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