5.3
7.In the alkaline-earth group, atoms with the smallest radii
a. are the most reactive.
b. have the largest volume.
c. are all gases.
d. have the highest ionization energies.
2. Which represents a neutral atom acquiring an electron in a process where energy is
released?
a.
b.
c.
d.
A+ + energy → A + e¯
A¯+ energy → A + e¯
A + e¯ → A¯ + energy
A + energy → A+ + e¯
6. In groups 13 through 18, valence electrons may be in sublevels
a.
b.
c.
d.
d and f.
p and d.
s and p.
s and d.
9.Which of the following has the largest radius?
a.
b.
c.
d.)
Rb+
BrSr2+
Se2-
3. Which is the best reason that the atomic radius generally increases with atomic number in
each group of elements?
a. The number of neutrons increases
b. A new octet forms.
c. The nuclear charge increases.
d. The number of occupied energy levels increases.
5. For groups 13 through 18, the number of valence electrons is equal to the group number
a.
b.
c.
d.
plus 1.
minus 10.
plus the period numbers
minus the period number.
4. As you move left to right in Period 4 from gallium through bromine, atomic radii
a.
b.
c.
d.
vary unpredictably
generally increase.
do not change.
generally decrease
1. One-half the distance between the nuclei of identical atoms that are bonded together is called
the
a.
b.
c.
d.
electron cloud
atomic diameter.
atomic radius.
atomic volume.
10. The following are data on elements X~Z. X~Z is one of S, Cl, and K, respectively.
Atomic Radius X>Y
Electronegativity Z>Y
What is true about comparing the atomic numbers of X~Z?
a.
b.
c.
d.
e.
Y>X>Z
X>Y>Z
Z>X>Y
Y>Z>X
X>Z>Y
8. The energy required to remove an electron from an atom is the atom's
a.
b.
c.
d.
ionization energy.
Electronegativity.
electron energy.
electron affinity.
6.1
6. Most chemical bonds are
b. purely covalent.
d. metallic.
a. purely ionic.
c. partly ionic and partly covalent.
4. When atoms share electrons, the electrical attraction of an atom for the shared electrons is
called the atom's
1/1
d. hybridization.
a. electron affinity.
b. electronegativity.
c. resonance.
7. The greater the electronegativity difference between two bonded atoms, the greater the
percentage of ____ in the bond.
a. ionic character
b. covalent character
d. electron sharing.
c. metallic character
2. A mutual electrical attraction between the nuclei and valence electrons of different atoms that
binds the atoms together is called a(n)
1/1
b. Lewis structure.
d. London force.
a. dipole
c. chemical bond.
8. In the three molecules, O₂, HCl, and MgS, what atom would have a partial negative charge?
1/1
c. chlorine
d. fluorine
b. hydrogen
a. oxygen
5. If the atoms that share electrons have an unequal attraction for the electrons, the bond is
called
*
1/1
b. polar
d. dipolar
c. ionic
a. nonpolar
10. What are shared in a covalent bond?
a. ions
b. Lewis structures
c. electrons
d. molecule
9. The pair of elements that forms a bond with the least ionic character is(Na:0.93, Mg:1.31,
K:0.82, Ca:1.00, Cl: 3.16)
1/1
a. Na and Cl.
b. K and Cl.
c. Ca and Cl.
d. Mg and Cl.
1. The electrons involved in the formation of a chemical bond are called
1/1
a. molecule
c. Lewis electrons.
b. s electrons.
d. valence electrons.
3. If two covalently bonded atoms are identical, the bond is
1/1
d. coordinate covalent.
c. dipole covalent.
a. nonpolar covalent.
b. polar covalent.
6.2
8. The following illustration shows a model of atom X. Which statement is not correct?
*
1/1
c. It can be combined with up to four atoms.
b. It is an element in the 2nd period.
d. It can triple bond with other X atoms.
a. It is a Group 16 element.
2. In the figure below, in which area is electrostatic force more dominant than repulsive force?
*
1/1
d. D
b. B
c. C
a. A
7. What is the correct Lewis structure for hydrogen chloride, HCl?
a. A
c. C
b. B
d. D
3. In a molecule of fluorine, the two shared electrons give each fluorine atom how many
electron(s) in the outer energy level?
*
1/1
a. 1
b. 2
d. 32
c. 8
4. To draw a Lewis structure, one must know the
*
1/1
c. bond length of each atom.
d. ionization energy of each atom.
b. atomic mass of each atom.
a. number of valence electrons in each atom.
10. Which is a correct Lewis structure for carbonic acid, H₂CO₃?
*
1/1
1. Which of the following is not an example of a molecular formula?
*
1/1
d. O₂
a. H₂O
c. NH₃
b. C
9. The figure below shows the Lewis structure of the X ion. The X ion has an electron
configuration of Ar. What is the atomic number of X?
*
1/1
b. 16
c. 18
a. 8
d. 20
6. The substance whose Lewis structure shows three covalent bonds is
*
1/1
c. PH₃.
a. H₂O.
b. CH₂Cl₂.
d. CCl₄.
5. Multiple covalent bonds may occur in atoms that contain carbon, nitrogen, or
*
1/1
a. chlorine.
c. oxygen.
d. helium.
b. hydrogen.
6.3&4
8. A chemical bond formed by the attraction between positive ions and surrounding mobile
electrons is a(n)
a. nonpolar covalent bond.
c. polar covalent bond.
b. ionic bond.
d. metallic bond.
9. If a material can be shaped or extended by physical pressure, such as hammering, which
property does the material have?
c. ductility
d. luster
b. malleability
a. conductivity
4. Compared with liquid ionic compounds, molecular compounds
b. are brittle.
a. have higher boiling points.
c. are harder.
d. have no electrical conductivity.
10. In which of the following states will electricity flow?
b. liquid molecules
a. solid ionic compounds
c. molecule solution
d. ionic compound solution
7. What is the name of SO₄²¯?
d. Nitrite
b. Sulfite
a. Sulfate
c. Nitrate
2. In an ionic compound, the orderly arrangement of ions in a crystal is the state of
d. zero potential energy.
a. maximum potential energy.
c. average potential energy.
b. minimum potential energy.
6. How many electrons must be shown in the Lewis structure of the hydroxide ion, OH¯?
d. 10
b. 8
c. 9
a. 1
1. In the NaCl crystal, each Na+ and Cl¯ion has how many oppositely charged ions clustered
around it?
b. 2
a. 1
d. 6
c. 4
5. How many extra electrons are in the Lewis structure of the phosphate ion, PO₄³¯?
d. 4
b. 2
c. 3
a. 0
3. The lattice energy is a measure of the
a. strength of an ionic bond.
b. strength of a metallic bond.
d. net charge on a crystal.
c. strength of a covalent bond.
CH6
e.
11. A formula that shows only the types and numbers of atoms combined in a single molecule is
called a(n)
a.
b.
c.
d.
Lewis structure
molecular formula.
ionic formula.
covalent formula.
18. In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)
a.
b.
c.
d.
electron cloud.
Dipole
electron sea.
Lewis structure.
5. The percentage ionic character and the type of bond in Br₂ (electronegativity for Br is 2.8) is
a.
b.
c.
d.
100%; pure ionic.
0%; nonpolar covalent.
100%; polar covalent
0%; pure ionic.
2. As atoms bond with each other, they
a.
b.
c.
d.
increase their potential energy, thus creating less-stable arrangements of matter.
decrease their potential energy, thus creating more-stable arrangements of matter.
increase their potential energy, thus creating more-stable arrangements of matter.
decrease their potential energy, thus creating less-stable arrangements of matter.
9. In drawing a Lewis structure, each nonmetal atom except hydrogen should be surrounded by
a. 2 electrons.
b. 8 electrons.
c. 10 electrons.
d. 4 electrons
15. The Lewis structure for the ammonium ion, NH4, has
a.
b.
c.
d.
metallic bond.
ionic bond.
nonpolar covalent bond.
polar covalent bond.
16. Compared with nonmetals, the number of valence electrons in metals is generally
a.
b.
c.
d.
about the same.
Smaller
Greater.
almost triple.
14. Compared with ionic compounds, molecular compounds
a.
b.
c.
d.
are brittle.
are harder.
have lower melting points.
have higher boiling points.
20. Which corresponds to the following A and B? The figure shows compounds AB and CD₃ as
a chemical bonding model. Choose only the right ones.
1. AB is an ionic compounds.
2. C₂ has a double bond.
3. A(s) has electrical conductivity.
a.
b.
c.
d.
e.
II, III
I
I, III
II
I, II, III
7. Bond length is the average distance between two bonded atoms
a.
b.
c.
d.
at which kinetic energy is at a maximum.
at which potential energy is at a minimum.
covalent bond
ionic bond
19. Metals are malleable because the metallic bonding
a.
b.
c.
d.
maximizes the repulsive forces within the metal.
allows one plane of ions to slide past another.
is easily broken.
holds the layers of ions in rigid positions
1. The electrostatic attraction between positively charged nuclei and negatively charged
electrons permits two atoms to be held together by a(n)
a.
b.
c.
d.
Ion.
chemical bond.
London force.
neutron.
6. Which of the following shows the types and numbers of atoms joined in a single molecule of a
molecular compound?
a.
b.
c.
d.
potential energy diagram
molecular formula
covalent bond
ionic bond
13. If the lattice energy of compound A is greater than that of compound B,
a.
b.
c.
d.
compound B is probably a gas.
the bonds in compound A are stronger than the bonds in compound B.
compound A has larger crystals than compound B.
compound A is not an ionic compound.
8. What group of elements satisfies the octet rule without forming compounds?
a.
b.
c.
d.
Halogen
noble gas
alkaline-earth metal
alkali metal
3. Nonpolar covalent bonds are not common because
a.
b.
c.
d.
polar covalent substances are rare in nature.
ions always form when atoms join.
one atom usually attracts electrons more strongly than the other.
the electrons usually remain equally distant from both atoms.
17. In metals, the valence electrons
a.
b.
c.
d.
form covalent bonds.
are attached to particular positive ions.
are shared by all of the atoms
are immobile.
12. The energy released when 1 mol of an ionic crystalline compound is formed from gaseous
ions is called the
a.
b.
c.
d.
bond energy.
potential energy.
energy of crystallization
lattice energy.
4. A bond that is less than 50% ionic is considered
a.
b.
c.
d.
Metallic.
nonpolar covalent.
Ionic.
polar covalent.
10. The chemical formula for an ionic compound represents the
a.
b.
c.
d.
ratio of the combined ions present in a sample.
total number of ions in the crystal lattice.
number of ions in each molecule.
number of atoms in each molecule.