Consider the molecule with skeletal structure C(1)-C(2)-N. The carbon atoms and the nitrogen atom are also bonded to hydrogen atoms to complete the octet and yield the formula C₂HyN. Which of the below is the best description of the bonding in this molecule? O sigma bond: C(2) sp³ to N sp O pi bond: C(2) sp³ to N sp O sigma bond: C(2) sp² to N sp O sigma bond: C(2) sp³ to N sp

Consider the molecule with skeletal structure C(1)-C(2)-N. The carbon atoms and the nitrogen atom are also bonded to hydrogen atoms to complete the octet and yield the formula C₂HyN. Which of the below is the best description of the bonding in this molecule? O sigma bond: C(2) sp³ to N sp O pi bond: C(2) sp³ to N sp O sigma bond: C(2) sp² to N sp O sigma bond: C(2) sp³ to N sp

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 109E: Predict the molecular structure and bond angles for each molecule or ion in Exercises 87 and 93. a....

See similar textbooks

Similar questions

Best 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.
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.)
Consider the following molecules: SiH4, PH3, H2S. In each case, a central atom is surrounded by four electron pairs. In which of these molecules would you expect the bond angle to be less than 109.5? Explain your reasoning.
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.
Consider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, IF5, and SCl6. These 12 compounds arc all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structure. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule docs not.) See Exercises 115 and 116 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.
The molecule shown here. 2-furylmelhanethiol, is responsible for the aroma of coffee: (a) What are the formal charges on the S and O atoms? (b) Give approximate values of angles 1, 2, and 3. (c) Which are the shorter carbon-carbon bonds in the molecule? (d) Which bond in this molecule is the most polar? (e) Is the molecule polar or nonpolar? (f) The four C atoms of the ring are all in a plane. Is the O atom in that same plane (making the five-member ring planar), or is the O atom bent above or below the plane?
Indicate which of the following molecules are polar. Draw the molecular structure of each polar molecule, including the arrows that indicate the bond dipoles and the molecular dipole moment. (a) HCN (b) I2 (c) NO
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.
Predict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. ICl5 b. XeCl4 c. SeCl6
As a general rule, MX molecules (where M represents a central atom and X represents terminal atoms; n = 2 5) are polar if there is one or more lone pairs of electrons on M. NH3 (M = N, X = H, n = 3) is an example. There are two molecular structures with lone pairs that are exceptions to this rule. What are they?
Predict the molecular structure (including bond angles) for each of the following. (See Exercises 115 and 116.) a. XeCl2 b. ICl3 c. TeF4 d. PCl5
It is possible to write a simple Lewis structure for the SO42- ion, involving only single bonds, which follows the octet rule. However, Linus Pauling and others have suggested an alternative structure, involving double bonds, in which the sulfur atom is surrounded by six electron pairs. (a) Draw the two Lewis structures. (b) What geometries are predicted for the two structures? (c) What is the hybridization of sulfur in each case? (d) What are the formal charges of the atoms in the two structures?