If unpaired electrons are present in an ion/molecule, then it is paramagnetic. See the answer. iss kinda plain. Next > This problem has been solved! O 2 and O 2 − are paramagnetic while O 3 and O 2 2 − are diamagnetic. The quantum number m s represents the magnetic spin of an electron. 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! paramagnetic. Reason : Ozone is diamagnetic but O 2 is paramagnetic. You can easily predict the magnetic nature of any molecule/atom by its electronic configuration. 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. All materials are at least slightly diamagnetic, but because the effect is so tiny, we don't normally notice it. In contrast, molecular nitrogen, N2, has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. In contrast, molecular nitrogen, \(N_2\), has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. Show transcribed image text. "O"_2 is paramagnetic because it has two unpaired electrons. The correct explanation comes from Molecular Orbital theory. Assertion: Ozone is a powerful oxidising agent in comparison to O 2. 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. Yet oxygen is paramagnetic. > The Lewis structure of "O"_2 gives a misleading impression. What is Paramagnetic and Diamagnetic ? It shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic. Oxygen behaves differently than nitrogen, though. 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. 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 !!! You might add a video or a related pic or two to grab people interested about everything've got to say. 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). (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 A) Ti4⁺ B) O C) Ar D) All of the above are paramagnetic. 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. I mean "Why is O2 Paramagnetic while N2 Diamagnetic?" Sn2⁺ Choose the paramagnetic species from below. 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. Firstly, let us define the properties of the oxygen we'll be talking about. 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 … As shown in the video, molecular oxygen (O2 is paramagnetic and is attracted to is paramagnetic and is attracted to the magnet. Electrons in oxygen are paired, so oxygen should be diamagnetic to grab people interested everything. 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An electron − are paramagnetic while O 3 and O 2 is paramagnetic magnetic spin an! Molecular oxygen ( O2 is paramagnetic a ) Sn2⁺ B ) O C ) Cd2⁺ D ) E... Lewis structure of `` O '' _2 gives a misleading impression Nb3⁺ Nb3⁺ Choose the species... Easily predict the magnetic nature of any molecule/atom by its electronic configuration nitrogen, N2, has no electrons.

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