Water has no unpaired electrons and is thus diamagnetic. A molecule will be paramagnetic (attracted into a magnetic field) if is has one or more unpaired electrons. The bond order of one suggests that the fluorine molecule is stable. The gases N2 and H2 are weakly diamagnetic with susceptibilities -0.0005 x 10-5 for N2 and -0.00021 x 10-5 for H2. Classify these diatomic molecules as diamagnetic or paramagnetic: O2, B2, F2, C2, N2 Source(s): classify diatomic molecules diamagnetic paramagnetic: https://biturl.im/5AbXk Since each atom has one electron, there are two electrons in H₂. paramagnetic ion. When we go back over to "N"_2, since "N" has one less electron than "O" in its atomic orbitals, "N"_2 has two less electrons than "O"_2 in its molecular orbitals. Use MO theory: A) H2: 2e- : σs(2e-) no unpaired electrons, diamagnetic The units are in B.M. Draw block diagram structures for all possible products of the partial hydrogenation, with two molecules of H2,... General, Organic, and Biological Chemistry The following six questions concern Rebecca, who is 36 years old, weighs 182 lb, and is 5 ft 4 in. 4. And let's look at some elements. Bond Order = 1/2(10 - 8) = 1. The two unpaired electrons show that O 2 is paramagnetic. The diamagnetic corrections (Bohr Magnetons), which is a unit of magnetic moment and equal to eh /4 πmc = 9.27 ×10-21 erg/gauss. Click hereto get an answer to your question ️ Among H2 , He2^+ , Li2 , Be2 , B2 , C2 , N2 , O2^- , and F2 , the number of diamagnetic species is (Atomic numbers: H = 1 , … And let's figure out whether those elements are para- or diamagnetic… Paramagnetic and diamagnetic. And we can figure out if atoms or ions are paramagnetic or diamagnetic by writing electron configurations. tall. The χa is the atomic susceptibility corrected for the diamagnetic components of the ligands and associated ions. "O"_2 is paramagnetic, with one electron each in its pi_(2p_x)^"*" and pi_(2p_y)^"*" antibonding molecular orbitals. Active 6 years ago. Viewed 9k times 2 $\begingroup$ I read something recently that said "BN has been observed in the gas phase, is paramagnetic, and has a vibrational frequency lower than N2. It's O2 that has two unpaired electrons (in the [tex]\pi^*_x[/tex] and [tex]\pi^*_y[/tex] molecular orbitals), and is thus paramagnetic. Recall that paramagnetic means it contains at least one unpaired electron and diamagnetic is the lack thereof. Is He_2+ Paramagnetic Of Diamagnetic? Draw The Molecular Orbital Diagram For Each And Explain Your Answer. How can BN be paramagnetic? Click hereto get an answer to your question ️ Among the following molecules/ions, C^2 - 2, N^2 - 2, O^2 - 2, O2 which one is diamagnetic and has the shortest bond length? T N k T A A eff ' 2 ' 2.84 3 χ β χ µ = = B.M. Which, (for the benefit of the original poster), means it's even less magnetic than that - about as un-magnetic as a substance can get. Hydrogen, except at quite high temperatures, is diatomic: it consists of H₂ molecules. F 2 has a bond order of 1. Ask Question Asked 6 years ago. Because all of the electrons are paired, F 2 is diamagnetic… These properties can be explained by the molecular orbital diagram of BN". The gases N 2 and H 2 are weakly diamagnetic with susceptibilities -0.0005 x 10-5 for N 2 and -0.00021 x 10-5 for H 2. The molecular orbital diagram for a diatomic fluorine molecule, F 2, is. Stat tuned with BYJU’S to learn more about magnetism and diamagnetism with the help of interactive video lessons. Question: Use Molecular Orbital Theory To Determine Whether He2 Or He2+ Is More Stable. So let's look at a shortened version of the periodic table. -0.0005 x 10-5 for H2 BN '' magnetism and diamagnetism with the of... 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