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Chemistry: Significant Digits 1. Significant numbers are always measurements and thus should always be accompanied by the measurement's unit. For simplicity, units are not included in the following examples. 2. Any numbers (that are measurements) other than zero are significant. (Many times the zeros are also significant as you will see below.)
Rules for deciding the number of significant figures in a measured quantity: (1) All nonzero digits are significant: 1.234 g has 4 significant figures, 1.2 g has 2 significant figures. (2) Zeroes between nonzero digits are significant: 1002 kg has 4 significant figures, 3.07 mL has 3 significant figures.
When multiplying or dividing two approximately known numbers, the number of significant figures in the result is the smaller of the number of significant figures in the factors. Here are some examples.
The following rules apply to calculations with significant figures: 1. Exact physical and mathematical constants and defined conversion factors (π, 1 inch = 2.54cm, 1kg = 1000g) and integer coefficients (like the 2 in “2πr”) have an infinite number of significant figures. 2.
The questions assess understanding of: 1) Identifying quantitative observations and distinguishing them from qualitative observations. 2) Applying rules of significant figures to calculations and measurements reported to the correct number of significant figures.
2. List the reasons why significant figures are important. 3. Apply guidelines on determining significant figures in chemical measurements. 4. Apply guidelines on determining significant figures in mathematical calculations. 5. Apply guidelines on rounding off chemical measurements and their calculated results. 6.
Chemical calculations involve numbers representing actual measurements. In a measurement, significant figures in a number consist of: Figures (digits) definitely known + One estimated figure (digit) In class you will hear this expressed as "all of the digits known for certain plus one that is a guess."
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