The bonding situation in C2 can be described with the bonds in Be2 that are enforced by. Combining the in-phase orbitals results in a bonding orbital. The bonding components in C2 consist of two weakly bonding bonds and two electron-sharing bonds. One contains the axis, and one contains the perpendicular. Combining the out-of-phase orbitals results in an antibonding molecular orbital with two nodes. Side-by-side overlap of each two p orbitals results in the formation of two π molecular orbitals. For the out-of-phase combination, there are two nodal planes created, one along the internuclear axis and a perpendicular one between the nuclei.įigure 7.7.6. Electrons in this orbital interact with both nuclei and help hold the two atoms together, making it a bonding orbital. In molecular orbital theory, we describe the \pi orbital by this same shape, and a \pi bond exists when this orbital contains electrons. In valence bond theory, we describe π bonds as containing a nodal plane containing the internuclear axis and perpendicular to the lobes of the p–\pi orbitals, with electron density on either side of the node. The side-by-side overlap of two p orbitals gives rise to a pi (\pi) bonding molecular orbital and a \pi* antibonding molecular orbital, as shown in Figure 7.7.6. Combining wave functions of two p atomic orbitals along the internuclear axis creates two molecular orbitals, σp and σ∗p. Just as with s-orbital overlap, the asterisk indicates the orbital with a node between the nuclei, which is a higher-energy, antibonding orbital.įigure 7.7.5. There is an \ce^* (antibonding) (read as “sigma-p-x” and “sigma-p-x star,” respectively). Li 2 + and Li 2 – ions have the same bond order ( 0.5).īut Li 2 – has more electrons in higher energy antibonding molecular orbital as compared to Li 2 +.This electronic structure adheres to all the rules governing Lewis theory. Li 2 + is more stable as compared to Li 2 – : Thus lithium molecule (Li2) is more stable. Therefore, Li2 has stronger single covalent bonding. Since the bond order of Li 2 is higher than Li 2 + and Li 2. The antibonding molecular orbital σ*2 s contains 1 electron.īond order = Number of electrons in BMO – Number ofīond order = 0.5 Arrange the following species in increasing order of stability: Li 2, Li2 +, Li 2 – Chemistry Class important question MO diagram Stability order of Li2,Li2-,Li2+ In the case of Li 2 -, the 2 electrons are present in σ 2s orbitals. In the case of Li 2 +, the 1 electrons are present in σ 2s orbitals.īond order = Number of electrons in BMO – Number of electrons in ABMO / 2
#C2 molecular orbital diagram how to#
How to draw the molecular orbital diagram of Li 2, Li2 +, Li2 – ? MO diagram MO diagram of Li2 ,Li2+ ,Li2. The antibonding molecular orbital σ*2 s is empty.īond order = Number of electrons in BMO – Number of electrons in ABMO /2īond order 1 shows that there is a single covalent bond between the lithium atoms in the Li 2 molecule. The 2 electrons are present in σ 2s orbitals. How do draw the Molecular Orbital Diagram of Lithium molecule (Li 2)?Īccording to the molecular orbital theory, the molecular orbital diagram of the lithium molecule is shown below: MO diagram Li2 bond order The electronic configuration of the Li atom is 1s 2 2s 1. The distribution of electrons in lithium electronic shells is as follows: The atomic number of Lithium (Li ) is 3 and the mass number is 6.941. Lithium is represented by the symbol “Li”. Lithium belongs to group 1 ( alkali metals), period 2 s-block element of the periodic table. How to draw Molecular Orbital Diagram of Li
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