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Knockout Review Questions Name: Date: 1. All of the Atoms of Argon

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Knockout Review Questions Name: Date: 1. All of the Atoms of Argon Knockout Review Questions Name: Date: 1. All of the atoms of argon have the same 6. The nucleus is the part of the atom that A. mass number A. consist mostly of empty space B. atomic number B. has a negative charge C. number of neutrons C. occupies most of the atom's total volume D. number of nucleons D. contains most of the atom's total mass 2. Which is the atomic number of an atom with six 7. What is the mass number of an ion that has valence electrons? 83 protons, 80 electrons, and 126 neutrons? A. 6 B. 8 C. 10 D. 12 A. 83 B. 206 C. 209 D. 289 3. Which of the following atoms has the greatest 127 8. The nucleus of an atom of 53I contains nuclear charge? A. 53 neutrons and 127 protons 14 12 2 4 A. 7N B. 6C C. 1H D. 2He B. 53 protons and 127 neutrons 4. What can be determined if only the atomic number C. 53 protons and 74 neutrons of an atom is known? D. 53 protons and 74 electrons A. the total number of neutrons in the atom, only 9. The atomic mass of an element is defined as the B. the total number of protons in the atom, only weighted average mass of that element's C. the total number of protons and the total number of neutrons in the atom A. most abundant isotope D. the total number of protons and the total B. least abundant isotope number of electrons in the atom C. naturally occurring isotopes 5. Which two particles have approximately the same D. radioactive isotopes mass? A. neutron and electron 10. In which list are the elements arranged in order of increasing atomic mass? B. neutron an deutron C. proton and neutron A. Cl, K, Ar B. Fe, Co, Ni D. proton and electron C. Te, I, Xe D. Ne, F, Na page 1 11. Base your answer(s) to the following question(s) 17. What is the total charge of the nucleus of a carbon on the data table below, which shows three atom? isotopes of neon. Isotope Atomic Mass Percent Natural A. 6 B. 0 C. +6 D. +12 (atomic mass units) Abundance 20Ne 19.99 90.9% 21Ne 20.99 0.3% 22Ne 21.99 8.8% 18. A proton has a charge that is opposite the charge of In terms of atomic particles, state one difference between these three isotopes of neon. A. an alpha particle B. a neutron 12. Which isotopic notation represents an atom of C. an electron D. a positron carbon-14? 19. The table below gives information about the 6 8 6 14 A. 8C B. 6C C. 14 C D. 6C nucleus of each of four atoms. Nuclei of Four Atoms 13. The atoms in a sample of an element must contain Atom Number of Number of nuclei with the same number of Protons Neutrons A 6 6 A. electrons B. protons D 6 7 C. neutrons D. nucleons E 7 7 G 7 8 14. In an experiment, alpha particles were used to How many different elements are represented by bombard gold foil. As a result of this experiment, the nuclei in the table? the conclusion was made that the nucleus of an atom is A. 1 B. 2 C. 3 D. 4 A. smaller than the atom and positively charged 20. Which nucleus contains the greatest number of B. smaller than the atom and negatively charged neutrons? C. larger than the atom and positively charged 31 32 31 32 A. 16S B. 16 S C. 15P D. 15P D. larger than the atom and negatively charged 21. Which particle can not be accelerated by the 15. Which kind of particle, when passed through an electric or magnetic fields in a particle accelerator? electric field, would be attracted to the negative electrode? A. neutron B. proton A. an alpha particle B. a beta particle C. alpha particle D. beta particle C. a neutron D. an electron 22. In which pair of atoms do both nuclei contain the same number of neutrons? 16. After bombarding a gold foil sheet with alpha particles, scientists concluded that atoms consist mainly of 7 9 40 40 A. 3Li and 4Be B. 19K and 17 Cl C. 40Ca and 38Ar D. 14N and 16O A. electrons B. empty space 20 18 7 8 C. protons D. neutrons page 2 Knockout Review Questions 23. Which nucleus is from an isotope of an atom with 29. Usually the term “kernel” includes all parts of the 6n atom except the the nucleus _6p ? A. neutrons B. protons 6n 4n A. _6p B. _8p C. valence electrons D. orbital electrons 8n 6n 2+ 0 C. _6p D. _8p 30. A Ca ion differs from a Ca atom in that the Ca2+ ion has 24. Neutral atoms of the same element can differ in A. more protons B. fewer protons their number of C. more electrons D. fewer electrons A. neutrons B. positrons C. protons D. electrons 31. When the electrons of an excited atom fall back to lower levels, there is an emission of energy that produces 25. Base your answer(s) to the following question(s) on the information below. A. beta particles B. alpha particles Naturally Occurring Isotopes of Copper C. spectral lines D. gamma radiation Isotope Percent Natural Atomic Mass Notation Abundance (%) (atomic mass units, u) Cu-63 69.17 62.930 32. What is the approximate mass of an electron? Cu-65 30.83 64.928 A. 1 atomic mass unit B. 1 of a C-12 atom State, in terms of subatomic particles, how an 12 atom of Cu-63 differs from an atom of Cu-65. 1 1835 C. 1836 of a proton D. 1836 of a proton 26. The maximum number of electrons that may be found in the third principal energy level is 33. What is the total number of electrons in an atom 19 of 9F? A. 8 B. 2 C. 18 D. 32 A. 9 B. 10 C. 19 D. 28 27. Which particle has a mass that is approximately 1 1,836 of the mass of a proton? 34. What is the most probable location of an electron? A. a gamma ray B. a neutron A. an orbital C. an alpha particle D. an electron B. a nucleus C. a sublevel 28. What is the total number of valence electrons in D. a principal energy level an atom of phosphorus in the ground state? A. 5 B. 2 C. 3 D. 7 page 3 Knockout Review Questions 35. In the wave-mechanical model, an orbital is a 40. Which principal energy level of an atom contains region of space in an atom where there is an electron with the lowest energy? A. a high probability of finding an electron A. n = 1 B. n = 2 C. n = 3 D. n = 4 B. a high probability of finding a neutron 41. An electron in a sodium atom moves from the C. a circular path in which electrons are found third shell to the fourth shell. This change is a result of the atom D. a circular path in which neutrons are found A. absorbing energy B. releasing energy 36. How many electrons are in an Fe2+ ion? C. gaining an electron D. losing an electron A. 24 B. 26 C. 28 D. 56 42. What is the net charge of an ion that consists of 10 electrons, 11 protons, and 12 neutrons? 37. Base your answer(s) to the following question(s) on the diagram below, which represents an atom + + of magnesium-26 in the ground state. A. 1 B. 2 C. 1 D. 2 43. How do the chemical properties of the Na atom and the Na+ ion compare? A. They are the same because each has the same atomic number. B. They are the same because each has the same electron configuration. C. They are different because each has a different What is the total number of valence electrons in atomic number. an atom of Mg-26 in the ground state? D. They are different because each has a different electron configuration. 38. What is the maximum number of electrons that can occupy the second principal energy level? 44. As an atom becomes an ion, its mass number A. 6 B. 8 C. 18 D. 32 A. decreases B. increases 39. The characteristic bright-line spectrum of an C. remains the same element is produced when electrons 45. Which element has an atom with the electron A. are given off as beta particles configuration 2 8 8 2? B. are gained from another atom A. Mg B. Ni C. Ca D. Ge C. move to higher energy levels D. fall back to lower energy levels 46. What is the electron configuration of a sulfur atom in the ground state? A. 2–4 B. 2–6 C. 2–8–4 D. 2–8–6 page 4 Knockout Review Questions 47. Which is the electron dot symbol of an atom of 53. Which statement best explains why most atomic boron in the ground state? masses on the Periodic Table are decimal numbers? . A. Atomic masses are determined relative to an A. B. : B. B C. B : D. B : H–1 standard. 48. Which electron-dot symbol correctly represents an B. Atomic masses are determined relative to an atom of its given element? O–16 standard. C. Atomic masses are a weighted average of the naturally occurring isotopes.
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