Single bonds carbon-hydrogen

Carbon, hydrogen, single bonds, and at least one -OH (may contain double and triple bonds and other structures)... 

Alkanes consist of carbon-carbon and carbon-hydrogen single bonds and are unreactive compounds. This is due to the fact that C-C and C-H bonds are covalent in nature and so there are no electrophilic or nucleophilic centres present. Since most reagents react with nucleophilic or electrophilic centres, so the alkanes are unreactive molecules. 

We can now completely specify the orbitals used to form the bonds in the ethylene molecule. As shown in Fig. 14.13, the carbon atoms are described as using sp2 hybrid orbitals to form the a bonds to the hydrogen atoms and to each other, and using p orbitals to form the 7t bond with each other. Note that we have accounted fully for the Lewis structure of ethylene with its carbon-carbon double bond and carbon-hydrogen single bonds. 

In all of these cases one carbon-hydrogen single bond is broken, one carbon-hydrogen single bond is formed, and a single bond turns into a double bond or a double bond turns into a triple bond. For example. 

Table 8.3 Carbon-Hydrogen Single Bond Lengths and Hybridization Compound Length, A Hybridization...

Single bonds are the most common type of bond, but many molecules (and ions) contain multiple bonds. Multiple bonds most frequently involve C, O, N, and/or S atoms. A double bond consists of two bonding electron pairs, four electrons shared between two atoms, so the bond order is 2. Ethylene (C2H4) is a simple hydrocarbon that contains a carbon-carbon double bond and four carbon-hydrogen single bonds ... 

Alkanes contain only carbon-carbon and carbon-hydrogen single bonds and have the general formula C H2 +2 where n is an integer other than zero. The smallest member of the alkane family is... 

In many cases, the choice of just where to localize the odd electron and charge is arbitrary, however. This is especially true if there are only carbon—carbon and carbon—hydrogen single bonds, as in propane. When possible, though, we write the structure showing the molecular ion that would result from the removal of one of the most loosely held valence electrons of the original molecule. Just which valence electrons are most loosely held can usually be estimated from ionization potentials (Table 9.3). The ionization potential of a molecule is the amount of energy (in electron volts) required to remove a valence electron from the molecule. 

Saturated fatty acid A fatty acid containing only carbon-hydrogen single bonds. 

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