Ground-state electronic configuration molecular

When N valence atomic orbitals overlap, they form N molecular orbitals. The ground-state electron configuration of a molecule is deduced by using the building-up principle to accommodate all the valence electrons in the available molecular orbitals. The bond order is the net number of bonds that hold the molecule together. 

The ground-state electron configurations of diatomic molecules are deduced by forming molecular orbitals from all the valence-sbell atomic orbitals of the two atoms and adding the valence electrons to the molecular orbitals in order of increasing energy, in accord ivith the building-up principle. 

A representative molecular orbital diagram for an octahedral d-block metal complex ML6 is shown in Figure 1.8. The MOs are classified as bonding (oL and ttL), nonbonding (jtM) and antibonding (o, nl and ). The ground-state electronic configuration of an octahedral complex... 

Figure 21-10 The vr-molecular-orbital energies and ground-state electronic configurations of (left) delocalized 1,3-butadiene and (right) localized 1,3-butadiene or 1,5-hexadiene.

The ground-state electron configuration of 02 is obtained by feeding its 12 valence electrons into the molecular orbitals shown in Fig. 3.36. The first 10 repeat the N2 configuration (apart from the change in order... 

The ground-state electron configurations of diatomic molecules are deduced by forming molecular orbitals from all the valence-shell... 

The ground state electron configuration of SiC is (5a)2 (6a)2 (7a)1 (2 r)3 so that the hyperftne constants will reflect the electron distribution in both a and n molecular orbitals. The hyperftne constants a and d are determined mainly by the unpaired n electron, the Fermi contact constant hv depends mainly on the a electron, whilst c is sensitive to both a and tt electrons. In fact the Fermi contact constant also depends, as usual, upon configurational mixing with excited electronic states, which makes... 

Give the ground-state electron configuration and the bond order of the HeJ molecular ion. 

The ground-state electron configuration of the Hj molecular ion is (cTgis). ... 

Having classified the elements according to their ground-state electron configurations, we can now look at the way chemists represent metals, metalloids, and nonmetals as free elements in chemical equations. Because metals do not exist in discrete molecular units, we always use their empirical formulas in chemical equations. The empirical formulas are the same as the symbols that represent the elements. For example, the empirical formula for iron is Fe, the same as the symbol for the element. 

Later in this section we will study molecules formed by atoms of the second-period elements. Before we do, it will be instructive to predict the relative stabilities of the simple species H2, H2, He, and Hc2, using the energy-level diagrams shown in Figure 10.24. The rri and of orbitals can accommodate a maximum of four electrons. The total number of electrons increases from one for H2 to four for He2. The Pauli exclusion principle stipulates that each molecular orbital can accommodate a maximum of two electrons with opposite spins. We are concerned only with the ground-state electron configurations in these cases. 

Fig. 6-7 rc-Electron, molecular-orbital energy-levels, and ground-state electronic-configuration of naphthalene. 

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