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17. The atomic mass of an element is the weighted average of the (1) number of protons in the isotopes of that element (2) number of neutrons in the isotopes of that element (3) atomic numbers of the naturally occurring isotopes of that element (4) atomic masses of the naturally occurring isotopes of that element 18. The modern model of the atom is based on the work of (1) one scientist over a short period of time (2) one scientist over a long period of time (3) many scientists over a short period of time (4) many scientists over a long period of time 19. In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability of finding a neutron (3) a circular path in which electrons are found (4) a circular path in which neutrons are found 20. During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is emitted by these ions in the flame when the electrons (1) gain energy as they return to lower energy levels (2) gain energy as they move to higher energy levels (3) emit energy as they return to lower energy levels (4) emit energy as they move to higher energy levels 21. Which of these phrases best describes an atom? (1) a positive nucleus surrounded by a hard negative shell (2) a positive nucleus surrounded by a cloud of negative charges (3) a hard sphere with positive particles uniformly embedded (4) a hard sphere with negative particles uniformly embedded 22. Recovering the salt from a mixture of salt and water could best be accomplished by (1) evaporation (3) paper chromatography (2) filtration (4) density determination 23. Which element is malleable and conducts electricity? (1) iron (3) sulfur (2) iodine (4) phosphorus 24. At STP, an element that is a brittle solid and a poor conductor of heat and electricity could have an atomic number of (1) 12 (3) 16 (2) 13 (4) 17 25. What are two properties of most nonmetals? (1) high ionization energy and poor electrical conductivity (2) high ionization energy and good electrical conductivity (3) low ionization energy and poor electrical conductivity (4) low ionization energy and good electrical conductivity 26. Which substance can not be decomposed by a chemical change? (1) Ne (3) HF (2) N2O (4) H2O Base your answers to questions 27 and 28 on the information below. Naturally occurring elemental carbon is a mixture of isotopes. The percent composition of the two most abundant isotopes is listed below. • 98.93% of the carbon atoms have a mass of 12.00 atomic mass units. • 1.07% of the carbon atoms have a mass of 13.00 atomic mass units. 27. Describe, in terms of subatomic particles found in the nucleus, one difference between the nuclei of carbon-12 atoms and the nuclei of carbon-13 atoms. The response must include both isotopes. 28. In the space provided in your answer booklet, show a correct numerical setup for calculating the average atomic mass of carbon. 29. Which pair of symbols represents a metalloid and a noble gas? (1) Si and Bi (3) Ge and Te (2) As and Ar (4) Ne and Xe 30. Which element is a solid at STP? (1) H2 (3) N2 (2) I2 (4) O2 31. Given the particle diagram: At 101.3 kPa and 298 K, which element could this diagram represent? (1) Rn (3) Ag (2) Xe (4) Kr 32. Which list consists of elements that have the most similar chemical properties? (1) Mg, Al, and Si (3) K, Al, and Ni (2) Mg, Ca, and Ba (4) K, Ca, and Ga 33. Which list of elements contains a metal, a metalloid, and a nonmetal? (1) Zn, Ga, Ge (3) Cd, Sb, I (2) Si, Ge, Sn (4) F, Cl, Br 34. The elements in Period 5 on the Periodic Table are arranged from left to right in order of (1) decreasing atomic mass (2) decreasing atomic number (3) increasing atomic mass (4) increasing atomic number 35. What is the density of N2 at STP? (1) .00100 g/cm 3 (3) .00143 g/cm 3 (2) .00125 g/cm 3 (4) .00198 g/cm 3 36. Explain, in terms of atomic structure, why germanium is chemically similar to silicon.
37. At STP, solid carbon can exist as graphite or as diamond. These two forms of carbon have (1) the same properties and the same crystal structures (2) the same properties and different crystal structures (3) different properties and the same crystal structures (4) different properties and different crystal structures 38. At 298 K, oxygen (O2 ) and ozone (O3 ) have different properties because their (1) atoms have different atomic numbers (2) atoms have different atomic masses (3) molecules have different molecular structures (4) molecules have different average kinetic energies 39. Which set of symbols represents atoms with valence electrons in the same electron shell? (1) Ba, Br, Bi (3) O, S, Te (2) Sr, Sn, I (4) Mn, Hg, Cu 40. How many electrons are contained in an Au 3+ ion? (1) 76 (3) 82 (2) 79 (4) 197 41. Which change occurs when a barium atom loses two electrons? (1) It becomes a negative ion and its radius decreases. (2) It becomes a negative ion and its radius increases. (3) It becomes a positive ion and its radius decreases. (4) It becomes a positive ion and its radius increases. 42. Which Lewis electron-dot diagram represents a boron atom in the ground state? (1) (2) 43. Which compound forms a green aqueous solution? (1) RbCl (3) NiCl2 (2) CaCl2 (4) ZnCl2 44. Which element forms an ion that is larger than its atom? (1) aluminum (3) magnesium (2) chlorine (4) sodium 45. As the elements in Group 17 on the Periodic Table are considered from top to bottom, what happens to the atomic radius and the metallic character of each successive element? (1) The atomic radius and the metallic character both increase. (2) The atomic radius increases and the metallic character decreases. (3) The atomic radius decreases and the metallic character increases. (4) The atomic radius and the metallic character both decrease. 46. The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s (1) electronegativity (3) heat of reaction (2) ionization energy (4) heat of formation (3) (4) 47. As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element generally (1) decreases (3) remains the same (2) increases 48. As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the (1) number of protons increases, and the number of shells of electrons remains the same (2) number of protons increases, and the number of shells of electrons increases (3) number of protons decreases, and the number of shells of electrons remains the same (4) number of protons decreases, and the number of shells of electrons increases 49. Compared to the nonmetals in Period 2, the metals in Period 2 generally have larger (1) ionization energies (3) atomic radii (2) electronegativities (4) atomic numbers 50. Which of these elements has the least attraction for electrons in a chemical bond? (1) oxygen (3) nitrogen (2) fluorine (4) chlorine 51. Most metals have the properties of (1) brittleness and high ionization energy (2) brittleness and low ionization energy (3) ductility and high ionization energy (4) ductility and low ionization energy 52. An unknown element X can form a compound with the formula XBr3 . In which group on the Periodic Table would element X be found? (1) 1 (3) 13 (2) 2 (4) 14 53. What is the chemical formula for copper(II) hydroxide? (1) CuOH (3) Cu2 (OH) (2) CuOH2 (4) Cu(OH) 2 54. Two different samples decompose when heated. Only one of the samples is soluble in water. Based on this information, these two samples are (1) both the same element (3) both the same compound (2) two different elements (4) two different compounds 55. The correct chemical formula for iron(II) sulfide is (1) FeS (3) FeSO4 (2) Fe2S3 (4) Fe2 (SO4 ) 3 56. The molecular formula of glucose is C6H12O6 . What is the empirical formula of glucose? (1) CHO (3) C6H12O6 (2) CH2O (4) C12H24O12 57. What is the molecular formula of a compound that has a molecular mass of 54 and the empirical formula C2H3 ? (1) C2H3 (3) C6H9 (2) C4H6 (4) C8H12
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