NAME MIDTERM REVIEW 1. 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 2. Which of the following statements contained in a student's laboratory report is a conclusion? A) A gas is evolved. B) The gas is insoluble in water. C) The gas is hydrogen. D) The gas burns in air. 3. The diagram below represents a portion of a 100-milliliter graduated cylinder. What is the reading of the meniscus? A) 35.0 mL B) 36.0 mL C) 44.0 mL D) 45.0 mL 4. An aluminum sample has a mass of 80.01 g and a density of 2.70 g/cm3. According to the data, to what number of significant figures should the calculated volume of the aluminum sample be expressed? A) 1 B) 2 C) 3 D) 4 5. A student in a laboratory determined the boiling point of a substance to be 71.8°C. The accepted value for the boiling point of this substance is 70.2°C. What is the percent error of the student's measurement? A) 1.60% B) 2.28% C) 2.23% D) 160.% MIDTERM REVIEW 6. Base your answer to the following question on the information below. A method used by ancient Egyptians to obtain copper metal from copper(I) sulfide ore was heating the ore in the presence of air. Later, copper was mixed with tin to produce a useful alloy called bronze. Calculate the density of a -gram sample of bronze that has a volume of cubic centimeters. Your response must include a correct numerical setup and the calculated result. 7. Compared to the charge of a proton, the charge of an 14. As a result of the gold foil experiment, it was concluded electron has that an atom A) a greater magnitude and the same sign A) contains protons, neutrons, and electrons B) a greater magnitude and the opposite sign B) contains a small, dense nucleus C) the same magnitude and the same sign C) has positrons and orbitals D) the same magnitude and the opposite sign D) is a hard, indivisible sphere 8. Which particle has no charge? 15. The gold foil experiment led to the conclusion that each atom in the foil was composed mostly of empty space A) electron B) neutron because most alpha particles directed at the foil C) positron D) proton A) passed through the foil 9. What is the overall charge of an ion that has 12 protons, 10 electrons, and 14 neutrons? B) remained trapped in the foil C) were deflected by the nuclei in gold atoms A) 2– B) 2+ C) 4– D) 4+ D) were deflected by the electrons in gold atoms 10. Which particles have approximately the same mass? 16. All phosphorus atoms have the same A) an electron and an alpha particle A) atomic number B) an electron and a proton B) mass number C) a neutron and an alpha particle C) number of neutrons plus the number of electrons D) a neutron and a proton D) number of neutrons plus the number of protons 11. Which phrase describes an atom? 17. Which electron configuration represents the electrons in A) a negatively charged nucleus surrounded by an atom of Ga in an excited state? positively charged protons A) 2-8-17-3 B) 2-8-17-4 B) a negatively charged nucleus surrounded by C) 2-8-18-3 D) 2-8-18-4 positively charged electrons C) a positively charged nucleus surrounded by 18. Which quantity represents the number of protons in an negatively charged protons atom? D) a positively charged nucleus surrounded by A) atomic number negatively charged electrons B) oxidation number 12. An ion that consists of 7 protons, 6 neutrons, and 10 C) number of neutrons electrons has a net charge of D) number of valence electrons A) 4– B) 3– C) 3+ D) 4+ 19. What is the charge of the nucleus of an oxygen atom? 13. Which subatomic particles are located in the nucleus of A) 0 B) –2 C) +8 D) +16 a carbon atom? 20. The notation for the nuclide 13755Cs gives information A) protons, only about B) neutrons, only A) mass number, only C) protons and neutrons B) atomic number, only D) protons and electron C) both mass number and atomic number D) neither mass number nor atomic number MIDTERM REVIEW 21. An atom of any element must contain 29. The nucleus of an atom of cobalt-58 contains A) an equal number of protons and neutrons A) 27 protons and 31 neutrons B) an equal number of protons and electrons B) 27 protons and 32 neutrons C) more electrons than neutrons C) 59 protons and 60 neutrons D) more electrons than protons D) 60 protons and 60 neutrons 22. In an atom of argon-40, the number of protons 30. Chlorine-37 can be represented as A) equals the number of electrons A) 1735Cl B) 2037Cl C) 3520Cl D) 3717Cl B) equals the number of neutrons 31. The atomic masses and the natural abundances of the C) is less than the number of electrons two naturally occurring isotopes of lithium are shown D) is greater than the number of electrons in the table below. 23. An atom contains 22 neutrons and 40 nucleons. What is the total number of protons in the atom? A) 18 B) 22 C) 40 D) 62 24. Which quantity can vary among atoms of the same element? A) mass number B) atomic number C) number of protons D) numbers of electrons Which numerical setup can be used to determine the 25. What is the mass number of a carbon atom that contains atomic mass of lithium? six protons, eight neutrons, and six electrons? A) (0.075)(6.02 u) + (0.925)(7.02 u) A) 6 B) 8 C) 14 D) 20 B) (0.925)(6.02 u) + (0.075)(7.02 u) 26. In which list are the elements arranged in order of C) (7.5)(6.02 u) + (92.5)(7.02 u) increasing atomic mass? D) (92.5)(6.02 u) + (7.5)(7.02 u) A) Cl, K, Ar B) Fe, Co, Ni 32. The atomic mass of an element is the weighted average C) Te, I, Xe D) Ne, F, Na of the 27. The table below shows the number of subatomic A) number of protons in the isotopes of that element particles in atom X and in atom Z. B) number of neutrons in the isotopes of that element C) atomic numbers of the naturally occurring isotopes of that element D) atomic masses of the naturally occurring isotopes of that element 33. Element X has two isotopes. If 72.0% of the element has an isotopic mass of 84.9 atomic mass units, and 28.0% of the element has an isotopic mass of 87.0 atomic mass units, the average atomic mass of element Atom X and atom Z are isotopes of the element X is numerically equal to A) aluminum B) carbon A) C) magnesium D) nitrogen B) 28. Atoms of different isotopes of the same element differ C) in their total number of D) A) electrons B) neutrons C) protons D) valence electrons MIDTERM REVIEW 34. An orbital is defined as a region of the most probable 42. In the wave-mechanical model of the atom, orbitals are location of regions of the most probable locations of A) an electron B) a neutron A) protons B) positrons C) a nucleus D) a proton C) neutrons D) electrons 35. What is the total number of valence electrons in an 43. Which group of atomic models is listed in historical atom of germanium in the ground state? order from the earliest to the most recent? A) 8 B) 2 C) 14 D) 4 A) hard-sphere model, wave-mechanical model, 36. Compared to an electron in the first electron shell of an electron-shell model atom, an electron in the third shell of the same atom has B) hard-sphere model, electron-shell model, wave-mechanical model A) less mass B) less energy C) electron-shell model, wave-mechanical model, C) more mass D) more energy hard-sphere model 37. What is the electron configuration of a sulfur atom in D) electron-shell model, hard-sphere model, the ground state? wave-mechanical model A) 2–4 B) 2–6 C) 2–8–4 D) 2–8–6 38. How many electrons are in the outermost principal energy level (shell) of an atom of carbon in the ground state? A) 6 B) 2 C) 3 D) 4 39. Which electron configuration represents an atom in an excited state? A) 2–7 B) 2–6–2 C) 2–8–1 D) 2–8–8–2 40. As an electron in an atom moves from the ground state to the excited state, the electron A) gains energy as it moves to a higher energy level B) gains energy as it moves to a lower energy level C) loses energy as it moves to a higher energy level D) loses energy as it moves to a lower energy level 41. 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 A) gain energy as they return to lower energy levels B) gain energy as they move to higher energy levels C) emit energy as they return to lower energy levels D) emit energy as they move to higher energy levels MIDTERM REVIEW Base your answers to questions 44 and 45 on the information and the bright-line spectra represented below.