C2+1. Take out one electron from the sigma_"2s"^"*" in this diagram: Diberyllium is thought to be non-existant. Asked by Aashna Anith Kumar | 4th Feb, 2014, 11:50: PM. Favorite Answer. Ask Question + 100. B2. Be2 is stable and paramagnetic, but Li2 is unstable. Re: Why is He2 not a stable molecule? Two superpositions of these two orbitals can be formed, one by summing the orbitals and the other by taking their difference. The MOs for the valence orbitals of the second period are shown in Figure 8.37. Both stable and unstable isotopes of beryllium are created in stars, but the radioisotopes do not last long. 1 Answer to li2 is stable but be2 is not stable . Answer Save. It should be noted that two hydrogen atoms can not be brought at a distance lesser than r Q (i.e. 2 Answers. Stable bonds have a positive bond order. The species in which the N atom is in a state of sp hybridization is: NO. 1 0. Post by Armo_Derbarsegian_3K » Thu Nov 17, 2016 6:10 am . Paramagnetic According to MO theory, the bond order is 1/2 and "Be"_2 has two bonding electrons with one antibonding electron. Whereas Be− is unstable with respect to electron detachment, Be2, Be3, and Be4, posses stable negative ions. A: No, Be2 is not expected to be stable according to molecular orbital theory. bond stability. 1 decade ago. It is stable. The following MO diagram is appropriate for Li2 and Be2. Anonymous. Ask Question + 100. Still have questions? Ask your question! An atom is more stable when its outer shell of electrons is full, as in the case of noble gases. 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. This means there is no bond, hence no stability as a molecule. C) Be2 is stable and diamagnetic, but Li2 is unstable. Still have questions? (a) Na22+ (b) Mg22+ (c) Al22+ (d) Si22+ (e) P22+ (f) S22+ (g) F22+ (h) Ar22+ Determine the bond order of each member of the following groups, and determine which member of each group is predicted by the molecular orbital model to have the strongest bond. However, this is not always the case. 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. Bond Order=2(bonding electrons)−0(anti−bonding e−)2=1. Anonymous. In other words, identify X in each of the following cases: X Electron Distributions Species X2. Predict the valence electron molecular orbital configurations for the following, and state whether they will be stable or unstable ions. 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. Get your answers by asking now. 2 Answers. = 0 unstable diamagnetic σ 1s ∗ σ 1s σ 1s. Return to … Thus, $\ce{Li2}$ should have been more stable than $\ce{B2}$ if we consider the number of electrons in the antibonding molecular orbital as the parameter of stability. Answer: be2 is a Diamagnetic What is Paramagnetic and Diamagnetic ? Armo_Derbarsegian_3K Posts: 35 Joined: Sat Jul 09, 2016 10:00 am. 2 posts • Page 1 of 1. 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+? Li2 is stable and diamagnetic, but Be2 is unstable. You are wrong. 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-. (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 Top. In He2 (dihelium), the two 1s atomic orbitals overlap to create two molecular orbitals: sigma(1s) and sigma(1s)*. = 1 stable diamagnetic b. 1 decade ago. Its molecular orbitals are constructed from the valence-shell orbitals of each hydrogen atom, which are the 1s orbitals of the atoms. 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). 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+) 74 pm) because the potential enthalpy of the system increases and curve shows an upward trend (dotted lines) and molecule becomes unstable. Is Be2+ stable or unstable? Explanation: Beryllium is the first element of Group 2 and. 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. It is believed that most of the stable beryllium in the universe was originally created in the interstellar medium when cosmic rays induced fission in heavier elements found in interstellar gas and dust. share | improve this question | follow | edited Apr 15 '17 at 19:58. airhuff. Li2+ is more stable than Li2− because Li2− has more numbers of antibonding electrons. So, the bond order is zero. You are wrong. Paramagnetic Paramagnetism is a form of magnetism whereby certain materials are weakly attracted by an externally applied magnetic field, and form internal, induced magnetic fields in the direction of the applied magnetic field. steviemarivie. Beryllium-9 is stable, and thus, not radioactive. explain, molecular orbital diagram ... the molecule is stable If Nb=Na, the molecule is unstable If Nb