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TE S T S F O R HI G H E R ST A N D A R D S P ROVIDE F OCUS + FACILITATE ACHIEVEMENT Tests for Higher Standards Halifax County Public Schools Chemistry GENERAL & CP 3rd Nine Weeks Benchmark Test 2008 - 2009 Dr. S. Stuart Flanagan, Professor Emeritus College of William and Mary Copyright 2005, S. Stuart Flanagan and David E. W. Mott Do not reproduce without permission. CH.1f 1. A certain chemistry student was performing an experiment to see whether a balance was precise and accurate, so she measured the mass of a 100 g metal weight. The data she recorded is below: Trial 1 2 3 4 5 mass in grams 101.0 101.1 100.9 100.9 101.1 When she looked at her data, she noticed that all the values were close together but all higher than the expected value. What can she say about the balance? A B C D It is accurate but not precise. It is precise but not accurate. It is neither precise nor accurate. It is both precise and accurate. CH.1f 2. If Agnes’s measure of the density of a substance is 1.81 g/cm3 and the accepted value is 2.06 g/cm3, what is the percent error of her measurement? F 12% G 14% H 88% J 114% CH.1g 3. The mass of 165.0 mL of ethyl alcohol, C2H6O, is 129.5 g. What is its density? A B C 0.7848 g / cm3 1.274 mL / g 21.38 kg / mL D 35.50 cc / kg3 _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 1 Do not reproduce without permission. Date CH.2i 4. Rutherford’s alpha-particle experiment, pictured below, helped support what idea? beam of alpha particles radioactive substance circular ZnS-coated fluorescent screen gold foil F G H J Electrons have mass. Electrons have a negative charge. The charge of an electron is 1. Atoms have a dense, positive nucleus. CH.2d 5. Each of the elements in a group or family of the periodic table have what characteristic in common? A B C D the same atomic radius very similar atomic masses similar half-lives the same number of valence electrons CH.2b 6. Different isotopes of an element differ from each other because they have a different number of which particles? F G H J protons electrons photons neutrons _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 2 Do not reproduce without permission. Date CH.2f 7. As you move from top to bottom and from left to right on the periodic table, how does the atomic radius of the atoms change? A B C D It decreases from top to bottom and increases from left to right. It increases from top to bottom and increases from left to right. It decreases from top to bottom and decreases from left to right. It increases from top to bottom and decreases from left to right. CH.2g 8. What is the most common oxidation state of the element described by the following electron configuration: [Ne] 3s2 3p4? F G H J –2 1 0 +2 CH.2h 9. Chlorine, Cl, is most like which of the following elements in its chemical and physical properties? A B C D Lithium, Li Helium, He Fluorine, F Sulfur, S CH.2i 10. Emission of light from an atom occurs when: F G H J an electron jumps from a lower to a higher energy level. an electron drops from a higher to a lower energy level. an electron falls into the nucleus. two electrons collide and are converted into pure energy. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 3 Do not reproduce without permission. Date CH.3c 11. The molecular formula for the sugar glucose is C6H12O6. What would be its empirical formula? A B CHO CH2O C D 6 CHO C2H12O2 CH.1a 12. Study the following drawing. What is the liquid volume indicated on this glass graduated cylinder? mL 10 9 8 7 F G H J 8.2 mL 8.0 mL 7 mL 8 mL _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 4 Do not reproduce without permission. Date CH.1b 13. Study the diagram of the Bunsen burner below. Which part of the flame is the hottest? A B C A B C D A B C None is hotter than any other. CH.1b 14. A student needed to dilute some concentrated hydrochloric acid. How should the student do this? F G H J add distilled water directly to the acid add acid to the distilled water first heat the acid and then add acid to the distilled water first heat the acid and then add distilled water to the acid CH.3a 15. In the formula MgCl2 • 2H2O, the compound is referred to as: A B C D a hydroxide. a hydrate. a dihydride. anhydrous. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 5 Do not reproduce without permission. Date CH.1d 16. What can be determined about a chemical reaction from the data and graph below? Volume of Hydrogen Produced (liters) Mass of Zinc Used (grams) 1 0.37 2 0.73 3 1.10 4 1.47 5 1.84 6 2.21 6 . 5 Mass of zinc 4 3 2 1 0 . . . . . 1 2 3 Volume of hydrogen (L) F G H J The mass of zinc used and hydrogen production are directly proportional. The mass of zinc used and hydrogen production are inversely proportional. The mass of zinc used and hydrogen production are related, but not proportional. The mass of zinc used and hydrogen production are unrelated. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 6 Do not reproduce without permission. Date CH.1g 17. How many significant digits are in the measurement 0.030010 cm? A B C D 7 6 5 4 CH.2a 18. The atomic mass of each element is based on the relative mass of which element? F G H J oxygen - 16 hydrogen - 1 carbon - 12 nitrogen - 14 CH.2h 19. Which of the following is a chemical property? A B C D boiling point resists corrosion dissolves in water melting point CH.2i 20. Of the following atomic models pictured below, which one is most accepted today? F H G J _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 7 Do not reproduce without permission. Date CH.2f 21. Electronegativity involves the difference in attraction of atoms for electrons in a bond. Which of the following bond pairs would have the greatest electronegativity difference? A B C D F-CI Cl-Cl Mg-Cl H-Mg CH.2g 22. What is the oxidation number for the polyatomic ion in the compound potassium permanganate? KMnO4 F G H J +1 –1 +4 –4 CH.2a 23. Consider the following entry for magnesium taken from the periodic table. 24.305 +2 Mg Magnesium 12 [Ne]3s2 The number 12 represents — A B C D the atomic mass number. the atomic number. the oxidation number. the number of neutrons. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 8 Do not reproduce without permission. Date CH.2e 24. Which of the following is considered a transition metal? F G H J magnesium silicon sodium gold CH.2g 25. Which of the following electron configurations represents an element in an excited state? A B C D 1s22s22p6 1s22s22p63s2 1s22s22p63s1 1s22s22p53s1 CH.2d 26. The following elements belong to which family (group) — Li, Na, K, Rb, Cs, or Fr? F G H J halogens alkali metals alkaline earth metals metalloids CH.2f 27. One of the periodic properties involves the amount of energy required to remove the most loosely held electron from the outer energy level of the atom (in the gas phase). This property is known as A B C D electronegativity. atomic radius. ionization energy. ionic radius. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 9 Do not reproduce without permission. Date CH.2i 28. Originally, Mendeleev arranged the families (columns) in the periodic table according to F G H J alphabetic order. atomic number. atomic mass. similar properties. CH.2a 29. An atom with 3 neutrons, 2 protons, and 2 electrons would have the mass of A B C D 2 amu. 5 amu. 7 amu. 4 amu. CH.2a, c 30. The number of neutrons in nickel-60 is F G H J 28. 30. 32. 60. CH.2g 31. When electrons enter orbitals of equal energy, one electron enters each orbital until all the orbitals contain one electron with parallel spins, according to — A B C D the Pauli Exclusion Principle Hund’s Rule The Heisenberg Uncertainty Principle. the Electron Affinity Rule. _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 10 Do not reproduce without permission. Date CH.2g 32. How many orbitals are located in the p sublevel? F G H J 3 5 7 10 CH.2 33. A B C D How many valence electrons does a carbon atom have? 2 3 4 6 CH.3a 34. Which is always named first, when naming an ionic compound? F G H J anion hydrogen atom the element that has a greater mass cation CH.3e 35. Consider the experiment below in which two iron nails are placed in a copper (II) chloride solution. Which of the following unbalanced reactions will represent the single replacement reaction that would occur? Copper (II) chloride solution iron nails A B C D CuCl2 + Fe Cu2Cl + Fe CuCl2 + Fe Fe + Cu → → Fe + Cl2 + Cu → Fe + CuCl2 → FeCl2 + Cu FeCl2 + Cu _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 11 Do not reproduce without permission. Date CH.3a 36. Name the following compound — CuO. F G H J copper (I) oxide copper (II) oxide copper (III) oxide copper (IV) oxide CH.3b 37. In order to balance the following equation, which coefficient would need to be placed in front of SO2? __ SO2(g) + O2(g) + 2H2O(l) → 2H2SO4(l) A B C D 1 2 3 4 CH.3a 38. The chemical formula for sulfur difluoride would be F G H J S2F. S2F2. SF2. SF. CH.3d 39. The type of bonding in sodium chloride is A B C D nonpolar covalent. polar covalent. ionic. metallic. CH.3d 40. When electrons are shared unevenly between atoms, what type of bond results? F G H J ionic nonpolar covalent metallic polar covalent _____________________________________________________________________________________________ Copyright ©2005, S.S. Flanagan & D.E. Mott 12 Do not reproduce without permission. Date