UNIT 1 - MATTER AND CHEMICAL BONDING- PART 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. The particle that has the smallest mass is the a. electron d. nucleus b. proton e. ion c. neutron 2. The atomic number of an element is defined as the a. number of neutrons in the nucleus b. number of protons in the nucleus c. number of electrons in the nucleus d. number of protons and neutrons in the nucleus e. electron to proton ratio 3. The relative atomic mass of chlorine (35.452 u) is a good indication that a. Chlorine is a compound, not an element. b. Chlorine is a mixture of isotopes. c. Chlorine nuclei contain fractions of a neutron. d. Chlorine consists of the molecule Cl 2. e. Chlorine is radioactive. 4. All fluorescent lights, when analyzed in a spectrometer, exhibit the same lines in the yellow, green, and blue spectral regions. This is evidence that a. Fluorescent lights contain fluorine gas. b. There are no gases present in fluorescent lights. c. The same elements are present in all fluorescent lights. d. Air is present in all fluorescent lights. e. Fluorescent lights are defective. 5. Which of the following elements requires the least amount of energy to remove an electron from an atom to form an ion? a. O d. H b. He e. Fr c. K + 6. Consider the equation X (g) + energy X + e. The "energy" term in the equation represents a. electron affinity d. sublimation energy b. heat of sublimation e. heat of vaporization c. ionization energy 7. Electron affinity increases as you go from left to right on the periodic table because a. atomic radius decreases d. all of the above b. ionization energy decreases e. none of the above c. of the periodic law 8. The person given credit for developing the first modern periodic table is a. Dalton d. Mendeleev b. Democritus e. Chadwick c. Thomson
9. Which of the following is NOT a metal? a. Li d. Mg b. Al e. C c. B 10. Two atoms are isotopes if they have a. different atomic numbers b. the same mass number, but different atomic numbers c. the same number of protons and neutrons d. the same number of electrons, but a different number of neutrons e. the same atomic number, but a different mass number 11. The element found in the periodic table in Group 4 and Period 6 is a. hafnium, Hf d. chromium, Cr b. selenium, Se e. aluminum, Al c. gadolinium, Gd 12. The element found in the periodic table in Group 6 and Period 4 is a. hafnium, Hf d. gadolinium, Gd b. selenium, Se e. chromium, Cr c. lithium, Li 13. Which of the following matches of group number and common name is incorrect? a. Group 2 - alkaline earth metals d. Group 17 - halogens b. Group 6 - lanthanides e. Group 18 - noble gases c. Group 1 - alkali metals 14. Which of the following matches of group number and common name is incorrect? a. Group 7 - transition metals d. Group 2 - actinides b. Group 2 - alkali earth metals e. Group 18 - noble gases c. Group 17 - halogens 15. An atomic mass unit (amu) is defined as the a. mass of a hydrogen atom b. mass of 12 hydrogen atoms c. mass of a carbon atom d. one-twelfth the mass of a hydrogen atom e. one-twelfth the mass of a carbon atom 16. According to the periodic law, chemical properties are repeated at regular intervals when a. elements are listed in order of their atomic radius b. elements are listed in order of their date of discovery c. families of elements are listed in order d. periods are arranged in order e. elements are arranged in order of increasing atomic number 17. A metalloid in Period 3 is a. scandium d. phosphorus b. aluminum e. silicon c. germanium 18. A metal in Group 15 is a. bismuth d. phosphorus b. lead e. tin c. arsenic
19. A nonmetal in Period 6 is a. astatine d. radon b. iodine e. rubidium c. polonium 20. The chemical family known as the halogens are the elements in Group a. 1 d. 17 b. 2 e. 18 c. 5 21. When elements are arranged in order of increasing atomic mass, their chemical properties repeat at regular intervals. This statement is the definition of a. atomic mass d. law of constant composition b. periodic law e. law of conservation of mass c. limitations of the periodic table 22. The atomic mass of barium is due to the number of a. neutrons and electrons in the nucleus d. protons and electrons in the atom b. electrons in the nucleus e. protons in the nucleus c. protons and neutrons in the nucleus 23. Isotopes with unstable nuclei are also referred to as a. nucleoisotopes d. radiation b. radioisotopes e. beta isotopes c. isotopic radiation 24. The properties of elements repeat periodically if they are arranged by a. atomic mass d. number of neutrons b. atomic charge e. number of electrons c. atomic number 25. The mass listed for each element in the periodic table is a. the mass of all of the isotopes of the element combined b. the mass of the average number of neutrons in all of the isotopes of the element c. the average of the atomic masses of all of the isotopes of the element d. the exact mass of the protons and neutrons in the most common isotope of the element e. the weighted average of the atomic masses of all of the isotopes of the element 26. The atomic number is the number of a. protons in the nucleus b. neutrons in the nucleus c. protons plus the number of neutrons in the nucleus d. electrons plus the number of protons in the nucleus e. electrons plus the number of neutrons in the nucleus 27. Why does atomic radius increase from top to bottom in a chemical family? a. Nuclear charge increases from top to bottom in a chemical family. b. Nuclear charge decreases from top to bottom in a chemical family. c. The number of energy levels increases from top to bottom in a chemical family. d. The number of energy levels decreases from top to bottom in a chemical family. e. The number of electrons decreases from top to bottom in a chemical family.
28. Why does atomic radius decrease from left to right in a period? a. Nuclear charge increases from left to right in a period. b. Nuclear charge decreases from left to right in a period. c. The number of energy levels increases from left to right in a period. d. The number of energy levels decreases from left to right in a period. e. The number of electrons decreases from left to right in a period. 29. Why does ionization energy increase from left to right in a period? a. Nuclear charge increases from left to right in a period. b. Nuclear charge decreases from left to right in a period. c. The number of energy levels increases from left to right in a period. d. The number of energy levels decreases from left to right in a period. e. The number of electrons decreases from left to right in a period. 30. Why does electron affinity increase from bottom to top in a chemical family? a. Nuclear charge increases from bottom to top in a chemical family. b. Nuclear charge decreases from bottom to top in a chemical family. c. The number of energy levels increases from bottom to top in a chemical family. d. The number of energy levels decreases from bottom to top in a chemical family. e. The number of electrons increases from bottom to top in a chemical family. 31. Which of the following is the most reactive element? a. helium d. hydrogen b. radon e. ununoctium c. francium 32. Why is it easier to remove an electron from potassium than it is to remove an electron from calcium? a. Potassium has a higher electron affinity. b. Potassium has a higher ionization energy. c. Potassium has a lower nuclear charge. d. Calcium has a lower electron affinity. e. Calcium is a metal, but potassium is not. 33. What effect does the waste heat from nuclear power stations have on the environment? a. It adds to the greenhouse effect. d. all of the above b. It affects aquatic life. e. none of the above c. It depletes the ozone layer. 34. Which of the following is a practical use of radioisotopes? a. determining the age of old objects d. all of the above b. medical diagnosis e. none of the above c. production of electricity 35. Atomic or ionic radius depends on a. nuclear charge d. all of the above b. number of populated energy levels e. none of the above c. number of valence electrons
36. Which of the following would have the highest electron affinity? a. potassium d. oxygen b. helium e. carbon c. fluorine 37. Consider the equation X (g) + e X + energy. The "energy" term in the equation represents a. electronegativity d. nuclear charge b. electron affinity e. none of the above c. ionization energy 38. Electronegativity is derived from a. ionization energies d. all of the above b. electron affinity e. none of the above c. reactivity 39. Elements X and Y are in the same chemical family. Element X has a first ionization energy of 7.646 ev. Element Y has a first ionization energy of 5.695 ev. Which is more reactive? a. X b. Y c. They are equally reactive. d. not enough information e. X will be more reactive provided it reacts with another member of its family. 40. Elements A, B, C, and D (found in Groups 1 17) have atomic radii of 265 m, 160 m, 185 m, and 175 m, respectively. Which element will most likely have the highest ionization energy? a. A d. D b. B e. not enough information c. C 41. One atomic mass unit is defined as a. exactly the mass of a C-12 atom b. exactly 14 times the mass of a C-12 atom c. exactly the mass of a C-12 atom d. exactly 12 times the mass of a C-12 atom e. none of the above 42. The SI symbol used for the atomic mass unit is a. au d. atm b. atu e. am c. u 43. Chlorine has two naturally occurring isotopes, namely and. The composition of chlorine is 25.0% and 75.0%. The average atomic mass of chlorine is a. 36.5 u d. 45.5 u b. 35.5 u e. 32.0 u c. 34.6 u
44. Silicon has three naturally occurring isotopes, as follows: 3.10% silicon-30 (atomic mass = 29.974 u); 4.67% silicon-29 (atomic mass = 28.976 u); and 92.23% silicon-28 (atomic mass = 27.977 u). The average atomic mass of silicon is a. 28.1 u d. 30.0 u b. 29.2 u e. 28.9 u c. 29.8 u 45. The relative atomic mass of a given element most closely resembles the total number of a. neutrons in the nucleus d. neutrons and protons in the nucleus b. neutrons and electrons e. neutrons and electrons c. protons in the nucleus 46. A new element, dmytrium, has two isotopes, Dm-350 and Dm-375. The composition of dmytrium is 62.0% Dm-350 and 38.0% Dm-375 by mass. The relative atomic mass of this new element is a. 351 u d. 366 u b. 354 u e. 360 u c. 357 u 47. An isotope that has three times the mass of an atom of C-12 is most likely an atom of a. chlorine d. carbon b. lithium e. fluorine c. calcium