Test Review Guide: Use your notes and the worksheets provided to complete your own study
guide for the test next Tuesday.
Predict what type of bond will occur between the elements in problems 1 – 10. Please
answer Ionic, Covalent, Metallic, Hydrogen or Van der Waals. You may use rule of thumb,
but hydrogen and Van der Waals bonds are not included in “Rule of Thumb”.
For this review sheet, please include all bond options.
1. Ca + O __ionic_________(intramolecular)_______________________
2.
3.
4.
5.
6.
7.
8.
9.
10.
Sc + P ___ionic_______(intramolecular )_______________________________
N + O ___covalent (polar)__ _______(intramolecular )__________________
Cs + Br _____Ionic__________(intramolecular )_____________________
Xe + Xe _Van der Waals___________(intramolecular )__________________________
W + Ir __metallic_____________(intramolecular )____________________
I + I ___covalent (non-polar)_____ _______(intramolecular )______________________
H2O + H2O __(between different molecules)___Hydrogen (intermolecular)_______________
H + H ___covalent (non-polar)_____ _______(intramolecular )__________________
O + H ____covalent (polar)____ _______(intramolecular )_____________________
Please list the bond type given by the description:
11. Bonds that are described by a "sea of electrons." Metallic
12. Bonds that do not melt from the heat of a candle. (Strong bonds) Ionic
13. Formed when 2 atoms share electrons Covalent
14. Bonds that dissolve in water ionic
15. If a conductivity test is performed, the light bulb will…light. ionic
16. Bonds that are described using large numbers of cations and anions. Ionic
17. Bonds that melt from the heat of a candle. Covalent
18. Bonds that transfer electrons from one element to another. Ionic
19. Intermolecular – attraction between molecules Hydrogen bonds
20. Electronegativity difference is between basically 0 non-polar covalent
21. Electronegativity difference is between 0.3 – 1.7 polar covalent
22. Electronegativity difference >1.7 ionic
23. Bonds that involve the noble gases. Van der Waals
24. If a conductivity test is performed, the light bulb will not light. Covalent
25. Bonds that will form solids, liquids, and gases. covalent
26. What is the electronegativity range for non-polar covalent bonds? 0-<0.3
27. What is the electronegativity range for polar covalent bonds? 0.3-1.7
28. What is the electronegativity range for ionic bonds? 1.8-4.0
29. Bond type that involves the unequal sharing of the valence shell electrons between the elements.
Polar covalent
30. Bond type in which the valence shell electrons are shared equally between the elements. Nonpolar
covalent
31. Electronegativity difference is between 0.4 – 1.7 polar covalent
32. Usually found between diatomic molecules – two of the same atoms non-polar covalent
33. The compound will fall apart (dissociate) into its original ions when dissolved in water ionic
34. These bonds are important for Noble Gases Van der Waals
35. What is the electronegativity difference in the compound NaCl? 3.0-0.9=2.1
36. Based on the electronegativity difference in the compound NaCl, what type of bond is
occurring? ionic
37. What is the electronegativity difference in the compound AlF? 4.0-1.5=2.1
38. Based on the electronegativity difference in the compound AlF, what type of bond is occurring?
ionic
39. What is the electronegativity difference in the compound I2?
0
40. Based on the electronegativity difference in the compound I2, what type of bond is occurring?
Non-polar covalent
41. What is the electronegativity difference in the compound CaS?
2.5-1.0=1.5
42. Based on the electronegativity difference in the compound CaS, what type of bond is occurring?
ionic
43. What is the electronegativity difference in the compound CuCl?
3.0-1.9=1.1
44. Based on the electronegativity difference in the compound CoBr, what type of bond is
occurring? 2.8-1.9=0.9 polar covalent
45. Since water is polar, which bonds break apart in it?
a. Ionic
b. Polar Covalent
c. Nonpolar Covalent
d. Both a and b
e. Both b and c
46. If ethanol is nonpolar, which bonds will dissolve in it?
a. Ionic
b. Polar Covalent
c. Nonpolar Covalent
d. Both a and b
e. Both b and c
47. Which compounds will conduct electricity? Ionic and metallic
48. Why does atomic radius change as you go down a group? Energy levels are added to hold the extra
electrons
49. A measure of the ability of an atom in a chemical compound to attract electrons is called
Electron affinity
50. Most chemical bonds are intramolecular
51. In a compound, the sum of the cation and anion charges will be Zero
52. What is the charge on a cation? +
53. What is the charge on an anion? 54. Metals bound metals to form these bonds. metallic
55. Nonmetals bound to nonmetals form these bonds. covalent
56. Metals bound to nonmetals form these bonds. ionic
57. Draw the electron cloud that would surround the following compounds and tell what the
type of bond it is and what the electronegativity difference is. Describe how these
bonds differ and why or if they should be drawn differently.
Au
I
H
H
EN of Au __2.4_______
EN of I ___2.5_______
Difference ___0.1______
bond type _non-polar covalent_______
EN of H _2.1______
EN of H___2.1_____
Difference _0_____
bond type _non-polar covalent_____
Fr
Br
EN of Fr __0.7_____
EN of Br ____2.8_____
Difference __2.1_____
bond type __ionic______
Description of differences or similarities between and among the three bonds you drew
______Francium and Bromine do not share electrons. They transfer electrons. Au and I
share as do the hydrogens. Sharing equally means non-polar covalent bonds are formed.
Transfer means ionic bonds form. ___________________________________
Based on the following atom’s nuclear symbol:
113
56
Ba
58. How many electrons does Barium have? 56
59. What is the mass number of Barium? 113
60. How many neutrons does Barium have? 57
61. How many protons does Barium have? 56
62. Based on the average atomic mass of Ba, what is the difference between the above atom and
elemental Barium found on the periodic table? Why? Average atomic mass from the table is
137amu. This isotope has fewer neutrons and represents only one isotope where the periodic
table’s number represents all the isotopes.
63. Given the quantum numbers, 3 2 -2 -½ , draw the correct electron (arrow):

_ __ _ _ _ _
3d
64. Draw the electron configuration for Bromine. Br = 35e1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5
65. Draw the noble gas notation for Bromine. [Ar] = 18e[Ar] 4s2 3d10 4p5
66. What is the quantum number for the last electron in Bromine?
4 1 0 -1/2
Based on the following atom’s hyphen notation:
Sc-21
67. How many neutrons does Sc have? __21____
68. How many protons? __21____________
69. How many electrons? ______21___________
70. What would the mass number of Sc be? ______42_______
71.
Given the three isotopes of element X, find its average atomic
mass. 60% =X-12, 25%= X-13, and 15% = X-11. Show your work.
Using only the Rule of Thumb, what type of bond will occur between the following
elements.
72. Mg + S 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
73. Ca + S 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
74. C + C 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
75. Rb + N 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
76. Mn + Rn 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
77. Ac + Sg 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
78. F + F 
a. Metallic Bond
b. Ionic Bond
c. Covalent Bond
d. No Bond
Most missed questions from the last test:
1. Which of the following is the least shiny metal?
a. Na
b. Cs
c. Fr
d. S
2. Which element is made in the laboratory (not found in nature)?
a. He
b. N
c. Es
d. Li
3. Which factor best accounts for the trend of atomic radius as you go down a group?
a. Fewer protons in the nucleus.
b. Electrons are being placed in higher energy levels.
c. More protons in the nucleus.
d. Ionization energy increase.
4. The energy needed to remove an electron from an atom is called
a. electronegativity
b. ionization
c. electron affinity
Use the choices to the right to classify the elements in questions 5-13
5.
6.
7.
8.
9.
10.
11.
12.
13.
Na
Si
Br
Ag
Ca
S
Ga
H
Ne
___a____________
___h_____________
___c_____________
___e_____________
___b_____________
___h_____________
___g____________
___h_____________
___d_____________
a. Alkali metal
b. Alkaline earth metal
c. Halogen
d. Noble gas
e. Transitional metal
f. Inner Transition Metal
g. Post Transition metal
h. Other nonmetal
i. Metalloid
More important review:
1.
Fill in the table below:
Mass Number
Nuclear Symbol
Notation
# of
Protons
# of Neutrons
# of
electrons
61
47
45
35
5
8
5
53
74
108
108
47
Ag
47
80
80
35
Br
35
13
13
5
127
127
53
B
I
2. Write the full electron configuration for Nickel (#28).
1s2 2s2 2p6 3s2 3p6 4s2 3d8
3. Write the noble gas notation for Phosphorus (# 15) [Ne] = 10
[Ne] 3s2 3p3
4. Identify this piece of lab equipment:
__crucible tongs________
5. Identify this piece of lab equipment
___graduated cylinder_______
*know all of the glassware we studied
53