8. The paramagnetic nature of O 2 is due to unpaired electrons. ... NEET 2020 Chemical Bonding and Molecular Structure. O 2 has, in total, 12 valence electrons (each oxygen donating six). The lowest excited state of the diatomic oxygen molecule is a singlet state.It is a gas with physical properties differing only subtly from those of the more prevalent triplet ground state of O 2.In terms of its chemical reactivity, however, singlet oxygen is far more reactive toward organic compounds. So these are diamagnetic. On electrolysis of dil.sulphuric acid using Platinum (Pt) electrode, the product obtained at anode will be: "O"_2 is paramagnetic because it has two unpaired electrons. Explanation: CN-, CO and NO + are isoelectronic with 14 electrons each and there is no unpaired electrons in the MO configuration of these species. B2 = 5 + 5 = 10e-= σ1s2 σ1s2 , σ2s2 σ2s2 , π2px1 π2py1Due to the presence of unpaired electrons, in π bonding orbitals, B2 shows paramagnetic behaviour. The common allotrope of elemental oxygen on Earth, O 2, is generally known as oxygen, but may be called dioxygen, diatomic oxygen, molecular oxygen, or oxygen gas to distinguish it from the element itself and from the triatomic allotrope ozone, O 3.As a major component (about 21% by volume) of Earth's atmosphere, elemental oxygen is most commonly encountered in the diatomic form. If the supply of oxygen is limited, $ {{H}_{2}}S $ reacts with $ {{O}_{2}} $ to form. NO 2 is paramagnetic due to the presence of unpaired electron on the nitrogen atom. 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. > The Lewis structure of "O"_2 gives a misleading impression. Due to their spin, unpaired electrons have a magnetic dipole moment and act like tiny magnets. It shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic. The quantum number m s represents the magnetic spin of an electron. Firstly, let us define the properties of the oxygen we'll be talking about. In contrast, molecular nitrogen, \(N_2\), has no unpaired electrons and is diamagnetic; it is therefore unaffected by the magnet. The atomic orbitals of the "O" atoms overlap to form the σ and π orbitals of the "O"_2 molecule … O-2 is paramagnetic due to the presence of one unpaired electron. As shown in the video, molecular oxygen (\(O_2\) is paramagnetic and is attracted to is paramagnetic and is attracted to the magnet. We now turn to a molecular orbital description of the bonding in \(\ce{O2}\). The correct explanation comes from Molecular Orbital theory. Correct option (a) O-2. Molecular Oxygen is Paramagnetic. The paramagnetic property of the oxygen molecule is due to the presence of unpiared electrons present in . NEET 2020 Chemical Bonding and Molecular Structure 8. Therefore, oxygen has two unpaired electrons and is paramagnetic. 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