Interpretation:
Why an addition product is normally not observed when an alkyne is treated with a peroxyacid in a way similar to the addition of a carbene is to be explained.
Concept introduction:
Alkenes also add a bridging oxygen in a similar way to form an
Alkynes, because of their similarity, would also be expected to react with peroxyacids in a similar way.
The stability of the ring formed is expected to be dependent on the nature of the
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ORGANIC CHEMISTRY E-BOOK W/SMARTWORK5
- The addition of water to aldehydes and ketones occurs rapidly, although it is not thermodynamically favored. What would be the product for the reaction above? Hint: Think of the self-ionization of water and the polarity of the carbonyl group.arrow_forwardorganic chemistry When learning about substitution or elimination reaction, hydrogen or carbon bonding in intimidate move to carbocation, making carbocation more substituted and stable. In here, I can't recall what this situation is calledarrow_forwardCan you give me detail about the chiral carbon step by step with an examples, please?arrow_forward
- For which isomer would you expect a greater equilibrium percentage of molecules with the alkyl group in the axial position, explain.arrow_forwardWhich of the following substitution reactions is not likely to occur? Explain.arrow_forwardCan you help me with the explanation of the alkane, alkene, alkyne, aromatic and all these terms give me examples too?arrow_forward
- The chiral molecular among the following isarrow_forwardThe skeleton of benzyldimethylamine is The number of available valence electrons is as follows: from the benzyl group, ___; from each of two methyl groups, ___; and, from the nitrogen atom, ___, for a total of ___. Filling in the skeleton with single bonds gives ____________________________ and adding the appropriate unshared pair gives ____________________________ The number of electrons in the functional group of this structure is ___, and the structure is (correct, incorrect).arrow_forwardThe skeleton is benzaldoxime is The number of valence electrons is as follows: from the phenyl group. ___; from each of two hydrogens, ___; from the carbon atom, ___; from the nitrogen atom, ___; and from the oxygen atom, ___, for a total of ___. Filling in the skeleton with single bonds and adding the appropriate unshared pairs gives _____________________ The number of electrons in the functional group of this trial structure is ___, which is ___ too many. Removing an unshared pair from carbon and nitrogen and adding a second bond between them gives _____________________ in which carbon, nitrogen, and oxygen have their customary valences of ___, ___, and respectively. The alternative structure with a double bond between nitrogen and oxygen is _____________________ This structure is not acceptable because it requires carbon and oxygen to exhibit the unfamiliar valences of ___ and ___. Derive Lewis structures for the compounds below.arrow_forward
- Nitrobenzene has the skeleton The number of available valence electrons is: from the phenyl group, ____; from the nitrogen atom, ____; and from each of two oxygen atoms, ____, for a total of ____. Filling in all single bonds and adding the appropriate unshared pairs gives ______________________________ The functional group of this structure contains ____ electrons. Therefore, unshared pairs are removed from the nitrogen atom and one of the oxygen atoms; a double bond is added giving ______________________________ which has the correct number of electrons. In this structure the nitrogen atom is sharing ____ pairs of electrons. From each shared pair the nitrogen owns ____ electron for a total of ____. Nitrogen is a Group ____ element and would have outer shell electrons in the unbonded, neutral state. Since the nitrogen atom in nitrobenzene has one fewer electron than it would in the neutral state, it has a formal charge of +1 . This is added to the Lewis structure as + giving Since an electron is negatively charged, a shortage of one electron results in a single positive charge on an atom. Conversely, an excess of one electron results in a single negative charge on an atom. When an atom in a Lewis structure “owns” two fewer electrons than it would have in the neutral, unbonded state, it is denoted by ++ or +2 and, conversely, or – 2.arrow_forwardBy drawing the lewis structure of the cyanide anion, interpret according to the molecular orbital theory on which atom the active end is on, that is, which atom it react in a reaction?arrow_forwardWhich of here is labelled incorrectly based on equivalent hydrogen of the ff structuresarrow_forward
- Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning