Chemical Bond Definitions, Parameters, and Hybridization

metallic bond: the bond strength between metal atoms, which owe their stability and properties of metallic lattices. Covalent bonding is the joining of two atoms q comprten one or more pairs of electrons. The salt bridge is the union resulting from the presence of electrostatic forces between positive and negative ions lead to the formation of a compound substituted ionic x a crystal lattice. The covalency of elmento is the number of covalent bonds can form q, which q depends on the number of unpaired electrons. Binding parameters: the binding energy of a diatomic molecule is the enthalpy q occurs when one mole dissociates of molecules in a gas of atoms in the same state. Bond length is the distance between the nuclei of 2 atoms linked by a covalent bond. · The link or is formed when two atomic orbitals overlap the ends so x q the electron density is concentrated between the two nuclei. All single bonds are of this type. Link form x ð lateral overlap of atomic orbitals. The electron density is concentrated at the top and bottom of the q plane containing the nuclei of bonded atoms. ð link is formed only when there is a link or between 2 atoms. Angulo liaison is the angle formed by the straight q x q passing atomic nuclei or link addresses. Polarity link: in the formation of covalent bonding, the q Delos electronegativity atoms involved will determine the polarity of the bond and the possible polarity of the resulting molecule. · Homonuclear diatomic molecules: the two atoms have the same electronegativity, mismatch distribution centers of positive and negative charge, and the molecules are nonpolar. The bond is nonpolar covalent bond electrons at q x as x seon shared the two atoms so q is symmetric electron density for the two nuclei. · Hetronucleares diatomic molecules: the two atoms have different electronegativities ls binding molecule is polarized and is a molecular dipole. The polar bond is aqel that one of the most lectro dosatomos be negative for the other q, to the dsplaza elctronica burden sharing. Sp3 Hybridization: The hybridization of an s orbital and three p orbitals yields four sp3 hybrid orbitals. Sp3 orbitals are directed toward the corners of a tetrahedron rgular, frmando Anglos of 109.5 º. CH4. Sp2 hybridization: when combining an s orbital with two p orbitals form three sp2 hybrid orbitals. The new orbitals are located on the same plane and are each other anguls of 120 °. It maintains a free p orbital hybridization. Hibriacion sp: sp hybrid orbitals from X combination is an s orbital with one p. The new orbitals are linear x lo qe forming an angle of 180 º. They stay two orbitals p without hybridize.