Download Part B: Periodic Trends

Part B: Periodic Trends Review
Name: ______________________________
Directions: Given the following periodic table, compare the given elements and indicate by circling
which element is larger, stronger, bigger and or greater to each other.
M
Z
Y
N
P
Q
A
O
S
F
C
L
H
I
1. IONIZATION ENERGY
L vs. Y
2. IONIZATION ENERGY
P vs. H
3. IONIZATION ENERGY
O vs. I
4. IONIZATION ENERGY
Z vs. A
5. ATOMIC RADIUS
S vs. H
6. ATOMIC RADIUS
A vs. 0
7. ATOMIC RADIUS
Y vs. N
8. ELECTRONEGATIVITY
A vs. O
9. ELECTRONEGATIVITY
C vs. H
10. ELECTRONEGATIVITY
M vs. L
11. ELECTRONEGATIVITY
S vs. H
12. ATOMIC RADIUS of P vs. IONIC RADIUS of P
13. ATOMIC RADIUS of O vs. IONIC RADIUS of O
Using the chart above answer the following questions also.
14. What is the symbol of the element with the highest ionization energy? _______
15. What element has the lowest electronegativity? _______
16. Who was given credit for first developing the periodic table of the elements? ______________
17. The energy that is required to remove an electron from it neutral atom is known as _______
18. The amount of pull an atom has for bonded electrons is known as _____________________
19. What are the period and group trends for atomic radius?
Across a period? _____________________ Down a group?_____________________
20. What are period and group trends for ionization energy.
Across a period? _____________________ Down a group?_____________________
21. What are period and group trends for electronegativity.
Across a period? _____________________ Down a group?_____________________
Part B: Periodic Trends Review
Directions: Given the following periodic table, compare the given elements and indicate by circling
which element is smaller, weaker, littler and or less than the other.
X
E
V
P
R
S
T
N
B
W
Z
K
M
O
H
F
L
22. IONIZATION ENERGY
E vs. N
29. ELECTRONEGATIVITY
F vs. O
23. IONIZATION ENERGY
W vs. L
30. ELECTRONEGATIVITY
V vs. T
24. IONIZATION ENERGY
X vs. R
31. ELECTRONEGATIVITY
F vs. L
25. IONIZATION ENERGY
B vs. Z
32. ELECTRONEGATIVITY
X vs. R
26. ATOMIC RADIUS
V vs. F
33. ATOMIC RADIUS of S vs. IONIC RADIUS of S
27. ATOMIC RADIUS
B vs. W
34. ATOMIC RADIUS of L vs. IONIC RADIUS of L
28. ATOMIC RADIUS
E vs. T
Using the chart above answer the following questions also.
35. What is the symbol of the element with the largest atomic radius? ____________________
36. What element has the lowest ionization energy? _____________________
Which atom in each pair has the larger atomic
radius?
Which atom in each pair has the larger
ionization energy?
37. Li or K
45. Na or O
38. Ca or Ni
46. Be or Ba
39. Ga or B
47. Ar or F
40. O or C
48. Cu or Ra
41. Cl or Br
49. I or Ne
42. Be or Ba
50. K or V
43. Si or S
51. Ca or Fr
44. Fe or Au
52. W or Se
Part B: Periodic Trends Review
How many valence electrons do each of these
elements have?
53. O _____
54. Na _____
55. F _____
56. N _____
57. Ca _____
58. Ar _____
What is the charge that each of these atoms
will for when it obeys the octet rule?
59. O _____
60. Na _____
61. F _____
62. N _____
63. Ca _____
64. Ar _____
65. Elements of Group 1A are ______________
66. Elements of Group 2A are ______________
67. Elements of Group 3-12 are _____________
68. Group 17 elements are ______________
69. Group 18 elements are _______________
70. A negative ion is (larger / smaller) than its
parent atom.
71. A positive ion is (larger / smaller) than its
parent atom.
72. Where is the highest electronegativity
found? _________________________
73. Where is the lowest electronegativity
found? _________________________
74. The majority of elements in the periodic
table are (metals / nonmetals).
75. Elements in the periodic table are
arranged according to their ______________
76. An element with both metallic and
nonmetallic properties is a _______________
77. As you go from left to right across a period
atomic size (decreases / increases). Why?
_________________________
78. As you travel down a group, atomic size
(decreases / increases). Why?
_________________________
79. As you go from left to right across a
period, ionization energy generally
(decreases / increases). Why?
_________________________
80. As you go down a group, ionization energy
generally (decreases / increases). Why?
_________________________
81. As you go from left to right across the
periodic table, the elements go from
(metals/nonmetals) to (metals/nonmetals)
82. Elements within a group have a similar
number of _________________________
83. Elements across a series have the same
number of _________________________
84. Between Cl, I, and Br: Which element is
(a) the smallest atom? (b) the atom with
the highest ionization energy?
85. Between P, S, and Se: Which element is
(a) the largest atom? (b) the atom with the
highest ionization energy?
86. (a) Which of the following atoms is
smallest: V, Cr, or W? (b) Which has the
highest ionization energy?
87. (a) Which of the following atoms is
smallest: N, P, or As? (b) Which has the
smallest ionization energy?
88. Between Al, Si, and P: Which is (a) the
largest atom? (b) the atom with the
highest ionization energy?
89. Explain why noble gases are inert and do
not form ions.