Chapter 2: Measurements and Calculations

Units of Measurement A standard system for measurements called Le Systeme Internatitional d’Unites was adopted by the General Conference on Weights and Measures in 1960. These units of measurements are abbreviated SI units.

Units of Measurement Table 2-1 on page 34 of your text lists the 7 base SI units. Quantity Unit Name Abbreviation Length meter m Mass kilogram kg Time second s Temperature Kelvin K Amount of Mole mol Substance

SI Prefixes (P35) Prefix- Symbol Exponent Factor Value Tera T 1012 1 000 000 000 000 Giga G 109 1 000 000 000 Mega M 106 1 000 000 Kilo k 103 1000 Hecto h 102 100 Deka da 101 10 Deci d 10-1 0.1 Centi c 10--2 0.01 Milli m 10-3 0.001 Micro μ 10-6 0.000 001 Nano n 10-9 0.000 000 001

Units of Measurement Page 36 The base SI units may be combined to form derived units. For example volume has three dimensions. Therefore volume can be expressed as m x m x m = m3 Table 2-2 on page 35 of your text lists the SI prefixes. Please review these.

Unit Conversions A conversion factor is a ratio derived from the equality between two different units of measurement and can be used to convert from one unit to another unit. For example 1 m = 1000 mm So the ratio and equal 1, and

Unit Conversions Your Turn: If you have 350 mg, how many grams do you have? Table 2-2 on page 35 of your text lists the SI prefixes.

DENSITY is an important and useful physical property Water Mercury Gold 13.6 g/cm3 19.3 g/cm3 1.0 g/cm3

Water Water is used as one of the bases for the SI unit system. The density of water is set to 1.0 g/cm3, in other words, 1 cm3 of water weighs 1 g. Also 1 mL is equivalent to 1 cm3. Therefore 1 g = 1 cm3 = 1 mL

Problem: A piece of copper has a mass of 57. 54 g. It is 9 Problem: A piece of copper has a mass of 57.54 g. It is 9.36 cm long, 7.23 cm wide, and 0.95 mm thick. Calculate its density (g/cm3).

SOLUTION 1. Get dimensions in common units. . 95 mm • 1 cm 10 mm = 095

SOLUTION 1. Get dimensions in common units. 2. Calculate volume in cubic centimeters. (9.36 cm)(7.23 cm)(0.095 cm) = 6.4 cm3 3. Calculate the density. . 95 mm • 1 cm 10 mm = 095 57 . 54 g = . 3 9 g / cm 3 6 . 4 cm

Your Turn: Mercury (Hg) has a density of 13. 6 g/cm3 Your Turn: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg in grams? Solve the problem using DIMENSIONAL ANALYSIS. Recall that 1.00 cm3 = 1.00 mL

First, recall that 1 cm3 = 1 mL PROBLEM: Mercury (Hg) has a density of 13.6 g/cm3. What is the mass of 95 mL of Hg? First, recall that 1 cm3 = 1 mL 95 ml = 95 cm3 Then, use dimensional analysis to calculate mass.

Practice What is the volume of a sample of liquid mercury that has a mass of 76.2 g given that the density of mercury is 13.6 g/mL?

Precision and Accuracy Precision is a measure of how nearly duplicate measurements agree with each other. Accuracy is a measure of how near a measurement is to the true value.

Percent Error Percent error is the relative difference between a measurement and the true value reported as a percentage. Percent error is calculated

Percent Error For example You obtain the value 5.55 g upon weighing a beaker full of water. The actual weight of the beaker full of water is 5.75 g. What is the percent error of you measurement? = 3.48 %

Significant Figures All nonzero digits are significant. All zeros that lie between nonzero digits are significant. None of the zeros that lie to the left, or in front, of the first nonzero digit are significant. Zeros to the right of the last nonzero digit are significant ONLY if they lie to the right of the decimal point.

Significant Figures For example how many significant figures are in each of the following numbers Number Significant Digits 3056 4 4000 1 0.035 2 30.00 4 1.0001 5 0.0001 1

Significant Figures Adding and Subtracting When adding and subtracting, line up the decimal points and round all numbers down to the one with the fewest decimal digits. For example Position of the least sig. fig. 1500 hundreds 25.5 tenths 100.2 tenths 1600 hundreds

Significant Figures Multiplying and Dividing Regardless of the locations of decimal points, the result must have no more significant digits than those in the factor with the smallest number of significant digits. For example 4.0 x 3.00 x 2.0 = 24 2 x 3.000 = 6

Scientific Notation Scientific notation is used to express very large or very small numbers. In scientific notation in the form M x 10n, where the factor M is a number equal to or greater than 1 and less and 10, and n is a whole number. For example 101,000 = 1.01 x 105, and 0.000004 = 4.0 x 106

Direct Proportions Two quantities are directly proportional to each other if dividing one by the other gives a constant value. This can be expressed mathematically as y/x = k, or y = kx Does the equation y = kx look familiar?

Inverse Proportions Two quantities are inversely proportional to each other if multiplying one by the other gives a constant value. This can be expressed mathematically as yx = k, or y = k/x