Ch. 5-3/6-1 Study Questions
1. Which of the following statements correctly compares the relative size of an ion to its neutral atom?
a. The radius of an anion is greater than the radius of its neutral atom.
b. The radius of an anion is identical to the radius of its neutral atom.
c. The radius of a cation is greater than the radius of its neutral atom.
d. The radius of a cation is identical to the radius of its neutral atom.
2. How does the energy required to remove an electron from an atom changer as you move left to right in Period 4
from potassium through iron?
a. It generally increases.
b. It generally decreases.
c. It does not change.
d. It varies unpredictably.
3. Two atoms will likely form a polar covalent bond if the electronegativity difference is
a. 0.1.
b. 1.0.
c. 2.5.
d. 4.0.
4. Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be
a. negatively charged compounds.
b. nonpolar-covalent compounds.
c. polar-covalent compounds.
d. ionic compounds.
5. Which is the correct Lewis structure for C2H4?
a.
b.
c.
d.
6. A single covalent bond involves the sharing of
a. only one electron.
b. two electrons.
c. three electrons.
d. a variable number of electrons, which depends on the bonding atoms.
7. Which of the following elements has an electron affinity of 0 kJ/m?
a. Br
b. As
c. Ar
d. I
8. Which is the correct Lewis structure for SiF4?
a.
b.
c.
d.
9. Atoms seldom exist as independent particles in nature because
a. as single particles, most atoms have low potential energy.
b. their electronegativity is much lower when they combine with other atoms.
c. atoms are more stable when they combine with other atoms.
d. neutral particles are rare.
10. Which of the following elements has the lowest electronegativity?
a. C
b. F
c. Li
d. O
11. To draw a Lewis structure, it is not necessary to know
a. which atoms are in the molecule.
c. the number of valence electrons for each atom.
b. bond energies.
d. the number of atoms in the molecule.
12. The principle that states that atoms tend to form compounds in which each atom has eight electrons in its
highest occupied energy level is called the
a. rule of eights.
b. configuration rule.
c. Avogadro principle.
d. octet rule.
13. When an atom completely gives up its valence electrons to another atom, what type of bond do they form?
a. purely ionic.
b. partially ionic.
c. polar-covalent.
d. nonpolar-covalent.
14. In which of these compounds is the bond between the atoms not a nonpolar covalent bond?
a. Cl2
b. H2
c. HCl
d. O2
15. A measure of the ability of an atom in a chemical compound to attract electrons from another atom in the
compound is called
a. electron affinity. b. electron configuration. c. electronegativity. d. ionization potential.
16. Use the table below to choose the pair of elements that will most likely have the greatest ionic character.
a. K and N b. K and S c. N and Br d. S and Br
17. Valence electrons are those s and p electrons
a. closest to the nucleus.
b. in the lowest energy level.
c. in the highest energy level.
d. combined with protons.
18. The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912
kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
a. sodium has four or five electrons.
b. the atomic radius has increased.
c. a d electron has been removed.
d. the noble gas configuration has been reached.
19. Use the table below to choose the pair of elements that will most likely have the least ionic character.
a. Na and Cl
b. O and Cl
c. H and O
d. Na and O
20. Of the elements below, __________ has the largest first ionization energy.
a. Li
b. Na
c. K
d. H
21. A positive ion is known as a(n)
a. ionic radius.
b. valence electron.
d. anion
c. cation.
22. The electrostatic attraction between positively charged nuclei and negatively charged electrons permits two
atoms to be held together by a(n)
a. chemical bond.
b. London force.
c. neutron.
d. ion.
23. For each successive electron removed from an atom, the ionization energy
a. increases.
b. decreases.
c. remains the same.
d. equals the nuclear charge.
24. A covalent bond is formed when two atoms
a. share an electron with each other.
b. share one or more pairs of electrons with each other.
c. gain electrons.
d. gain and lose electrons.
25. The percentage ionic character and the type of bond in Br2 (electronegativity for Br is 2.8) is
a. 0%; nonpolar covalent. b. 100%; polar covalent. c. 0%; pure ionic. d. 100%; pure ionic.
26. The charge on an ion is
a. always positive.
b. always negative.
c. either positive or negative.
d. zero.
27. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called
a. nonpolar.
b. polar.
c. ionic.
d. dipolar.
28. You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the
a. distance between the atoms’ nuclei.
b. difference in the atoms’ electronegativities.
c. atoms’ atomic radii.
d. number of atoms in the compound.
29. Which of the following elements has the smallest first ionization energy?
a. sodium
b. calcium
c. potassium
d. magnesium
30. As atoms bond with each other, they
a. increase their potential energy, thus creating less-stable arrangements of matter.
b. decrease their potential energy, thus creating less-stable arrangements of matter.
c. increase their potential energy, thus creating more-stable arrangements of matter.
d. decrease their potential energy, thus creating more-stable arrangements of matter.
31. A negative ion is known as a(n)
a. ionic radius.
b. valence electron.
c. cation.
d. anion.
32. The ionization energies required to remove successive electrons from one mole of calcium atoms are 590
kJ/mol, 1145 kJ/mol, 4912 kJ/mol, and 6474 kJ/mol. The most common ion of calcium is probably
a. Ca+.
b. Ca2+.
c. Ca3+.
d. Ca4+.
33. What is the element with the highest electronegativity value?
a. cesium b. helium c. calcium d. fluorine
34. What is the element with the lowest electronegativity value?
a. cesium b. helium c. calcium d. fluorine
35. In which of the following sets are the charges given correctly for all the ions?
a. Na , Mg , Al b. K , Sr , O
c. Rb , Ba , P
d. N , O , F
36. The electrons involved in the formation of a chemical bond are called
a. dipoles. b. s electrons. c. Lewis electrons. d. valence electrons.
37. Which ionization energy is generally the largest?
a. first ionization energy b. second ionization energy c. third ionization energy d. fourth ionization energy
38. Which of the following elements has the greatest ionization energy?
a. Ga b. K c. Bi d. As
39. Given the electronegativities below, which covalent single bond is most polar?
Element:
H C N O
Electronegativity: 2.1 2.5 3.0 3.5
a. C-H b. O-H c. O-C d. N-H
40. Which of the following elements has the greatest atomic radius?
a. Al b. S c. Si d. C
41. An ionic bond results from electrical attraction between
a. cations and anions. b. atoms. c. dipoles. d. orbital.
42. What can be removed from an atom if ionization energy is supplied?
a. a proton b. a neutron c. an electron d. an ion
43. What is the apparent charge on the chlorine atom in the molecule HCl?
a. +1 b. -1 c. 1 d. 2
44. What are shared in a covalent bond?
a. ions b. Lewis structures c. electrons d. dipoles
45. The measure of an atom’s ability to attract electrons is its
a. electronegativity b. polarization. c. ionization d. electron affinity
46. Ionic bonds form as a result of the electrostatic attraction between
a. dipoles. b. electrons. c. ions. d. nuclei.
47. Which of the following has the largest second ionization energy?
a. Si b. Al c. Na d. Mg
48. For multiple covalent bonds to form in molecules, the molecules must contain carbon, nitrogen, or
a. chlorine. b. hydrogen. c. oxygen. d. helium.
49. In general, as you go across a period in the periodic table from left to right:
(1) the atomic radius __________;
(2) the electron affinity becomes __________ negative; and
(3) the first ionization energy __________.
a. decreases, decreasingly, increases
b. decreases, increasingly, increases
c. decreases, increasingly, decreases
d. increases, increasingly, increases
50. One-half the distance between the nuclei of identical atoms that are bonded together is called the
a. atomic radius. b. atomic diameter. c. atomic volume. d. electron cloud.
Ch. 5-3/6-1 Answer Section
1. A
2. A
3. B
4. B
5. C
6. B
7. C
8. A
9. C
10. C
11. B
12. D
13. A
14. C
15. C
16. A
17. C
18. D
19. B
20. D
21. C
22. A
23. A
24. B
25. A
26. C
27. B
28. B
29. C
30. D
31. D
32. B
33. D
34. A
35. B
36. D
37. D
38. D
39. B
40. A
41. A
42. C
43. D
44. C
45. A
46. C
47. C
48. C
49. B
50. A