UNIT 3 REVIEW SHEET
MODERN PERIODIC TABLE AND TRENDS
1. What was the basis for Mendeleev’s arrangement of elements in his early periodic table?
2. Know the modern basis for the arrangement of the periodic table.
3. What sublevel is being filled by elements in each transition series and in each inner transition series (lanthanides
and actinides)?
4. Give the outer level electron configuration for the following elements:
A. Ge (z = 32)
C. Te (z = 52)
B. Ra (z = 88)
D. Br (z = 35)
5. Classify the following elements as metals, nonmetals, or metalloids.
A. As (z = 33)
E. Sn (z = 50)
B. Xe (z = 54)
F. Li (z = 3)
C. F (z = 9)
G. Te (z = 52)
D. Pt (z = 78)
H. Np (z = 93)
6. State the octet rule. What group of elements has this electron arrangement?
7. Give the outer level electron configuration and “d” sublevel configuration for each of the following.
A. V (z = 23)
C. Zr (z = 40)
B. Os (z =76)
D. Pd (z = 46)
8. Give the outer level electron configuration and “f” sublevel configuration for each of the following.
A. Pm (z = 61)
C. U (z = 92)
B. Es (z = 99)
D. No (z = 102
9. State the general rule for number of outer level electrons for metals and nonmetals.
10. Know where each of the following groups are found on the periodic table and which elements belong to the
group.
A. Alkali metals
D. Noble gases
B. Alkaline earth metals
E. Lanthanides
C. Halogens
F. Actinides
11. Give the symbol of each of the elements for each of the following outer level electron configurations and “d” or
“f” sublevel configurations.
A. 2s2
C. 3s2 3p6
2
8
B. 5s 4d
D. 6s2 4f10
12. Give the following ending configurations for unknown elements A-D, answer each of the questions below.
A. 3s2 3p4
B. 5s1
C. 7s1 D. 3s2
(1) Which if any of these elements belong to the same period? Identify the period.
(2) Which, if any belong to the same group? Identify the group.
(3) Which, if any are nonmetals?
(4) Which if any are metals?
(5) Which if any are metalloids or semimetals?
(6) Which if any belong to the alkali family?
(7) Which if any belong to the alkaline family?
13. Know what is the most important factor in determining the properties of an element?
14. Know what happens to the size of atoms as you move across a period or down a group. Know which member of
the following pairs of particles is larger: Pd, Rb; Mg, Ba; Cs, Lu; Se, O
15. Which of the following atoms would we expect to have the largest radius? Li, B, O, or F
16. Know which are larger, metal atoms or their ions. Also, know which are largest, non metal atoms or their ions.
Which member of the following pairs of particles is larger? Br, Br-; Na, Na+; F, F-; Al, Al+3
17. Which of the following electron configurations would be the most stable chemically?
A. 1s2 2s2 2p6
C. 1s2 2s2
2
2
6
2
1
B. 1s 2s 2p 3s 3p
D. 1s2 2s2 2p5
18. Know the various properties of metal discussed in this chapter including malleability, ductility, luster and
electrical conductivity.
19. Know how electronegativity varies within a group and within a period on the periodic table (i.e., the trend).
20. Know what element on the periodic table has the highest electronegativity and ionization energy. Know which
has the lowest electronegativity and ionization energy.
IONIC, COVALENT, METALLIC BONDING AND LEWIS STRUCTURES
1. Know the various properties of metals discussed in this chapter including malleability, ductility, luster, and
electrical conductivity.
2. Know the differences between ionic, covalent, and metallic bonds.
a. What kinds of bonds are found between (1) metal cations and delocalized electrons, (2) between nonmetal
atoms, (3) metal and nonmetal ions
b. What phases conduct electricity in ionic and covalent compounds and in metals?
c. Which bond type is found in materials with extremely high boiling points?
d. What bond type forms molecules?
e. In which bond type is electrons shared and in which are electrons transferred.
3. How are ions arranged in a crystal lattice structure?
4. Where are the hardest metals found?
5. What type of bonds are found in the following compounds? NaCl, NaOH, BaSO4, LiCl, CaS, CH4, CO2, C6H12O6.
6. When given the electronegativities of several elements, be able to predict what kind of bond would form between
them. As an example look up the electronegativities of the following elements and determine the type of bond
that would form between them: C-N, K-F, H-O, Ca-F, Na-Cl, Ba-Br.
7. Give the Lewis Dot Structures for Cl2, SiO2, H2O, and NO3-1.
8. Give the correct formula for a compound composed of Ba+2 and OH-1.
9. In a properly written formula for a compound all the charges add up to what number?
10. Give the names of the following covalent compounds containing sulfur and oxygen
a. SO
c. S2O3
b. SO2
d. S2O5
11. Give the names of the compounds from the following formulas.
a. BaCl2
d. Ba(ClO3)2
b. Ba(ClO2)2
e. Ba(ClO4)2
c. Ba(ClO)2
12. Give the formulas for the following compounds.
a. Cobalt (III) Sulfate
d. Cobalt (II) Sulfite
b. Cobalt (II) Sulfate
e. Cobalt (III) Sulfide
c. Cobalt (III) Sulfite
f. Cobalt (II) Sulfide
13. Know the names of the five acids that were assigned and be able to recognize their formulas. SKIP
a. Acetic acid
b. Hydrochloric acid
c. Nitric acid
d. Sulfuric acid
e. Phosphoric acid
14. Be able to match the name to the formula for the hydrocarbons containing 1-10 carbon atoms. Be able also to
give the name of a hydrocarbon in a ring structure. As an example give the name of the following hydrocarbons.
a. C2H6
SKIP
b. C5H12
c. C6H14
d. C3H8
15. Give the charges on the unknown ions below indicated as “X”. Use the charge on the given ion to determine the
answer.
a. XCl
e. XPO4
b. X2(SO4)2
f. X(NO3)2
c. BaX
g. Cd2X
d. Al2X
h. X2S3
16. Sodium is atomic number 11 and chlorine is atomic number 17?
a. What are their electron configurations?
b. When they react what are their resulting electron configurations?
c. What is the advantage to each in the resulting electron configurations?
d. What type of bond is formed between these two elements?
e. What is the name of the resulting structure that forms? Describe its arrangement of particles.