Reactivity in Chemistry

Carbonyl Addition

CO27.  Solutions to Selected Problems, Part A

Problem CO1.1. 

The HO-C=O or CO2H group present in all of the amino acids is called a carboxylic acid.

An additional carboxylic acid is present in aspartic acid and glutamic acid.

The H2N-C=O or CONH2 group present in asparagine and glutamine is called an amide.

Problem CO1.2. 

a) aldehyde    b) ketone    c) ketone    d) aldehyde  

Problem CO1.3.

Problem CO1.4.

Problem CO2.1.

a)  The double bond means two pairs of electrons are shared between the carbon and oxygen, instead of just one.  As a result, the oxygen is able to pull more electron density away from the carbon.  The carbon becomes much more positive in this case than in the case of a double bond.

Not only that, but the second bond between the carbon and the oxygen is a pi bond.  Those electrons are farther from the nucleus than a sigma bond, in which the electrons are tightly held between the atoms.  That means the pi electrons are more easily drawn toward the oxygen, so the bond becomes even more polarized.

b)  A C=N bond would be very similar to a C=O bond, because nitrogen is the third most electronegative element after oxygen and fluorine (ignoring noble gases).

Problem CO2.2.

 

Problem CO2.3.

Problem CO2.4.

Problem CO2.5.

a)  2-hexanone or hexan-2-one        b)  5-methylhexan-2-one    c)  3-methylhexan-2-one

d)  hexan-3-one    e)  heptan-4-one    f)  4-methylhexan-3-one

g)  hexanal    h)  3-methylbutanal    i)  2-methylbutanal

j)  2-ethylpentanal    k) 4,4-dimethylpentanal    l) 2,3-dimethylpentanal

m)  3-ethoxypropanal    n)  4-chloropentan-2-one    o)  4-aminohexan-3-one

p)  hex-4-en-2-one (in the solution above, (E)-hex-4-en-2-one is shown first and (Z)-hex-4-en-2-one is shown second).

q)  hept-4-yn-2-one    r) benzaldehyde (this is a common name adopted for formal naming.  Benz means a carbon attached to a benzene ring.)

Problem CO2.6.

Problem CO3.1.

Problem CO3.2.

Problem CO4.1.

 

Problem CO4.2.

 

Problem CO4.3.

Problem CO4.4.

Problem CO5.1.

The LUMO in this case is the π*, an antibonding level. If electrons populate this level, the π bond will break.

Problem CO5.2.

Problem CO5.3.

Both the imine (b) and nitrile (c) have a low-lying pi antibonding level (π*), similar to a carbonyl.

Problem CO6.1.

a)  On the basis of steric crowding, the first one is most reactive, then the last one, then the middle.

b)  On the basis of steric crowding, the last one is most reactive, then the first one, and then the middle. 

Although there is a large group on the nitrogen in that last compound, the site of reactivity is the carbon, which is less crowded.

c)   On the basis of electronics, the middle one is most reactive, then the last, and then the first.  The fluorine atom is very electronegative and pulls electron density towards itself.  That leaves more positive charge on the nearby carbonyl carbon.  The more fluorines on that nearby carbon, the more positive the carbon.  The more positive the carbon, the more it attracts electrons from a nucleophile.

Problem CO6.2.

a) propanal    b) butanal    c) propanal, again!

d) pentanal    e) hexanal    f) heptanal

Problem 6.3.

a) 3-pentanone    b) 3-hexanone    c) 4-heptanone

d) 2-butanone    e) 3-octanone    f) 5-decanone

Problem 6.4.

a) 2-methyl-3-pentanone or  2-methylpentan-3-one    b) 4-ethyl-3-hexanone or 4-ethylhexan-3-one  

c) 3,3-dimethyl-2-butanone or 3,3-dimethylbutan-2-one      d) 2,5,5-trimethyl-4-heptanone or 2,5,5-trimethylheptan-4-one

e) 6-ethyl-4-methyl-3-octanone or 6-ethyl-4-methyloctan-3-one    f) 6-ethyl-4,5-dimethyl-3-octanone or 6-ethyl-4,5-dimethyloctan-3-one

Problem CO7.1.

Problem CO8.1.

Problem CO8.2.

Problem CO8.3.

Problem CO8.4.

Problem CO9.1.

a)  In acetylide, the lone pair is on a linear carbon or sp carbon.  In methyl anion, the lone pair is on a tetrahedral carbon or sp3 carbon.  The description "sp" indicates that sigma bonding to neighbours involves a 2s orbital and a 2p orbital on carbon; there is a 50% contribution from the s orbital. 

The description "sp3", on the other hand, indicates that sigma bonding to neighbours involves a 2s orbital and three 2p orbitals; there is a 25% contribution from the s orbital. 

The 2s orbital is lower in energy than the 2p orbital.  The greater the s orbital contribution to the bond (or in this case to the lone pair), the lower it is in energy.  Thus, a lone pair on an sp carbon is lower in enrgy than a lone pair on an sp3 carbon.

b)  In cyanide, the same argument outlined in pary (a) hold true.  In addition, the nearby electronegative nitrogen stabilizes the charge by drawing electron density toward itself.

Problem CO9.2.

a)  CH3OK, because of the ionic O-K bond.  This is an anionic nucleophile.  It is more reactive and nucleophilic than the corresponding neutral nucleophile.

b)  CH3NH2, because nitrogen is less electronegative than oxygen.  Its lone pair is held less tightly and is more easily donated to the electrophile.

c)  NaCCH, because the neighbouring carbon in this case does not have the inductive electron-withdrawing effect that the nitrogen does in the case of NaCN.  In that case, the lone pair is stabilized and made less reactive.

d)  c-C6H11ONa, because the negative charge is localized on one atom.  In c-C6H5ONa, the negative charge is delocalized over four different positions in the molecule.  Delocalization of charge stabilizes the anion and makes it less reactive.

Problem CO11.1.

Problem CO11.2.

Problem CO11.3.

Problem CO11.4.

Problem CO11.5.

Problem CO11.6.

Problem CO11.7.

Problem CO11.9.

Problem CO12.1.

a) pentanol        b) 2-butanol        c)  4-octanol

d)  2-methylpropan-2-ol or 2-methyl-2-pronanol        e) 3-methylhexan-2-ol or 3-methyl-3-hexanol

f)  5,6-dimethylheptan-1-ol or 5,6-dimethyl-1-heptanol

Problem CO12.1.

Problem CO12.2.

 

Problem CO12.3.

Problem CO12.4.

Problem CO12.5.

 

Problem CO12.6.

Problem CO12.7.

Problem CO12.8.

Problem CO12.9.

Some of these compounds do not have alpha-protons, so they cannot form enolate ions.

Problem CO12.10.

Problem CO12.11.

Problem CO12.12.

Problem CO12.13.

Problem CO12.14.

Problem CO12.15.

Problem CO12.16.

 

This site is written and maintained by Chris P. Schaller, Ph.D., College of Saint Benedict / Saint John's University (with contributions from other authors as noted).  It is freely available for educational use.

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Structure & Reactivity in Organic, Biological and Inorganic Chemistry by Chris Schaller is licensed under a Creative Commons Attribution-NonCommercial 3.0 Unported License

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This material is based upon work supported by the National Science Foundation under Grant No. 1043566.

Any opinions, findings, and conclusions or recommendations expressed in this material are those of the author(s) and do not necessarily reflect the views of the National Science Foundation.

 

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