Practice Periodic Table Review

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1 Practice Periodic Table Review Name 1. An electron will emit energy in quanta when its energy state changes from 4p to A) 5s B) 5p C) 3s D) 6p 2. Which electron configuration represents an atom in the excited state? A) 1s 2 2s 2 2p 6 3s 2 B) 1s 2 2s 2 2p 6 3s 1 C) 1s 2 2s 2 2p 6 D) 1s 2 2s 2 2p 5 3s 2 3. In the electron-dot symbol, the dots represent electrons located in A) s sublevels, only B) p sublevels, only C) s and p sublevels, only D) s, p, and d sublevels 4. What is the highest principal quantum number assigned to an electron in an atom of zinc in the ground state? A) 1 B) 2 C) 5 D) 4 5. Which orbital notation represents a noble gas in the ground state? A) B) C) D) 6. Which orbital notation represents a boron atom in the ground state? A) B) C) D) 7. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 8. The elements in Group 2 are classified as A) metals B) metalloids C) nonmetals D) noble gases 9. Which element has chemical properties that are most similar to the chemical properties of sodium? A) beryllium B) calcium C) lithium D) magnesium 10. 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. 11. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? A) nonmetal metalloid metal B) metalloid metal nonmetal C) metal metalloid nonmetal D) metal nonmetal metalloid 12. At STP, which element is a good conductor of electricity? A) chlorine B) iodine C) silver D) sulfur 13. Which element is a liquid at 305 K and 1.0 atmosphere? A) magnesium B) fluorine C) gallium D) iodine 14. At STP, which element is solid, brittle, and a poor conductor of electricity? A) Al B) K C) Ne D) S 15. 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

2 16. 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 17. Arsenic and silicon are similar in that they both A) have the same ionization energy B) have the same covalent radius C) are transition metals D) are metalloids 18. At STP, which list of elements contains a solid, a liquid, and a gas? A) Hf, Hg, He B) Cr, Cl2, C C) Ba, Br2, B D) Se, Sn, Sr 19. The carbon atoms in graphite and the carbon atoms in diamond have different A) atomic numbers B) atomic masses C) electronegativities D) structural arrangements 20. The valence electron of which atom in the ground state has the greatest amount of energy? A) cesium B) lithium C) rubidium D) sodium 21. Which set of properties is most characteristic of transition elements? A) colorless ions in solution, multiple positive B) colorless ions in solution, multiple negative C) colored ions in solution, multiple positive D) colored ions in solution, multiple negative 22. What is the net charge of an ion that has 8 protons, 9 neutrons, and 10 electrons? A) 1+ B) 2+ C) 1- D) Compared to the radius of a chlorine atom, the radius of a chloride ion is A) larger because chlorine loses an electron B) larger because chlorine gains an electron C) smaller because chlorine loses an electron D) smaller because chlorine gains an electron 24. As the elements is Period 3 are considered in order of increasing atomic number, there is a general decrease in A) atomic mass B) atomic radius C) electronegativity D) first ionization energy 25. Which of the following ions has the smallest radius? A) F B) Cl C) K + D) Ca 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 27. Which term represents the attraction one atom has for the electrons in a bond with another atom? A) electronegativity B) electrical C) first ionization energy D) mechanical energy 28. Based on Reference Table S, atoms of which of these elements have the strongest attraction for the electrons in a chemical bond? A) Al B) Si C) P D) S

3 29. The graph below represents the relationship between atomic radii, in picometers, and increasing atomic number for elements in Group 15. Which element is most metallic A) A B) B C) D D) E 30. Base your answer to the following question on the information below and on your knowledge of chemistry. There are six elements in Group 14 on the Periodic Table. One of these elements has the symbol Uuq, which is a temporary, systematic symbol. This element is now known as flerovium. Explain, in terms of electron shells, why each successive element in Group 14 has a larger atomic radius, as the elements are considered in order of increasing atomic number. Base your answers to questions 31 and 32 on the information below. 31. Calculate the volume of a tin block that has a mass of grams at STP. Your response must include both a numerical setup and the calculated result 32. Identify one element from this table for each type of element: metal, metalloid, and nonmetal.

4 Base your answers to questions 33 through 35 on the information below. The ionic radii of some Group 2 elements are given in the table below. 33. Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomic radius. 34. State the trend in ionic radius as the elements in Group 2 are considered in order of increasing atomic number. 35. Estimate the ionic radius of strontium.

5 Answer Key Periodic Table 1. C 2. D 3. C 4. D 5. A 6. B 7. B 8. A 9. C 10. A 11. A 12. C 13. C 14. D 15. A 16. D 17. D 18. A 19. D 20. A 21. C 22. D 23. B 24. B 25. A 26. C 27. A 28. D 29. D 30. The atomic radius of these elements increases down the group because each successive element has one more electron shell. The number of shells per atom increases g/cm 3 = 32. Metal: Tin or Sn or Lead or Pb Metalloid: Silicon or Si or Germanium or Ge Nonmetal: Carbon or C 33. The valence electron shell of a Group 2 atom is lost when it becomes an ion. A Group 2 ion has two fewer electrons than the atom from which it was formed. 34. As the atomic number of elements in Group 2 increases, the ionic radius increases. The ionic radius increases pm 2 pm

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