Examine the sigma bonding in ethene. What types of orbitals does each C atom use when forming sigma bonds to the H atoms? s orbial p orbitals O hybrid orbitals Submit What type of orbital does each C atom use to form a sigma bond to the other C atom? s orbial p orbitals hybrid orbitals Submit Now examine the pi bonding in ethene. What types of orbitals on the C atoms are used to form the pi bond? s orbital p orbitals hybrid orbitals

Examine the sigma bonding in ethene. What types of orbitals does each C atom use when forming sigma bonds to the H atoms? s orbial p orbitals O hybrid orbitals Submit What type of orbital does each C atom use to form a sigma bond to the other C atom? s orbial p orbitals hybrid orbitals Submit Now examine the pi bonding in ethene. What types of orbitals on the C atoms are used to form the pi bond? s orbital p orbitals hybrid orbitals

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter23: Carbon: Not Just Another Element

Section: Chapter Questions

Problem 116SCQ

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The bond lengths of ethane, ethene, and ethyne were determined, and a graph of the C-H bond length vs. % s-character of the C hybrid orbital was made. Comment on the observed trend, additionally. How would this trend change if C-H bond energy vs. % s-character of the C hybrid orbital was graphed? Which hydrocarbon has the strongest carbon-carbon bond?
Why is the C-C bond length of an alkyne shorter than the C-C bond length of an alkene? O The orbitals are physically smaller due to mores character. O Pi bonds are weaker so more pi bonds creates a shorter bond. O There's a triple bond instead of a double bond.
what is the molecular geometry of cyclopropane and the hybridization ?
(a) How does the structure of diborane (B2H6) differ fromthat of ethane (C2H6)? (b) Explain why diborane adoptsthe geometry that it does. (c) What is the significance ofthe statement that the hydrogen atoms in diborane aredescribed as “hydridic”?
4. Octatetraene, C8H10, is an 8-membered linear carbon chain with alternating single and double bonds. As a result, each carbon is left with an unhybridized p-orbital containing one electron. This problem will take you through steps to construct and fill the molecular orbital diagram for octatetraene based on the way these different p-orbitals can come together. a) The various molecular orbitals formed from octatetraene’s 8 unhybridized p-orbitals are shown on the next page. Draw the nodal planes for each molecular orbital. Hint: A nodal plane is a line through the molecule that denotes the sites of destructive interference. An example is shown below with ethylene. b) Based on the nodal planes, arrange the energy levels corresponding to the 8 molecular orbitals on the energy level diagram (label them using the numbering provided on the left side of the molecular orbitals) on the next page, in order of lowest to highest energy. c) Populate your molecular…
What type of atomic or hybridized orbital is each lone pair indicated below in? Compound A Compound B Compund A (unhybridized p-orbital) and Compound B (sp3-hybridized orbital) O Compund A (sp2-hybridized orbital) and Compound B (sp3-hybridized orbital) Compund A (sp3-hybridized orbital) and Compound B (unhybridized p-orbital) O Compund A (unhybridized p-orbital) and Compound B (sp2-hybridized orbital)
Two useful organic compounds that contain Cl atoms are vinyl chloride (CH2 = CHCI) and chloroethane (CH;CH;CI). Vinyl chloride is the starting material used to prepare poly (vinyl chloride), a plastic used in insulation, pipes, and bottles. Chloroethane (ethyl chloride) is a local anesthetic. Why is the C- Cl bond of vinyl chloride stronger than the C– CIl bond in chloroethane.
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sketch and label the orbitals in ethene according to valence bond theory?
The alkene C=C double bond and the carbonyl (C=O) group are both sp2 hybridized BUT have different chemistry. Which statement explains best this difference? A) The bond angle of the carbonyl is larger than the bond angle of the alkene and this accounts for the difference in their reactions. B) The electronegative oxygen of the C=O group makes this bond polar and this polar bond accounts for the difference in their reactions. C) The bond of the C=C is longer that the bond of the C=O and this accounts for the differences in their reactions. D) There is more steric crowding in the carbonyl than in the alkene and this accounts for the differences in their reactions.