Relevance. So, the bond order is zero. 2 Answers. (a) Is O2 stable or unstable? In the case of the hydrogen molecule, the bond length is 74 pm. According to it's molecular orbital configuration, Be+2 is paramagnetic and its bond order is zero so it is considered to be unstable. Answer. Two superpositions of these two orbitals can be formed, one by summing the orbitals and the other by taking their difference. B2 is a known molecule in gas phase, although not very stable, whose existence has been predicted in terms of MOT because it has a Bond Order greater than zero (in the case of B2, the bond order is 1).Ah, the B2 molecule does not complete its octet indeed. Take out one electron from the sigma_"2s"^"*" in this diagram: Return to … 32) Given that O2 is paramagnetic and has a bond order of 2, and its highest occupied molecular orbital is antibonding, what would be the expected bond orders for O22- and O22+? Expert Answer: According to Molecular Orbital theory, only those molecule can exists which have net positive bond order while the molecules with negative or zero bond order will not exists. Top. According to J.D Lee, compounds with fraction bond number are unstable--Li2+ BOND ORDER = 0.5 Li2 BOND ORDER =1 Hence Li2+ must be unstable than Li2 but then why Li2 is more stable than Li2+. Even rather simple molecular orbital (MO) theory can be used to predict which homonuclear diatomic species – H 2, N 2, O 2, etc. Its molecular orbitals are constructed from the valence-shell orbitals of each hydrogen atom, which are the 1s orbitals of the atoms. which response lists all the following diatomic molecules and ions that are paramagnetic (Be2, B2, B2+2, C2+2, C2-2, O2-, O2-2) B2, C2+2, and O2 which response lists all the following diatomic molecules and ions that have at least one unpaired electron (Be2, B2, B2+, C2, N2, N2+) Is Be2+ stable or unstable? 5 years ago. The species in which the N atom is in a state of sp hybridization is: NO. 3- H 2 is the most stable because it has the highest bond order (1), in comparison with the bond orders (1/2) of H 2 + and H 2-. Bond order is an index of bond strength and is used extensively in valence bond theory. C2+1. = 1 stable diamagnetic b. It depends on what isotope you are talking about. O 2 + is more stable than O 2-.Because According to molecular orbital theory O 2 + has 15 electrons &it has one electron in antibonding orbital. 0 0. Key Terms. 1 0. Anonymous. 2 Answers. Whereas Be− is unstable with respect to electron detachment, Be2, Be3, and Be4, posses stable negative ions. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. A: No, Be2 is not expected to be stable according to molecular orbital theory. According to it's molecular orbital configuration, Be+2 is paramagnetic and its bond order is zero so it is considered to be unstable. Bond Order=2(bonding electrons)−0(anti−bonding e−)2=1. Which homonuclear diatomic molecules or ions of the second period have the following electron distributions in MOs? In other words, identify X in each of the following cases: X Electron Distributions Species X2. B2-1. ANSWERS TO MOLECULAR ORBITALS PROBLEM SET 1. Ask your question! 74 pm) because the potential enthalpy of the system increases and curve shows an upward trend (dotted lines) and molecule becomes unstable. Top. molecular orbital diagram of O 2 + Electronic configuration of O 2 + In the case of O 2-17 electrons are present &3 electrons are present in antibonding orbitals. In He2 (dihelium), the two 1s atomic orbitals overlap to create two molecular orbitals: sigma(1s) and sigma(1s)*. Molecular Orbital Diagram – Cl2, Br2, I2 3s & 3p and higher atomic orbitals are not so widely separated in energy and allow significant mixing (hybridization) to occur. This means that it has 2 electrons in its last layer. He 2 B.O. Get your answers by asking now. Is Be2+ stable or unstable? Favorite Answer. Still have questions? The following MO diagram is appropriate for Li2 and Be2. A bonding molecular orbital is always lower in energy (more stable) than the component atomic orbitals, whereas an antibonding molecular orbital is always higher in energy (less stable). C) Be2 is stable and diamagnetic, but Li2 is unstable. You are wrong. Ask Question + 100. Part of this theory is the concept of bond order which gauges whether a molecular bond would be stable or unstable. It is a paramagnetic diradical. If number of electrons more in antibonding orbital the molecule become unstable. Beryllium-9 is stable, and thus, not radioactive. The MOs for the valence orbitals of the second period are shown in Figure 8.37. Please explain reasons. You are wrong. (a) N2 +(13 e-): σ2 1sσ*21sσ22sσ*22sπ22pπ22pσ12p N2 2+(12 e-): σ2 1sσ*21sσ22sσ*22sπ22pπ22p N2 (14 e-): σ2 1sσ*21sσ22sσ*22sπ22pπ22pσ22p N2-(15 e-): σ21sσ*21sσ22sσ*22sπ22pπ22pσ22pπ*12p N2 2-(16 e-): σ21sσ*21sσ22sσ*22sπ22pπ22pσ22pπ*12pπ*12p (b) Bond orders are: N2 + = 2.5 ; N 2 2+ = 2.0 ; N explain, molecular orbital diagram ... the molecule is stable If Nb=Na, the molecule is unstable If Nb