Please correct answer and don't use hand rating Which of following does NOT suggest that another resonance structure exists?Select one:O a. a lone pair of electrons adjacent to a multiple bondO b. an incomplete octet on an atom adjacent to a multiple bondO c.a lone pair of electrons on an atom adjacent to an atom with an incomplete octetO d.a ring containing an atom with an incomplete octetO e.a ring of alternating single and double bonds

Option a: It can suggest that the another resonance structure exists because lone pair of electrons…

Answered: Which of following does NOT suggest…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 100AP

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Similar questions

In the Lewis structure for chloromethane, the chlorine atom is sharing _____ electron pair and “owns” _____ of those electrons. Also, the chlorine atom possesses two electrons from each of _____ unshared pairs. The total number of electrons that belong to chlorine is 7 . Chlorine is a Group ____ element. The formal charge on chlorine in chloromethane is ____.
Draw the Lewis structure of a neutral molecule that is a naturally occurring combination ofhydrogen atoms and one sulfur atom. What is the shape of this molecule?
a model of each of the following molecules: a. Based on your model, draw a bond-line representation with as many atoms as possible in the plane of the paper. Use wedge and dash bonds to represent any atoms that do not lie in the plane of the paper. b. Indicate each unique bond angle and the shape of each unique central atom.
What is the most polar bond in the molecule?
It is impossible to draw a legitimate Lewis structure of a neutral NH4 molecule. Hypothetically,how many valence electrons would such a neutral NH4 molecule have ifit could exist? a. The +1 cation, NH4+ , does exist. How many valence electrons does one NH4+ ion have? b. Draw the Lewis structure for NH4+
C4H10O is the formula of diethyl ether. The same group of atoms is attached on either side of the oxygen atom. Draw the Lewis diagram. Diethyl ether was among the first anesthetics used in surgery, but it has been largely replaced by safer anesthetics today.
Use Table 4.4 and classify the bonds in the following compounds as nonpolar covalent, polar covalent, or ionic: a. MgI2 each I is bonded to Mg b. NCl3 each Cl is bonded to N c. H2S each H is bonded to S d. RbF e. SrO
1.Which type of atom will form a bond? Group of answer choices a. An atom whos outer shell is empty b. An atom that has an outer shell. c. An atom that has electrons
If a molecule requires two or more resonance structures to draw it, which of the following statements is true? Select one: A. The molecule does not have a single structure but dynamically oscillates between the resonance structures drawn for it. B. The molecule has lower energy than the computed energy of any of the resonance structures that are drawn for it. O C. The molecule is less stable than any of the resonance structures drawn for it. D. The molecule's resonance structures coexist in an equilibrium with the lower energy form predominating.
Which of the following statements is true? A. An atom with high electronegativity is an electron donor because it has high ionization energy B. An atom with a high electronegativity is an electron donor because it has already has too many electrons C. An atom with a high electronegativity is an electron acceptor because it has a high affinity for electrons. D. An atom with high electronegativity can be a electron acceptor or donor because electron affinity can be (+) or (-)
Consider the compounds and ions with curved arrows drawn below. When the curved arrows give a second valid resonance structure, draw the resonance structure. When the curved arrows generate an invalid Lewis structure, explain why the structure is unacceptable.
The formal charge of an atom in a Lewis structure is defined as ________ Select one: a. the difference between the number of bonding electrons and nonbonding electrons assigned to an atom. b. the difference between the number of valence electrons in a free atom and the number of nonbonding electrons assigned to it. c. the difference between the number of valence electrons in a free atom and the number of electrons assigned to it in a Lewis structure. d. the difference between the number of valence electrons in a free atom and the number of bonding electrons assigned to it. e. the difference between the number of valence electrons in a free atom and the total number of valence electrons in the molecule.

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