Test 7: Periodic Table Review Questions

Transcription

1 Name: Wednesday, January 16, 2008 Test 7: Periodic Table Review Questions 1. Which halogen is a solid at STP? 1. fluorine 3. bromine 2. chlorine 4. iodine 2. Element M is a metal and its chloride has the formula MCl 2. To which group of the Periodic Table does element M most likely belong? 1. 1 (IA) (VA) 2. 2 (IIA) (VIIA) 3. As the atomic number of elements within Group 2 increases, the metallic character of each successive element 1. decreases 2. increases 3. remains the same 4. Which characteristics describe most nonmetals in the solid phase? 1. They are malleable and have metallic luster. 3. They are brittle and have metallic luster. 2. They are malleable and lack metallic luster. 4. They are brittle and lack metallic luster. 5. Which group in the Periodic Table contains elements that are all gases at STP? (IB) (IIB) (VIIA) (0)

2 6. Compared to the radius of a chlorine atom, the radius of a chloride ion is 1. larger because chlorine loses an electron 3. smaller because chlorine loses an electron 2. larger because chlorine gains an electron 4. smaller because chlorine gains an electron 7. Which of these elements has an atom with the most stable outer electron configuration? 1. Ne 3. Ca 2. Cl 4. Na 8. Which of the following ions has the smallest radius? - 1. F + 3. K - 2. Cl Ca 9. Arsenic and silicon are similar in that they both 1. have the same ionization energy 3. are transition metals 2. have the same covalent radius 4. are metalloids 10. As the elements in Period 3 are considered from left to right, they tend to 1. lose electrons more readily and increase in metallic 3. gain electrons more readily and increase in metallic character character 2. lose electrons more readily and increase in 4. gain electrons more readily and increase in nonmetallic character nonmetallic character

3 11. The atom of which element has an ionic radius smaller than its atomic radius? 1. N 3. Br 2. S 4. Rb 12. Which property is characteristic of nonmetals? 1. They have a high electronegativity. 3. They have a low first ionization energy. 2. They lose electrons easily. 4. They are good conductors of electricity. 13. Which group in the Periodic Table contains elements that are all monatomic gases at STP? The amount of energy required to remove the outermost electron from a gaseous atom in the ground state is known as 1. first ionization energy 3. conductivity 2. activation energy 4. electronegativity When an atom of phosphorus becomes a phosphide ion (P ), the radius 1. decreases 2. increases 3. remains the same

4 16. At 25 C, in which phase of matter do most of the known elements exist? 1. solid 3. gas 2. liquid 4. supercooled liquid 17. Which of these Group 14 elements has the most metallic properties? 1. C 3. Si 2. Ge 4. Sn 18. Which period of the Periodic Table contains more metallic elements than nonmetallic elements? 1. Period 1 3. Period 3 2. Period 2 4. Period Nonmetals in the solid state are poor conductors of heat and tend to 1. be brittle 3. have a shiny luster 2. be malleable 4. have good electrical conductivity 20. In which list are the elements arranged in order of increasing atomic mass? 1. Cl, K, Ar 3. Te, I, Xe 2. Fe, Co, Ni 4. Ne, F, Na

5 21. Which group contains a metalloid? As the atoms of the Group 17 elements in the ground state are considered from top to bottom, each successive element has 1. the same number of valence electrons and similar 3. an increasing number of valence electrons and similar chemical properties chemical properties 2. the same number of valence electrons and identical 4. an increasing number of valence electrons and identical chemical properties chemical properties 23. Draw a Lewis electron-dot structure for an atom of phosphorus Which halogens are gases at STP? 1. chlorine and fluorine 3. iodine and fluorine 2. chlorine and bromine 4. iodine and bromine

6 25. 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 3. number of protons decreases, and the number of shells of electrons remains the same of electrons remains the same 2. number of protons increases, and the number of shells 4. number of protons decreases, and the number of shells of electrons increases of electrons increases 26. The chemical properties of the elements are periodic functions of their atomic 1. masses 3. numbers 2. weights 4. radii 27. Which is a property of most nonmetallic solids? 1. high thermal conductivity 3. brittleness 2. high electrical conductivity 4. malleability 28. Which element is in Group 2 (IIA) and Period 7 of the Periodic Table? 1. magnesium 3. radium 2. manganese 4. radon 29. What is the total number of valence electrons in a fluorine atom in the ground state?

7 30. An atom in the ground state contains 8 valence electrons. This atom is classified as a 1. metal 3. noble gas 2. semimetal 4. halogen 31. A strontium atom differs from a strontium ion in that the atom has a greater 1. number of electrons 3. atomic number 2. number of protons 4. atomic mass 32. Which trends appear as the elements in Period 3 are considered from left to right? 1. Metallic character decreases, and electronegativity 3. Metallic character increases, and electronegativity decreases. decreases. 2. Metallic character decreases, and electronegativity 4. Metallic character increases, and electronegativity increases. increases. 33. Which statement is true about the properties of the elements in any one period of the Periodic Table? 1. They are determined by the number of neutrons. 3. They change in a generally systematic manner. 2. They are determined by the number of electrons in the first 4. They change in a random, unpredictable shell. manner. 34. What are two properties of most nonmetals? 1. high ionization energy and poor electrical 3. low ionization energy and poor electrical conductivity conductivity 2. high ionization energy and good electrical 4. low ionization energy and good electrical conductivity conductivity

8 35. Which list of elements is arranged in order of increasing atomic radii? 1. Li, Be, B, C 3. Sc, Ti, V, Cr 2. Sr, Ca, Mg, Be 4. F, Cl, Br, I 36. Which list of elements contains two metalloids? 1. Si, Ge, Zr, Pb 3. Si, P, S, Cl 2. As, Bi, Br, Kr 4. Zr, Sb, I, Xe 37. Which of these elements has physical and chemical properties most similar to silicon (Si)? 1. germanium (Ge) 3. phosphorus (P) 2. lead (Pb) 4. chlorine (Cl) 38. In which shell are the valence electrons of the elements in Period 2 found? The elements of the Periodic Table are arranged in horizontal rows according to each successive element's greater 1. atomic mass 3. number of protons 2. atomic radius 4. number of neutrons

9 40. The element in Period 4 and Group 1 of the Periodic Table would be classified as a 1. metal 3. nonmetal 2. metalloid 4. noble gas 41. What is the total number of electrons in the valence shell of an atom of aluminum in the ground state? The metalloids that are included in Group 15 (VA) are antimony (Sb) and 1. N 3. As 2. P 4. Bi 43. Which element in Period 5 of the Periodic Table is a transition element? 1. Sr 3. Ag 2. Sb 4. Xe 44. The properties of elements are periodic functions of their 1. mass numbers 3. atomic radii 2. atomic masses 4. atomic numbers

10 45. Which group contains elements in three phases of matter at STP? 1. noble gases 3. alkaline earth metals 2. transition elements 4. halogens 46. The atoms of the elements in Group 2 have the same 1. mass number 3. number of protons 2. atomic number 4. number of valence electrons 47. Which element is so active chemically that it occurs naturally only in compounds? 1. potassium 3. copper 2. silver 4. sulfur 48. A characteristic of most nonmetallic solids is that they are 1. brittle 3. malleable 2. ductile 4. conductors of electricity 49. For which element is the radius of its ion larger than the radius of its atom? 1. K 3. Na 2. F 4. Ca

11 50. Which electron-dot symbol represents an atom of argon in the ground state?

12 Answer Key for Test 7: Periodic Table Review Questions Test 7: Periodic Table Review Questions

13 Test 7: Periodic Table Review Questions