notation

  8. Convert to Scientific Notation

  9. Convert to Standard Form

  10. Convert to Standard Form

  11. Significant Figures • Scientists report measurements using significant figures • SF: a measurement that includes all the precisely known digits plus a last digit that must be estimated

  12. Measuring using Sig Figs

  13. What is the length of each object?

  14. Sig Fig Rules • Every nonzero digit is significant • Zeros between nonzero digits are significant • Zeros in front of all nonzero digits are NOT significant • Zeros at the end of a number and to the right of a decimal are significant • Zeros at the end of a measurement and to the left are NOT significant if there is no decimal at the end

  15. How many Sig Figs? • 123 m e. 4.5600 m • 0.123 m f. 0.078 m c. 40506 m g. 0.070 80 m d. 9.8000 x 104 h. 98 000 m

  16. How many Sig Figs? • 123 m (3) e. 4.5600 m (5) • 0.123 m (3) f. 0.078 m (2) c. 40506 m (5) g. 0.070 80 m (4) d. 9.8000 x 104 (5) h. 98 000 m (2)

  17. Addition and Subtraction The answer can have no more digits to the right of the decimal point than the measurement with the least number of digits after the decimal. • ex. 1 12.52 + 349.0 + 8.24 = • ex. 2 740626 - 86.34 =

  18. Multiplication and Division The answer must contain no more significant figures that the measurement with the least number of significant figure a. 7.44 m x 0.34 m = b. 2.4526 m / 8.4 =

  19. Practice Problems Page 840, #1 Page 841, #1, 2

More Related