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Pure Element Mixture Suspensions, Heterogeneous Mixture Solution

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Pure Element Mixture Suspensions, Heterogeneous Mixture Solution ACP and Chemistry 1 Unit 1 Review Name: ________________________________________ Equipment, Safety, Density, Sig. Fig.’s, Matter & Properties Date: _________________________________________ Classify each of the materials below. In the center column, state whether the materials is a pure substance or a mixture. If the material is a pure substance, further classify it as either an element or a compound in the column to the right. Similarly, if the material is a mixture, further classify it as homogeneous or heterogeneous in the column to the right and note if it is a solution, colloid or suspension. Element or Compound, Material Pure Substance or Mixture Homo/Heterogeneous, solution colloid or suspension 1. Iron filings (Fe) Pure Element 2. Orange Juice (with pulp) Mixture Suspensions, Heterogeneous 3. Pacific Ocean Mixture Solution, Homogeneous 4. Air inside a balloon Mixture Solution, Homogeneous 5. Brass (Cu mixed with Zn) Mixture Solution, Homogeneous 6. Muddy water Mixture Suspensions, Heterogeneous 7. Baking soda (NaHCO3) Pure Compound 8. Lucky Charms Mixture Heterogeneous 9. Milk Mixture Colloid, Homogeneous 10. Chromium (Cr) Pure Element 11. Using the equipment from your lab drawers, what item would be the best to use for each of the following: a. Measuring 120 mL of water ___________Graduated Cylinder_____________________________________________ b. Storing 300 mL of NaOH solution _______ Beaker or Erlenmeyer Flask________________________________ c. ‘Topping off’ a graduated cylinder to 10.00 mL _____ Eye Dropper_______________________________________ d. Transferring a small sample of a solid from its container to a beaker______ Spatula or Tweezers____ 12. A 5.61-gram sample is placed in 14.56 ml of water making the water rise to 17.22 ml. What is the density of the sample? 2.10902255639 g/mL 2.11 g/mL g 13. An object with a density of 2.720 /mL has a mass of 12.66 g. If the object is placed in 20.00 mL of water, to what volume will the water rise? 4.65441176471 mL 4.65 mL 14. A rectangular solid has a mass of 264.1252 g and the dimensions of 1.31 cm by 2.2 cm by 10.45 cm. Determine the density of the solid providing you answer with appropriate significant figures. 8.804173333333 g/mL 8.8 g/mL 15. Determine the number of significant figures in each of the following numbers. a. 5.9100 __4_____ c. 0.0001200 __4___ e. 203 __3_____ b. 0.00385 __3_____ d. 391000 __3___ f. 3010 _3_____ 16. Round the following value to the required number of significant figures: a. 86753090 to 3 sig. fig. __86800000 or 8.68x107_ c. 45319001 to 3 sig. fig. _45300000 or 4.53x107____ b. 0.00087642 to 2 sig. fig. __0.00088 or 8.8x10-4___ d. 0.3718912 to 4 sig. fig. _0.3719 or 3.719x10-1____ 17. Perform the following calculations providing the answer with appropriate number of significant figures. a. 5.40 + 9.811 + 6.2114 + 4.211 = 25.6334 25.63 c. 0.00212 x 0.0073 x 0.001321 = 2.0x10-8 b. 0.00212 + 0.0073 – 0.001321 = 0.008099 0.0081 d. (5.40 x 9.811 x 6.2114) / 4.211 = 78.1 18. Compare and contrast the following terms: a. mass & matter: mass is the measure of the amount of matter, matter is anything that takes up space & has mass__ b. atom & compound _an atom is the smallest form of matter & 2 or more different atoms chemically bonded make compounds__ c. physical property & chemical property __Physical property can be observed w/o changing the compound, Chemical property can only be observed upon reaction___ d. mixture & pure substance __A mixture is multiple substances physically mixed where a pure substance is simply one substance___ e. physical change & chemical change __A physical change is the change in appearance but not chemical make up where chemical change is the change of a substance chemically to make a new substance ____________ 19. Using circles to represent particles, draw diagrams that illustrate the arrangements of particles in solids, liquids, and gases. 20. Explain how energy involved in chemical and physical change. In matter, solids have the lowest energy and slowest movement of particles and Gases have the highest energy and fastest movement of particles. So, the more energy put in, the faster the movement and the change of state occurs. For chemical change, energy is usually put off as in chemical reactions (exothermic) and sometimes taken in (endothermic). 21. Classify each as chemical change (cc) or physical change (pc): a. Ice melting __pc____________________ d. Paper burning __cc_________________ b. Metal rusting __cc__________________ e. Liquid evaporating __pc____________ c. Gas pressure increasing __pc______ f. Food digesting __cc__________________ 22. What is the difference between intensive and extensive properties? Intensive properties do not change when the amount of the substance changes (density, color, etc.), Extensive properties change when the amount changes (mass, volume, etc.) 23. Consider the burning of gasoline and the evaporation of gasoline. Which process represents a chemical change and which represents a physical change? Explain your answer. Gasoline burning produces new compounds (CO2 and H2O) meaning it is a chemical change. Evaporation of gasoline is a physical change because you still have gasoline; it is just changed state from liquid to vapor. 24. Describe the difference between a homogenous mixture and a heterogeneous mixture and give an example of each. An example of a homogeneous mixture is a cup of coffee where it is the same throughout. An example of a heterogeneous mixture would be a chocolate chip cookie where you can see different chips and cookie areas (Every bite is not the same). .
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