You can easily predict the magnetic nature of any molecule/atom by its electronic configuration. All of the electrons are spin-paired in diamagnetic elements so their subshells are completed, causing them to be unaffected by magnetic fields. Table 1: Magnetic moments of homonulcear and heteronuclear diatomic species; Species (Molecules or ions) Total Number of electrons. Answer (a): The O atom has 2s 2 2p 4 as the electron configuration. Therefore, a simple rule of thumb is used in chemistry to determine whether a particle (atom, ion, or molecule) is paramagnetic or diamagnetic: If all electrons in the particle are paired, then the substance made of this particle is diamagnetic; If it has unpaired electrons, then the substance is paramagnetic. Chapter 9.3, Problem 4RC. As all the electrons are now paired, CN- is diamagnetic (it is weakly repelled by a magnetic field). Why don't libraries smell like bookstores? Relevance. Since it posses 2 unpaired electrons, it is Paramagnetic in nature. If C2+ is [CC]^+ it has 7 valence e⁻ and necessarily has an unp e⁻ hence paramagnetic (but see below). which o the following diatomic species are paramagnetic and which are diamagnetic? Click hereto get an answer to your question ️ Assuming that Hund's rule is violated, the bond order and magnetic nature of the diatomic molecule B2 is: Is CN- paramagnetic or diamagnetic. I would say B2- is paramagnetic, since when you draw the molecular bond diagram you get an unpaired electron All Chemistry Practice Problems Bond Order Practice Problems. If you want to quickly find the word you want to search, use Ctrl + F, then type the word you want to search. True or false ? arrow_back. Who is the longest reigning WWE Champion of all time? H 2 + 1. 4 years ago. Answer Save. Magnetic property: Since bond order is zero, Be 2 molecule does not exist. arrow_back. you need to write the molecular orbital configuration of B2 = [ sigma (1s) ]^2 [ sigma*(1s) ]^2 [ sigma(2s) ]^2 [ sigma*(2s) ]^2 [ π(2px) ]^1 [ π(2py) ]^1. Any time two electrons share the same orbital, their spin quantum numbers have to be different. Explanation: We can work this out by looking at the molecular orbital diagram of O2 O2 (2+) has two fewer electrons than O2 which is what it gives it positive charge. As another example of this, you mention that lead is diamagnetic. Want to see this answer and more? (a) O 2 (b) B 2 (c) C 2 (d) N 2 + check_circle Expert Solution. paramagnetic. molecular bond diagram you get an unpaired electron. arrow_forward. If you want to quickly find the word you want to search, use Ctrl + F, then type the word you want to search. Answer: B2 2- is a Diamagnetic What is Paramagnetic and Diamagnetic ? Show Answer Hide Answer; Workspace ; Answer : Explanation : B2+ is a Paramagnetic. The two boron atom is B2 molecules are linked by one covalent bond. 1) and * orbital can have maximum of 2 electrons and * orbital can have maximum of 4 electrons 1 F atom have 9 electrons … It is also described as the property of a substance which is equal to the magnetic flux density established inside the material. drakepwgreen PLUS. Table 1: Magnetic moments of homonulcear and heteronuclear diatomic species; Species (Molecules or ions) Total Number of electrons. Answer: B2 2- is a Diamagnetic What is Paramagnetic and Diamagnetic ? I would say B2- is paramagnetic, since when you draw the molecular bond diagram you get an unpaired electron Basically, know your isoelectronic species: #"O"_2^(2+)#, #"CO"#, #"NO"^(+)#, and #"CN"^(-)# are all diamagnetic with zero #pi^"*"# antibonding electrons. Hey guys! Want to see this answer and more? Solution for Classify these diatomic molecules as diamagnetic or paramagnetic: B2, O2, F2, N2, C2 Magnetism origin lies in the spin motion and orbital of the electrons and also the interaction of electrons with each other. Question: Is B2 2- a Paramagnetic or Diamagnetic ? The other two are diamagnetic. electronic configuration of B2 molecule isB2: [KK (σ2s)2 (σ2s)2 (2px)1(2py)1]Since each 2px and 2py MO contains unpaired electron, therefore B2 molecule is paramagnetic. 1) and * orbital can have maximum of 2 electrons and * orbital can have maximum of 4 electrons 1 F atom have 9 electrons … Favorite Answer. Therefore, Br has 1 … The M.O. Number of unpaired electrons (n) Magnetic moment (μs) in Bohr Magneton (\(\mu_B\)) Magnetic Behavior. Which is the light metal available with better Hardness ? Q. paramagnetic are those elements which have one unpaired electrons while diamagnetic have paired electrons . Marks 8 How many valence electrons in the O 2 molecule? 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