1. Compared to the atoms of nonmetals in Period 3, the atoms of metals in Period 3 have A) fewer valence electrons B) more valence electrons C) fewer electron shells D) more electron shells 2. The elements on the Periodic Table are arranged in order of increasing A) atomic number B) mass number C) number of isotopes D) number of moles 3. Which element has chemical properties that are most similar to the chemical properties of sodium? A) beryllium B) calcium C) lithium D) magnesium 4. Which list of elements contains a metal, a metalloid, a nonmetal, and a noble gas? A) Be, Si, Cl, Kr B) C, N, Ne, Ar C) K, Fe, B, F D) Na, Zn, As, Sb 5. The chemical properties of calcium are most similar to the chemical properties of A) Ar B) K C) Mg D) Sc 6. Which two elements have the most similar chemical A) Be and Mg B) Ca and Br C) Cl and Ar D) Na and P 7. Which statement explains why sulfur is classified as a Group 16 element? A) A sulfur atom has 6 valence electrons. B) A sulfur atom has 16 neutrons. C) Sulfur is a yellow solid at STP. D) Sulfur reacts with most metals. 8. Which substance can be decomposed by chemical means? A) tungsten B) antimony C) krypton D) methane 9. Which elements are malleable and good conductors of electricity? A) iodine and silver B) iodine and xenon C) tin and silver D) tin and xenon 10. Which Group 14 element is classified as a metal? A) carbon B) germanium C) silicon D) tin 11. An element that has a low first ionization energy and good of heat and electricity is classified as a A) metal B) metalloid C) nonmetal D) noble gas 12. A sample of an element is malleable and can conduct electricity. This element could be A) H B) He C) S D) Sn 13. Which two characteristics are associated with metals? A) low first ionization energy and low B) low first ionization energy and high C) high first ionization energy and low D) high first ionization energy and high 14. Which element is malleable and can conduct electricity in the solid phase? A) iodine B) phosphorus C) sulfur D) tin 15. The elements located in the lower left corner of the Periodic Table are classified as A) metals B) nonmetals C) metalloids D) noble gases 16. What is a property of most metals? A) They tend to gain electrons easily when bonding. B) They tend to lose electrons easily when bonding. C) They are poor conductors of heat. D) They are poor conductors of electricity. 17. At STP, which element is solid, brittle, and a poor conductor of electricity? A) Al B) K C) Ne D) S 18. Which element is classified as a nonmetal? A) Be B) Al C) Si D) Cl
19. Which is a property of most nonmetallic solids? A) high thermal B) high electrical C) brittleness D) malleability 20. What are two properties of most nonmetals? A) high ionization energy and poor electrical B) high ionization energy and good electrical C) low ionization energy and poor electrical D) low ionization energy and good electrical 21. Which property is characteristic of nonmetals? A) They have a high. B) They lose electrons easily. C) They have a low first ionization energy. D) They are good conductors of electricity. 22. The table below shows some properties of elements A, B, C, and D. 26. Which Lewis electron-dot diagram represents an atom in the ground state for a Group 13 element? 27. An atom in the ground state contains a total of 5 electrons, 5 protons, and 5 neutrons. Which Lewis electron-dot diagram represents this atom? 28. Which Lewis electron-dot diagram is correct for a S 2 ion? A) B) C) D) 29. Which Lewis electron-dot structure is drawn correctly for the atom it represents? 30. Which electron-dot symbol correctly represents an atom of its given element? Which element is most likely a nonmetal? A) A B) B C) C D) D 23. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has A) more protons than neutrons B) more neutrons than protons C) a total of two valence electrons D) a total of eight valence electrons 24. Which element is a metalloid? A) Al B) Ar C) As D) Au 25. Which element has both metallic and nonmetallic A) Rb B) Rn C) Si D) Sr 31. Aqueous solutions of compounds containing element X are blue. Element X could be A) carbon B) copper C) sodium D) sulfur 32. Which compound forms a green aqueous solution? A) RbCl B) CaCl2 C) NiCl2 D) ZnCl2 33. An atom of which element has the largest atomic radius? A) Fe B) Mg C) Si D) Zn 34. Which characteristics both generally decrease when the elements in Period 3 on the Periodic Table are considered in order from left to right? A) nonmetallic properties and atomic radius B) nonmetallic properties and ionization energy C) metallic properties and atomic radius D) metallic properties and ionization energy
35. As atomic number increases within Group 15 on the Periodic Table, atomic radius A) decreases, only B) increases, only C) decreases, then increases D) increases, then decreases 36. As the elements of Group 17 are considered in order of increasing atomic number, there is an increase in A) atomic radius B) C) first ionization energy D) number of electrons in the first shell 37. How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? A) Sodium has a larger atomic radius and is more B) Sodium has a larger atomic radius and is less C) Sodium has a smaller atomic radius and is more D) Sodium has a smaller atomic radius and is less 38. Which grouping of circles, when considered in order from the top to the bottom, best represents the relative size of the atoms of Li, Na, K, and Rb, respectively? 39. An ion of which element has a larger radius than an atom of the same element? A) aluminum B) chlorine C) magnesium D) sodium 40. An atom with the electron configuration 2-8-2 would most likely A) decrease in size as it forms a positive ion B) increase in size as it forms a positive ion C) decrease in size as it forms a negative ion D) increase in size as it forms a negative ion 41. An Mg atom differs from an Mg 2+ ion in that the atom has a A) smaller radius B) larger radius C) smaller nucleus D) larger nucleus 42. Which atom has the weakest attraction for the electrons in a bond with an H atom? A) Cl atom B) F atom C) O atom D) S atom 43. Which statement describes the general trends in and metallic properties as the elements in Period 2 are considered in order of increasing atomic number? A) Both and metallic properties decrease. B) Both and metallic properties increase. C) Electronegativity decreases and metallic properties increase. D) Electronegativity increases and metallic properties decrease. 44. An atom of which element has the greatest attraction for electrons in a chemical bond? A) As B) Ga C) Ge D) Se 45. Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to bottom on the Periodic Table? A) a decrease in atomic radius B) a decrease in C) an increase in first ionization energy D) an increase in nonmetallic behavior 46. An atom of which element has the greatest attraction for the electrons in a bond with a hydrogen atom? A) chlorine B) phosphorus C) silicon D) sulfur 47. Atoms of which element have the greatest tendency to gain electrons? A) bromine B) chlorine C) fluorine D) iodine 48. Which atom in the ground state requires the least amount of energy to remove its valence electron? A) lithium atom B) potassium atom C) rubidium atom D) sodium atom
49. Which element requires the least amount of energy to remove the most loosely held electron from a gaseous atom in the ground state? A) bromine B) calcium C) sodium D) silver 50. Samples of four Group 15 elements, antimony, arsenic, bismuth, and phosphorus, are in the gaseous phase. An atom in the ground state of which element requires the least amount of energy to remove its most loosely held electron? A) As B) Bi C) P D) Sb 51. In the ground state, each atom of an element has two valence electrons. This element has a lower first ionization energy than calcium. Where is this element located on the Periodic Table? A) Group 1, Period 4 B) Group 2, Period 5 C) Group 2, Period 3 D) Group 3, Period4 52. Which general trend is found in Period 2 on the Periodic Table as the elements are considered in order of increasing atomic number? A) decreasing atomic mass B) decreasing C) increasing atomic radius D) increasing first ionization energy 53. Which Period 4 element has the most metallic A) As B) Br C) Ge D) Sc
Answer Key Chapter 6 Practice Questions 1. A 2. A 3. C 4. A 5. C 6. A 7. A 8. D 9. C 10. D 11. A 12. D 13. A 14. D 15. A 16. B 17. D 18. D 19. C 20. A 21. A 22. C 23. D 24. C 25. C 26. C 27. C 28. D 29. D 30. B 31. B 32. C 33. B 34. C 35. B 36. A 37. A 38. A 39. B 40. A 41. B 42. D 43. D 44. D 45. B 46. A 47. C 48. C 49. C 50. B 51. B 52. D 53. D