What do resonance structures represent, such as the one shown? Please select allthe correct statements.Rapidly interconverting structures|A way of representing delocalized electrons in a structureA way to show how electrons shift back and forth between atoms in a molecule| To be considered correct, all resonance structures must be consideredsimultaneously (resonance hybrid)To be considered correct, the resonance structures should be consideredseparately; the resonance hybrid is a simplificationZI

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Answered: What do resonance structures represent,…

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 8STP

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Methanol, CH3OH, is a compound in which the formal charge on all the atoms is zero. Consider what results when a proton, H+, becomes bonded to methanol by way of one of the unshared electron pairs on the oxygen atom, i.e., This time we use the curved arrow to signify bond making. Now a pair of unshared electrons on oxygen is pushed toward the region between the oxygen atom and the hydrogen ion. It becomes an OH covalent bond. In the resulting structure the oxygen atom owns one electron from each of ____ shared pairs and two electrons from ____ unshared pair. The total number of electrons that belong to the oxygen atom is ____. Oxygen is a Group ____ element. Since the number of electrons that the oxygen atom owns in this structure is one fewer that it would have in the neutral, unbonded state, the charge on oxygen is ____. The correct Lewis structure for the conjugate acid of methanol is _________________________ Once again charge is conserved. Joining a neutral molecule and a cation must yield a cation. Again the formal charge distribution on the resulting ion is predictable from the arrow. Electrons are pushed away from the oxygen atom, leaving it with a positive charge. Electrons are pushed toward the hydrogen ion, neutralizing its erstwhile positive charg.
Use VSEPR to explain why the HBH bond angle of BH3 is 120°. (Hint: What is one-third of360°?)
For each of the following molecules, complete the Lewis structure and use the VSEPR model to determine the bond angles around each central atom. Note that the drawings are only skeleton structures and may depict the angles incorrectly.
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+
The C=O double bond is called a “carbonyl bond.” Acetone and othercarbonyl compounds are introduced in some texts along with this structure a. Is this an important resonance structure of acetone? Explain. b. Does this structure convey any useful information about acetone? If so, what?
You need to devise a 3-D model that demonstrates the bonding between atoms, as well as any lone pairs. Please note that your individual assignment may be for an ion (don't forget about charges) or a neutral atom. Your assigneed ion is : AlCl4-
Determin the total number of resonance structures for the following image below?
Your assigneed ion is : AlCl4- please give a brief description that includes: (a) total valence electron count, (b) the Lewis structure, (c) the arrangement (or shape) of the electron grouping (includes lone pairs), (d) ideal bond angle, (e) actual molecular geometry (may be the same or different than answer (c), (f) actual bond angles (may use > or< symbols where appropriate). Please note that for an ion don't forget about charges.
Our class has just touched on molecular shapes/geometries and the last HW question contains this Nitrogen atom with a + formal charge. How would the VSEPR Molecular Shape look like? Also, If the same number of bonds and charge were kept and the Nitrogen was swapped with a Carbon, would both shapes be the same? Thank you.
What is agostic interaction, draw a structure to explain the bonding in terms of number of electron and how strong the bond is as compare to C-H bond and H bond.
1. Conjugated radicals, ions, or molecules are more stable than non-conjugated ones, why? 2. Charge separation decreases stability, why? 3. Structures in which all of the atoms have a complete valence shell of electrons are especially stable and make large contributions to the hybrid, why?
In consideration of the overall resonance hybrid OCN(^-), which is the proposed resonance structure that's most important? In lewis Dot Form*

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