general chemistry lecture
DESCRIPTION
Scientific MeasurementsTRANSCRIPT
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Scientific Measurements
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1. All numbers excluding the zero are significant.
2. Zero is significant if it is between 2 non-zero digits.
3. Zero’s to the right of an expressed decimal points are significant.
4. Zero’s to the right of a decimal point and to the right of a non-zero digit is significant
Significant Figures Rules
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Significant Figures Rules
5. Zero’s with bar on the top are significant.6. Zero’s to the left of a decimal point but to the left of a non-zero decimal are not significant.7. When a number ends with a zero, the zeros are not significant
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• Addition and Subtraction–Least Decimal Places
• Multiplication and Division–Least Significant figures
Operations on Significant Figures
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- Short hand way of writing large and small numbers
- (+ large numbers), base (- decimal numbers)- Example:- Mass of an electron
0.00000000000000000000000000000911or
Speed of light :
Scientific Notation
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Operation on Scientific Notation
Addition1. If the same exponent, add the main and
copy the exponent2. If not the same exponent, make the same
exponent copying the larger exponent
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Operation on Scientific Notation
Subtraction1. If the same exponent, subtract the main and
copy the exponent2. If not the same exponent, make the same
exponent copying the larger exponent
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Operation on Scientific Notation
MultiplicationMultiply the M’s (bases) and add the
exponents algebraically
DivisionDivide the M’s and subtract the
exponents algebraically
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Length10mm=1cm 1yard=3ft10cm=1dcm 1km=0.62miles10dcm=1m10m=1hm10hm=1km1inch=2.54cm12inches=1ft
Conversion
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Mass1g=1000mg1000g=1kg1kg=2.2lb
Volume1L=1000mL1cm³=1mL=1cc
Conversion
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Temperature
°C → °F °F = °C +32K= °C +273.15R=°F + 460.67
Conversion
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Prepared by:Novilyn M. Villanueva