ance-mole-mol
· Volume-cubic meter-m^3 *In chem the mL and the L are the most important non-SI units. 1L = 1dm = 10^(-3) m^3. 1mL = 1cm^3 = 10^(-3) dm^3 = 10^(-3) L = 10^(-6) m^3
· Density- mass divided by volume. ( Intensive property)
D= mass/volume (*mass and volume are extensive)
· 1.6 Uncertainty in Measurement: Significant Figures
* The greater the number of SF (significant figures) in a measurement, the greater the certainty.
(WARNING !) YOU CANNOT GIVE A VALUE MORE PRECISE THAN THE TOOL
· always estimate the rightmost digit (assume uncertainty of one unit in the rightmost digit)
· All digits are significant, except zeros that are not measured but are used only to position the decimal point.
· Zeros are NOT significant when:
· They're used as placeholders
· Ex: 0.5 (1 SF), 500 (1SF), 500.01 ( 5 SF )* the decimal point made the zeros after count, and the five made the ones before count
· TEACHER'S CONVENTION FACTOR IS FOUR SIG FIGS (ex. 1.000 L = 1.057 qt)
· In addition and subtraction:
· The number of decimal places in result can be no more than that of the operator with the least number of decimal places.
· In Multiplication and division:
· The result can have as many SF as the least SF digit.
· Precision How close all trial of measurement are to each other (deviation from other obtained values)
· Accuracy The closer a value is to a true (theoric) value, the more accurate it is.
· Systematic Error - Produces values that are either all higher or all lower than the actual value. (causes: faulty measuring device, or consistent mistake in taking a reading)
· Random Error- I the absence of systematic error, produces some values that are higher and some values that are lower than the actual value. (always occur)
· PRECISE MEASUREMENTS HAVE LOW RANDOM E...