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