chapter 3 scientific measurement qualitative measurements- give results in a descriptive,...
TRANSCRIPT
Chapter 3Scientific Measurement
• Qualitative measurements- give results in a descriptive, non-numerical form
• Quantitative measurements- give results in a definite form, as numbers and units.
• Scientific notation- a number is written as the product of two numbers- a coefficient and 10 raised to a power.
Ex: 3.6 x 10^4
• 3.6 represent the coefficient- always greater than or equal to 1 and less than 10
• 4 represents the exponent- indicates how many times the coefficient must be x by 10 to = the original number.
• For numbers greater than 10, the exponent is + and equals the number of places the original decimal point has been moved to the left. Ex: 36000= 3.6x10^4
• For numbers less than 10, the exponent is negative and equals the number of places the original decimal point has been moved to the right. Ex: 0.0081= 8.1x10^-3
• To multiply numbers written in scientific notation, multiply the coefficients and add the exponents.
• Ex: (3.0x10^4)(2.0x10^2)=(3.0x2.0)x 10^(4+2)= 6.0 x 10^6
• To divide numbers written in scientific notation, first divide the coefficients. Then subtract the exponent in the denominator (bottom) from the exponent in the numerator (top).
Multiplication & Division
Addition & Subtraction• Before adding or subtracting numbers
written in scientific notation, the exponents must be the same.
• Ex: (5.40 x 10^3) + (6.0 x 10^2)
• Make the exponents the same by choosing one to change
• Ex: (5.40 x 10^3) + (0.60 x 10^3)= 6.0 x 10^3
Accuracy & Precision
• Accuracy- a measure of how close a measurement comes to the actual or true value of whatever is measured.
• Precision- a measure of how close a series of measurements are to one another.
• Ex: playing darts (text pg. 54)
• Good accuracy and good precision if the darts are close to the bulls eye and to one another
• Poor accuracy yet good precision if the darts are far from the bulls eye but close to one another.
• Poor accuracy and poor precision if the darts are far from the bulls eye and from one another.
Accepted value, Experimental value and Percent Error
• Accepted value- the correct value based on reliable references.
• Experimental value- the value measured in the lab.
• Error= experimental value – accepted value (can be + or – value).
• Percent Error=([error]/accepted value) x 100. (will always be +)
Significant figures in measurements
• Include all of the digits that are known, plus a last digit that is estimated
• Measurements must always be reported to the correct number of significant figures.
Rules of Significant Figures
• Every nonzero digit in a measurement is assumed to be significant
Ex: 24.7 meters, 0.743 meter, 714 meters
All have 3 significant figures
• Zeros appearing between nonzero digits are significant
Ex: 7003 meters, 40.79 meters, 1.503 meters all have 4 significant figures
• Leftmost zeros appearing in front of nonzero digits are not significant. They act as placeholders
Ex: 0.0071 meter, 0.42 meter, 0.000099 meter all have 2 significant figures
*write in scientific notation to get rid of the placeholding zeros
Ex: 7.1 x10^-3, 4.2 X10^-1, 9.9 x10^-5• Zeros at the end of a number and to the right of
a decimal point are always significant
Ex: 43.00 m, 1.010 m, 9.000 m all have 4 significant figures
• Zeros at the rightmost end of a measurement that lie to the left of an understood decimal point are not significant if they serve as placeholders to show the magnitude of the number.
Ex: 300. m—has one sig.fig. 7000. m—has one sig.fig. 27210. m—has 4 sig.figs.*the zeros are not significant. If the zeros were
known measured values, then they would be significant
Ex: if all of the zeros in the measurement 300 m were significant (not rounded)
Writing the value in scientific notation makes it clear the zeros are significant (3.00 x 10^2)
Significant figures in calculations
• Rounding: less than 5 do not round up, greater than 5 round up
• In addition, subtraction, multiplication, and division, round the answer to the same number of sig.figs. as the measurement with the least amount of sig.figs.
Ex: 12.52 + 349.0 + 8.24 =369.76, the answer should be rounded to 369.8 because 349.0 has the least amount of sig.figs (being one sig.fig. After the decimal point)
Metric System
• Standard system used by scientists
• aka International System of Units (SI)
• Decimal system based on the number 10, multiples of 10
• Used to measure length, volume, mass, density, and temperature
Length • Basic unit is the meter (m)• Metric ruler• 1m= 39.4 inches• 1m=100cm• 1m=1000mm• 1000m=1km• 1x10^-6m=1um(micrometer) or 1x10^6um=1m• 1x10^-9m=1nm(nanometer) or 1x10^9nm=1m• K H D M D C M * * um * * nm L cc g (text pg. 64)
Volume• Amount of space an object takes up• V=LxWxH• Basic unit is the Liter (L) or cm^3, mL• Graduated cylinder is used to measure volume
of liquids or irregular shaped solids by water displacement
• Read water level on graduated cylinder at the meniscus
• Use metric ruler to measure volume of solids: LxWxH
• 1 cubic centimeter= 1 milliliter• 1cubic meter= 1000 Liters• (text pg. 65)
Mass• Amount of matter in an object (remains
constant)• Different from weight- a force that
measures the pull of gravity on a given mass (can change)
• Basic unit Kilogram, gram• Use triple beam balance• 1Kg=2.2lbs.• 1Kg=1000g• 1000Kg=1 metric ton• (text pg. 67)
Density
• Mass per unit volume
• D=M/V
• Units g/cm^3, g/mL
• Density of water= 1g/mL
• Float< 1g/mL < Sink
• Density table on pg. 69
Specific Gravity• The comparison of the density of a substance
with the density of a reference substance at the same temp.
• Common reference substance is water• Specific gravity= density of substance/ density of water • No units because they cancel out
(g/cm^3/g/cm^3)• Hydrometer measures specific gravity of liquid• Hydrometer is a sealed tube with a weight in the
bottom. The higher it floats the higher the specific gravity of the liquid being tested
• Specific gravity measurements (no units)
• Used by physicians to diagnose certain diseases (diabetes)
• Check antifreeze condition in radiator
• Measure acid in an automobile battery
Temperature• Kelvin (K) scale or degrees Celsius
• Use thermometer with degrees Celsius
• 0 degrees Celsius= 273 K
• 100 degrees Celsius= 373K
• Water freezes 0 degrees Celsius or 273K
• Water boils 100 degrees Celsius or 373K
• 0 Kelvin or absolute zero= -273K
• K=Celsius + 273
• C=K - 273