Nitrogen triple covalent bond

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. 

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). 

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. 

In some molecules, atoms have noble-gas configurations when they share more than one pair of electrons with one or more atoms. Sharing multiple pairs of electrons forms multiple covalent bonds. A double covalent bond and a triple covalent bond are examples of multiple bonds. Carbon, nitrogen, oxygen, and sulfur atoms often form multiple bonds with other nonmetals. How do you know if two atoms will form a multiple bond In general, the number of valence electrons needed to form an octet equals the number of covalent bonds that can form. 

Nitrogen shortage is caused by the fact that most of it on the surface is in the form of N. In this molecule, the atoms have a strong triple covalent bond. Because of it xmder normal conditions nitrogen practically does not participate in redox reactions w/o catalysts and almost is not used by plants and animals. This property defines drastic domination of over other forms of nitrogen on Earth. 

A triple covalent bond, or simply a triple bond, is a covalent bond in which three pairs of electrons are shared between two atoms. For example, elemental nitrogen, N2, like hydrogen and the halogens, normally exists as diatomic molecules. In this case, however, each nitrogen atom, which has five valence electrons, acquires three electrons to complete an octet by sharing three pairs of electrons with its partner. This is illustrated in the Lewis structure and the formula structure for N2, as shown below. 

Atoms can also bond together by sharing three pairs of electrons. We call this a triple covalent bond. Figure 4.12 shows a dot-and-cross diagram for the triple-bonded nitrogen molecule. 

The electronic configuration of a nitrogen atom is ls 2s 2p. Its atoms need to gain three electrons to achieve the noble gas configuration of neon. Nitrogen atoms do this by forming a triple covalent bond between two atoms (see Figure 13.2). 

The triple covalent bond is very strong its bond energy is almost 1000 kj mol It is difficult to break and so nitrogen gas will only react under extreme conditions. For example, the nitrogen and oxygen in the air react together during... 

The triple covalent bond in N2 is a very strong bond that is difficult to break in a chemical reaction. The unusual strength of this bond makes N2(g) quite inert. As a result, N2(g) coexists with 02(g) in the atmosphere and forms oxides of nitrogen only in trace amounts at high temperatures. The lack of reactivity of N2 with O2 is an essential condition for life on Earth. The inertness of N2(g) lso makes if difficulf to synthesize nitrogen compounds. 

The Lewis structure of N2 indicates that the nitrogen-to-nitrogen bond is a triple covalent bond. Other evidence suggests that the a bond in this molecule involves the overlap of sp hybrid orbitals. 

The substance from which all nitrogen compounds are ultimately derived, NiCg), is unusually stable. One explanation of the limited reactivity of the N2 molecule is based on its electronic structure. As discussed in Chapter 10, the bond between the two N atoms in N2 is a triple covalent bond, which is unusually strong and difficult to break. In thermochemical terms, the enthalpy change associated with breaking the bonds in one mole of N2 molecules is very high—the dissociation reaction is highly endothermic. 

Of course, in all cases each carbon has a full octet of electrons. Carbon also forms double and triple bonds with several other elements that can exhibit a covalence of two or three. The carbon-oxygen (or carbonyl) double bond appears in carbon dioxide and many important organic compounds such as methanal (formaldehyde) and ethanoic acid (acetic acid). Similarly, a carbon-nitrogen triple bond appears in methanenitrile (hydrogen cyanide) and eth-anenitrile (acetonitrile). 

A triple bond is a covalent bond in which six electrons are shared. The nitrogen that is 80 percent of our atmosphere is N2and is an example of a molecule having a triple bond. Each nitrogen atom has five valence electrons, and so each needs to acquire another three electrons in order to satisfy the octet rule. Because both nitrogen atoms are in the same situation, a sharing of six total electrons works. 

When atoms share three pairs of electrons, they form a triple bond. Diatomic nitrogen contains a triple bond, as you can see in Figure 3.19. Try the following problems to practise representing covalent bonding using Lewis structures. Watch for multiple bonding ... 

The covalent bond is directional and multiple covalent bonds are considerably shorter than the corresponding single ones. For carbon as well as for nitrogen, oxygen, or sulfur, the decrease on going from a single bond to a double and a triple bond amounts to about 10 and 20%, respectively. 

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