Some of the content of this guide was modeled after a guide originally created by Openstax and has been adapted for the NWP Learning Commons in September 2020. This work is licensed under a Creative Commons BY NC SA 4.0 International License.
Significant figures, or significant digits, are used in science as a way to account for the uncertainty in numbers obtained through measurement. All measurements have some level of uncertainty. How much uncertainty depends on how the measurement was made - the equipment used and the skill of the person making the measurement.
1. All non-zero digits are significant.
52.76 and 2367 both have four significant figures.
2. Captive zeros (zeros that are between non-zero digits) are significant.
502 and 2.07 both have three significant figures.
3. Leading zeros (to locate the decimal point) are not significant.
0.0527 and 0.205 both have three significant figures.
4. Trailing zeros (located to the right of significant figures by the other three rules) are only significant if a decimal is present.
5.60, 520. and 5760 all have three significant figures.
Examples
Exceptions
Exact numbers, those that are counted or defined rather than measured, do not have uncertainty. Because they are exact, they are considered to have infinite significant figures.
Rounding Rules
Identify the first digit to be dropped (immediately to the right of the last significant figure). If it is:
example: rounding 52.51 to three significant figures becomes 52.5
example: rounding 52.57 to three significant figures becomes 52.6
examples: rounding to three significant figures
52.55 becomes 52.6 (round up to make last sig. fig. even)
52.65 becomes 52.6 (round down to make last sig. fig. even)
52.6500 becomes 52.6 (round down to make last sig. fig. even)
52.6501 becomes 52.7 (round up because there is a non-zero digit following the 5 to be dropped)
These rules are designed to reduce bias and rounding error. Rounding error can be further reduced by carrying extra digits through your calculations and rounding only at the last step. Keep track of the required number of significant figures at each calculation step (according to the rules below) so you know how many significant figures you need in your final value. For greater explanation of the reasoning around these rounding rules (and a practice quiz!), check out the University of Calgary Chemistry Textbook.
Addition and Subtraction
Example I
2.550 + 3.5001 = 6.0501 (We are not done yet!)
Therefore the answer should have three digits after the decimal. The fourth number is one. Since it's less than five we should round down the final answer to 6.050
Example II
52.36095 - 32.232 = 20.12895
Therefore the answer should have three digits after the decimal. The fourth number is nine. Since it's greater than five we should round up the final answer to 20.129
Multiplication and Division
The significant figures in the result, for both multiplication and division, are determined by the least number of significant figures in any number.
Example I
An object has a mass of 35.5324 g and a volume of 15.0 cm3, then find the density.
15.0 cm3 has the least number of significant figures (three significant figures), therefore the answer has three significant figures.