Unit 3 Review
1. An atom of fluorine is smaller than an atom of oxygen. One possible explanation is that, compared with oxygen,
fluorine has_____.
2. The trend in atomic radii you move down a group of elements on the periodic table is partially due to ____.
3. The atomic radius of an element can be measured by ______.
4. Explain the atomic radii trend ____.
5. Given the same conditions, which of the Group 17 elements has the least tendency to gain electrons?
6. Which of the following elements have the largest atomic radius: sodium or potassium?
7. Which alkaline earth metal lowing atoms will lose an electron most readily?
8. The element in Period 3 that has the highest ionization energy is belongs to what group?
9. Which group of elements contains the element with the highest ionization energy?
10. Which element in Period 4 has the highest ionization energy?
11. Fluorine has a higher ionization energy than chlorine because ____.
12. Which element in Group 15 has the greatest tendency to gain electrons?
13. Which of the elements in Group 2 has the highest electronegativity?
14. As one proceeds from left to right across a given period on the Periodic Table the electronegativity of the
element generally _____.
15. Which of the elements in period 2 has the lowest electronegativity?
16. As one proceeds from fluorine to iodine in Group 17 the electronegativity____.
17. The elements characterized as metals are located in what portion of the periodic table.
18. Elements that have properties of both metals and non—metals are called ______.
19. The alkaline earth metal having the largest atomic radius is found in Period _______.
20. The elements known as the Alkali metals are found in Group _____.
21. Which element in Group 17 has the greatest nuclear charge?
22. Which element in Period 3 has both metallic and nonmetallic properties?
23. The elements in the present periodic table are arranged according to their ____.
24. What is the total number of electrons found in the valence shell of an alkaline earth metal in the ground state?
25. Which Period contains four elements which are gases at room temperature?
26. Which elements are a liquid at room temperature?
27. All elements whose atoms in the ground state have a total of 5 e- in their outer most p sublevel are called?
28. Beryllium is classified as a ____.
29. What is the total number of elements in Period 2 that are gases at room temperature and standard pressure?
30. Which group contains elements in the solid, liquid, and gas phases at room temperature?
31. An element with two valence electrons is in what Group?
32. What elements are members of the halogen family?
33. Which are the properties of most nonmetals?
34. What elements are alkaline earth metal?
35. The element found in Group 14 and also in Period 3 is ______.
36. Elements in the same group or family have similar chemical properties because ___.
37. What is the difference between electronegativity and ionization energy?
38. Where is the highest electronegativity found?
39. Where is the lowest electronegativity found?
40. Elements of group 1 are called ___.
41. Elements of Group 2 are called_____.
42. Elements found in Group 3-12 are called____.
43. Elements in Group 17 are called ____.
44. Elements in Group 18 are called ____.
45. Rank the following elements by increasing atomic radius: Carbon, Aluminum, Oxygen, Potassium.
46. Rank the following elements by increasing electronegativity: Carbon, Aluminum, Oxygen, Potassium.
47. Why do elements in the same family have similar properties?
48. Arrange the following elements in order of increasing ionization energy: Be, Mg, Sr
49. Arrange the following elements in order of increasing electronegativity: Na, Al, S
50. Explain why noble gases are inert (unreactive) and do not form ions.