Illustrate, by drawing, how the orbitals in thefollowing carbon-to-carbon bonds look like ina three-dimensional space. Also include theunhybridized p orbitals, if any, in the drawing.Shade the hybrid orbitals and leave theunhybridized orbitals unshaded. Show onlythe large lobes of the hybrid orbitals.a. sp^2-sp^2b. sp^3-sp

Answered: Image /qna-images/answer/e97ea9ce-1e78-4773-9527-d26be6e73f9c.jpg

Answered: Illustrate, by drawing, how the…

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter4: Molecular Structure And Orbitals

Section: Chapter Questions

Problem 5RQ: What hybridization is required for central atoms that have a tetrahedral arrangement of electron...

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Similar questions

Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals: a. Which is the bonding molecular orbital and which is the antibonding molecular orbital? Explain how you can tell by looking at their shapes. b. Which of the two molecular orbitals is lower in energy? Why is this true?
Why are d orbitals sometimes used to form hybrid orbitals? Which period of elements does not used orbitals for hybridization? If necessary, which d orbitals (3d, 4d, 5d, or 6d) would sulfur use to form hybrid orbitals requiring d atomic orbitals? Answer the same question for arsenic and for iodine.
Consider acetyl salicylic acid, better known as aspirin. Its structure is (a) How many sigma and pi bonds are there in aspirin? (b) What are the approximate values of the angles marked (in blue) A, B, and C? (c) What is the hybridization of each atom marked (in red) 1, 2, and 3?
In the hybrid orbital model, compare and contrast bonds with bonds. What orbitals form the bonds and what orbitals form the bonds? Assume the z-axis is the internuclear axis.
Give the shape that describes each hybrid orbital set: (a) sp2 (b) sp3d (c) sp (d) sp3d2
What hybridization is required for central atoms that have a tetrahedral arrangement of electron pairs? A trigonal planar arrangement of electron pairs? A linear arrangement of e lectron pairs? How many unhybridized p atomic orbitals are present when a central atom exhibits tetrahedral geometry? Trigonal planar geometry? Linear geometry? What are the unhybridized p atomic orbitals used for? Describe the bonding in H2S, CH4, H2CO, and HCN, using the localized electron model.
Pelargondin is the molecule responsible for the red color of the geranium flower. It also contributes to the color of ripe strawberries and raspberries. The structure of pelargondin is: How many and bonds exist in pelargondin? What is the hybridization of the carbon atoms marked 14?
Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.39.
Numerous molecules are detected in deep space. Three of them are illustrated here. (a) Are these compounds isomers? (b) Indicate the hybridization of each C atom in each molecule. (c) What is the value of the HCH angle in each of the three molecules? (d) Which of these molecules is/are polar? (e) Which molecule should have the strongest carbon-carbon bond? The strongest carbon-oxygen bond?
Consider the following computer-generated model of caffeine: Complete a Lewis structure for caffeine in which all atoms have a formal charge of zero (as is typical with most organic compounds). How many C and N atoms are sp2 hybridized? How many C and N atoms are sp3 hybridized? sp hybridized? How many and bonds are there?
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.
Two isomers share the molecular formula C3H4. In Structure A two ofthe carbon atoms are sp hybridized and one carbon atom is sp3 hybridized. In Structure B, two of the carbon atoms are sp2 hybridized and one carbon atom is sphybridized. b)Draw “3D”-looking structures on paper, make a sketch of each of the isomers. (This should be a sketch of themolecules, not diagrams of overlapping orbitals!) Your drawing should show thecorrect molecular geometry around each carbon atom. [HINT: NEITHER of thesemolecules is planar!!! To draw them correctly, you will have to consider why!]

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