University:
Missouri State University
Course:
CHM 160 | General Chemistry I
Academic year:

2020
Views:

369

Pages:

4
Author:

Nesbyenvkk

Name KEY Date Periodic Trends Worksheet ections: Use your notes to answer the following questions. 1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium. O, C, A, K 2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. Ne, Al, S 3. Why does fluorine have a higher ionization energy than iodine? Fluorine has a smaller atomic radius, so the pt can exert a greater pull on e (val. shell is close) 4. Why do elements in the same family generally have similar properties? They have the same valence shell e arrangement. 5. Indicate whether the following properties increase or decrease from left to right across the periodic table. a. atomic radius (excluding noble gases) decrease b. first ionization energy increase. c. electronegativity increase 6. What trend in atomic radius occurs down a group on the periodic table? What causes this trend? Atomic radius increases down a group because energy levels (shells) are added 7. What trend in ionization energy occurs across a period on the periodic table? What causes this trend? lonization energy increases across a period because as elements become less metallic, it requires remove ane. 8. Circle the atom in each pair that has the largest atomic radius. more energy to a. Alor B b. Na or Al c. Sor O d. Oor F e. Br or Cl f. Mg or (Ca Name Date 9. Circle the atom in each pair that has the greater ionization energy. a. Li or (Be) b. Ca or Ba c. (Na) or K d. Por Ar e. (C or Si f. Lior K 10. Define electronegativity. The ability of an atom to gain an e- 11. Circle the atom in each pair that has the greater electronegativity. a. Ca or Ga b. Br or As c. Li or O d. Ba or Sr e. C or S f. Oor S