The electronic configuration of N2 is KK (σ(2s)) 2 (σ ∗(2s)) 2 (π(2p x)) 2 (π(2p y)) 2 (σ(2p z)) 2īond order value of 3 means that N 2 contains a triple bond. The double bond in C 2 consist of both Pi bonds because the four electrons are present in the two pi molecular orbitals. The electronic configuration of Be 2 is KK (σ(2s)) 2 (σ ∗(2s)) 2 The electronic configuration of Li 2 is (σ(1s)) 2 (σ ∗(1s)) 2 (σ(2s)) 2Īs inner closed closed shells do not participate in bonding therefore the configuration is written as:Īs the K closed shells do not take part in bonding, they are called non-bonding orbitals.ģ)It has no unpaired electron ,it should be diamagnetic. The electronic configuration of He 2 + is (σ(1s)) 2 (σ ∗(1s)) 1 No bond is formed between two helium therefore He 2 does not exist. The electronic configuration of H 2 – is ( σ(1s) ) 2 (σ ∗(1s)) 1Ģ) Smaller positive value of bond order indicates that it is somewhat stable.ģ) Since it has one unpaired ,it is paramagnetic.Įlectronic configuration of helium is (σ(1s)) 2 (σ ∗(1s)) 2 Greater value of bond order for H 2 molecule than H 2 + ion shows that two H 2 molecule is more stable than H 2 +.īond length of H 2 is smaller than that of H 2 + ion.Īs no unpaired electron is present, the H 2 molecule should be diamagnetic. Positive value of bond order indicates that H 2 molecule is stable.īond order value of 1 means that two hydrogen atoms are connected by a single bond. 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:
Energy level diagram for Molecular orbitals
0 kommentar(er)
