N-C- H H H 141 HÖ: Based on formal charges, the Lewis Structure above is [Select] Draw a resonance structure for the structure above. The resonance structure you drew is the [Select] resonance structure and the structure shown above is the [Select] resonance structure. The C-N bond order is [Select] >

N-C- H H H 141 HÖ: Based on formal charges, the Lewis Structure above is [Select] Draw a resonance structure for the structure above. The resonance structure you drew is the [Select] resonance structure and the structure shown above is the [Select] resonance structure. The C-N bond order is [Select] >

Pushing Electrons

4th Edition

ISBN:9781133951889

Author:Weeks, Daniel P.

Publisher:Weeks, Daniel P.

Chapter1: Lewis Structures

Section: Chapter Questions

Problem 34EQ: Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4...

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Formamide, HC(O)NH2, is prepared at high pressures from carbon monoxide and ammonia, and serves as an industrial solvent (the parentheses around the O indicate that it is bonded only to the carbon atom and that the carbon atom is also bonded to the H and the N atoms). Two resonance forms (one with formal charges) can be written for formamide. Write both resonance structures, and predict the bond angles about the carbon and nitrogen atoms for each resonance form. Are they the same? Describe how the experimental determination of the HNH bond angle could be used to indicate which resonance form is more important.
(a) Draw a Lewis structure for the ozone molecule, O3. (The order of atom attachment is OOO, and they do not form a ring.) Chemists use ozone to cleave carbon-carbon double bonds (Section 6.5C). (b) Draw four contributing resonance structures; include formal charges. (c) How does the resonance model account for the fact that the length of each OO bond in ozone (128 pm) is shorter than the OO single bond in hydrogen peroxide (HOOH, 147 pm) but longer than the OO double bond in the oxygen molecule (123 pm)?
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
Aspartame is an artificial sweetener marketed under the name Nutra-Sweet. A partial Lewis structure for aspartame is shown below. Aspartame can be classified as an organic compound (a compound based on carbon atoms). The majority of Lewis structures for simple organic compounds have all atoms with a formal charge of zero. Therefore, add lone pairs and multiple bonds to the structure above to give each atom a formal charge of zero when drawing the Lewis structure. Also note that the six-sided ring is shorthand notation for a benzene ring (C6H5). Benzene is discussed in Section 4-7. Complete the Lewis structure for aspartame. How many C and N atoms exhibit sp1 hybridization? How many C and O atoms exhibit sp3 hybridization? How many and bonds are in aspartame?
Consider the pyrosulfate ion, S2O72-. It has no sulfurâ€“sulfur nor oxygenâ€“oxygen bonds. (a) Write a Lewis structure for the pyrosulfate ion using only single bonds. (b) What is the formal charge on the sulfur atoms for the Lewis structure you drew in part (a)? (c) Write another Lewis structure using six bonds and two Oâ€”S bonds. (d) What is the formal charge on each atom for the structure you drew in part (c)?
Predict die molecular structure and bond angles for each molecule or ion in Exercises 88 and 94. a. POCl3, SO42, XeO4, PO43, ClO4 b. NF3, SO32, PO33, ClO3 c.ClO2, SCl2, PCl2 d. Considering your answers to parts a, b, and c. what conclusions can you draw concerning the structures of species containing the same number of atoms and the same number of valence electrons? (O3), sulfur dioxide, and sulfur trioxide.
Carbon monoxide (CO) is an example of an overall neutral molecule (netcharge=0) that hasnon-zero formal charges. Draw a Lewis structure of carbon monoxide (CO).
Cyanamide (H2NCN), an important industrial chemical, is produced by the following steps: Calcium cyanamide (CaNCN) is used as a direct-application fertilizer, weed killer, and cotton defoliant. It is also used to make cyanamide, dicyandiamide, and melamine plastics: a. Write Lewis structures for NCN2, H2NCN, dicyandiarnide, and melamine, including resonance structures where appropriate. b. Give the hybridization of the C and N atoms in each species. c. How many bonds and how many bonds are in each species? d. Is the ring in melamine planar? e. There are three different CN bond distances in dicyandiamide, NCNC(NH2)2, and the molecule is nonlinear. Of all the resonance structures you drew for this molecule, predict which should be the most important.
Chloromethane has the Lewis structure _______________________________ The carbon atom is sharing 4 electron pairs. In each shared pair the carbon atom “owns” 1 electron. The number of electrons that “belong” to carbon is ___. Carbon, being a Group ___ element would have 4 , outer shell electrons in the unbonded, neutral state. Therefore, the carbon atom in chloromethane has a formal charge of zero.
Predict the molecular structure and bond angles for each molecule or ion in Exercises 87 and 93. a. CCl4 b. NCl3 c. SeCl2 d. ICl a. NO2, NO3, N2O4 (N2O4 exists as O2NNO2.) b. OCN, SCN, N3 (Carbon is the central atom in OCN and SCN.)
The possible resonance structures for the cyanate ion, OCN, are: N=c=ö :NEC-0: :N-CEO: Structure A Structure B Structure C Which structure is the most stable? [Select ] What are the formal charges on the oxygen (O), carbon (C), and nitrogen (N) atoms, respectively, in the resonance structure that contributes most to the stability of the cyanate ion, OCN ? O: [ Select ] C [ [ Select ] N [ Select ] >
Draw all the equivalent resonance structures for BrO 3¯ on a piece of paper and then fill in the blanks. Draw the structure in such a way that the formal charge on the central atom is zero. Molecular geometry: Number of equivalent resonance structures: Bond order of Br-O bond(s): (fractions rounded to 2 decimal places, e.g. 1/2 will be 0.50 , 4/3 will be 1.33 and 5/3 will be 1.67) Formal charge on terminal atoms participating in resonance