![]() ![]() Hence from bond order we see that O2 molecule is more stable than O 2 2- ion. 1 sigma bond and 1 pi bond is formed and in O 2 2- ion the bond order is 1. Conclusionįrom O2 bond order diagram we see that the bond order in O2 molecule is 2 i.e. When we see the O2 bond order diagram, all the MO’s are fulfilled expect ∏ 2py * and ∏ 2pz * MO’s which are singly occupied. Higher energy orbitals are unstable in nature where as lower energy orbitals are stable. some goes to higher energy level and some goes to lower energy level. When atomic orbitals of O atom are mixed to form O2 molecule the energies of atomic orbitals changes i.e. How many orbitals are singly occupied in O2? To find out O2 bond order we can use the following formula,īond Order= (Total no of electrons in bonding MO-Total no of electrons in antibonding MO)/2. The ∏ bond is higher in energy as well as weakly bonded than σ bond. The σ bond is formed by overlap of 2p x orbital of each O atom and the ∏ bond is formed by the overlap of either 2p y and 2p z orbitals of each O atom. These 2 covalent bonds contains a total of 4 electrons. Hence 1 σ bond and 1 ∏ bond is formed between 2 O atoms. Covalent bond in O2 moleculeįrom O2 bond order diagram we see that there 2 covalent bonds between 2 O atoms. Hence there is only 1 bond which is σ bond is formed in O 2 2- ion. Total no of electrons in antibonding MO of O 2 2- ion=8. Total no of electrons in bonding MO of O 2 2- ion=10. Use the molecular orbital diagram shown to determine which of the following are paramagnetic. The bond order of O 2 2- ion is calculated by the above mentioned formula. These 18 electrons are filled similar way as in O 2 with extra 2 electrons in ∏ 2py * and ∏ 2pz * MO’s. By the addition of these 2 electrons O 2 2- ion contains a total of 18 electrons. These 2 electrons are added 1 electron each in higher energy ∏ 2py * and ∏ 2pz * MO’s. When 2 electrons are added in O2 molecule O 2 2- ion is formed. The electron configurations for the four species are contrasted below. The bond order is determined from the the electron configurations. Hence one σ bond and 1 ∏ bond is formed between 2 O atom. This diagram shows 8 electrons in bonding orbitals and 4 in antibonding orbitals, resulting in a predicted bond order of 2. Total no of electrons in antibonding MO of O2 molecule= 6. Total no of electrons in bonding MO of O2 molecule= 10. The formula through which bond order is calculated is given below:īond Order= (Total no of electrons in bonding Mo-Total no of electrons in antibonding MO)/2. Molecular orbital diagram of O2 Mot O2 bond order ∏ 2py * and ∏ 2pz * each contain 1 electron making a total of 2 electrons in ∏ *Mo’s. ∏ 2py and ∏ 2pz MO’s each contain 2 electrons making a total of 4 electrons in ∏ MO’s. out of which 2 are ∏ 2py and ∏ 2pz and their corresponding antibonding MO’s i.e. Then 2p y and 2p z atomic orbitals of each O atom mixed together to form 4 MO’s. Out of these 2 MO only bonding σ 2px MO is filled with 2 electrons but antibonding σ 2px * MO remains vacant. σ 2px is bonding in nature and σ 2px * MO is antibonding in nature. one 2p x orbital of each O atom combined to form 1 σ 2px, and 1 σ 2px * MO. When 2p orbitals of each O atom are combined total 6 MO’s are formed, each 2p subshell contain 3 atomic orbitals i.e. Similarly σ 2s which is always lower in energy and σ 2s * is always higher in energy. Then 2s orbitals of each O atoms are coupled to form 1 σ 2s bonding MO and 1 σ 2s * antibonding MO. σ 1s bonding MO is lower in energy and σ 1s * MO is higher in energy. Both molecular orbitals contains 2 electrons. In a sigma (σ) orbital, (i.e.O2 bond order diagram Molecular orbital diagram O2 bond orderĪt first, 1s orbital of both O atom are mixed to form 1 bonding MO i.e. ![]()
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