Name:_______________________________________
Date:_____________
Chapter 7
Guided Reader- Honors Chemistry
Directions: Please answer the questions to the guided reading activity as you read chapter 7 of your
textbook. A word of advice: write page numbers by your answers so you can reference them later.
1. Elements in the same group have the same number of valence electrons in their ______________.
2. Electron configurations can be used to explain differences and similarities in the _______________
of elements.
3. How many elements had been discovered by 1865?
4. Mendeleev and __________ noticed similar chemical and physical properties when elements were
arranged by increasing _________________.
5. What two elements did Mendeleev call eka-aluminum and eka-silicon, respectively?
6. Who developed the concept of atomic numbers?
7. The force of attraction between an electron and the nucleus depends on the _____________of the
______________________ acting on the electron and on the average _____________ between the
nucleus and the electron.
8. In a many electron atom, electrons are both __________ to the nucleus and repulsed by the
__________________.
9. The net electric field as if it results from a single positive charge located at the nucleus is called the
______________________________.
10. The effective nuclear charge acting on an electron in an atom is __________ than the _________
nuclear charge because the effective nuclear charge also accounts for the _____________ of the
electron by the other electrons in the atom. THIS IS A VERY IMPORTANT CONCEPT!!!
11. For what is Z the symbol?
12. Inner electron partially _________ the outer electrons from the attraction of the nucleus.
13. For what is S the symbol?
14. The value of S is usually close to___________________________________.
15. What is S for a sodium atom?
16. What is Z for a sodium atom?
17. What is Zeff for a sodium atom?
18. Effective nuclear charge___________ as we move across periods on the periodic table.
19. Effective nuclear charge increases slightly/greatly as we move down groups. CIRCLE 1
20. What is the bonding atomic radius?
21. Atomic radius tends to ___________ from top to bottom within a group due to the increase in the
_____________________________.
22. Atomic radius tends to ___________ from left to right within a period due to the increase in the
_____________________________.
23. Cations are __________ than their parent atoms.
24. Anions are __________ than their parent atoms.
25. For ions carrying the same charge, size __________ as we go down a group.
26. What is an isoelectronic series?
27. In an isoelectronic series, we can list the members in order of increasing atomic number, and
therefore the ionic radii will be in _______________ order.
28. What is ionization energy?
29. The energy needed to remove the third electron would be called the _______ ionization energy.
30. Ionization energies increase/decrease for a given element.
31. There is a sharp increase in ionization energy when the first ______________ electron is removed.
32. The first ionization energy generally __________ across a period.
33. The first ionization energy generally __________ down a group.
34. Smaller atoms typically have lower ionization energies. TRUE/FALSE
35. One irregularity to the pattern in #32 is that Be, Mg, and Ca are _________ in first ionization
energy than B, Al, and Ga, respectively.
36. Another irregularity to the pattern in #32 is that O, S, and Se are __________ in first ionization
energy than N, P, and As, respectively.
37. How is electron affinity different from ionization energy?
38. The more negative/positive the electron affinity, the greater the attraction of the atom for an
electron.
39. Why do group 5A elements have relatively low affinity?
40. What is metallic character?
41. List four characteristics of metals.
42. Metals tend to have ______ ionization energies and then to form __________ ions.
43. Give two examples of substances that can oxidize metals.
44. Metal oxides are acidic/basic. CIRCLE 1
45. A metal oxide and water react to form ______________.
46. Metal oxides and acids react to form _________________________.
47. List three characteristics of nonmetals.
48. Nonmetal oxides are acidic/basic. CIRCLE 1
49. Nonmetal oxides and water react to form _______.
50. Nonmetal oxides and bases react to form ________________________.
51. ______________ have intermediate properties between those of metals and nonmetals.
52. Melting point increases/decreases as we go down the group of alkali metals.
53. Alkali metals react with hydrogen to form _____________.
54. Alkali metals react with sulfur to form ______________.
55. What is a hydride ion?
56. When oxygen reacts with metals, __________ are usually formed.
57. Except for lithium, all alkali metals react with oxygen to form _____________________.
58. Name the three alkali metals that can form compounds containing superoxides.
59. Beryllium reacts with steam but not water. TRUE/FALSE.
60. Magnesium reacts with steam but not water. TRUE/FALSE.
61. Calcium in water reacts to form ______________________.
62. Magnesium in oxygen reacts to form ______________.
63. _______________ salts are used in fireworks to produce a red color.
64. What two alkaline earth metals are important in living organisms?
65. Hydrogen can have metallic properties under tremendous _____________.
66. Hydrogen reacts with metals to form ____________________.
67. Metallic character increases/decreases as we go down the group of chalcogens. CIRCLE 1
68. What are the two allotropes of oxygen?
69. What are the three ions of oxygen?
70. What is the most stable and common isotope of sulfur?
71. What does the word halogen mean?
72. What is the most reactive halogen?
73. What is the most industrially useful halogen?
74. The noble gases are monatomic. TRUE/FALSE
75. Noble gases used to be called _______________.
76. Bartlett synthesized compounds containing what two elements?