Significant Figure Notes With scientific notation too.

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Presentation transcript:

Significant Figure Notes With scientific notation too

Sig Figs Rule 1: “Non-Zeroes Count” NON-ZERO numbers ARE significant How many sig figs? ____3.14 ____469 ____

Sig Figs Rule 2: “Sandwiched Zeroes Count” All zeros BETWEEN significant digits ARE significant. How many sig figs? x 10 3 ____70501 ____ 3020 ____ Only count the numbers to the left of the multiplication sign!

Sig Figs Rule 3: “Lefty Zeroes Don’t Count” Zeroes to the LEFT of significant figures are NOT significant. How many sig figs? ____ ____ ____

Sig Figs Rule 4: “Righty Zeroes…Sometimes Count” Zeroes on the far right ARE significant if the number contains a DECIMAL POINT Zeroes on the far right are NOT significant if the number has NO decimal point How many sig figs? x ____ 200 ____ ____78020 ____

Practice We Do: mL _____ g _____ 82,000 s _____ 6.19 x 10 1 years ______ Next, try the “You Do” problems on your own!!

Scientific Notation I Do:  

Scientific Notation I Do:   We Do:  55, 000  Now try the “You Do” problems on your own!

Scientific Notation IN REVERSE! Make sure you know how to go in both directions! 4.78 x  5.50 x 10 4  This can also be done with a calculator!

Addition/Subtraction When you add or subtract numbers with different precision, you must round your final answer to the least precise number place. Ex g g  g

Addition/Subtraction When you add or subtract numbers with different precision, you must round your final answer to the least precise number place. We Do: What is the total mass of 33.0 g of KCl and g of H 2 O 2 ? Now try the “You Do!”

Multiplication/Division When you multiply or divide numbers with different precision, you must round your final answer to the least number of sig figs. We Do: What is the density (D = m/V) of a g metal sample with a volume of 2.0 cm 3 ? Now try the “You Do!”