Organic Chemistry
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A Lewis acid is a substance that can accept an electron pair. One example of a Lewis acid is SiH3+. Which orbital will the new electron occupy if SiH3+ accepts an electron pair?
i. How are electrons excited? ii. Fill the electrons on the π and/or π* orbitals in the incomplete molecular orbital diagram to show the excited state.
The molecular orbital drawing for the C—F bond of fluoromethane is given below. If there were two more electrons in this bond, where would these electrons go in the molecular orbital drawing?
Determine which kind of molecular orbitals are formed when the following atomic orbitals are combined with each other.
Explain the cause of the rotational behaviors around the C−C bond in propane, which has a free rotation, and around the C=C bond in propene, which has an extremely high rotational barrier.
Show how pi orbitals are involved in the formation of pi bonds in the given molecules.a. HCOOHb. CH3CN
Provide a molecular orbital diagram for trans−hex−3−ene and label all σ and π bonds. Determine and explain whether there will be a free rotation around the C3−C4 bond or none.
Illustrate the given orbitals:
(i) 2s
(ii) 3s
(iii) 2p
True or false: He22+ does not exist.
Draw the orbitals used in the π bonds of the molecule shown below:
CH2=CHCH2CH2CH=C=CH2
Draw the orbitals used in the π bonds of the compound with the formula N≡CCH2CH=C=O.
Part of the molecular orbital diagram of F2 is shown below.
i. Identify σ and σ* on the diagram
ii. Identify which is lower in energy between the two and explain.