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Name: ____________________________________ 1. Given the electron dot diagram: The valence electrons represented by the electron dot diagram could be those of atoms in Group A. B. C. D. 13 15 3 16 2. An atom in the ground state contains 8 valence electrons. This atom is classified as a A. metal B. semimetal C. noble gas D. halogen 3. Which substance can be decomposed by chemical change? A. beryllium B. boron C. methanol D. magnesium 4. Which element is an active nonmetal? A. neon B. oxygen C. zinc D. chromium 5. To which group do the alkaline earth metals belong? A. 1 B. 2 C. 11 D. 12 6. What is the total number of electrons present in an atom of ? A. B. C. D. 27 32 39 86 8. Which formula represents a substance that contains covalent bonds? A. LiCl B. CaCl2 C. K2 O D. CO2 9. Neutral atoms of 35Cl and 37Cl differ with respect to their number of A. electrons B. protons C. neutrons D. positrons 10. Spectral lines produced from the radiant energy emitted from excited atoms are thought to be due to the movements of electrons A. from lower to higher energy levels B. from higher to lower energy levels C. in their orbitals D. out of the nucleus 11. Which is the correct electron-dot formula for a molecule of chlorine? A. C. B. D. 12. All samples of an element are composed of atoms with the same A. atomic mass B. atomic number C. number of nucleons D. number of neutrons 13. The mass of a solid is 3.60 grams and its volume is 1.8 cubic centimeters. What is the density of the solid, expressed to the correct number of significant figures? A. 2 g/cm3 B. 2.0 g/cm3 C. 0.5 g/cm3 D. 0.50 g/cm3 7. What is the correct formula for ammonium carbonate? A. NH4 (CO3 )2 B. NH4 CO3 C. (NH4 )2 (CO3 )2 D. (NH4 )2 CO3 14. What is the gram formula mass of Li2 SO4 ? A. B. C. D. 54g 55g 110g 206g 15. The formula for calcium cyanide is A. CaCN2 B. CaSCN2 C. Ca(CN)2 D. Ca(SCN)2 16. What is the correct formula for chromium (III) oxide? A. CrO3 B. Cr3 O C. Cr2 O3 D. Cr3 O2 17. When the pressure exerted on a confined gas at constant temperature is doubled, the volume of the gas is A. halved B. doubled C. tripled D. quartered 18. Which is an example of a binary compound? A. acetic acid B. nitric acid C. potassium hydroxide D. potassium oxide 19. The volume of a sample of gas is 1.0 liter at STP. If the pressure remains constant and the temperature is raised to 547 K, the new volume of the gas will be A. 0.25 L B. 2.0 L C. 0.50L D. 4.0 L 22. Compared to the entire atom, the nucleus of the atom is A. smaller and contains most of the atom’s mass B. smaller and contains little of the atom’s mass C. larger and contains most of the atom’s mass D. larger and contains little of the atom’s mass 23. The atomic number of any atom is equal to the number of A. neutrons in the atom, only B. protons in the atom, only C. neutrons plus protons in the atoms D. protons plus electrons in the atom 24. What is the correct formula for iron (II) bromide? A. FeBr2 B. Fe2 Br C. FeBrO2 D. Fe2 BrO2 25. In an experiment, alpha particles were used to bombard gold foil. As a result of this experiment, the conclusion was made that the nucleus of an atom is A. smaller than the atom and positively charged B. smaller than the atom and negatively charged C. larger than the atom and positively charged D. larger than the atom and negatively charged 26. An example of a heterogeneous mixture is A. soil B. sugar C. carbon monoxide D. carbon dioxide 27. In the compound shown in the diagram: 20. Neutral atoms of the same element can differ in their number of A. neutrons B. positrons C. protons D. electrons 21. Which element is in Group 2 (IIA) and Period 7 of the Periodic Table? A. magnesium B. manganese C. radium D. radon Which element that could be represented by X would have the greatest attraction for electrons in the bond? A. B. C. D. iodine chlorine bromine fluorine 28. Which graph best represents a change of phase from a gas to a solid? A. 31. During which change is energy absorbed? A. the melting of ice B. the cooling of ice C. the freezing of water D. the condensation of water B. 32. Which of the following atoms has the greatest nuclear charge? A. Al B. Ar C. Si D. Na 33. An atom of carbon-14 contains A. 8 protons, 6 neutrons and 6 electrons B. 6 protons, 6 neutrons and 8 electrons C. 6 protons, 8 neutrons and 8 electrons D. 6 protons, 8 neutrons and 6 electrons C. 34. When the equation __C8 H16 + __O2 → __CO2 + __H2 O is correctly balanced using the smallest whole number coefficient, the coefficient of O2 is D. A. B. C. D. 1 8 12 16 35. Which pair must represent atoms of the same element? 29. Which statement best describes an electron? A. It has a smaller mass than a proton and a negative charge. B. It has a smaller mass than a proton and a positive charge. C. It has a greater mass than a proton and a negative charge. D. It has a greater mass than a proton and a positive charge. 30. Element X is in Group 2 (IIA) and element Y is in Group 17 (VIIA). A compound formed between these two elements is most likely to have the formula A. X2 Y B. XY2 C. X2 Y7 D. X7 Y2 A. and B. and C. D. and and 36. A student observing the behavior of paradichlorobenzene first heats 10 grams of the substance in a hot water bath until it is completely liquified. The data in the table are recorded as paradichloro-benzene cools. 40. A white crystalline salt conducts electricity when it is melted and when it is dissolved in water. Which type of bond does this salt contain? A. ionic B. metallic C. covalent D. network 41. Which substance is composed of atoms that all have the same atomic number? A. magnesium B. methane C. ethane D. ethene 42. When the equation: __Al2 (SO4 )3 + __ZnCl2 → __AlCl3 + __ZnSO4 is correctly balanced using the smallest whole number coefficients, the sum of the coefficients is What is the freezing point of paradichlorobenzene? A. B. C. D. 42°C 53°C 58°C 65°C 37. What is the formula mass of Al2 (SO4 )3 ? A. B. C. D. 123 150. 214 342 38. Which term refers to the region of an atom where an electron is most likely to be found? A. orbital B. orbit C. quantum D. spectrum 39. A student investigated the physical and chemical properties of a sample of an unknown gas and then identified the gas. Which statement represents a conclusion rather than an experimental observation? A. The gas is colorless. B. The gas is carbon dioxide. C. When the gas is bubbled into limewater, the liquid becomes cloudy. D. When placed in the gas, a flaming splint stops burning. A. B. C. D. 9 8 5 4 43. Which phase change represents sublimation? A. solid to gas B. solid to liquid C. gas to solid D. gas to liquid 44. More than two-thirds of the elements of the Periodic Table are classified as A. metalloids B. metals C. nonmetals D. noble gases 45. When metals form ions, they tend to do so by A. losing electrons and forming positive ions B. losing electrons and forming negative ions C. gaining electrons and forming positive ions D. gaining electrons and forming negative ions 46. The graph represents the uniform cooling of water at 1 atmosphere, starting with water as a gas above its boiling point. 51. What is the maximum number of electrons that may be present in the fourth principal energy level of an atom? A. 8 B. 2 C. 18 D. 32 52. Which substance takes the shape of and fills the volume of any container into which it is placed? A. H2 O ( ) B. I2 (s) C. CO2 (g) D. Hg ( ) Which segments of the cooling curve represent the fixed points on a thermometer? A. B. C. D. AB and CD BC and DE AF and EF CD and EF 47. What is the gram formula mass of (NH4 )2 SO4 ? A. B. C. D. 66.0 g 94.0 g 114 g 132 g 48. Which electronegativity is possible for an alkali metal? A. 1.0 B. 2.0 C. 3.0 D. 4.0 49. Compared to atoms of metals, atoms of nonmetals generally have A. higher electronegativities and lower ionization energies B. higher electronegativities and higher ionization energies C. lower electronegativities and lower ionization energies D. lower electronegativities and higher ionization energies 50. A sample of a gas has a volume of 2.0 liters at a pressure of 1.0 atmosphere. When the volume increases to 4.0 liters, at constant temperature, the pressure will be A. 1.0 atm B. 2.0 atm C. 0.50 atm D. 0.25 atm 53. Given the equation: __FeCl2 + __Na2 CO3 → __FeCO3 + __NaCl When the equation is correctly balanced using the smallest whole numbers, the coefficient of NaCl is A. B. C. D. 6 2 3 4 54. The correct electron dot formula for hydrogen chloride is A. B. C. D. 55. During a laboratory activity, a student combined two solutions. In the laboratory report, the student wrote "A yellow color appeared." The statement represents the student's recorded A. conclusion B. observation C. hypothesis D. inference