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30/12/2020

the fact that o2 is paramagnetic can be explained by

Gaseous oxygen is paramagnetic also but is moving too fast to be affected by the magnets. Materials that display paramagnetism are called paramagnetic. Oxygen is paramagnetic means , it is attracted by the magnetic field but does not remain magnetic once it leaves the field. I hope you have seen the video of the link I had given you in previous post. Because this measurement is a purely physical effect, nothing is consumed and in principle the cell has an unlimited life. Since paramagnetic has an unpaired electron, it is always alone ! O2 and F2 both stabilise high oxidation states with metal but the tendency is greater in oxygen than fluorine. A further study on the protein itself revealed that crystalline $\ce{HbO2}$ mainly has $\ce{Fe(II)-O2}$ character, whereas solution $\ce{HbO2}$ has $\ce{Fe(III)-O2-}$ character. Paramagnetism, kind of magnetism characteristic of materials weakly attracted by a strong magnet, named and extensively investigated by the British scientist Michael Faraday beginning in 1845. In this way, the MO theory successfully explains the paramagnetic nature of oxygen. I wanted to add in something because it is silly but all my professor's have given our classes tricks to always remember on exams. E) hybridization of atomic orbitals in O2… And let's look at some elements. The person above ^ explained it perfectly. Whereas valence bonding theory predicts that all electrons will be paired, using the molecular orbital theory, you can … It so happens that the molecular orbital description of this molecule provided an explanation for a long-standing puzzle that could not be explained using other bonding models. So let's look at a shortened version of the periodic table. This may leave the atom with many unpaired electrons. All types of materials and substances posses some kind of magnetic properties which are listed further down in this article. the The fact that O2 is paramagnetic can be explained by A) the Lewis structure of O2. It is because O2 bears -2 charges for each oxygen atom while F2 bears only -1 for each atom thus the force of attraction between the metal atom and O2-ion is greater than the force between the same metal atom and F- ion. Therefore, O2 molecule has paramagnetic nature. This capability allows paramagnetic atoms to be attracted to magnetic fields. First observed by S.J. The MG8G paramagnetic oxygen analyzer measures the concentration of oxygen based on the fact that a magnet attracts gaseous oxygen. Paramagnetic and diamagnetic. We can explain the paramagnetic nature of oxygen molecule by molecular orbital theory. Oxygen is a paramagnetic gas and is attracted into a strong magnetic field. (The well-known Meissner Effect is a special example of diamagnetism involving superconductivity). Brugmans (1778) in bismuth and antimony, diamagnetism was named and O2+, O2 and O22 ions O2+, is formed by the loss of one electron from O2 molecule. Diatomic oxygen, \(O_2\) is a good example of paramagnetism (described via molecular orbital theory). Paramagnetic properties are due to the realignment of the electron paths caused by the external magnetic field. When you draw molecular orbital diagram of O 2 we can see there are two unpaired electrons are present in the last molecular orbital which shows us that it is paramagnetic in nature. Incorporating several design improvements, an effective precision of 0.2 ppm O2 from repeated measurements over a 1‐hour interval was achieved. The Molecular Orbital Diagram of oxygen molecule is shown in Fig 35. Whereas zirconia oxygen analyzers cannot measure oxygen in flammable gas mixtures, the MG8G can measure oxygen concentration in flammable gas mixtures. And we can figure out if atoms or ions are paramagnetic or diamagnetic by writing electron configurations. However, true paramagnets display magnetic susceptibility according to the Curie or Curie-Weiss laws and exhibit paramagnetism over a wide temperature range. 19 They therefore concluded that the bonding was multiconfigurational in nature, and that "secondary changes in the protein environment, crystal packing, and so forth, can tip the electronic structure in either direction". d) the molecular-orbital diagram for O 2. e) hybridization of atomic orbitals in O 2. the Lewis structure of O 2 . a violation of the octet rule . Fig 35 M.O diagram for O2 molecule 1. This phenomenon can be explained by the fact that ball-milling treatment can induce large strain levels both in SiO 2 and ε-Fe 2 O 3 lattices, however, the lattice strain in SiO 2 may be effectively released during subsequent alkali-etching process . Answer 1) O2 molecule has two unpaired electrons which is only proved by Molecular orbitals theory (M.O.T). The measurement methods of the oxygen analyzers currently available in the industry can be classified into the following categories. You can determine whether the net effect in a sample is diamagnetic or paramagnetic by examining the electron configuration of each element. Paramagnetism is a form of magnetism whereby some materials are weakly attracted by an externally applied magnetic field, and form internal, induced magnetic fields in the direction of the applied magnetic field. c . Strong paramagnetism (not to be confused with the Paramagnetic materials characteristically align with and strengthen an external magnetic field, while diamagnetic substances partially expel an applied field and always align themselves so that they are perpendicular to its lines of magnetic force. However, you will not be able to observe this paramagnetism at anything but the highest possible fields (I'm only guessing that the required magnetic field is even achievable...but I'll have to do a calculation to make sure). d . resonance . The fact that O 2 is paramagnetic can be explained by (5 points) a) the Lewis structure of O 2. b) resonance. The Molecular Orbital Diagram of oxygen molecule is shown in Fig 35. We now turn to a molecular orbital description of the bonding in \(\ce{O2}\). 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