Chapter 1 review

Matter States of Matter: solid, liquid, gas How do we classify matter? Physical Properties of Matter Physical Change vs Chemical Change Measurements

Measurements Dimensional Analysis Density Temperature: K, ºF, ºC ºC = (ºF – 32)/1.8 K = ºC + 273 ºC = K – 273

Common Units and Their Equivalents Length 1 kilometer (km) = 0.6214 mile (mi) 1 meter (m) 39.37 inches (in.) 1.094 yards (yd) 1 foot (ft) 30.48 centimeters (cm) 1 inch (in.) 2.54 centimeters (cm) exactly

Common Units and Their Equivalents Mass 1 kilogram (km) = 2.205 pounds (lb) 1 pound (lb) 453.59 grams (g) 1 ounce (oz) 28.35 grams (g) Volume 1 liter (L) = 1000 milliliters (mL) 1000 cubic centimeters (cm3) 1.057 quarts (qt) 1 U.S. gallon (gal) 3.785 liters (L)

Scientific Notation Locate the decimal point Move the decimal so that there is only one number to the left of it Write “x 10” behind you new number Count the number of places you’ve moved your decimal point and make this number the exponent on your 10 Assign a + or – sign to your exponent If your original # is larger than your SN #, the exponent is + If your original # is smaller than your SN #, the exponent is –

Significant Figures Numbers up to and including the “uncertain” number are significant All non-zero numbers are significant Zeros may or may not be significant Zeros are significant if They are between two non-zero digits They are at the end of a decimal number

Zeros are not significant if They are used as place holders in large numbers without a decimal point They are at the beginning of decimal numbers All numbers displayed in a number written in scientific notation are significant

Calculation With Significant Digits Multiplication and Division The final answer has the same number of sig figs as the measurement with the fewest sig figs Addition and Subtraction The final answer is written so that it has the same number of decimal places as the measurement having the fewest decimal places

Write these numbers using standard scientific notation. 0.0468   0.0468 6,600,000 (two significant figures) Round off these numbers to the number of significant figures indicated. 0.08965 (two significant figures) 88.015 (three significant figures)

Write how many significant figures the answer should contain for each of these calculations.   1200. + 6.34 _________ 94.5 _________ 1.2 119.1 – 3.44 _________

How many centimeters are in 2.00 ft? For the following numbers, tell whether the zeros are significant or are not significant.   0.007 8.00 x 102 100.00 4200 3.0030

  Calculate the following. (Show all work for full credit. Answers should show the correct number of significant figures.) At 35 cents per liter how much will it cost to fill a 15.8 gal tank with gasoline?   How much would 1.0 kg of potatoes cost if the price is $1.78 for 10 pounds? Normal body temperature for humans is 98.6 oF. What is this temperature on the Celsius scale?

Make the following conversions showing mathematical setups 0.606 cm to km 35.6 m to ft. 35 km to mm 1000. m to km 0.64 mi to inches 3.5 quarts to ml

Convert 78oF to degrees Celsius An object weighs 8.22 lbs. What is the mass in grams? A graduated cylinder was filled to 25.0 mL with liquid. A solid object weighing 73.5 grams was immersed in the liquid, raising the liquid level to 43.9 mL. Calculate the density of the solid object. The density of carbon tetrachloride, CCl4, is 1.59 grams/mL. Calculate the volume of 100.0 grams of CCl4.