You can easily predict the magnetic nature of any molecule/atom by its electronic configuration. A) Ca B) O2⁻ C) Cd2⁺ D) Zn E) Nb3⁺ Nb3⁺ Choose the diamagnetic species from below. 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 !!! Show transcribed image text. And, just like nitrogen, each molecule of oxygen behaves like a tiny magnet when it's exposed to a magnet's magnetic field. "O"_2 is paramagnetic because it has two unpaired electrons. If it has any unpaired electrons it will be paramagnetic and otherwise it Next > This problem has been solved! I mean "Why is O2 Paramagnetic while N2 Diamagnetic?" Reason : Ozone is diamagnetic but O 2 is paramagnetic. As shown in the video, molecular oxygen (O2 is paramagnetic and is attracted to is paramagnetic and is attracted to the magnet. paramagnetic. For something to be magnetic (we say 'paramagnetic'), it must have an inequality in the total electron spin. You might add a video or a related pic or two to grab people interested about everything've got to say. All materials are at least slightly diamagnetic, but because the effect is so tiny, we don't normally notice it. 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. If unpaired electrons are present in an ion/molecule, then it is paramagnetic. Steve: Just like nitrogen, oxygen isn't normally magnetic. O 2 and O 2 − are paramagnetic while O 3 and O 2 2 − are diamagnetic. See the answer. A) Ti4⁺ B) O C) Ar D) All of the above are 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 If all electrons are paired, then the ion/molecule is diamagnetic The MO electronic configurations are given. Sn2⁺ Choose the paramagnetic species from below. iss kinda plain. In contrast, molecular nitrogen, N2, has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. Paramagnetic molecules get attracted towards external magnetic field and diamagnetic repel the external magnetic field. The correct explanation comes from Molecular Orbital theory. You ought to look at Yahoo's front page and note how they create article headlines to geet viewers interested. A) Sn2⁺ B) Br C) P D) Cr E) None of the above are diamagnetic. Choose the paramagnetic species from below. The atomic orbitals of the "O" atoms overlap to form the σ and π orbitals of the "O"_2 … Assertion: Ozone is a powerful oxidising agent in comparison to O 2. > The Lewis structure of "O"_2 gives a misleading impression. O 2 has, in total, 12 valence electrons (each oxygen donating six). Diamagnetic Up to date, curated data provided by Mathematica 's ElementData function from Wolfram Research, Inc. Click here to buy a book, photographic periodic table poster, card deck, or 3D print based on the images you see here! In contrast, molecular nitrogen, \(N_2\), has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. It shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic. As shown in the video, molecular oxygen (\(O_2\) is paramagnetic and is attracted to is paramagnetic and is attracted to the magnet. What is Paramagnetic and Diamagnetic ? Firstly, let us define the properties of the oxygen we'll be talking about. 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