Chapter 09 – Chemical Bonding I: Basic Concepts
116.
The following Lewis structure for OF2 uses how many valence electrons?
Chapter 09 – Chemical Bonding I: Basic Concepts
117.
Carbonic acid, H2CO3, is a weak acid that contributes to the taste and produces the carbon dioxide bubbles in all carbonated
beverages. How many valence electrons are used to show the Lewis structure for H2CO3?
Chapter 09 – Chemical Bonding I: Basic Concepts
118.
Select True or False: The structure below depicts the correct Lewis structure for Dichloromethane, CH2Cl2 (an important
solvent in synthetic chemistry).
Chapter 09 – Chemical Bonding I: Basic Concepts
119.
The Lewis structure for the nitrate ion, NO3–, showing all non-zero formal charges is shown here. Select True or False: This
structure shows a violation of the octet rule.
Chapter 09 – Chemical Bonding I: Basic Concepts
120.
A Lewis structure for SO3 that obeys the octet rule, showing all non-zero formal charges, is shown here. How many
resonance structures for SO3 that obey the octet rule, are possible?
121.
Shown here is a Lewis structure for SO3 that expands the octet to minimize formal charges. Select True or False: The formal
charge on the sulfur atom is zero.
Chapter 09 – Chemical Bonding I: Basic Concepts
122.
Shown here is a Lewis structure for the chlorite ion, ClO2–, that obeys the octet rule, showing all non-zero formal charges.
How many resonance structures for ClO2– that obey the octet are possible?
Chapter 09 – Chemical Bonding I: Basic Concepts
123.
Select True or False: Shown here is the Lewis structure for the chlorite ion, ClO2–, that expands the octet to minimize formal
charge and if necessary places negative formal charges on the most electronegative atom(s).
Chapter 09 – Chemical Bonding I: Basic Concepts
124.
Shown here is a Lewis structure for the chlorate ion, ClO3–, that obeys the octet rule, showing all non-zero formal charges.
How many resonance structures for ClO3– are possible that obey the octet rule?
Chapter 09 – Chemical Bonding I: Basic Concepts
125.
Shown here is a Lewis structure for the chlorate ion, ClO3–, that expands the octet to minimize formal charge and if necessary
places negative formal charges on the most electronegative atom(s). What is the formal charge on Cl?
126. How many resonance phosphate Lewis structures can be drawn for the phosphate ion,
PO43–, that obey the octet rule?
Chapter 09 – Chemical Bonding I: Basic Concepts
127.
Examine this Lewis structure for the phosphate ion, PO43–. How many valence electrons are around the P atom in this
structure?
Chapter 09 – Chemical Bonding I: Basic Concepts
128.
A Lewis structure of boron trifluoride is shown here. How many valence electrons are shown directly around the B atom?
Chapter 09 – Chemical Bonding I: Basic Concepts
129.
Select True or False: The Lewis structure shown here is correct for ammonia (nitrogen trihydride).
Chapter 09 – Chemical Bonding I: Basic Concepts
130.
The following Lewis structure depicts the product when boron trifluoride combines with ammonia. How many total valence
electrons are shown in this structure?
Chapter 09 – Chemical Bonding I: Basic Concepts
131. Select True or False: The polarity of covalent bonds increases as the percent ionic
132. Select True or False: Of the following substances, KCl, KBr, and KF, KF will have the
Chapter 09 – Chemical Bonding I: Basic Concepts
134.
Select True or False: Of the species NO2, NO, and N2, only NO2 is an exception to the octet rule.
135. Select True or False: The Si — Cl bond has less ionic character than the C — Cl bond.
136. Select True or False: A molecule with two resonance structures is shifting quickly back
Chapter 09 – Chemical Bonding I: Basic Concepts
137. Select True or False: The properties and chemical reactivity of a molecule is best
explained by analyzing all possible resonance structures for that molecule.