"O"_2 is paramagnetic because it has two unpaired electrons. The quantum number m s represents the magnetic spin of an electron. Assertion: Ozone is a powerful oxidising agent in comparison to O 2. If unpaired electrons are present in an ion/molecule, then it is paramagnetic. The atomic orbitals of the "O" atoms overlap to form the σ and π orbitals of the "O"_2 … Yet oxygen is paramagnetic. iss kinda plain. 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. As shown in the video, molecular oxygen (\(O_2\) is paramagnetic and is attracted to is paramagnetic and is attracted to the magnet. Firstly, let us define the properties of the oxygen we'll be talking about. And, just like nitrogen, each molecule of oxygen behaves like a tiny magnet when it's exposed to a magnet's magnetic field. It shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic. Question: Classify Each Of The Species Given Below As Paramagnetic Or Diamagnetic O2 12 C2 F2 F2 N2 N2 B2 F:2- N2 На C₂2- 0,2- B.2- C2 Nz O, Paramagnetic Diamagnetic Reset < Prev 8 Of 12 !!! If all electrons are paired, then the ion/molecule is diamagnetic The MO electronic configurations are given. Reason : Ozone is diamagnetic but O 2 is paramagnetic. Choose the paramagnetic species from below. A) Ca B) O2⁻ C) Cd2⁺ D) Zn E) Nb3⁺ Nb3⁺ Choose the diamagnetic species from below. O 2 has, in total, 12 valence electrons (each oxygen donating six). I mean "Why is O2 Paramagnetic while N2 Diamagnetic?" In contrast, molecular nitrogen, N2, has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. You might add a video or a related pic or two to grab people interested about everything've got to say. What is Paramagnetic and Diamagnetic ? If it has any unpaired electrons it will be paramagnetic and otherwise it You ought to look at Yahoo's front page and note how they create article headlines to geet viewers interested. For something to be magnetic (we say 'paramagnetic'), it must have an inequality in the total electron spin. Sn2⁺ Choose the paramagnetic species from below. O 2 and O 2 − are paramagnetic while O 3 and O 2 2 − are diamagnetic. In contrast, molecular nitrogen, \(N_2\), has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. You can easily predict the magnetic nature of any molecule/atom by its electronic configuration. Next > This problem has been solved! paramagnetic. (a) Both A and R are true and R is the correct explanation of A (b) Both A and R are true but R is not correct explanation of A The correct explanation comes from Molecular Orbital theory. All materials are at least slightly diamagnetic, but because the effect is so tiny, we don't normally notice it. 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