Ethanol Lewis structure

Write the Lewis structure for acetic acid, CH COOH, the carboxylic acid in vinegar formed when the ethanol in wine is oxidized. In the —COOH group, both O atoms are attached to the same C atom, and one of them is bonded to the final H atom. The two C atoms are bonded to each other. 

Write the Lewis structure of each of the following organic compounds (a) ethanol, Cl IjCLLOH, which is also called ethyl alcohol or grain alcohol (b) methylamine, CH3NH2, a putridsmelling substance formed when flesh decays (c) formic acid, HCOOH, a component of the venom injected by ants. 

Write the Lewis structures of the following organic compounds (a) ethanol, CH3CH2OH, which is also called ethyl alcohol or grain alcohol ... 

As expected, because the parent acids of these two anions can be reasonably well described by a single Lewis structure, they have much smaller delocalisation energies. In ethanol and its deprotonated anion, for which no resonance between low-lying Lewis structures may be expected, the delocalisation energy is relatively small. 

Both are valid Lewis structures, and both molecules exist. One is called ethanol, and the other, dimethyl ether. These two compounds are called isomers. 

A third factor that determines acidity is resonance. Recall from Section 1.5 that resonance occurs whenever two or more different Lewis structures can be drawn for the same arrangement of atoms. To illustrate this phenomenon, compare ethanol (CH3CH2OH) and acetic acid (CH3COOH), two different compounds containing O-H bonds. Based on Table 2.1, CH3COOH is a stronger acid than CH3CH2OH ... 

Draw the conjugate bases of these acids to illustrate the importance of resonance. For ethoxide (CH3CH20, the conjugate base of ethanol, only one Lewis structure can be drawn. The negative charge of this conjugate base is localized on the O atom. 

Our best acid in the solution is the solvent, ethanol. The proton transfer path again gives us the Lewis structure of the product. The p Ta of the product is known to be 17.6, and the pATg of ethanol (our acid) is at 16, so that gives a of = lO -, ... 

Special Topic 3.1 describes how the shape of ethanol molecules allows them to attach to specific sites on nerve cell membranes and slow the transfer of information from one neuron to another. Special Topic 5.2 describes how the shapes of the molecules in our food determine whether they taste sweet or bitter. You will find out in Special Topic 17.2 that the fat substitute Olestra is indigestible because it does not fit into the enzyme that digests natural fat. The purpose of this section is to show you how to use Lewis structures to predict three-dimensional shapes of simple molecules and polyatomic ions. Let s start with a review of some of the information from Section 3.1, where this topic was first introduced. 

In contrast, if two liquids mix endothermically, it indicates that the solute-solvent interactions are weaker than the interactions among the molecules in the pure liquids. More energy is required to expand the liquids than is released when the liquids are mixed. In this case the molecules in the solution have a higher tendency to escape than expected, and positive deviations from Raoult s law are observed (see Fig. 11.13). An example of this case is provided by a solution of ethanol and hexane, whose Lewis structures are as follows ... 

The framework of covalent bonds revealed by the connectivity information accounts for 16 of the 20 valence electrons in C2H6O (step 4). The remaining four valence electrons are assigned to each oxygen as two unshared pairs in step 5 to complete the Lewis structures of ethanol and dimethyl ether. 

Draw Lewis structures for the following organic t ARiS molecules (a) methanol (CH3OH) (b) ethanol... 

The functional group of an alcohol is an —OH (hydroxyl) group bonded to a tetrahedral carbon atom (a carbon having single bonds to four other atoms). Here is the Lewis structure of ethanol. 

PROBLEM 2.42 Write Lewis structures for ethane, ethylene, acetylene, ethanol, ethanethiol, tetraethylammonium ion, diethylphosphine, the imine of diethyl ketone, diethylborane, tetraethylborate ion, diethyl ether, diethyl sulfide, acetaldehyde, acetone, acetic acid, ethyl acetate, acetamide, acetyl chloride, propanenitrile, ethyl fluoride, and ethyl chloride. Show nonbonding electrons as dots and electrons in bonds as lines. 

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