![]() The electronic configuration of H 2 is ( σ(1s) ) 2 The electronic configuration of H 2 + is ( σ(1s) ) 1Ģ) Positive bond order means it is stable.ģ) One unpaired electron is present. Greater the number of unpaired electrons present in the molecular or ion, greater is its paramagnetic nature.Įlectronic configuration of Homonuclear Diatomic Molecules If the molecules has some unpaired electrons ,it is paramagnetic in nature. If all the electrons in the molecule are paired, it is diamagnetic in nature. Greater the bond order, shorter is the bond length.Ħ) Diamagnetic and paramagnetic nature of the molecules the bond order is negative or zero.ģ) Relative stability of molecule in terms of bond orderįor diatomic molecules ,the stability is directly proportional to the bond order.Ī molecule with the bond order of 3 is more stable than a molecule with bond order of 2 and so on.Ĥ) Nature of bond in terms of bond order :īond order 1 ,2 and 3 mean single ,double and triple bond.īond length is found to be inversely proportional to the bond order. The molecule is unstable if N b < Na i.e. Σ(1s) Na ,the molecule is stable because greater number of bonding orbitals are occupied than antibonding orbital, resulting in a net force of attraction.Ģ) If N b Na ie. The first ten molecular orbitals may be arranged in order of energy as follow: Therefore, theĮlectronic configuration of O 2 is as follows.Energy level diagram for Molecular orbitals Hence, in O 2 molecule there are 16 electrons. The electronic configuration of oxygen (Z = 8) in the ground state is 1s 22s 22p 4. The bond order of N 2 can be calculated as follows.Ī triple bond is present in a molecule ofĤ. The molecular orbital energy level diagram of N 2 is given in Fig. In calculating bond order, weĬan ignore KK, as it includes two bonding and two antibonding electrons. The configuration is abbreviated as KK, which denotes the K shells of the two atoms. Molecular orbitals in order of increasing energy. Therefore, the total number of electrons present in nitrogen molecule (N 2) is 14. The electronic configuration of nitrogen (Z=7) in the ground state is 1s 2 2s 2 2p 1x 2p 1y 2p 1z . ![]() Level diagram of He 2 (hypothetical) is givenīond order = N b - N a / 2 = 2 - 2 / 2 = 0.Īs the bond order for He 2 comes out to be zero, this molecule does not exist.ģ. Keeping in view the Aufbau principle and Pauli'sĮxclusion principle its electronic configuration would be as follows. As each helium atom contains two electrons, there will be fourĮlectrons in He2 molecule. The electronic configuration of helium (Z =Ģ) in the ground state is 1s 2. The bond order of H 2 molecule can be calculated as follows.īond : This means that the two hydrogen atoms in a moleculeĮlectron is present in hydrogen molecule,ĭiatomic helium molecule, He 2 (Hypothetical). Molecular orbital energy level diagram of H 2 molecule is given in Fig. The molecular orbital electronic configuration of These two electrons should have opposite spins. Therefore, in all there are two electrons in hydrogen molecule which are present in lower most s 1s molecular orbital.Īccording to Pauli's exclusion principle, It is formed by the combination of two hydrogen atoms. Now, let us consider some examples of homo nuclear (iii)Hund's rule of maximum multiplicity. The filling of molecular orbitals is governed by the ![]() Orbital energy level diagrams of certain diatomic Homo nuclear molecules and molecular ions
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |