5. (2 points) Consider ethylene, and acetylene ethylene acetylene (a) Draw three-dimensional diagrams of each molecule. Label the hybridization of each carbon, and show all sigma and pi bonds. (b) Which of these molecules has the shortest bond length? Which has the longest? In each of these molecules, where is the largest electron density located in space?

5. (2 points) Consider ethylene, and acetylene ethylene acetylene (a) Draw three-dimensional diagrams of each molecule. Label the hybridization of each carbon, and show all sigma and pi bonds. (b) Which of these molecules has the shortest bond length? Which has the longest? In each of these molecules, where is the largest electron density located in space?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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ASK YOUR TEACHER Choose the selection which correctly identifies the sets of hybrid orbitals used by central atoms to form bonds in both of the molecules and/or ions whose formulas are given below:HCN and NO2- a) The central atom of HCN uses sp hybridization and the central atom of NO2- uses sp2 hybridization. b) The central atom of HCN uses sp hybridization and the central atom of NO2- uses sp hybridization. c) The central atom of HCN uses sp2 hybridization and the central atom of NO2- uses sp2 hybridization. d) The central atom of HCN uses sp3 hybridization and the central atom of NO2- uses sp hybridization. e) The central atom of HCN uses sp hybridization and the central atom of NO2- uses sp3 hybridization.
What is the hybridization of the N atom in this molecule? What are the hybridizations of the other 4 atoms indicated? ............................ H-G-C-ċ-ċ-ö-H H H :N-H 2 E→:ö: HHO: A H
For the indicated atoms, what is their hybridization? In what orbital do the lone pairs reside?
Draw the Lewis structure of CH₃CCH and then choose the appropriate set of hybridization states for the three central atoms. Your answer choice is independent of the orientation of your drawn structure.
7)How many molecules from the list below are polar ?
Consider a molecule AB3, where both element A and B have 7 valent electrons. Predict the shape and bond hybridization 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, c) bond hybridization.
6.For the molecules shown below: L=molecule on left, R=molecule on the right H. CH3 at C H' ******* C%3Cd H -CH3 N. PCL R. (a) Add the lone pair of electrons to all atoms in both structures that have lone pairs (b) What hybrid orbital is used by the C in the CN group of L? (c) How many o (d) What is the approximate bond angle shown as “c" in L? - (e) What is the approximate bond angle shown as "f' in R? --- (f) What hybrid orbital is used by the O in the OCH3 group in R and how many t - bonds are there in L? --- -- -
Consider the following Lewis structure. (Lone pairs are not drawn in.) What is the hybridization of each C, N, and O atom? They have been labelled with subscript numbers for convenience. H-C,-H H-0,-Ċ2=C3=N,-H I
1.5 Draw the molecular orbital electron configuration for (a)H2, (b) B
A, B, and C
2) a) Consider the following molecule . Given what you have learned about hybridization theory, draw an image or images explaining the bonding situation in this molecule. I want you to draw out all of the orbitals, hybrid orbitals and how they overlap to form the bonds in the molecule. Indicate the % s or p character in the given atomic and hybrid orbitals. Which C-C bond or bonds are the longest? In a paragraph or so explain the image or images you just drew. b) Lastly, consider the molecule below. Indicate the Molecular formula, the molar mass, label the hybridization of each atom except for hydrogen, indicate any chiral centers with a *, which bond or bonds are the shortest, identify by name of each functional group with an arrow pointing to the group.
a) Consider a molecule of acetone cyanohydrin, shown below. What is the hybridization and molecular geometry at CA, CB, and O? (b) For Carbon B (CB) and nitrogen (N), draw orbital energy diagrams showing the orbitals involved in bonding after hybridization. Be sure to fill the orbitals appropriately with valence electrons. c) In your diagrams in part (b), which orbitals are involved in sigma and pi bonding? Orbitals Involved in Sigma Bonding Orbitals Involved in Pi Bonding 2p sp sp2 sp3 2p sp sp2 sp3 (d) In a sample containing many molecules of acetone cyanohydrin (and no other substances), what type(s) of intermolecular forces could be present? Choose all that apply. Covalent Bonds Hydrogen Bonds Dipole-Dipole Forces London Dispersion Forces