Use your knowledge of Lewis structure and valence bond theory to predict the characteristics of acetonitrile (NCCH:) and its isomer methyl isocyanide (CNCH:). a. Determine the best Lewis structure for acetonitrile. Include the formal charge on each carbon and nitrogen atom. b. Using valence bond theory, determine the hybridization on the nitrogen atom in acetonitrile and state the number of pi and sigma bonds in the nitrogen-carbon bond. C. Determine the best Lewis structure for methyl isocyanide. Include the formal charge on each carbon and nitrogen atom. d. Using valence bond theory, determine the hybridization on each carbon atom in methyl isocyanide and state the hybrid orbitals in which you would expect to find nonbonding electrons. e. Based on the Lewis structures which molecule would you expect to be more reactive: acetonitrile or methyl isocyanide? Briefly explain your answer.

Use your knowledge of Lewis structure and valence bond theory to predict the characteristics of acetonitrile (NCCH:) and its isomer methyl isocyanide (CNCH:). a. Determine the best Lewis structure for acetonitrile. Include the formal charge on each carbon and nitrogen atom. b. Using valence bond theory, determine the hybridization on the nitrogen atom in acetonitrile and state the number of pi and sigma bonds in the nitrogen-carbon bond. C. Determine the best Lewis structure for methyl isocyanide. Include the formal charge on each carbon and nitrogen atom. d. Using valence bond theory, determine the hybridization on each carbon atom in methyl isocyanide and state the hybrid orbitals in which you would expect to find nonbonding electrons. e. Based on the Lewis structures which molecule would you expect to be more reactive: acetonitrile or methyl isocyanide? Briefly explain your answer.

Organic Chemistry: A Guided Inquiry

2nd Edition

ISBN:9780618974122

Author:Andrei Straumanis

Publisher:Andrei Straumanis

Chapter3: Electron Orbitals

Section: Chapter Questions

Problem 8E

See similar textbooks

Similar questions

how is molecular orbital theory an improvement of valence bond theory? valence bond theory is too complicated because the orbital overlap is hard to draw. MO is easier MO theory allows us to directly solve schrodingers equation for a molecule valence bond theory is oversimplification because it uses atomic orbitals in a molecular context. mo corrects for this or MO theory is not an improvement becayse it requires too much math
how is molecular orbital (MO) theory an improvement of valence bond theory? A.) valence bond theory is an oversimplification because it uses atomic orbitals in a molecular context MO theory corrects for this B.) valence bond theory is too complicated because the orbital overlap is hard to draw, MO theory is easier. C.) MO theory is not an improvement because it requires too much math. OR D.) MO theory allows us to directly solve schrodingers equation for a molecule
(a) Dihydrogen cation H2+ is commonly found in interstellar space. It can be generated by ionization of dihydrogen molecule H2. What electromagnetic radiation can be used to generate the H2+ cation? (b) Construct an energy level diagram for the molecular orbitals of the H2+ cation. What is the bond order of the HH bond in the H2+ cation? (c) Suggest a spectroscopic method for differentiation of H2 gas and the H2+ cation. Explain your answers.
The molecule shown below is called furan. It is represented intypical shorthand way for organic molecules, with hydrogenatoms not shown, and each of the 4 vertices representing acarbon atom. (a) What is the molecular formula for furan? (b) How manyvalence electrons are there in the molecule? (c) What isthe hybridization at each of the carbon atoms? (d) Howmany electrons are in the π system of the molecule? (e) TheC¬C¬C bond angles in furan are much smaller than thosein benzene. The likely reason is which of the following: (i) Thehybridization of the carbon atoms in furan is different fromthat in benzene, (ii) Furan does not have another resonancestructure equivalent to the one above, or (iii) The atoms in afive-membered ring are forced to adopt smaller angles than ina six-membered ring.
Given the molecule CH2CHCN Please draw a Lewis structure for this compound with CORRECT GEOMETRY and label all sigma and pi bonds with the orbitals it is made from (what orbitals are overlapping to form the bond). You may draw the hybridized sigma orbitals as sticks and the unhybridized p-orbitals as lobes for clarity. For this question, you DO need to draw out the orbitals.
In the hydrocarbon: (a) What is the hybridization at each carbon atom in themolecule? (b) How many σ bonds are there in the molecule?(c) How many π bonds? (d) Identify all the 120° bond anglesin the molecule.
Consider the Lewis structure shown below. (a) Does the Lewis structure depict a neutral molecule or anion? If it is an ion, what is the charge on the ion? (b) What hybridizationis exhibited by each of the carbon atoms? (c) Arethere multiple equivalent resonance structures for the species?(d) How many electrons are in the π system of the species?
How many sp, sp2, and sp3 carbons are present in a Capsaicin? What is the hybridization around N atom? How many pi bonds are present over the whole molecule (Capsaicin)? sp: sp2: sp3: N: pi bonds: Note: The image below contains a Capsaicin Lewis Structure for the question above. Thank you.
(a) If you combine two atomic orbitals on two different atomsto make a new orbital, is this a hybrid orbital or a molecularorbital? (b) If you combine two atomic orbitals onone atom to make a new orbital, is this a hybrid orbital or amolecular orbital? (c) Does the Pauli exclusion principle apply to MOs? Explain.
CH3+ and CH3- are two highly reactive carbon species. a. What is the predicted hybridization and geometry around each carbon atom? b. Two electrostatic potential plots are drawn for these species. Which ion corresponds to which diagram and why?
An organic chemist synthesizes the molecule below:(a) Which of the orientations of hybrid orbitals shown below a represent in the molecule? (b) Are there any present that are not shown below? If so, what are they? (c) How many of each type of hybrid orbital are present?
15. How many hybrid orbitals do we use to describe each molecule? Enter in integer form! -BrCN