Question 3 Hybrid orbitals are formed by combining the valence orbitals on an atom.A molecule has sp³ d hybridization with 1 lone pair.The electron pair geometry of this molecule is:The geometry of this molecule is:This molecule will have approximate bond angles of (Choose all that apply.):090°0000109.5°120°180°

A molecule with sp³d hybridization typically has a trigonal bipyramidal electron pair geometry. This…

Answered: Hybrid orbitals are formed by combining…

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 35QRT: The hybridization of the two carbon atoms differs in an acetic acid, CH3COOH, molecule. (a)...

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Methylcyanoacrylate is the active ingredient in super glues. Its Lewis structure is (a) How many sigma bonds are in the molecule? (b) How many pi bonds are in the molecule? (c) What is the hybridization of the carbon atom bonded to nitrogen? (d) What is the hybridization of the carbon atom bonded to oxygen? (e) What is the hybridization of the double-bonded oxygen?
7.96 Consider the hydrocarbons whose structures are shown below. Which of these molecules would be planar, meaning that all of the atoms must lie in the same plane? Explain your answer in terms of orbital hybridizations.
The hybridization of the two carbon atoms differs in an acetic acid, CH3COOH, molecule. (a) Designate the correct hybridization for each carbon atom in this molecule. (b) What is the approximate bond angle around each carbon?
7.59 What type of hybrid orbital is generated by combining the valence s orbital and all three valence p orbitals of an atom? How many hybrid orbitals result?
• explain how hybridization reconciles observed molecular shapes with the orbital overlap model.
In propene CH3CH=CH2, the first carbon has sp3 hybrid orbitals and the second carbon has sp2 hybrid orbitals. These orbitals interact to make a bond. Why are these hybrid orbitals not orthogonal?
Lets look more closely at the process of hybridization. (a) What is the relationship between the number of hybrid orbitals produced and the number of atomic orbitals used to create them? (b) Do hybrid atomic orbitals form between different p orbitals without involving 5 orbitals? (c) What is the relationship between the energy of hybrid atomic orbitals and the atomic orbitals from which they are formed?
Aspartame is a compound that is 200 times sweeter than sugar and is used extensively (under the trade name NutraSweet) in diet soft drinks. The skeleton structure of the atoms in aspartame is (a) Complete the Lewis structure and give the number of and bonds in aspartame. (b) What is the hybridization about each carbon atom that forms a double bond with an oxygen atom? (c) What is the hybridization about each nitrogen atom?
What hybrid orbitals would be expected for the central atom in each of the following molecules or ions?

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