2014 Chemistry 1 st Semester Exam Review Packet

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1 Name: Date: Hour: 2014 Chemistry 1 st Semester Exam Review Packet 1. What percentage of the water on Earth is salt water? (1 point) A. 97.2% B % C. 2.11% D. 2.8 % 2. One similarity between all mixtures and compounds is that both. (1 point) A. are heterogeneous B. are homogeneous C. combine in a definite ratio D. consist of two or more substances 3. An atom of carbon-12 and an atom of carbon-14 differ in. (1 point) A. atomic number B. mass number C. nuclear charge D. number of electrons 4. How many times more acidic is a solution of ph 8 than a solution of ph 5? (1 point) A. 3X B. 30X C. 300X D. 1,000X E. 100X 5. Which of the following elements is most chemically similar to magnesium? (1 point) C4.9A A. calcium B. manganese C. sodium D. aluminum 6.. The density of tin is 7.3 g/ml. The density of lead is g/ml. The density of silicon is 2.33 g/ml. Therefore, the density of germanium must be. (1 point) C4.9c A. 1.5 g/ml B. 5.3 g/ml C g/ml D g/ml 7. Since an atom is electrically neutral, the number of protons is equal to the number of. (1 point) C4.10A A. neutrons B. electrons C. neutrons + electrons D. neutrons electrons 8. Fact 1: Zinc releases hydrogen gas when exposed to hydrochloric acid. Fact 2: Zinc s density is 7.14 g/ml. The 1 st fact describes a, and the 2 nd fact describes a. (1 point) C5.2B A. physical change, physical property D. chemical change, chemical property B. physical property, chemical change E. physical property, physical property C. chemical change, physical property F. chemical property; physical change 9. Which list of elements consists of nonmetals only? (1 point) C4.9b A. boron, gallium, germanium B. oxygen, sulfur, selenium C. aluminum, boron, silicon D. boron, silicon, germanium 10. Which of the following atoms represent the same element? (1 point) C4.10B Atoms Protons Neutrons Electrons A B C D A. Element A & Element B B. Element C & Element D C. Element B & Element C D. Element B & Element D E. Element A & Element C F. Element A & Element D 11. In an atom of argon-40, the number of protons. (1 point) A. equals the number of electrons B. equals the number of neutrons C. is less than the number of electrons D. is greater than the number of electrons 1

2 12. Which statement describes a chemical property of bromine? (1 point) A. bromine is soluble in water B. bromine has a reddish-brown color C. bromine combines with aluminum to produce AlBr 3 D. bromine changes from a liquid to a gas at 23 0 C 13. A sample of an element is malleable and can conduct electricity. This element could be. (1 point) A. H B. He C. S D. Sn 14. Given the balanced particle diagram below: + Which statement describes the type of change and the chemical properties of the product and reactants? (1 point) A. the equation represents a physical change, with the product and reactants having different chemical properties B. The equation represents a physical change, with the produce and reactants having identical chemical properties C. The equation represents a chemical change, with the product and reactants having different chemical properties D. The equation represents a chemical change, with the product and reactants having identical chemical properties 15. An element that is malleable and a good conductor of heat and electricity could have an atomic number of. (1 point) A. 16 B. 29 C. 18 D. 35 E On the modern Periodic Table, the elements are arranged in order of increasing. (1 point) A. atomic mass B. mass number C. charge D. atomic number 17. What can be determined if only the atomic number of an ion is known? (1 point) A. the total number of neutrons only B. the total number of protons only C. the total number of protons and neutrons D. the total number of protons and electrons 18. Chlorine-37 can be represented as. (1 point) A. Cl B. Cl C. Cl D. Cl Sodium and potassium have similar chemical properties because an atom of each element has the same. (1 point) A. oxidation number B. # of neutrons C. # of protons D. # of electrons Which quantity identifies an element? (1 point) A. atomic number B. mass number C. number of neutrons D. total number of electrons 22. What is the total charge of the nucleus of a nitrogen atom? (1 point) A. +5 B. +14 C. 0 D. +2 E Which of the following isotopes will be in greatest abundance in nature? (1 point) C4.10b A. P-30 B. P-31 C. P-15 D. P

3 24. Which of the following drawings represents krypton at room temperature? (1 point) A. B. C. 25. Which of the following is the products side of the chemical equation of solid calcium in aqueous copper (II) nitrate is shown below. (1 point) C5.6b Ca (s) + Cu(NO 3) 2 (aq) A. Cu (s) + Ca(NO 3) 2(aq) B. Ca (aq) + Cu (aq) + 3 N 2 (g) + 9 O 2 (g) C. Cu 3Al 2 (s) + 2 NO 3 (aq) D. Ca (s) + Cu (s) + N 2O 6 (aq) E. Cu (s) + CaNO 3 (aq) 26. What element on the periodic table will have very similar properties to copper, Cu? (1 point) (C4.9A) A. iron B. silver C. nickel D. zinc E. aluminum 27. What trend in metallic reactivity is apparent as you move from left to right across a horizontal row (period) of the periodic table? (1 point) A. Reactivity decreases B. Reactivity increases C. Reactivity stays the same D. Impossible to predict 28. Which of the following metals would be the most difficult to extract from their ores? (1 point) A.) aluminum B.) silver C.) gold D.) iron 29. In which part of the periodic table are the most reactive-metals found? (1 point) A. Bottom left B. Top right C. Middle D. Top left E. Bottom right Identify each of the following as being a physical (A) or chemical (B) change. (1 point each) 30. a cut apple left out in the air turns brown 31. dry cleaning removes oils from clothing 32. an opened carbonated beverage fizzes 33. as shoes wear out, holes appear in the soles What is happening to the average kinetic energy of the molecules in the sample during section 2? (1 point) A. increasing B. decreasing C. staying the same D. impossible to tell 3

4 35. As a substance goes from step 3-4, what happens to the distance between the particles?(1 point) A. increasing B. decreasing C. staying the same D. impossible to tell 36. What is the condensing point (temperature) of this substance? (1 point) A C B C C C D C E C Identify each of the following as being an element (A), mixture (B), or compound (C). (1 point each) 37. milk 38. CO silver 40. concrete Identify each of the following compounds as being soluble (A) or insoluble (B) in water. (1 point each) 45. silver sulfate 46. potassium hydroxide 47. CuNO Na 2CO 3 Use each element s electronegativity to identify whether each of the following molecules are polar covalent (A), nonpolar covalent (B), or ionic (C). (1 point each) 49. H 2O 50. LiF 51. NH O 2 Identify each of the following statements as referring to an acid (A), base (B) or neither (C). (1 point each) 53. KOH 59. ph = HNO sour tasting 55. NaCl 61. [H+] = [OH-] 56. H 2SO slippery to touch 57. red litmus turns blue 63. ph = ph = [H+] < [OH-] 65. Where is most of Earth s fresh water located? (1 point) A. lakes & ponds B. rivers and streams C. glaciers D. ocean Match the following terms. (8 points) 66. supersaturated A. substance being dissolved (in lesser quantity) 67. saturated B. maximum amount of solute dissolved 68. unsaturated C. not able to dissolve 69. soluble D. homogeneous mixture 70. insoluble E. excess solute dissolved at higher temperature, then cooled 71. solvent AB. able to dissolve 72. solution AC. more solute is still able to be dissolved 73. solute AD. substance doing the dissolving (in greater quantity) 4

5 74. Which substance in the solubility curve above is least soluble at 10 0 C? (1 point) A. KI B. Ce 2(SO 4) 3 C. KClO 3 D. NH 3 E. KNO Ammonia, NH 3, is a gas. What happens to the solubility of gases as temperature decreases? (1 point) A. increases B. decreases C. stays the same 76. At 40 0 C, 70 g KNO 3 is dissolved in 100 g of water. Is this solution? (1 point) A. saturated B. supersaturated C. unsaturated? 77. Which substance s solubility changes the least from 0 0 C to C? A. KI B. Ce 2(SO 4) 3 C. KClO 3 D. NH 3 E. NaCl 78. Which of the following is the best method to purify water that is contaminated with insoluble solid (can t dissolve) substances such as sand? (1 point) A. distillation B. precipitation C. filtration D. decanting 1. Calculate the density of a substance that has a mass of 4.5 g and a volume of 2.4 ml. (2 points) 2. Calculate the mass of a 5.5 ml nugget of aluminum that has a density of 1.9 g/ml. (2 points) 3. In each of the following beakers, draw what the same sample of water, H 2O, would look like on a molecular scale as a solid, liquid, and gas. C2.2B (3 points) Solid Water Liquid Water Water Vapor 5

6 4. Convert the following measurements. You must show your work and use the fence method to receive full credit. (4 points) 46.3 hours = years 65 mi/hr = km/s 5. Complete the chart. (8 points) Substance S Fe Atomic number 13 Mass number Protons Neutrons Electrons Metal, Nonmetal, Metalloid Name the following ionic compounds. (6 points) CoCl 2: Mn 3(PO 4) 2: MgBr 2: NaOH: (NH 4) 2Cr 2O 7: AuP: 7. Write formulas for the following ionic compounds. (6 points) calcium iodide: tin (IV) carbonate: copper (II) nitrate: aluminum oxide: lead (IV) sulfide: barium hydroxide: 8. In beakers A and B draw two different compounds, one in each box, using the representations for atoms of element X and element Z given below. In beaker C draw a mixture of these two compounds. (3 points) Atom of element X = Atom of element Z = A B C 6

7 9. How many moles of CaCl 2 are in 150 g of CaCl 2? (2 points) 10. What is the molarity of a solution containing 70 g of CaCl 2 in 275 ml of solution? (2 points) Atom/Ion/Element A B C D E F G # electrons # protons # neutrons Table Which of the substances in Table 1 represent the same element? (1 point) 12. Write the correct isotopic symbol for substances A, C, and E listed in Table 1. Include in your symbol the element symbol, atomic number, mass number, and charge if applicable. (An example is given for reference.) (3points) 2 Ex: 1 H +1 A C E 13. Using the metal reactivity series, write the products of the reactions that will occur. Balance all reactions. If a reaction will not occur, write NR after the arrow. (3 points) C5.6b (Use the following charge for the transition metal: Pt +4 ) Al (s) + Zn(NO 3) 2 (aq) Pt (s) + Sn(NO 3) 2 (aq) Br 2 + KI 14. Assign oxidation numbers for all elements in each compound. (5 points) NaClO 3 Na = Cl= O= -3 PO 4 P = O = H 5P 3O 10 H = P = O = -1 SbF 6 Sb = F= 7

8 liter (giga) (mega) (kilo) (hecto) (deka) meter (deci) (centi) (milli) (micro) (nano) (pico) G- M- k- h- da- gram d- c- m- - n- p- byte 0 F = 9/5( 0 C) cm 3 = 1mL 0 C = ( 0 F-32)5/9 1 dm 3 = 1,000 ml = 1L K = 0 C m 3 = 1,000,000 ml = 1,000 L 1 lb 1 kg 1 m 1 in 1 mile 1 mile 2.54 cm 5,280 ft km g 2.2 lbs 3.28 ft density = mass volume Molarity = # moles # liters moles = # grams molar mass Electronegativity difference Ionic = > 1.7 Polar = 0.51 to 1.69 Nonpolar = < 0.5 8

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