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Physical Science Final ____ ____ 1. Ninety-nine percent of all the matter that can be observed in the universe exists as 2. Hydrochloric acid, HCl, is added to solid NaOH. After the reaction is complete, NaCl dissolved in water remains. What are the products of this chemical reaction? ____ 3. In an electron dot diagram, the symbol for an element is used to represent ____ 4. Which statement is true about the metalloid silicon? ____ 6. To find the number of neutrons in an atom, you would subtract ____ 7. What is a heterogeneous mixture? ____ the 8. Boyle’s law states that the volume of a gas is inversely proportional to its pressure if ____ 9. How many grams of CO2 are in 2.1 mol of the compound? ____ 10. The heat of fusion for water is the amount of energy needed for water to ____ 11. Raising the temperature of a gas will increase its pressure if the volume of the gas ____ 12. shoelaces? ____ What physical properties of nylon and leather make them good materials to use for 13. You see a structural formula in which the symbols for elements are connected by a long dash. You can assume that the chemical bonds in the compound are ____ 14. Democritus thought that matter was made of tiny particles ____ 15. Which of the following Group 1A elements is the most reactive? ____ 16. How does increasing the amount of carbon in steel affect its properties? ____ 17. The phase change in which a substance changes from a solid to a liquid is ____ 18. What is true about metals ____ 20. The standard on which the atomic mass unit is based is the mass of a ____ 21. The water molecule H2O is polar because it contains two polar single bonds and ____ ____ 22. Which of the following Group 7A elements is the most reactive? 23. What is the difference between an atom in the ground state and an atom in an excited state? ____ 24. The unit for atomic mass is ____ ____ 25. Metallic bonding is similar to ionic bonding because 26. A substance that is made up of only one kind of atom is a(an) ____ 27. To keep them from reacting, some highly reactive elements are stored in ____ 28. For the chemical reaction C2H6 + 137 kJ → C2H4 + H2, the chemical energy of the ____ 29. Which halogen is most likely to react? ____ 30. The name iron(II) indicates that a compound contains ____ 31. What is about subatomic particles is NOT true? ____ 32. The phase change in which a substance changes from a solid to a gas or vapor without changing to a liquid first is ____ ____ 33. Group 7A of the periodic table contains the 34. What is the result of a force distributed over an area? ____ 35. If a solid piece of naphthalene is heated and remains at 80°C until it is completely melted, you know that 80ºC is the ____ 36. When magnesium carbonate, MgCO2, reacts with nitric acid, HNO3, magnesium nitrate and carbonic acid form. Carbonic acid then breaks down into water and carbon dioxide. Which two types of reactions take place in this process? Figure 7-1 ____ 37. The reaction in Figure 7-1 shows the formation of ammonia from nitrogen and hydrogen in the Haber process. What will be the effect on the equilibrium if the temperature is increased and some of the ammonia is removed from the system? ____ ____ 38. Which of the following is a typical property of an ionic compound? 39. As you move from left to right across a period, the number of valence electrons ____ 40. Which element is found in nature only in compounds? ____ orderly? 41. During which phase change does the arrangement of water molecules become more ____ 42. Which of the following is a clue of a chemical change? ____ 43. Moving from left to right across a row of the periodic table, which of the following values increases by exactly one from element to element? ____ 44. most likely A substance has a melting point of 0ºC and a boiling point of 100ºC. The substance is ____ 45. What is the law of conservation of mass? ____ 46. Atoms of the most reactive elements tend to have ____ 47. What are pure substances? ____ 48. compound? Fluorine, F, forms a binary ionic compound with lithium, Li. What is the name of this ____ 49. The tendency of an element to react is closely related to ____ 50. In an atomic model that includes a nucleus, positive charge is ____ 51. describes a metallic bond? ____ 52. The Greek philosopher Democritus coined what word for a tiny piece of matter that cannot be divided? ____ ____ 53. In the compound MgCl2, the subscript 2 indicates that ____ 54. Which statement about subatomic particles is true? 55. 55. If you move a substance from one container to another and its volume changes, the substance is a ____ 56. Which of the following statements is true about what happens during a chemical reaction? ____ 57. Which element is found in most of the compounds in your body except for water? ____ 58. What is the symbol for aluminum? ____ 59. An industrial process makes calcium oxide by decomposing calcium carbonate. Which of the following is NOT needed to calculate the mass of calcium oxide that can be produced from 4.7 kg of calcium carbonate? ____ 60. A mixture that appears to contain only one substance is a(an) ____ 61. What does NOT contain molecules? ____ 62. What ormulas represents a compound whose molecules contain a triple bond? ____ 63. What has the highest viscosity? ____ 64. What will cause a decrease in gas pressure in a closed container? ____ 65. What does NOT state what the arrow means in a chemical equation? ____ 66. What is true about oxygen-17 and oxygen-18 ____ 67. What groups contain three elements with stable electron configurations? ____ 68. Alkali metals, alkaline earth metals, and aluminum all form ions with positive charges equal to the ____ 69. The coefficients in a balanced chemical equation always can express the ratio of ____ 70. A gas has ____ 71. One twelfth the mass of a carbon-12 atom is used to define a(an) ____ 72. Many metals can be drawn into thin wires without breaking because ____ 73. Ionization energies tend to ____ 74. The reaction H2CO3 + H2O ↔ H3O+ + HCO3– takes place in water. What happens to the equilibrium when the pressure is increased? ____ 75. Mendeleev gave the name eka-aluminum to a(an) Figure 6-1 ____ 76. Study the electron dot diagrams for lithium, carbon, fluorine, and neon in Figure 6-1. Choose the statement that correctly identifies the most stable of the elements. ____ ____ ____ 77. 78. Compared with Group 2A elements, Group 6A elements have 79. Two highly reactive elements in Period 2 are the metal lithium and the ____ 80. Which of the following takes place during a redox reaction? ____ 81. from Na and Br2? ____ Which of the following is a balanced chemical equation for the synthesis of NaBr 82. During a phase change, the temperature of a substance ____ 83. Which of the following provides the best analogy for an electron in an atomic orbital? ____ ____ The formation of an ionic bond involves the 84. Flammability is a material’s ability to burn in the presence of 85. In general, if the temperature of a chemical reaction is increased, the reaction rate ____ 86. Reaction rates do NOT tell you how fast ____ 87. What electrons and atomic orbitals is NOT true? ____ 88. Which columns have only metals? ____ 89. What is John Dalton’s atomic theory? ____ 90. When a physical change in a sample occurs, what does not change? ____ 91. What type of change occurs when water changes from a solid to a liquid? ____ 92. What is NOT always true about a synthesis reaction? ____ 93. Methane, CH4, burns in oxygen gas to form water and carbon dioxide. What is the correct balanced chemical equation for this reaction? ____ ____ doubt? 94. Suppose an atom has a mass number of 23. Which statement is true beyond any ____ 95. Forces of attraction limit the motion of particles most in ____ 96. What is a physical change? ____ 97. Water has a higher boiling point than expected because 98. In a periodic table, a set of properties repeats from ____ 99. Matter that has a definite volume but no definite shape is a ____ 100. You are about to open a container of soy milk but notice that there are instructions to “shake well before serving.” The soy milk is most likely a Essay 101. Suppose you want to separate the leaves, acorns, and twigs from a pile of soil. Filtration and distillation are two processes of separating mixtures. Explain which process you would use and why. 102. Fluorine is the most reactive nonmetal. To fluorine’s immediate right in the periodic table is neon, a noble gas that does not form chemical bonds. Explain this contrast in reactivity in terms of atomic structure. 103. Explain why rust forms in steel tanks that hold seawater in ships. How can nitrogen be used to reduce rust in these tanks? 104. In science lab, your teacher gives you two small pieces of matter and tells you that one piece is a metal and one is a nonmetal. Without changing the size or shape of the pieces, how could you test them to determine which is the metal? 105. A sample of calcium contains calcium-40, calcium-44, calcium-42, calcium-48, calcium-43, and calcium-46 atoms. Explain why these atoms can have different mass numbers but must have the same atomic number. 106. point. Describe how water can change from a liquid to a vapor at temperatures lower than its boiling 107. Why were the elements gallium (Ga), scandium (Sc), and germanium (Ge) important to Mendeleev?