Chapter One Review PDF

Chapter One Review 1) Differentiate and characterize the three physical states of matter. 2) Classify a sample of matter as a substance or a mixture, and classify mixtures as homogeneous or heterogeneous. 3) List and describe several techniques used to separate mixtures. 4) State the difference...

Chapter One Review 1) Differentiate and characterize the three physical states of matter. 2) Classify a sample of matter as a substance or a mixture, and classify mixtures as homogeneous or heterogeneous. 3) List and describe several techniques used to separate mixtures. 4) State the difference between an element and a compound. 5) Classify substances as elements or compounds. 6) Memorize the names of the first 36 elements on the periodic table and their location. 7) Know the seven diatomic elements (H2, N2, O2, F2, Cl2, Br2 and I2) 8) Distinguish between potential and kinetic energy. 9) State and apply the law of conservation of matter and energy. 10) Classify properties of and change in matter as physical or chemical. 11) Distinguish between extensive and intensive physical properties of matter. 12) Name SI units for length, mass, time, volume, and density. 13) List and define the common metric units. 14) Distinguish between mass and weight. 15) Perform density calculations and identify substances using density. 16) Distinguish between accuracy and precision. 17) Determine the number of significant figures in measurements. 18) Perform mathematical operations involving significant figures. 19) Convert measurements into scientific notation. 20) Distinguish between inversely and directly proportional relationships. 21) Determine percent error of a measurement from experimental data. 22) Construct conversion factors from equivalent measurements. 23) Apply the techniques of dimensional analysis to a variety of conversion factors. 24) Use dimensional analysis to solve multi-step problems. Matter and Change 1. Classify each of the following as a physical or a chemical property. a) Iron and oxygen form rust. b) Iron is more dense than aluminum c) Oil and water do not mix d) Magnesium burns brightly when ignited e) Mercury melts at -39°C f) Silver tarnishes. g) A sheet of copper can be pounded into a bowl. h) Potassium metal is kept submerged in oil to prevent contact with oxygen or water. i) Helium does not react with any other element. j) A bar of lead is more easily bent than is a bar of aluminum of the same size. 2. Identify each physical property as extensive or intensive. a) melting point b) mass c) density d) length 3. Classify each of the following as a physical or a chemical change. a) breaking a pencil b) water freezing c) frying an egg d) burning wood e) leaves changing color f) recycling an aluminum can g) Moisture in the air forms beads of water on a cold windowpane. h) An electric current changes water into hydrogen and oxygen. i) Yeast cells in bread dough make carbon dioxide and ethanol from sugar. j) Molten bronze is poured into a mold and solidifies to form a statue. 4. Solve each of the following based on conservation of mass: a) In the complete reaction of 22.99 g of sodium with 35.45 g of chlorine, what mass of sodium chloride is formed? b) A 12.2 g sample of X reacts with a sample of Y to form 78.9 g of XY. What is the mass of Y that reacted? 5. Classify each of the following as either a heterogeneous or homogeneous mixture. a) brass b) concrete c) saltwater d) air e) milk f) sand 6. Identify each of the following as an example of an element or a compound. a) sucrose b) helium in a balloon c) a diamond d) aluminum foil e) table salt 7. Describe the separation technique that could be used to separate each of the following mixtures. a) two colorless liquids b) an insoluble solid mixed with a liquid Scientific Measurements and Calculations in Chemistry 1. How many centigrams are in a gram? 2. How many liters are in a kiloliter? 3. How many nanoseconds are in a second? 4. How many meters are in a kilometer? 5. Calculate the density of a piece of a bone with a mass of 3.8 g and a volume of 2.0 cm3. 6. A spoonful of sugar with a mass of 8.8 grams is poured into a 10 mL graduated cylinder. The volume reading is 5.5 mL. What is the density of the sugar? 7. A 10.0 g pat of butter raises the water level in a 50 mL graduated cylinder by 11.6 mL. What is the density of the butter? 8. A sample of metal has a mass of 34.65 g. When placed in a graduated cylinder containing water, the water level rises 3.3 mL. Which of the following metals is the sample made from: silver, d=10.5 g/cm3; tin, d=7.28 g/cm3; or titanium, d=4.5 g/cm3? 9. Rock salt has a density of 2.18 g/cm3. What would the volume be of a 4.8 g sample of rock salt? 10. A piece of lead displaces 1.5 mL of water in a graduated cylinder. Lead has a density of 11.34 g/cm3. What is the mass of the piece of lead? 11. Express each answer in scientific notation with correct significant figures and units. a) (1.26 x104 kg) + (2.5 x 106 g) in kg c) (4.39 x 105 kg) – (2.8 x 107 g) in kg b) (7.06 g) + (1.2 x 10 kg) in kg -4 d) (5.36 x 10-1 kg) – (7.40 x 10-2 kg) in g 12. Use dimensional analysis to determine the following: a) The speedometer in a car reads 63 miles per hour. What is the speed in km/hr? (1 mile = 1609 m) b) The density of a material is 0.821 g/mL. How many cubic millimeters would you have with 71.3 g of this material? c) How many millimeters are there in 2.5 x 102 km? 13. Determine the number of significant figures in each measurement. a) 508.0 L b) 820,400.0 L c) 1.0200 x 105 kg d) 807,000 kg e) 0.049450 s f) 3.1587 x 10 g -4 g) 0.000482 mL h) 0.00084 mL 14. Round each number to four significant figures. a) 84,791 kg b) 38.5432 g c) 256.75 cm d) 4.9356 m 15. Round each number to four significant figures and write in scientific notation. a) 0.00054818 g b) 308,659,000 mm c) 136,758 kg d) 2.0145 mL 16. Perform the following calculations. Round to the correct significant figure. Write the correct units. a) 24 m x 3.26 m b) 120 m x 0.10 m c) 1.23 m x 2.0 m d) 53.0 m x 1.53 m e) 4.84 m / 2.4 s f) 60.2 m / 20.1 s g) 102.4 m / 51.2 s h) 168 m / 58 s 17. Four students made the following measurements of a string: 76.48 cm; 76.47 cm; 76.48 cm; 76.46 cm. The actual length of the string is 76.58 cm. Are the measurements precise? Explain. Are the measurements accurate? Explain. 18. Students collected mass data for a group of coins. The mass of a single coin is 5.00 g. Determine the accuracy and precision of the measurements. Number of coins 5 10 20 30 50 Mass (g) 23.5 54.5 105.9 154.5 246.2 19. The accepted density for copper is 8.96 g/mL. Calculate the percent error for each of these measurements. a) 8.86 g/mL b) 9.00 g/mL c) 8.92 g/mL d) 8.98 g/mL 20. Answer the following using dimensional analysis; a) A troy ounce is equal to 480 grains, and 1 grain is equal to 64.8 milligrams. If the price of gold is $560 per troy ounce, what is the cost of 1.0 g of gold? b) The average mass of a kernel of popcorn is 0.125 g. If 1 pound = 16 ounces, and 1 ounce = 28.3 g, then how many kernels of popcorn are there in 0.500 pounds of popcorn? c) You have 15 g of hemoglobin in every 100 mL of your blood, 10.0 mL of your blood can carry 2.01 mL of oxygen. How many milliliters of oxygen does each gram of hemoglobin carry? d) The recommended calcium intake for teenagers is 1300 mg per day. A glass of milk contains 305 mg of calcium. One glass contains a volume of 8 fluid ounces. How many liters of milk should a teenager drink per day to get the recommended amount of calcium? One fluid ounce equals 29.6 mL.