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Because there are no unpaired electrons, Zn atoms are diamagnetic. Here, for H2 the number of unpaired electron is 0. An atom could have ten diamagnetic electrons, but as long as it also has one paramagnetic electron, it is still considered a paramagnetic atom. O$_2$, and NO. Tell whether each is diamagnetic or paramagnetic. You cannot really work it out from the valence electronic structure. Only NO^- is the paramagnet, so "option A". Para magnetic ( Those who have unpaired electrons in last shell) Diamagnetic ( U know those who have paired) C2+ & C2- are paramagnetic! The F-ion has 2s 2 2p 6 has the electron configuration. Paramagnetic materials, those with unpaired electrons, are attracted by magnetic fields whereas diamagnetic materials, those with no unpaired electrons, are weakly repelled by such fields. Here is a breakdown of each classification. An atom is considered paramagnetic if even one orbital has a net spin. In our beautiful universe, most elements are considered paramagnetic, ferromagnetic, or diamagnetic. The key difference between paramagnetic and diamagnetic materials is that the paramagnetic materials get attracted to external magnetic fields whereas the diamagnetic materials repel from the magnetic fields.. Materials tend to show weak magnetic properties in the presence of an external magnetic field.Some materials get attracted to the external magnetic field, whereas some … Jul 25, 2007 58 0 Status Pre-Dental Jul 31, 2009 #6 That being said, the magnetic properties don’t stay within the elements once the magnet is removed. e.g. Classify these diatomic molecules as diamagnetic or paramagnetic: O2, B2, F2, C2, N2 Source(s): classify diatomic molecules diamagnetic paramagnetic: https://biturl.im/5AbXk By constructing a molecular orbital picture for each of the following molecules, determine whether it is paramagnetic or diamagnetic. Step 4: Determine whether the substance is paramagnetic or diamagnetic. However, molecules with an even number of electrons can also be paramagnetic, the most famous being dioxygen (O$_2$). Paramagnetic Elements – These items have a small, weak attraction to magnets. NO^- has 5+6+1=12*"valence electrons"; ""^(-)C-=N has 4+5+1=10*"valence electrons"; ""^(-)C-=O^+ has 4+6=10*"valence electrons". But in option 3 in H2 there's no unpaired electron. Paramagnetism is a consequence of having one or more un-paired electrons in the outer electronic configuration. For O=O we also have "12 valence electrons": And thus highest occupied molecular orbitals are the … (paramagnetic transition and inner transtion metal ions), orbital filling footnotes (elemental dioxygen), or nitrogen (for its odd number of electrons) and some pluck (NO, NO2 monomer, DPPH, TEMPO; nitronyl nitroxides, verdazyls, etc.). This is something you know or you don't know. Number of valance electrons in N O + = 5 + 6 − 1 = 1 0 All electrons can be paired up and there is no free electron. A paramagnetic electron is an unpaired electron. But in all other case there's an unpaired electron. Give the number of unpaired electrons of the paramagnetic … Answer. Diamagnetic … R. ResidentPersian. For diamagnetic character, there should not be any unpaired electron in the molecules formation. Because it has no unpaired electrons, it is diamagnetic. Exercise \(\PageIndex{2}\) Indicate whether F-ions are paramagnetic or diamagnetic. Depict high spin and low spin configurations for each of the following complexes. An an odd number of electrons can clearly produce a paramagnetic ion, radical or molecule. N O 2 + molecule is therefore diamagnetic. Isn't paramagnetic one arrow and diamagnetic 2 arrow in an orbital? In non-stoichiometric low density, paramagnetic free … Let it be H2- ,H2+ or He2+ ; there's an unpaired electron i.e, they are paramagnetic. 10+ Year Member. 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