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General AB Molecules

2-19 GENERAL AB MOLECULES We shall now describe the bonding in a general diatomic molecule, AB, in which B has a higher electronegativity than A, and both A and B have s and f valence orbitals. The molecular-orbital energy [Pg.78]

The ground-state electronic configuration for BN is ( a y(as y (jCie,fyy( z ) This gives a ir state and a prediction of two bonds [Pg.80]

The BN molecule is thus electronically similar to C2. The bond lengths of C2 and BN are I.3I and 1.28 A, respectively. The BN bond energy is only 92 kcal/mole, as compared to 150 kcal/mole [Pg.81]

The CO, NO+, and CN molecules are isoelectronic with N2, having a ground state. The configuration [Pg.81]

The electronic configuration of NO is Co s ) (crs ) (xj,/) (o-j ) (irx,y )t giving a V ground state. Since the eleventh electron goes into a IT orbital, the number of bonds is now 1, or less than for NO+. The bond length of NO is 1.15 A, longer than either the CO or NO+ distances. The bond energy of NO is 162 kcal/mole, considerably less than the CO value. [Pg.81]


Figure 2-24 Relative orbital energies i a general AB molecule, with B more electronegative than A. Figure 2-24 Relative orbital energies i a general AB molecule, with B more electronegative than A.

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