Recall that for a lone pair to be involved in resonance, it must be in a p orbital, which requires the atom it is on to be sp² or sp hybridized. This means that for a situation with resonance, the actual hybridization of the atom is determined from the resonance structure where that atom has the lowest steric number (so it can use the required number of p orbitals to form pi bonds as shown in some of its resonance structures). This could be the situation in your initial drawing, or in one of the resonance structures you draw from it. All of the oxygens in the following molecules are sp² hybridized except one. Which of the following structures has an sp³ hybridized oxygen atom? НО. (A) (B) (D)

Recall that for a lone pair to be involved in resonance, it must be in a p orbital, which requires the atom it is on to be sp² or sp hybridized. This means that for a situation with resonance, the actual hybridization of the atom is determined from the resonance structure where that atom has the lowest steric number (so it can use the required number of p orbitals to form pi bonds as shown in some of its resonance structures). This could be the situation in your initial drawing, or in one of the resonance structures you draw from it. All of the oxygens in the following molecules are sp² hybridized except one. Which of the following structures has an sp³ hybridized oxygen atom? НО. (A) (B) (D)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter10: Molecular Structure And Bonding Theories

Section: Chapter Questions

Problem 10.108QE: Aspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the...

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Aspirin, or acetylsalicylic acid, has the formula C9H8O4 and the skeleton structure (a) Complete the Lewis structure and give the number of bonds and bonds in aspirin. (b) What is the hybridization about the CO2H carbon atom (colored blue)? (c) What is the hybridization about the carbon atom in the benzene-like ring that is bonded to an oxygen atom (colored red)? Also, what is the hybridization of the oxygen atom bonded to this carbon atom?
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.
Draw an MO diagram to explain the existence of the trihydrogen cation (H3+). Hint: it forms a cyclic structure. Use individual 1s orbitals from H atoms to form your molecular orbitals (don’t worry about forming LGOs; determine the symmetries of the MOs using the projection operator method and sketch approximate wavefunctions for each). How many electrons are present in this molecule? What is the bond order? What type of bonding is this?
Consider the T-system of the radical (a molecule with one unpaired electron) shown below. Note: the dot in this drawing represents an unpaired electron What is the best description of the following n molecular orbital (hint: consider the resonance structures of the radical)? ㅇ Note: each dot in this drawing represents a carbon nucleus bonding and filled with two electrons bonding and empty non-bonding and contains one electron antibonding and empty antibonding and filled with two electrons
According to valence bond theory, what is the total number of sp2 hybridized orbitals on all the atoms in formaldehyde, CH2O? Sketch and explain why. According to valence bond theory, how many lone pairs of electrons reside in sp hybridized orbitals in formaldehyde? explain why?
Out of p-orbital and sp-hybrid orbital which has greater directional character and Why?
What is the hybridization of the highlighted atoms in the following structure? What are your estimates for the bond angles around these highlighted atoms? in what kind of orbital does the lone pair of electrons on the nitrogen reside?
Use the References to access important values if needed for this question. Answer the following questions about the hybrid orbitals on the chlorine atom in the ClO3+ and ClO2+ molecular ions. What are the expected geometries of these ions? ClO3+: Central atom = Cl Type of hybrid orbitals on the chlorine atom = Number of hybrid orbitals used in overlap with atomic orbitals = Number of hybrid orbitals accomodating unshared electrons = Hybrid orbital geometry = Molecular geometry = ClO2+: Central atom = Cl Type of hybrid orbitals on the chlorine atom = Number of hybrid orbitals used in overlap with atomic orbitals = Number of hybrid orbitals accomodating unshared electrons = Hybrid orbital geometry = Molecular geometry =
The hydrogen molecular ion, H2+, can be detected spectroscopically. Write the electron configuration of the ion in molecular orbital terms. What is the bond order of the ion? Is the hydrogen-hydrogen bond stronger or weaker in H2+ than in H2? Electron configuration = Bond order Hydrogen-hydrogen bond is in H2 than in H2+. Drag and drop your selection from the following list to complete the answer: 1 (T1,) 2 (T1,)" * (01,)? 1s
TOPIC: QUANTUM, ATOMIC AND MOLECULAR PHYSICIS In C-C bonds of organic molecules, there are orbitals of carbon atoms with different { that degenerate and combine with each other, forming so-called hybridized orbitals that give rise to o -type bonds. Consider hydrogen functions with n = 2, that is, 2s and 2p orbitals of carbon. In sp hybridization of carbon (as in graphite), these linear combinations ypi (i = 1, 2, 3) are the following: 1 1 1 1 2 =. 22s+ P2px + Pzpy 1 V3 ==42s + V3 1 1 Vzpy V6 Note that the Y2pz orbital does not participate in this hybridization. Show that the points of maximum probability density for this hybridization are contained in the XY plane and form the vertices of an equilateral triangle whose geometric center is at the origin.
How many hybrid orbitals are represented in the picture, hoe many s,p,d atomic orbitals corresponding to what hybridization, what electron pair, and what bond angle(s)?
Does it matter which of the two sp3 hybrid orbitals are used tohold the two nonbonding electron pairs?