Valence bond theory The skeletal structure for methyleneimine (CH2NH) is shown. Draw for yourself the best Lewis structure. Propose a bonding scheme by indicating the hybridization of the central atoms and the orbital overlaps for each bond. H. | H-cN H (a) (b) (c) | The bond labeled (a) forms from o + -overlap of a C sp2 orbital and a H 1s + orbital. The bond labeled (b) forms from: • one o-overlap of a C sp2 + orbital and a N sp2 + orbital, and one + T-overlap(s) of a C sp2 orbital and a N sp2 + orbital. The bond labeled (c) forms from o + - overlap of a N sp2 + orbital and a H 1s + orbital. There is/are + lone pair(s) around the one N atom. Lewis structures do not attempt to portray 3D shape, but you can predict the molecular geometry from VSEPR theory. The ideal bond angle <(H-C-H) around the C atom is 120 + degrees. The ideal bond angle <(C-N-H) around the N atom is 120 • degrees.

Valence bond theory The skeletal structure for methyleneimine (CH2NH) is shown. Draw for yourself the best Lewis structure. Propose a bonding scheme by indicating the hybridization of the central atoms and the orbital overlaps for each bond. H. | H-cN H (a) (b) (c) | The bond labeled (a) forms from o + -overlap of a C sp2 orbital and a H 1s + orbital. The bond labeled (b) forms from: • one o-overlap of a C sp2 + orbital and a N sp2 + orbital, and one + T-overlap(s) of a C sp2 orbital and a N sp2 + orbital. The bond labeled (c) forms from o + - overlap of a N sp2 + orbital and a H 1s + orbital. There is/are + lone pair(s) around the one N atom. Lewis structures do not attempt to portray 3D shape, but you can predict the molecular geometry from VSEPR theory. The ideal bond angle <(H-C-H) around the C atom is 120 + degrees. The ideal bond angle <(C-N-H) around the N atom is 120 • degrees.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter7: Molecular Structures

Section: Chapter Questions

Problem 26QRT

See similar textbooks

Similar questions

(a) Construct a Lewis structure for O2 in which each atomachieves an octet of electrons. (b) How many bondingelectrons are in the structure? (c) Would you expect theO¬O bond in O2 to be shorter or longer than the O¬Obond in compounds that contain an O¬O single bond?Explain.
The structure of caffeine is shown below. (a) Complete the Lewis structure. (b) How many pi bonds are present in caffeine? How many sigma bonds? (c) Identify the hybridization of the carbon atoms. (d) What is the value of the O-C-N angle?
indicate the approximate values for the indicated bond angles in the following molecules. 1 (a) H 0-N=ö 2. Н 4 H. (b) H C-c=0 H H H (c) H-N-O–H . H. (d) H-C-C=N: H.
The structural formulas for ethanol, CH3CH2OH, and propene, CH;CH=CH,2, are нн H Н—С—С—0—н H-C-C=C-H нн H H H Ethanol Propene (a) Complete the Lewis structure for each molecule showing all valence electrons. (b) Using the VSEPR model, predict all bond angles in each molecule.
(a) Methane (CH4) and the perchlorate ion (ClO4- ) are bothdescribed as tetrahedral. What does this indicate about theirbond angles? (b) The NH3 molecule is trigonal pyramidal, while BF3 is trigonal planar. Which of these molecules is flat?
Consider the reaction BF3 + NH3 -> F3B-NH3 (a) Describe the changes in hybridization of the B and N atoms as a result of this reaction. (b) Describe the shapes of all the reactant molecules with their bond angles. (c) Draw the overall shape of the product molecule and identify the bond angles around B and N atoms. (d) What is the name of the bond between B and N. (e)Describe the bonding orbitals that make the B and F, B and N & N and H bonds in the product molecule.
In the following compounds, the C atoms form a single ring.Draw a Lewis structure for each compound, identify cases for which resonance exists, and determine the carbon-carbon bondorder(s): (a) C₃H₄; (b) C₃H₆; (c) C₄H₆; (d) C₄H₄; (e) C₆H₆.
(a) What orbitals are overlapping to form each of the following bonds? b) Classify whether the bond formed is sigma or pi? (a) (b) H. : 3 1 2 H 4 5 6 7 10 H 8 9 10
Consider a molecule AB6, where element A has 6 valence electrons and B has 7 valence electrons. If the ΔEn for each bond = 1.2, predict the shape, bond hybridization and polarity (polar or non-polar) of the molecule. Your answer should follow the format: a) number of total electrons for bonding; b) Steric Number and Lone Pairs; c) name of shape based on the VSEPR chart, d) bond hybridization and e) molecular polarity.
Propylene, C3H6, is a gas that is used to form the importantpolymer called polypropylene. Its Lewis structure is given. (a) What is the total number of valence electrons in the propylenemolecule? (b) How many valence electrons are usedto make σ bonds in the molecule? (c) How many valenceelectrons are used to make π bonds in the molecule? (d) Howmany valence electrons remain in nonbonding pairs in themolecule? (e) What is the hybridization at each carbon atomin the molecule?
Bond energy : 4. (a) Draw the Lewis structure of NH,BCI, and name the bond between N and B. (b) State the type of orbital hybridization of N in NH3 and in NH3BCI3. NH3: NH;BCI3:
Identify the set that shows the correct trend in increasing polarity of covalent bonds: (A) B―F < C―F < C―Cl < N―Cl (B) C―F < C―Cl < N―Cl < B―F; (C) N―Cl < C―Cl < C―F < B―F; (D) C―Cl < N―Cl < B―F < C―F;