Concept explainers
(a)
Interpretation: The Lewis structure and the molecular structure with polarity of molecule needs to be determined.
Concept Introduction:
Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.
The hybridization and molecular structure of molecule determine the molecular structure of molecule.
For a molecule to be polar, it should have polar bond with no symmetry in the molecule.
(a)
Answer to Problem 109E
Explanation of Solution
In
Hence the best Lewis structure for
It is a polar molecule as it has two O-F polar bonds with bent geometry.
In
Hence the best Lewis structure for
In
Hence the best Lewis structure for
In
Hence the best Lewis structure for
(c)
Interpretation: The Lewis structure and the molecular structure with polarity of molecule needs to be determined.
Concept Introduction:
Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.
The hybridization and molecular structure of molecule determine the molecular structure of molecule.
For a molecule to be polar, it should have polar bond with no symmetry in the molecule.
(c)
Answer to Problem 109E
Explanation of Solution
In
Hence the best Lewis structure for
In
Hence the best Lewis structure for
In
Hence the best Lewis structure for
(d)
Interpretation: The Lewis structure and the molecular structure with polarity of molecule needs to be determined.
Concept Introduction:
Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.
The hybridization and molecular structure of molecule determine the molecular structure of molecule.
For a molecule to be polar, it should have polar bond with no symmetry in the molecule.
(d)
Answer to Problem 109E
Explanation of Solution
According to the given molecular formula, the structure of
Hence the best Lewis structure for
According to the given molecular formula, the structure of
Hence the best Lewis structure for
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Chapter 13 Solutions
Chemical Principles
- Write Lewis structures and predict the molecular structures of the following. (See Exercises 115 and 116.) a. OCl2, KrF2, BeH2, SO2 b. SO3, NF3, IF3 c. CF4, SeF4, KrF4 d. IF5, AsF5 Which of these compounds are polar?arrow_forwardWrite Lewis structures and predict the molecular structures of the following. (See Exercises 25 and 26.) a. OCl2, KrF2, BeH2, SO2 b. SO3, NF3, TF3 c. CF4 SeF4, KrF4 d. IF5, AsF5 Which of these compounds are polar?arrow_forwardWhich of the molecules in Exercise 121 have net dipole moments (are polar)?arrow_forward
- There are several molecular structures based on the trigonal bipyramid geometry (see Table 8.9). Three such structures are Which of the compounds in Exercises 91 and 92 have these molecular structures? PF5, SF4, ClF3 and Br3 SF6, ClF5, and XeF4arrow_forwardAn important observation supporting the concept of resonance in the localized electron model was that there are only three different structures of dichlorobenzene (C6H4C10). How does this fact support the concept of resonance (see Exercise 89)?arrow_forwardWhich of the molecules in Exercises 21 and 22 have net dipole moments (are polar)?arrow_forward
- Among the following, which has the shortest bond and which has the longest: Li2, B2, C2, N2, O2?arrow_forwardThe most common exceptions to the octet rule are compounds or ions with central atoms having more than eight electrons around them. PF5, SF4, CIF3, and Br3 are examples of this type of exception. Draw the Lewis structure for these compounds or ions. Which elements, when they have to, can have more than eight electrons around them? How is this rationalized?arrow_forwardGive two requirements that should be satisfied for a molecule to be polar. Explain why CF4 and XeF4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has a net dipole moment). Is CO2 polar? What about COS? Explain.arrow_forward
- hy do atoms form bonds with one another? What can make a molecule favored compared with the lone atoms?arrow_forwardBest Lewis Formula and Molecular Geometry A student writes the Lewis electron-dot formula for the carbonate anion, CO32, as a Does this Lewis formula obey the octet rule? Explain. What are the formal charges on the atoms? Try describing the bonding for this formula in valence bond terms. Do you have any difficulty doing this? b Does this Lewis formula give a reasonable description of the electron structure, or is there a better one? If there is a better Lewis formula, write it down and explain why it is better. c The same student writes the following resonance description for CO2: Is there something wrong with this description? (What would you predict as the geometries of these formulas?) d Is one or the other formula a better description? Could a value for the dipole moment help you decide? e Can you write a Lewis formula that gives an even better description of CO2? Explain your answer.arrow_forwardExplain why CF4 and Xef4 are nonpolar compounds (have no net dipole moments) while SF4 is polar (has a net dipo le moment). Is CO2 polar? What about COS?arrow_forward
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