Chemistry
Periodic Table Review Ms. Pollock
2013 ­ 2014 1. On what basis did Mendeleev organize his periodic table? ​
atomic mass / mass number 2. What are the horizontal rows on the periodic table? ​
periods 3. What are the vertical columns on the periodic table? ​
families / groups 4. Name a halogen. ​
fluorine, chlorine, bromine, iodine 5. Name a noble gas. ​
helium, neon, argon, krypton, xenon, radon 6. Name the period (horizontal row) and the sub­level (s, p, d, f ) of the valence electrons for the following elements. Then indicate the number of valence electrons for that element. a. hydrogen ​
1s, 1 b. carbon ​
2p, 4 c. sulfur ​
3p, 6 d. barium ​
6s, 2 e. iodine ​
5p, 7 7. Which sublevel (s, p, d, or f) contains most of the nonmetals? ​
p 8. Why are there no transition elements in periods 1 and 2? ​
Transition metals form more than one oxidation state and have valence electrons in the d sublevel. 9. Why do many of the transition elements have similar chemistry? ​
They all have varying numbers of electrons. 10. Use the periodic table to determine the energy level and sub­level of the highest energy electrons in each of the following elements: a. N ​
2p b. Ca ​
4s c. Rb ​
5s d. P ​
3p e. In ​
5p 11. Decide whether each of the following statements is true or false. a. Li has valence electrons in the n = 1 energy level. ​
false b. Si has valence electrons in the n = 3 energy level. ​
true c. Ga has valence electrons in the n = 3 energy level. ​
false d. Xe has valence electrons in the n = 5 energy level. ​
true e. P has valence electrons in the n = 2 energy level. ​
false 12. Why is the table of elements called “the periodic table”? ​
Properties of the elements repeat periodically. 13. Name a nonmetal. ​
chlorine, fluorine, iodine, nitrogen, carbon, sulfur, oxygen 14. Name a metalloid. ​
boron, silicon, germanium, arsenic, antimony, tellurium 15. Why is the atomic size considered to have “no definite boundary”? ​
Electrons can move from one atom to another without crossing a set barrier. 16. How is atomic size measured? ​
from the center of one nucleus to the center of the next nucleus 17. Which of the following would be smaller: indium or gallium? ​
Indium 18. Which of the following would be smaller: potassium or cesium? ​
Potassium 19. Which of the following would be smaller: titanium or polonium? ​
Polonium 20. Explain why iodine is larger than bromine. ​
Iodine has more energy levels. 21. What are three factors that affect atomic size? ​
number of electron shells (energy levels), nuclear charge (more protons = greater electron attraction), nuclear shielding 22. Arrange the following in order of increasing atomic radius: Tl, B, Ga, Al, In. ​
B, Al, Ga, In, Tl 23. Arrange the following in order of increasing atomic radius: Ga, Sn, C. ​
Sn, Ga, C 24. Which of the following would be larger: Rb or Sn? ​
Rb 25. Which of the following would be larger: Ca or As? ​
Ca 26. Describe the trend for the atomic size of elements in a row in the periodic table. ​
Size decreases from left to right because of the increase in nuclear charge. 27. Arrange the following in order of decreasing atomic radius: Ba, Tl, Se, Bi, Cs. ​
Ca, Ba, Tl, Bi, Se 28. How is the size of a cation different from the size of the atom from which it was formed? Why? ​
A cation is smaller than the atom from which it was formed because it has emptied the outer shell. The valence shell is now closer to the nucleus. 29. How is the size of an anion different from the size of the atom from which it was formed? Why? ​
An anion is larger than the atom from which it formed because it has filled the outer shell. The valence shell is now farther from the nucleus. 2+​
­​
30. Mg​
has the same number of electrons as F​
(they are said to be isoelectric). Which ion ­​
is larger and why? ​
The F​
ion is larger. Mg has lost electrons, while F has gained them. 31. Which of the following has the smallest ionic radius? 2­ a. O​
2­ b. S​
2+ c. Mg​
2+
d. Ca​
32. Which of the following has the largest ionic radius? 2+ a. Ba​
+ b. Cs​
­ c. I​
2­ d. Te​
33. Define ionization energy. ​
the energy required to remove an electron from the outer energy level 34. Which of the following would have the largest ionization energy? a. Na b. Al c. H d. He 35. Which of the following would have the smallest ionization energy? a. K b. P c. S d. Ca 36. Place the following elements in order of increasing ionization energy: Na, O, Mg, Ne, K. Ne, O, Mg, Na, K 37. Place the following elements in order of decreasing ionization energy: N, Si, P, Mg, He. He, N, P, Si, Mg 38. Using experimental data, the first ionization energy for an element was found be 600 kJ/mol. The second ionization energy was found to be 1800 kJ/mol. The third, fourth, and fifth ionization energies were found to be, respectively, 2700 kJ/mol, 11;600 kJ/mol, and 15;000 kJ/mol. To which family of elements does this element belong? Explain. ​
Group 13, large jump in ioziation energy after third electron removed 39. Using electron configurations and your understanding of ionization energy, which would you predict to have a higher second ionization energy: Na or Mg? ​
Na 40. Comparing the first ionization energies of Ca and Mg. ​
Ca higher 41. Comparing the first ionization energies of Be and B. ​
B higher 42. Define electronegativity. ​
strength with which an element hold to its electrons 43. Choose the element in each pair that has the lower electronegativity. a. ​
Li​
or N b. Cl or ​
Na c. Ca or ​
K d. ​
Mg​
or F 44. Which of the following will have the largest electronegativity? a. Se b. F c. Ne d. Br 45. Which of the following will have the smallest electronegativity? a. Na b. Ne c. Al d. Rb 46. Describe the general trend for electronegativity in period 2.Define electron affinity. increasing left to right 47. Choose the element in each pair that has the lower electron affinity. a. ​
Li​
or N b. Cl or ​
Na c. Ca or ​
K d. ​
Mg​
or F 48. Why is the electron affinity for calcium higher than that of potassium? ​
Calcium has two valence electrons, so it has a stronger attraction to the nucleus and more electrons to move to achieve stability. 49. Which of the following will have the largest electron affinity? a. Se b. F c. Ne d. Br 50. Which of the following will have the smallest electron affinity? a. Na b. Ne c. Al d. Rb 51. Place the following elements in order of increasing electron affinity: Tl, Br, S, K, Al. ​
Tl, K, Al, S, Br 52. Describe the general trend for electron affinities in period 2. ​
increasing left to right 53. Why does sulfur have a greater electron affinity than phosphorus does? ​
Sulfur has a greater number of valence electrons and a stronger attraction to the nucleus.