WebDec 21, 2024 · 1) H2- 2) H2+ 3) H2 4) He2+. A species is said to be diamagnetic when it has all the paired electrons. Similarly if the species contain unpaired electron it is said to be paramagnetic. To know the magnetic character of molecules we can use MO diagram. When we draw MO diagram for dihydrogen anion ( H2-) we find one unpaired electron in ... WebOct 27, 2024 · To summarize, diamagnetic refers to paired electrons in an orbital, whereas paramagnetic refers to an unpaired electron in an orbital. To solve these problems, I …
Are the following ions diamagnetic or paramagnetic? - Socratic
WebQuestion: 1. (2.0 point) Determine whether each of the following ions is diamagnetic or paramagnetic. a.S2- b. Fe3+ to receive full credit for this question, you must show the following steps: a) Write the short-hand electron configuration of the neutral atom. (0.2 points for each atom) b) write the short-hand electron configuration of the ion ... WebFour complexes containing Dy(III) and Pr(III) ions and their Ln(III) -Zn(II) analogs have been synthesized in order to study the influence that a diamagnetic Zn(II) ion has on the electronic structure and hence, the magnetic properties of the Dy(III) is freelance data entry jobs genuine
is S2 is he paramagnetic or diamagnetic - BYJU
WebApr 15, 2013 · Which one of the following molecules is expected to exhibit diamagnetic behaviour ? (1) C2 (2) N2 (3) O2 (4) S2 why. Asked by TARUN Garg 15 Apr, 2013, 03:17: PM Expert Answer So, C 2 and N 2 are diamagnetic in nature since they have no unpaired electrons. Answered by 16 Apr, 2013, 10:04: AM Application Videos ... http://dentapoche.unice.fr/keep-on/is-f2-paramagnetic-or-diamagnetic WebIn vapour state, sulphur (S 2) shows paramagnetic behaviour due to: A presence of one unpaired electron in the antibonding σ orbitals B presence of two unpaired electrons in the bonding π orbitals C presence of one unpaired electron in the antibonding π orbitals D presence of two unpaired electrons in the antibonding π orbitals Medium Solution s20 sim free deals