Simple picture is adequate for many diatomic molecules with univa-lent atoms,īut it is not sufficient to describe the bonding in most polyatomic molecules. The type of bond formed is called a σ bond because the region of greatestĮlectron density falls on the internuclear axis. This is shown both by using Lewis structuresĪnd by using orbital pictures. With a singly occupied 2p orbital of fluorine to give a bond between the twoĪtoms that contains two electrons. The reaction of a chlorine atom with aįluorine atom occurs by the overlap of a singly occupied 3p orbital of chlorine Each atom inĮssence gains an electron by sharing. Occupied AOs to form new MOs that contain a pair of electrons. Covalent bonds are formed by the overlap of singly Sharing electrons is a way to enable each atom of theīonded pair to reach an octet electronic configuration without having to give (Based on functional groupīehavior, any other alcohol is predicted to react with potassium in the sameīonds in organic molecules, however, are covalent bonds in which elec-trons are Hydrogen has the electronic configuration of helium. Has an octet structure (three lone pairs and one pair of shared electrons), and By losing anĮlectron, potassium gains the octet electronic configuration of argon, oxygen Gives an ionic bond between the tert-butoxyĪnion and a potassium cation by transfer of electrons from potas-sium to the Reaction of potassium metal with tert-butanol The “bond” between cesium and chlorine is due to the electrostaticĪttraction of the cesium and chloride ions.
Octet electronic configuration of xenon, and the chlorine has been converted toĪ negatively charged chloride ion with the octet electronic configuration ofĪrgon. The cesium atom has been converted to a positively charged cesium ion with the By doing so,īoth cesium and chlorine have reached a valence octet electron configuration. Transfer of an electron from the cesium atom to the chlorine atom. ForĮxample, the reaction of a cesium atom with a fluorine atom occurs by the Reach an octet electronic configuration (as a negatively charged ion). Positively charged ion) and a second atom accepts one or more electrons to Gives up one or more electrons to reach an octet electronic configuration (as a An atom can achieve an inert-gasĮlectronic configuration by giving up electrons, accepting electrons, or Inert gas electron configuration in the valence level (a valence octet for allĮlements except hydrogen which requires only two electrons to achieve theĮlectronic configuration of helium). The quadrivalent valence state of carbon atom, along with the four hydrogen atoms ready to form bonds, is represented in Figure 2.Bonding Schemes| Home | | Organic Chemistry |Ĭhapter: Organic Chemistry : Functional Groups and Chemical Bondingīond formation between atoms occurs primarily to enable each atom to achieve an inert gas electron configuration in the valence level (a valence octet for all elements except hydrogen which requires only two electrons to achieve the electronic configuration of helium).įormation between atoms occurs primarily to enable each atom to achieve an Moffitt 4, as the conceptual precursor of bond formation to hydrogen atoms (or other elements). The carbon atom with the four singly-occupied tetrahedral hybrids is now in what can be designated as its "valence state," a construct introduced independently by J. These are called sp 3-hybrid orbitals, which can be designated t 1, t 2, t 3, and t 4. A further transformation, first suggested by Linus Pauling 2 is the linear combination of the nearly degenerate 2 s and three 2 p orbitals into four identically-shaped hybrid orbitals, directed toward the corners of a tetrahedron. But much more stable compounds can be formed if carbon invests a relatively small amount of energy to excite one of its 2 s-electrons to the remaining unoccupied 2 p orbital, and thereby becomes quadrivalent, thus recouping the 2 s-2 p excitation energy in the formation of two additional chemical bonds. Carbon, with its two unpaired electrons, appears to be a naturally divalent atom, and indeed the compound CH 2 can exist in the gas phase.
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