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CHAPTER 5 REVIEW
The Periodic Law
SECTION 5-3
SHORT ANSWER
1.
Answer the following questions in the space provided.
When an electron is added to a neutral atom, energy is
(a) always absorbed
(b) always released
2.
.
(c) either absorbed or released
(d) burned away
The energy required to remove an electron from an atom is the atom’s
(a) electron affinity
(b) electron energy
.
(c) electronegativity
(d) ionization energy
3. Moving from left to right across a period on the periodic table,
a. electron affinity values tend to become
more positive).
b. ionization energy values tend to become
c. atomic radii tend to become
4.
(more negative or
(larger or smaller).
(larger or smaller).
a. Name the halogen with the least-negative electron affinity.
b. Name the alkali metal with the highest ionization energy.
c. Name the element in Period 3 with the smallest atomic radius.
d. Name the Group 14 element with the largest electronegativity.
5. Write the electron configuration of the following:
a. Na
b. Na
c. O
d. O2
e. Co2
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SECTION 5-3 continued
6. a. Compare the size of the radius of a positive ion to its neutral atom.
b. Compare the size of the radius of a negative ion to its neutral atom.
7. a. Give the approximate positions and blocks where metals and nonmetals reside in the periodic
table.
b. Of metals and nonmetals, which tend to form positive ions? Which tend to form negative ions?
8. Table 5-3 on page 145 of the text lists successive ionization energies for several elements.
a. Identify the electron that is removed in the first ionization energy of Mg.
b. Identify the electron that is removed in its second ionization energy.
c. Identify the electron that is removed in its third ionization energy.
d. Explain why the second ionization energy is higher than the first, the third is higher than the
second, and so on.
9. Explain the role of valence electrons in the formation of chemical compounds.
38
SECTION 5-3 REVIEW
MODERN CHEMISTRY
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Name
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CHAPTER 5 REVIEW
The Periodic Law
SECTION 5-3
SHORT ANSWER
1.
c
Answer the following questions in the space provided.
When an electron is added to a neutral atom, energy is
(a) always absorbed
(b) always released
2.
d
.
(c) either absorbed or released
(d) burned away
The energy required to remove an electron from an atom is the atom’s
(a) electron affinity
(b) electron energy
.
(c) electronegativity
(d) ionization energy
3. Moving from left to right across a period on the periodic table,
more negative
4.
a. electron affinity values tend to become
more positive).
larger
b. ionization energy values tend to become
smaller
c. atomic radii tend to become
(more negative or
(larger or smaller).
(larger or smaller).
At
a. Name the halogen with the least-negative electron affinity.
Li
b. Name the alkali metal with the highest ionization energy.
Ar
c. Name the element in Period 3 with the smallest atomic radius.
C
d. Name the Group 14 element with the largest electronegativity.
5. Write the electron configuration of the following:
a. Na
1s22s22p63s1
b. Na
1s22s22p6
c. O
1s22s22p4
d. O2
1s22s22p6
e. Co2
1s22s22p63s23p63d7
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SECTION 5-3 continued
6. a. Compare the size of the radius of a positive ion to its neutral atom.
In positive ions, the radius is smaller than its corresponding neutral atom.
b. Compare the size of the radius of a negative ion to its neutral atom.
In negative ions, the radius is larger than its corresponding neutral atom.
7. a. Give the approximate positions and blocks where metals and nonmetals reside in the periodic
table.
Metals are on the left-hand side of the periodic table, mostly in the s, d, and f
blocks. Nonmetals are on the right-hand side of the periodic table, all in the p block.
b. Of metals and nonmetals, which tend to form positive ions? Which tend to form negative ions?
Metals tend to form positive ions; nonmetals tend to form negative ions.
8. Table 5-3 on page 145 of the text lists successive ionization energies for several elements.
3s2
a. Identify the electron that is removed in the first ionization energy of Mg.
3s1
b. Identify the electron that is removed in its second ionization energy.
2p6
c. Identify the electron that is removed in its third ionization energy.
d. Explain why the second ionization energy is higher than the first, the third is higher than the
second, and so on.
As electrons are removed in successive ionizations, fewer electrons remain within
the atom to shield the attractive force of the nucleus. Each successive electron
removed from an ion experiences an increasingly strong, effective nuclear charge.
9. Explain the role of valence electrons in the formation of chemical compounds.
Valence electrons are the electrons most subject to the influence of nearby atoms
or ions. They are the electrons available to be lost, gained, or shared in the
formation of chemical compounds.
38
SECTION 5-3 REVIEW
MODERN CHEMISTRY
HRW material copyrighted under notice appearing earlier in this work.