Survey
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
* Your assessment is very important for improving the workof artificial intelligence, which forms the content of this project
Regents Review Periodic Table Worksheet 1. Which two characteristics are as sociated with metals? A. low first ionization energy and low electronegativity B. low first ionization energy and high electronegativity C. high first ionization energy and low electronegativity D. high first ionization energy and high electronegativity Mr. Beauchamp 14. Which isotopic no tation identifies a metalloid that i s matched with the corresponding number of protons in each of its atoms? A. 24Mg and 12 protons C. 75As and 75 protons 28 B. Si and 14 protons D. 80Br and 80 protons 2. Which element is malleable and can conduct electricity in the solid phase? A. iodine C. sulfur B. phosphorus D. tin 3. Which substance can not be decomposed by ordinary chemical means? A. methane C. ethanol B. mercury D. ammonia 4. The elements located in the l ower left corner of the Periodic Table are classified as A. metals C. metalloids B. nonmetals D. noble gases 15. At standard pressure, which element has a melting point higher than standard temperature? A. F2 C. Fe B. Br 2 D. Hg 16. According to Reference Ta ble N, which pair of isotopes spontaneousl y decays? A. C-12 and N-14 C. C-14 and N-14 B. C-12 and N-16 D. C-14 and N-16 17. Which of these elements has the lowest melting point? A. Li C. K B. Na D. Rb 18. Which element is a solid at STP? A. B. 5. Which statement describes a chemical property of iron? A. Iron can be flattened int o sheets. B. Iron conducts electri city and heat. C. Iron combines wi th oxygen to form rust. D. Iron can be drawn into a wire. H2 I2 C. D. N2 O2 19. The elements on the Periodic Table are arr anged in order of increasing A. boiling point C. atomic number B. electronegativity D. atomic mass 6. What is a propert y of most metals? A. They tend to gain electrons easil y when bonding. B. They tend to lose electrons easi ly when bonding. C. They are poor conductors of heat. D. They are poor conductors of electricity. 20. Which element has chemical properties that are most similar to those of calcium? A. Co C. N B. K D. Sr 7. At STP, which elem ent is brittl e and not a conductor of electricity? A. S C. Na B. K D. Ar 21. The carbon atoms in graphite and the carbon atoms in diamond have different A. atomic numbers C. electronegativities B. atomic masses D. structural arrangements 8. Which element is classified as a nonmetal? A. Be C. Si B. Al D. Cl 22. A 10.0-gram sample of which element has the smallest volume at STP? A. aluminum C. titanium B. magnesium D. zinc 9. At STP, an element that is a bri ttle solid and a poor co nductor of heat and electri city could have an a tomic number of A. 12 C. 16 B. 13 D. 17 10. Which element is a noble gas? A. krypton B. chlorine C. D. antimony manganese 11. Which substance can not be decomposed by a chemical change? A. Ne C. HF B. N2O D. H2O 12. Which group in the Periodic Table contains elements t hat are all monatomic gases at STP? A. 15 C. 17 B. 16 D. 18 13. Which element has both metallic and nonmetallic properties? A. Rb C. Si B. Rn D. Sr 23. Lithium and potassium have similar chemical properties because the atoms of both elements have the same A. mass number B. atomic number C. number of electron shells D. number of valence electrons 24. An atom of argon rarel y bonds to an atom of ano ther el ement because an argon atom has A. 8 valence electrons B. 2 electrons in the first shell C. 3 electron shells D. 22 neutrons 25. What is the t otal number of valence electrons in an atom of sulfur in the ground state? A. 6 C. 3 B. 8 D. 4 Page 1 Periodic Table Worksheet 26. When an atom loses one or more electrons, this a tom becomes a A. positive ion with a radius smaller than the radius of this atom B. positive ion with a radius larger than the radius of this atom C. negative ion with a radius smaller than the radius of this atom D. negative ion with a radius larger than the radius of this atom 27. Which list of elements from Group 2 on the Periodic Table is arranged in order of increasing atomic radius? A. Be, Mg, Ca C. Ba, Ra, Sr B. Ca, Mg, Be D. Sr, Ra, Ba 34. Which Period 4 element has the most metallic properties? A. As C. Ge B. Br D. Sc 35. Which group on the Periodic Table of the Elements contains elements t hat react wit h oxygen to form compounds with the general formula X20? A. Group 1 C. Group 14 B. Group 2 D. Group 18 36. Element X reacts wit h iron to form two different compounds with the formulas FeX and Fe 2X3 . To which group on the Periodic Table does element X belong? 28. Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? A. Their metallic properties decrease and their atomic radii decrease. B. Their metallic properties decrease and their atomic radii increase. C. Their metallic properties increase and their atomic radii decrease. D. Their metallic properties increase and their atomic radii increase. 29. Atoms of which element have the gr eatest tendency to gain electrons? A. bromine C. fluorine B. chlorine D. iodine A. B. Group 8 Group 2 C. D. Group 13 Group 16 37. As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there i s a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the A. number of protons increases, and the number of shells of electrons remains the same B. number of protons increases, and the number of shells of electrons increases C. number of protons decreases, and the number of shells of electrons remains the same D. number of protons decreases, and the number of shells of electrons increases 30. The strength of an atom’s attraction for the electrons in a chemical bond is the atom’s A. electronegativity C. heat of reaction B. ionization energy D. heat of formation 38. As the atoms in Period 3 of the Periodic Table are considered from left to right, the atoms generall y show A. an increase in radius and an increase in ionization energy B. an increase in radius and a decrease i onization energy C. a decrease in radius and an increase i n ionization energy D. a decrease in radius and a decrease in i onization energy 31. As the elements of Group 1 on the Periodic Table are considered in order of increasing atomic radius, the ionization energy of each successive element genera lly A. decreases C. remains the same B. increases 39. Based on Reference Table S, atoms of which of these el ements have the strongest attraction for the electrons in a chemical bond? A. Al C. P B. Si D. S 32. How do the atomic radius and meta llic properties of sodium compare to the atomic radius and metallic properties of phosphorus? A. Sodium has a larger atomic radius and is more metallic. B. Sodium has a larger atomic radius and i s less metallic. C. Sodium has a smaller atomic radius and is more metallic. D. Sodium has a smaller atomic radius and is less metallic. 40. What is the correct Lewis electron-dot structure for the compound magnesium fluoride? 33. Which trends are observed when the elements in Peri od 3 on the Periodic Table are considered in order of increasing atomic number? A. The atomic radius decreases, and the first ionization energy generally increases. B. The atomic radius decreases, and the first ionization energy generally decreases. C. The atomic radius increases, a nd the first ionization energy generally increases. D. The atomic radius increases, a nd the first ionization energy generally decreases. Page 2 A. C. B. D. Periodic Table Worksheet Answer Key 1. A 31. A 2. D 32. A 3. B 33. A 4. A 34. D 5. C 35. A 6. B 36. D 7. A 37. A 8. D 38. C 9. C 39. D 40. C 10. A 11. A 12. D 13. C 14. B 15. C 16. D 17. D 18. B 19. C 20. D 21. D 22. D 23. D 24. A 25. A 26. A 27. A 28. D 29. C 30. A