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1 st Semester Exam in High School Chemistry

1 st Semester Exam in High School Chemistry. Examination in January of 2012 . 1. Substance A is a liquid, Substance B is a gas and Substance C is a solid. .

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1 st Semester Exam in High School Chemistry

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  1. 1st Semester Exam in High School Chemistry Examination in January of 2012

  2. 1. Substance A is a liquid, Substance B is a gas and Substance C is a solid. All of the substances are at the same temperature and pressure. Which of the following shows the correct relationship between the strength of the intermolecular forces in each substance? A. A > B > C B. B > A > C C. C > B > A D. C > A > B

  3. 2. A balloon is inflated with room temperature air, and is placed outside in the sun. The balloon expands due to the rise in temperature. Which of the following describes what happens to the molecules of air as the temperature rises? A. The molecules of air stop colliding with the balloon wall. B. The molecules of air increase in size. C. There are fewer interactions between the air molecules. D. The molecules of air move more quickly.

  4. 3. Condensation occurs when _____________________ . A. a gas loses energy to become a liquid B. a solid gains energy to become a liquid C. a liquid gains energy to become a gas D. a gas loses energy to become a solid

  5. 4. As liquid carbon dioxide freezes, its molecules ________________ . A. absorb heat energy and move farther apart B. absorb heat energy and move closer together C. release heat energy and move farther apart D. release heat energy and move closer together

  6. Compared to the particles in a gas, the particles in a solid move_____________ . A. at the same speed as the gas B. quicker and farther than the gas C. quicker than the gas D. slower than the gas

  7. 6. Which one of the following is a TRUE statement? A. Gas molecules move around freely. B. Liquids do not change shape easily. C. Gas molecules move more slowly as they are heated. D. Solids change shape easily.

  8. 7. Which of the following BEST describes what happens when most substances change from a solid state to a liquid state? A. The molecules slow down. B. The molecules move farther apart. C. The molecules get smaller. D. The molecules lose energy.

  9. 8. Unlike most substances, water is unusual because it ____ when it goes from the liquid to solid state. A. contracts B. melts C. expands D. diffuses

  10. 9. Which of the following is an example of a chemical change? A. filling a balloon with helium B. freezing a glass of water C. a plant collecting energy from the sun to create food D. a dog ripping a newspaper

  11. 10. What happens to the atoms of the reactants in a chemical reaction? A. They change into new atoms. B. They recombine to form the products. C. They change names. D. Some are lost to the environment.

  12. 11. When two substances react chemically, what type of products will be formed? A. Products will be very similar to the reactants. B. Products will be very different from the reactants. C. The products will vary from one reaction to another. D. Products of a chemical reaction cannot be predicted.

  13. 12. A good hypothesis _____________ . A. can be tested by experiment B. can be an educated guess predicting the outcome of an experiment C. can only be formed when you know something about what is going to happen D. may be described by all of the above

  14. 13. In the late nineteenth century, Dmitri Mendeleev spent two years developing a table that could be used to predict which of the following? A. age of mineral samples B. movements of planets C. composition of stars D. properties of elements

  15. 14. Is science limited only to ideas and concepts that are testable? A. Yes, because scientists can only make theories about things that have been measured. B. Yes, because scientists cannot create new theories from nothing. C. No, because natural phenomena can be observed, but not always measured. D. No, because scientific theories change as public opinion changes.

  16. 15. Which family correctly labels the elements in Group 1 on the Periodic Table? A. transition metals B. alkali series C. lanthanide elements D. actinide series

  17. 16. Which is the BEST conclusion that can be made from the information shown on the graph below? A. Electrons in Period 3 are more difficult to remove from an atom than electrons in Period 2. B. In general, going from left to right across a period on the Periodic Table, electrons become increasingly difficult to remove from an atom. C. Period 2 atoms are larger in size than Period 3 atoms, decreasing the attraction of the valence electrons for the nucleus. D. As the number of valence electrons increases, the electron removal energy decreases.

  18. 17. Melting Point of Elements Use the data shown below to create a graph on the element’s melting point. Students should make a bar graph of the data.

  19. 18. Explain how the melting point of a metal compares to the melting point of a nonmetal. 18. The melting point of a metal is generally higher, except for the nonmetal that is next to the metalloid.

  20. 19. Why is an atom considered electrically neutral? A. neutrons equal the number of protons B. proton forces pull on the neutrons C. electrons equal the number of protons D. electrons equal the number of neutrons

  21. 20. Which of the following statements describes isotopes of an atom? A. different chemical properties B. different numbers of protons C. different masses D. different numbers of electrons

  22. 21. Using the Periodic Table, predict which elements will have similar chemical properties or reactivity. A. cadmium, calcium and carbon B. magnesium, strontium and barium C. rubidium, yttrium and zirconium D. nitrogen, sulfur and bromine

  23. 22. Choose the correct Lewis Dot diagram for NaCl. A. B. C. D.

  24. 23. As the atomic number increases, within a group of elements, the atomic radius usually ________________ . A. decreases B. remains the same as the one above it C. increases D. decreases, then increases

  25. Which of the following increases as the electronegativity difference between 2 atoms increases? A. ionic nature of the bond B. covalent nature of the bond C. metallic nature of the bond D. electron sharing between the 2 atoms

  26. What is the formula for potassium fluoride? A. KF B. KF2 C. K2F D. K2F2

  27. 26. What is the formula for the compound formed by iron (II) ions and chromate ions? A. FeCrO4 B. Fe2CrO4 C. Fe2(CrO4)3 D. Fe(CrO4)2

  28. 27. What is the formula for aluminum hydroxide? A. AlOH B. Al(OH)3 C. A l2(OH)3 D. A l3OH

  29. What is the name of the compound: N2O3? A. sodium dioxide B. dinitrogen oxide C. nitrous oxide D. dinitrogen trioxide

  30. 29. What is the formula for tin (IV) oxide? A. Tn4O2 B. SnO C. TnO2 D. SnO2

  31. 30. What is the formula for barium nitrate? A. Ba(NO3)2 B. BaNO2 C. Ba2NO3 D. Ba(NO4)2

  32. 31. What is the name of the compound AlPO4? A. aluminum phosphide B. aluminum phosphate C. aluminum phosphite D. aluminum phosphoroxide

  33. 32. Which of the following is the metallic ion in scandium (II) chloride? A. Sd2 + B. Cl2- C. Sc 2 + D. Cl1-

  34. 33. Using the Nutrition Facts label to the right, which of the following formulas is CORRECT for the highlighted ingredient? A. Na2PO3 B. Na3PO4 C. NaPO D. Na3(PO4)2

  35. 34. Select the correct name for this compound. A l2(SO4)3 A. dialuminumtrisulfate B. aluminum trisulfide C. aluminum sulfate D. sulfuric aluminate

  36. 35. Choose the correct name for the following. HClO3 A. hydrogen chloroxide B. hydrogen trichlor C. hypochlorite D. chloric acid

  37. 36. What is the name of the compound NiSO4 ? A. nickel (II) sulfite B. nickel (II) sulfide C. nickel (II) sulfate

  38. 37. What is the oxidation number of nitrogen in most compounds? A. -3 B. -2 C. -1 D. + 1

  39. 38. What is the oxidation number of hydrogen in HCl? A. 0 B. +1 C. + 2 D. + 3

  40. Name the compound. H2O A. dihydrogen monoxide B. hydrogen oxide C. hydrogen oxalate D. hydrogen dioxide

  41. 40. Name the following. Li2S A. dilithiummonosulfide B. lithium sulfide C. lithium disulfide D. sulfuric lithate

  42. 41. Which of the following is a possible compound formed from Calcium (2+) and the polyatomic ion Nitrate, NO3 (-1)? A. Ca2NO3 B. Ca3NO2 C. CaNO D. Ca(NO3)2

  43. 42. Carbon tetrachloride is a solvent which is used as a refrigerant and also as a cleaning agent. Prior to the 1950s, carbon tetrachloride was manufactured by the chlorination of carbon disulfide: CS2 + 3 Cl2 → CCl4 + S2Cl2 but now it is mainly produced from methane: CH4 + 4 Cl2 → CCl4 + 4 HCl How many grams of carbon tetrachloride can be produced from reacting 709.0 grams of Chlorine (Cl2) with excess methane? A. 3.845 g B. 61.53 g C. 384.5 g D. 6153 g

  44. 43. What is the coefficient for potassium in the balanced equation? ____ Na + ____K2S → ____ K + ____ Na2S A. 2 B. 4 C. 6 D. 8

  45. For the reaction HCl + NaOH > NaCl + H2O, which reactant is the limiting reactant given 100.0 g of sodium hydroxide and 100.0 g of hydrochloric acid? A. hydrochloric acid B. sodium hydroxide C. sodium chloride D. water

  46. 45. In the reaction A + B → C + D, if element B is in excess, then — A. A is the limiting reactant. B. B is the limiting reactant. C. C is the limiting reactant. D. both A and B are limiting reactants.

  47. In the reaction 2RbNO3 → 2RbNO2 + O2 how many moles of O2 are produced when 5.0 mol of RbNO3 decompose? A. 1.0 mol B. 2.5 mol C. 3.0 mol D. 7.5 mol

  48. 47. How many molecules are represented by 3.00 moles of oxygen, O2? A. 4.98 x 1024 B. 3.00 C. 6.32 x 102 1 D. 1.81 x 1

  49. 48. White phosphorous is used as an incendiary weapon and smoke tracer. It can also be used to create smoke screens to mask troop movement or hide platoon position. Robert Boyle was the first to use phosphorus to ignite sulfur tipped wooden splints, forerunners of our modern matches, in 1680. One of the ways in which it can be made involves the fusion of calcium phosphate with carbon and sand in an electric furnace. 2Ca3(PO4)2 + 6SiO2 + 10C → 6CaSiO3 + P4 + 10CO Starting with 100.0 grams of calcium phosphate and assuming excess silicon dioxide and carbon, how many moles of phosphorous will be produced? A. 0.1612 moles B. 0.3224 moles C. 15510 moles D. 1.551 moles

  50. 49. Calcium hydroxide and hydrochloric acid react to form calcium chloride and water as shown in the chemical reaction. If the chemicals are present in exactly the correct ratios to fully use all of the ingredients, how many moles of water would be formed from 5 moles of HCl? __ Ca(OH)2 + __ HCl → __ CaCl2 + __ H2O A. 1 mole B. 2 moles C. 5 moles D. 10 moles

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