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1 Name: Chemistry, PERIODIC TABLE 1. A solid element that is malleable, a good conductor of electricity, and reacts with oxygen is classified as a (1) noble gas (2) metalloid (3) metal (4) nonmetal 2. Which ion has the largest radius? (1) K + (2) Mg 2+ (3) Ca 2+ (4) Na + 3. Which statement explains why neon is a Group 18 element? (1) Neon atoms have two electrons in the first shell. (2) Neon has a low melting point. (3) Neon is a gas at STP. (4) Neon atoms have a stable valence electron configuration. 4. How much energy is required to remove the most loosely bound electron from a neutral atom of carbon in the gaseous phase? (1) 363 kj (2) 1242 kj (3) 441 kj (4) 1086 kj 5. Which of the following Group 2 elements has the lowest first ionization energy? (1) Be (2) Ca (3) Ba (4) Mg 6. As atomic number increases within Group 15 on the Periodic Table, atomic radius (1) decreases, only (2) increases, only (3) decreases, then increases (4) increases, then decreases 7. Which Group 14 element is a metalloid? (1) carbon (2) lead (3) silicon (4) tin 8. Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to bottom on the Periodic Table? (1) an increase in nonmetallic behavior (2) a decrease in electronegativity (3) an increase in first ionization energy (4) a decrease in atomic radius 9. Which list of elements consists of a metal, a metalloid, and a nonmetal? (1) O, S, Te (2) Sn, Si, C (3) Li, Na, Rb (4) Cr, Mo, W Date: Pd: Spring, Regents Prep 10. Which particle diagram represents a sample of matter that can not be broken down by chemical means? (1) (2) (3) (4) 11. The valence electrons of a germanium atom in the ground state are located in the (1) first shell (2) second shell (3) third shell (4) fourth shell 12. If an element, X, can form an oxide that has the formula X 2O3, then element X would most likely be located on the Periodic Table in the same group as (1) In (2) Cd (3) Ba (4) Na HSVD Ms. Chang Page 1

2 13. Which elements have the most similar chemical properties? (1) N2, O2, and F2 (2) Ca, Cs, and Cu (3) Mg, Sr, and Ba (4) Si, As, and Te 14. Which list includes elements with the most similar chemical properties? (1) Br, Ga, Hg (2) Cr, Pb, Xe (3) N, O, F (4) O, S, Se 15. Which diagram represents a mixture of two different molecular forms of the same element? 22. What is the number of electrons in an Al 3+ ion? (1) 10 (2) 13 (3) 3 (4) Which atom has the largest atomic radius? (1) cesium (2) francium (3) rubidium (4) potassium 24. Which Lewis electron-dot diagram represents a nitrogen atom in the ground state? (1) (2) (3) (4) 25. The elements on the Periodic Table are arranged in order of increasing (1) (2) (1) oxidation number (2) molar mass (3) atomic number (4) atomic mass 26. Given four particle models: (3) (4) 16. 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? (1) (2) (3) (4) 17. Which element is a metalloid? (1) Au (2) Ar (3) As (4) Al 18. In the formula X 2(SO4)3, the X represents a metal. This metal could be located on the Periodic Table in (1) Group1 (2) Group 2 (3) Group 13 (4) Group In the ground state, which atom has a completely filled valence electron shell? (1) C (2) Ne (3) V (4) Sb 20. Which atom in the ground state has a stable electron configuration? (1) neon (2) carbon (3) magnesium (4) oxygen 21. Which two gases can not be broken down by chemical means? (1) CO and He (2) CO and NH3 (3) Xe and NH3 (4) Xe and He Which two models can be classified as elements? (1) I and II (2) II and IV (3) II and III (4) I and IV 27. Which element has chemical properties that are most similar to the chemical properties of fluorine? (1) chlorine (2) oxygen (3) boron (4) neon 28. When an atom of lithium loses an electron, the atom becomes a (1) negative ion with a radius smaller than the radius of the atom (2) negative ion with a radius larger than the radius of the atom (3) positive ion with a radius smaller than the radius of the atom (4) positive ion with a radius larger than the radius of the atom 29. Which atom has the weakest attraction for the electrons in a bond with an H atom? (1) Cl atom (2) S atom (3) F atom (4) O atom 30. Which element forms an ion that is larger than its atom? (1) chlorine (2) sodium (3) aluminum (4) magnesium HSVD Ms. Chang Page 2

3 31. Explain, in terms of subatomic particles, why the radius of a chloride ion is larger than the radius of a chlorine atom. 32. Base your answer to the following question on the information below. The atomic and ionic radii for sodium and chlorine are shown in the table below. Write the ground state electron configuration for the ion that has a radius of 181 picometers. 33. Base your answer to the following question on the Reference Tables for Physical Setting/Chemistry. a Complete the data table provided for the following Group 18 elements: He, Ne, Ar, Kr, Xe b Using information from your data table in part a, construct a line graph on the grid provided, following the directions below. Mark an appropriate scale on the axis labeled "First Ionization Energy (kj/mol). " Plot the data from your data table. Circle each point and connect the points. c Based on your graph in part c, describe the trend in first ionization energy of Group 18 elements as the atomic number increases. HSVD Ms. Chang Page 3

4 34. Base your answer to the following question on the data table provided. On the same grid, plot the data from the data table. Circle and connect the points. 35. Explain, in terms of atomic structure, why Group 18 elements on the Periodic Table rarely form compounds. 36. Base your answer to the following question on the information below and on your knowledge of chemistry. The diagram below represents three elements in Group 13 and three elements in Period 3 and their relative positions on the Periodic Table. Some elements in the solid phase exist in different forms that vary in their physical properties. For example, at room temperature, red phosphorus has a density of 2.16 g/cm 3 and white phosphorus has a density of g/cm 3. Consider the Period 3 elements in the diagram in order of increasing atomic number. State the trend in electronegativity for these elements. HSVD Ms. Chang Page 4

5 37. Base your answer to the following question on the information below. Identify one element from this table for each type of element: metal, metalloid, and nonmetal. 38. Explain, in terms of electrons, why the radius of a potassium atom is larger than the radius of a potassium ion in the ground state. 39. In the 19th century, Dmitri Mendeleev predicted the existence of a then unknown element X with a mass of 68. He also predicted that an oxide of X would have the formula X 2O3. On the modern Periodic Table, what is the group number and period number of element X? HSVD Ms. Chang Page 5

6 40. Base your answer to the following question on the information below. The ionic radii of some Group 2 elements are given in the table below. On the grid, mark an appropriate scale on the axis labeled "Ionic Radius (pm)." HSVD Ms. Chang Page 6

7 Chemistry Name Class Date Diagram on Separate Sheet HSVD Ms. Chang Page 7

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