General Chemistry Lecture
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Transcript of General Chemistry Lecture
Scientific Measurements
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
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
• Addition and Subtraction–Least Decimal Places
• Multiplication and Division–Least Significant figures
Operations on Significant Figures
- 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
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
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
Operation on Scientific Notation
MultiplicationMultiply the M’s (bases) and add the
exponents algebraically
DivisionDivide the M’s and subtract the
exponents algebraically
Length10mm=1cm 1yard=3ft10cm=1dcm 1km=0.62miles10dcm=1m10m=1hm10hm=1km1inch=2.54cm12inches=1ft
Conversion
Mass1g=1000mg1000g=1kg1kg=2.2lb
Volume1L=1000mL1cm³=1mL=1cc
Conversion
Temperature
°C → °F °F = °C +32K= °C +273.15R=°F + 460.67
Conversion
Prepared by:Novilyn M. Villanueva