Handout 4-1 Periodic Table 1. The elements on the Periodic Table are arranged in order of increasing 1) atomic mass 2) atomic number 3) molar mass 4) oxidation number 2. Which element exists as a diatomic molecule at STP? 1) bromine 2) argon 3. The element in Group 14, Period 3, of the Periodic Table is classified as a 1) metal 2) noble gas 3) neon 4) carbon 1) Li, Na, Rb 2) Cr, Mo, W 4. Which list of elements consists of a metal, a metalloid, and a nonmetal? 3) metalloid 4) nonmetal 3) Sn, Si, C 4) O, S, Te 5. Which list includes elements with the most similar chemical properties? 1) Br, Ga, Hg 3) O, S, Se 4) N, O, F 2) Cr, Pb, Xe 6. Which statement identifies the element arsenic? 1) Arsenic has an atomic number of 33. 2) Arsenic has a melting point of 84 K. 3) An atom of arsenic in the ground state has eight valence electrons. 4) An atom of arsenic in the ground state has a radius of 146 pm. 7. Which statement explains why sulfur is classified as a Group 16 element? 1) A sulfur atom has 6 valence electrons. 2) A sulfur atom has 16 neutrons. 3) Sulfur is a yellow solid at STP. 4) Sulfur reacts with most metals. 1) hydrogen 2) calcium 8. Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element. X be found? 2) 2 3) 15 4) 16 1) 1 9. Which element is an alkali metal? 3) sodium 4) zinc 10. Most of the groups in the Periodic Table of the Elements contain 1) nonmetals, only 2) metals, only 3) nonmetals and metals 4) metals and metalloids 11. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? 1) nonmetal → metalloid → metal 2) metalloid →→ metal → nonmetal 3) metal metalloid →→> nonmetal 4) metal →→nonmetal → metalloid 12. Which group contains both metals and nonmetals? 1) 1 2) 3 3) 15 4) 7 13. Which element is in Group 2 and Period 7 of the Periodic Table? 1) magnesium 3) radium 2) manganese 4) radon 14. Bromine has chemical properties most similar to 1) fluorine 2) potassium 3) krypton 4) mercury 15. Which group is known as the halogens? 1) 1 2) 2 3) 17 4) 18 16. An atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This element is in Group 1) 1 2) 2 3) 4 4) 18 17. Which element is malleable and ductile? 1) S 2) Si 3) Au 4) C 18. Which of these elements is the best conductor of electricity? 1) Sb 3) Si 4) Zn 2) I/n19. What is a property of most metals? 1) They tend to gain electrons easily when bonding. 2) They tend to lose electrons easily when bonding. 3) They are poor conductors of heat. 4) They are poor conductors of electricity. 20. Which element has properties of electrical conductivity and luster and exists as a liquid at STP? 1) Hg 2) Br 3) C 4) I 21. Metallic substances will conduct electricity in 1) the solid phase, only 2) the liquid phase, only 3) both the solid and the liquid phase 4) neither the solid nor the liquid phase 22. At STP, graphite and diamond are two solid forms of carbon. Which statement explains why these two forms of carbon differ in hardness? 1) Graphite and diamond have different ionic radii. 2) Graphite and diamond have different molecular structures. 3) Graphite is a metal, but diamond is a nonmetal. 4) Graphite is a good conductor of electricity, but diamond is a poor conductor of electricity. 23. Which particle diagram represents the arrangement of F2 molecules in a sample of fluorine at 95 K and standard pressure? Key O atom of fluorine = त O 8 3) 4) 24. At STP, which element is brittle and not a conductor of electricity? 1) S 2) K 3) Na 4) Ar 25. Which characteristics describe most nonmetals in the solid phase? 1) They are malleable and have metallic luster. 2) They are malleable and lack metallic luster. 3) They are brittle and have metallic luster. 4) They are brittle and lack metallic luster. 26. Which element tends not to react with other elements? 1) neon 2) hydrogen 3) phosphorous 4) potassium 27. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has 1) more protons than neutrons 2) more neutrons than protons 3) a total of two valence electrons 4) a total of eight valence electrons 28. Which element has both metallic and nonmetallic properties? 1) Rb 2) Rn 3) Si 4) Sr 29. At 25°C, in which phase of matter do most of the known elements exist? 1) solid 2) liquid 3) gas 4) supercooled liquid 30. Which group in the Periodic Table contains elements that are all gases at STP? 1) 11 2) 17 3) 12 4) 18 31. Which group on the Periodic Table has at least one element in each of the three phases of matter at STP? 1) 1 2) 2 3) 17 4) 18 32. Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)? 1) They have different molecular structures, only. 2) They have different properties, only. 3) They have different molecular structures and different properties. 4) They have the same molecular structure and the same properties./n33. Which element has the greatest density at STP? 1) calcium 2) carbon 3) chlorine 4) copper 34. An atom that has an electron configuration of 2-8-13-2 is classified as 1) an alkali metal 2) an alkaline earth metal 3) a transition element 4) a noble gas element 35. Magnesium and calcium have similar chemical properties because their atoms in the ground state have 1) equal numbers of protons and electrons 2) equal numbers of protons and neutrons 3) two electrons in the first shell 4) two electrons in the outermost shell 36. Which compound forms a green aqueous solution? 1) RbCl 2) CaCl2 3) NiCl24) ZnCl2 37. Based upon your knowledge of metallic activity, which element would most readily react with water? 1) Zn 2) Cu 3) Fe 4) Li 38. Which ionic compound dissolves in water to form a colored solution? 1) Ca(NO3)2 2) Cu(NO3)2 3) KNO3 4) AI(NO3)3 39. Which set of properties is most characteristic of transition elements? 1) colorless ions in solution, multiple positive oxidation states 2) colorless ions in solution, multiple negative oxidation states 3) colored ions in solution, multiple positive oxidation states 4) colored ions in solution, multiple negative oxidation states 40. Compared to the radius of a chlorine atom, the radius of a chloride ion is 1) larger because chlorine loses an electron 2) larger because chlorine gains an electron 3) smaller because chlorine loses an electron 4) smaller because chlorine gains an electron 41. Compared to an atom of potassium, an atom of calcium has a 1) larger radius and lower reactivity 2) larger radius and higher reactivity 3) smaller radius and lower reactivity 4) smaller radius and higher reactivity 42. As an atom becomes an ion, its mass number 3) remains the sam 1) decreases 2) increases 43. Which two characteristics are associated with metals? 1) low first ionization energy and low electronegativity 2) low first ionization energy and high electronegativity 3) high first ionization energy and low electronegativity 4) high first ionization energy and high electronegativity 44. As the elements in Period 2 of the Periodic Table are considered in order from left to right, which property generally decreases? 1) atomic radius 3) ionization energy 2) electronegativity 4) nuclear charge 45. Which of the following Period 4 elements has the most metallic characteristics? 1) Ca 2) Ge 3) As 4) Br 46. Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? 1) Their metallic properties decrease and their atomic radii decrease. 2) Their metallic properties decrease and their atomic radii increase. 3) Their metallic properties increase and their atomic radii decrease. 4) Their metallic properties increase and their atomic radii increase. Page 3/n47. 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 48. Which of the following electron configurations represents the element with the smallest atomic radius? 1) 2-4 2) 2-5 3) 2-6 4) 2-7 49. An atom with the electron configuration 2-8-7 would most likely 1) decrease in size as it forms a positive ion 2) increase in size as it forms a positive ion 3) decrease in size as it forms a negative ion 4) increase in size as it forms a negative ion 50. Which ion has the largest radius? 1) Br 2) Cl- 3) F- 4) 1- 51. Which ion has the largest radius? 1) Na+ 2) Mg²+ 3) K+ 4) Ca²+ 52. As the elements in Group I of the Periodic Table are considered from top to bottom, each successive element has a 1) smaller first ionization energy 2) larger first ionization energy 3) smaller number of protons 4) larger number of valence electrons 53. Elements that readily gain electrons tend to have 1) high ionization energy and high electronegativity 2) high ionization energy and low electronegativity 3) low ionization energy and low electronegativity 4) low ionization energy and high electronegativity 54. How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? 1) Sodium has a larger atomic radius and is more metallic. 2) Sodium has a larger atomic radius and is less metallic. 3) Sodium has a smaller atomic radius and is more metallic. 4) Sodium has a smaller atomic radius and is less metallic. 55. As the elements of Group 16 are considered in order from top to bottom, the covalent radius of each successive element increases. This increase is primarily due to an increase in 1) atomic number 2) mass number 3) the number of protons occupying the nucleus 4) the number of occupied electron shells 56. Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having 1) a larger nuclear charge 2) a smaller nuclear charge 3) more principal energy levels 4) fewer principal energy levels 57. Which term represents the strength of the attraction an atom has for the electrons in a chemical bond? 1) electrical conductivity 2) electronegativity 3) first ionization energy 4) specific heat capacity 58. Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond? 1) chlorine 2) nitrogen 3) oxygen 4) selenium 59. Which element requires the least amount of energy to remove the most loosely held electron from a gaseous atom in the ground state? 1) Na 2) Ar 3) P 4) CI Page 4/nShort Answers Base your answers to questions 1 through 3 on the information below and on your knowledge of chemistry. A technician recorded data for two properties of Period 3 elements. The data are shown in the table below. Element Ionic Radius (pm) Reaction with Cold Water Na 95 reacts vigorously Two Properties of Period 3 Elements Si P 41 Mg Al 51 66 S 184 no no no reacts no very observable observable observable observable slowly reaction reaction reaction reaction 1. Identify the element in this table that is classified as a metalloid. CI 181 reacts slowly Ar no observable reaction 2. State evidence from the technician's data which indicates that sodium is more active than aluminum. 3. State the phase of chlorine at 281 K and 101.3 kPa. (hint: use Reference Table S) Explain. Base your answers to questions 4 through 7 on the information below and on your knowledge of chemistry. Sir William Ramsey is one scientist credited with identifying the noble gas argon. Sir Ramsey separated nitrogen gas from the air and reacted it with an excess of magnesium, producing solid magnesium nitride. However, a small sample of an unreactive gas remained with a density different from the density of the nitrogen gas. Sir Ramsey identified the unreactive gas as argon and later went on to discover neon, krypton, and xenon. 4. Compare the chemical reactivities of nitrogen gas and argon gas based on Sir Ramsey's experiment using magnesium. 5. Compare the density of nitrogen gas to the density of argon gas when both gases are at 298 Kand 101.3 kPa. 6. State, in terms of valence electrons, why the noble gases that Sir Ramsey discovered have similar chemical properties. 7. State the trend, at standard pressure, of the boiling points of these noble gases, as they are considered in order of increasing atomic number. Page 1/nchemistry. Some properties of the element sodium are listed below. • is a soft, silver-colored metal • melts at a temperature of 371 K • oxidizes easily in the presence of air • forms compounds with nonmetallic elements in nature • forms sodium chloride in the presence of chlorine gas 8. Identify one chemical property of sodium from this list. 9. Convert the melting point of sodium to degrees Celsius. Base your answers to questions 10 and 11 on the information below. Densities of Group 14 Elements Density at STP (g/cm³) 3,51 Element C Si Ge Sn Pb 2.33 5.32 7.31 11.35 10. Identify one element from this table for each type of element: metal, metalloid, and nonmetal. 11. Calculate the volume of a tin block that has a mass of 95.04 grams at STP. Your response must include both a numerical setup and the calculated result. Round your answer to the correct number of significant figures. Base your answers to questions 12 through 14 on the information below and on your knowledge of chemistry. Periodic trends are observed in the properties of the elements in Period 3 on the Periodic Table. These elements vary in physical properties, such as phase, and in chemical properties, such as their ability to lose or gain electrons during a chemical reaction. 12. Identify the metals in Period 3 on the Periodic Table. 13. Identify the element in Period 3 that requires the least amount of energy to remove the most loosely held electrons from a mole of gaseous atoms of the element in the ground state. 14. State the general trend in atomic radius as the elements in Period 3 are considered in order of increasing atomic number. Page 2/nBase your answers to questions 15 through 17 on the information below and on your knowledge of chemistry. The elements in Group 2 on the Periodic Table can be compared in terms of first ionization energy, electronegativity, and other general properties. 15. Describe the general trend in electronegativity as the metals in Group 2 on the Periodic Table are considered in order of increasing atomic number. 16. Explain, in terms of electron configuration, why the elements in Group 2 have similar chemical properties. 17. Explain, in terms of atomic structure, why barium has a lower first ionization energy than magnesium. Base your answers to questions 18 through 20 on the information below and on your knowledge of chemistry. Rubidium and iodine have different chemical and physical properties. Some of these properties are shown in the table below. Some Physical and Chemical Properties of Rubidium and lodine Rubidium lodine silvery-white solid forms ionic compounds with nonmetals reacts with oxygen in the air specific heat = 0.363 J/g+K 18. State the chemical property of iodine listed in this table. bluish-black lustrous solid forms ionic bonds with active metals sublimes at room temperature specific heat = 0.214 J/g.K 19. Compare the atomic radius of an atom of iodine to the atomic radius of an atom of rubidium when both atoms are in the ground state. 20. Compare the electrical conductivity of these two elements at STP. Page 3

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Handout 4-1 Periodic Table 1. The elements on the Periodic Table are arranged in order of increasing 1) atomic mass 2) atomic number 3) molar mass 4) oxidation number 2. Which element exists as a diatomic molecule at STP? 1) bromine 2) argon 3. The element in Group 14, Period 3, of the Periodic Table is classified as a