Covalent bond triple

Double and triple covalent bonds can be formed between elements by the sharing of two or three electron pairs respectively. Consider the formation of ethene (ethylene), C2H4 ... 

Of course, when multiple pairs of electrons participate in double or triple covalent bonds, those electrons stay within the same bonding axis. Lone pairs repel other lone pairs more strongly than they repel bonding pairs, and the weakest repulsion is between two pairs of bonding electrons. Two lone pairs separate themselves as fcir apart as they can go, on exact opposite sides of an atom if possible. Electrons involved in bonds also separate themselves as far apart as they can go but with less force than two lone pairs. In general, all electron pairs try to maintain the maximum mutual separation. But when an atom is bonded to many other atoms, the ideal of maximum separation isn t always possible because bulky groups... 

Double covalent bonds in molecules of oxygen, Oz, and carbon dioxide, C02, and a triple covalent bond in a molecule of nitrogen, N2. 

Some atoms can form triple covalent bonds, in which six electrons—three from each atom—are shared. One example is molecular nitrogen, N2. Most of the air surrounding you right now (about 78 percent) is gaseous molecular nitrogen, N2. 

How many electrons are shared in a triple covalent bond ... 

Unsaturated hydrocarbon A hydrocarbon molecule which contains double or triple covalent bonds between carbon atoms. 

The triple covalent bond with two atoms bonded by three pairs of electrons is known for instance in the case of nitrogen (N N-.) or of acetylene (H C C H). 

Alkynes Unsaturated hydrocarbon compounds with the general formula CH2n 2 in the simplest cases. They contain triple covalent bonds. Uncommon in essential oil components. 

Notice that in this case each atom shares three electrons there are three shared pairs, or a triple covalent bond between the two atoms, N=N. 

Explain the differences between single, double, and triple covalent bonds. 

Double and triple covalent bonds are examples of multiple bonds. A double covalent bond occurs when two pairs of electrons are shared. The atoms in an oxygen molecule (O2) share two electron pairs, forming a double bond. Each oxygen atom has six valence electrons and must obtain two additional electrons for a noble-gas configuration. If each oxygen atom shares two electrons, a total of two pairs of electrons is shared between the two atoms. A double covalent bond results. See Figure 9-5a. 

A triple covalent bond is formed when three pairs of electrons are shared between two atoms. Nitrogen (N2) shares three electron pairs, producing a triple bond. One nitrogen atom needs three additional electrons to attain a noble-gas configuration. Figure 9-5b shows the triple bond formed between two nitrogen atoms. 

A double covalent bond results when two pairs of electrons are shared between atoms. Sharing three pairs of electrons results in a triple covalent bond. 

Carbon atoms can bond to each other not only by single covalent bonds but also by double and triple covalent bonds. In a double bond, atoms share two pairs of electrons in a triple bond, they share three pairs of electrons. The following diagram shows Lewis structures and structural formulas for single, double, and triple covalent bonds. 

Modem chemists can explain the results of the chemists of 170 years ago. Hydrocarbons that reacted with bromine had double or triple covalent bonds. Those that took up no bromine had only single covalent bonds. Today, a saturated hydrocarbon is defined as a hydrocarbon having only single bonds— in other words, an alkane. An unsaturated hydrocarbon is a hydrocarbon that has at least one double or triple bond between carbon atoms. You will learn more about unsaturated hydrocarbons in Section 22.3. 

Naming alkynes Straight-chain alkynes and branched-chain alkynes are named in the same way as aikenes. The only difference is that the name of the parent chain ends in -yne rather than -ene. Study the examples in Table 22-5. Alkynes with one triple covalent bond form a homologous series with the general formula C H2 2- What are the molecular formulas for... 

By the middle of the nineteenth century, chemists had a basic understanding of the structures of hydrocarbons with single, double, and triple covalent bonds. However, a fourth class of hydrocarbon compounds remained a mystery. The simplest example of this class of hydrocarbon is benzene, which the English physicist Michael Faraday (1791-1867) had first isolated in 1825 from the gases given off when either whale oil or coal was heated. 

Addition reactions Another type of organic reaction appears to be an elimination reaction in reverse. An addition reaction results when other atoms bond to each of two atoms bonded by double or triple covalent bonds. Addition reactions typically involve double-bonded carbon atoms in alkenes or triple-bonded carbon atoms in alkynes. Addition reactions occur because double and triple bonds have a rich concentration of electrons. Therefore, molecules and ions that attract electrons tend to form bonds that use some of the electrons from the multiple bonds. The most... 

This notation uses atomic symbols or group abbreviations joined by single, double or triple lines to represent single, double or triple covalent bonds. All atoms are included in a stylised manner at an... 

C.]—Answer C represents the compound ethyne, which has a molecular formula of C2H2. The three pairs of dots found between the carbon atoms represent a triple covalent bond. 

Other pairs of nonmetal atoms share electron pairs to form covalent bonds. The result of this sharing is that each atom attains a more stable electron configuration—frequently the same as that of the nearest noble gas. This results in a more stable arrangement for the bonded atoms. (This is discussed in Section 7-5.) Most covalent bonds involve sharing of two, four, or six electrons—that is, one, two, or three pairs of electrons. Two atoms form a single covalent bond when they share one pair of electrons, a double covalent bond when they share two electron pairs, and a triple covalent bond when they share three electron pairs. These are usually called simply single, double, and triple bonds. Covalent bonds that involve sharing of one and three electrons are known, but are relatively rare. 

Vukicevic, D. and Graovac, A. (2005) Compact valence sequences for molecules with single, double and triple covalent bonds. Croat. Chem. Acta, 78, 203-209. 

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