Practice Periodic Table Review Name______
1. An electron will emit energy in quanta when its 8. The elements in Group 2 are classified as energy state changes from 4p to A) metals B) metalloids A) 5s B) 5p C) 3s D) 6p C) nonmetals D) noble gases 2. Which electron configuration represents an atom 9. Which element has chemical properties that are in the excited state? most similar to the chemical properties of sodium? A) 1s22s22p63s2 B) 1s22s22p63s1 A) beryllium B) calcium C) 1s22s22p6 D) 1s22s22p53s2 C) lithium D) magnesium 3. In the electron-dot symbol, the dots represent 10. Which statement explains why sulfur is classified electrons located in as a Group 16 element? A) A sulfur atom has 6 valence electrons. B) A sulfur atom has 16 neutrons. A) s sublevels, only C) Sulfur is a yellow solid at STP. B) p sublevels, only D) Sulfur reacts with most metals. C) s and p sublevels, only D) s, p, and d sublevels 11. As the elements in Group 15 are considered in order of increasing atomic number, which 4. What is the highest principal quantum number sequence in properties occurs? assigned to an electron in an atom of zinc in the ground state? A) nonmetal ® metalloid ® metal A) 1 B) 2 C) 5 D) 4 B) metalloid ® metal ® nonmetal C) metal ® metalloid ® nonmetal 5. Which orbital notation represents a noble gas in D) metal ® nonmetal ® metalloid the ground state? 12. At STP, which element is a good conductor of A) B) electricity? A) chlorine B) iodine C) C) silver D) sulfur
D) 13. Which element is a liquid at 305 K and 1.0 atmosphere?
6. Which orbital notation represents a boron atom in A) magnesium B) fluorine the ground state? C) gallium D) iodine A) 14. At STP, which element is solid, brittle, and a poor conductor of electricity? B) A) Al B) K C) Ne D) S 15. What are two properties of most nonmetals? C) A) high ionization energy and poor electrical conductivity D) B) high ionization energy and good electrical conductivity 7. The elements on the Periodic Table are arranged in C) low ionization energy and poor electrical order of increasing conductivity D) low ionization energy and good electrical A) atomic mass B) atomic number conductivity C) molar mass D) oxidation number 16. An atom of argon in the ground state tends not to 23. Compared to the radius of a chlorine atom, the bond with an atom of a different element because radius of a chloride ion is the argon atom has A) larger because chlorine loses an electron A) more protons than neutrons B) larger because chlorine gains an electron B) more neutrons than protons C) smaller because chlorine loses an electron C) a total of two valence electrons D) smaller because chlorine gains an electron D) a total of eight valence electrons 24. As the elements is Period 3 are considered in 17. Arsenic and silicon are similar in that they both order of increasing atomic number, there is a general decrease in A) have the same ionization energy B) have the same covalent radius A) atomic mass C) are transition metals B) atomic radius D) are metalloids C) electronegativity 18. At STP, which list of elements contains a solid, a D) first ionization energy liquid, and a gas? 25. Which of the following ions has the smallest radius? A) Hf, Hg, He B) Cr, Cl2, C – – + 2+ C) Ba, Br2, B D) Se, Sn, Sr A) F B) Cl C) K D) Ca 19. The carbon atoms in graphite and the carbon 26. Which element requires the least amount of atoms in diamond have different energy to remove the most loosely held electron from a gaseous atom in the ground state? A) atomic numbers B) atomic masses A) bromine B) calcium C) electronegativities C) sodium D) silver D) structural arrangements 27. Which term represents the attraction one atom 20. The valence electron of which atom in the ground has for the electrons in a bond with another state has the greatest amount of energy? atom? A) cesium B) lithium A) electronegativity C) rubidium D) sodium B) electrical conductivity C) first ionization energy 21. Which set of properties is most characteristic of D) mechanical energy transition elements? 28. Based on Reference Table S, atoms of which of A) colorless ions in solution, multiple positive these elements have the strongest attraction for oxidation states the electrons in a chemical bond? B) colorless ions in solution, multiple negative oxidation states A) Al B) Si C) P D) S C) colored ions in solution, multiple positive oxidation states D) colored ions in solution, multiple negative oxidation states 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) 2- 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 95.04 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. 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. Answer Key Periodic Table
1. C 31. 7.31 g/cm3 = 2. D 32. –Metal: Tin or Sn or 3. C Lead or Pb –Metalloid: Silicon or 4. D Si or Germanium or 5. A Ge 6. B –Nonmetal: Carbon or C 7. B 33. – The valence 8. A electron shell of a 9. C Group 2 atom is lost 10. A when it becomes an ion. – A Group 2 ion 11. A has two fewer 12. C electrons than the 13. C atom from which it was formed. 14. D 34. – As the atomic 15. A number of elements in 16. D Group 2 increases, the ionic radius increases. 17. D – The ionic radius 18. A increases. 19. D 35. – 117 pm 2 pm 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.