Their paramagnetism comes from the spin of conduction electrons, so is strongly limited by the Pauli exclusion principle ("Pauli paramagnetism"). Among Cl 2, Cl 2-, Cl 2 +, paramagnetic species are Cl 2-, Cl 2 +.This can be explained according to MOLECULAR ORBITAL THEORY as follows: Cl 2 has two chlorine atoms each with 17 electrons, therefore total electrons are 34(17+17). If an atom has one or more unpaired electrons, the magnetic dipoles of the unpaired electrons will line up with an applied magnetic field. Q: A chemist adds 0.30 L of a 0.865 mol/L iron(II) bromide (FeBr,) solution to a reaction flask. Step 4: Determine whether the substance is paramagnetic or diamagnetic All of the electrons in its molecular orbitals are paired up. Cl Titanium ( ti ) Diamagnetic List C2 Potassium Ne2 CO silicon sulfur neon ( Ne ) h2 hydrogen zinc zn si helium ( he ) beryllium Nitrogen N2 be2 carbon s2 ag Copper zn2+ cu V3+ Cadmium ... Is Aluminum (Al) a Paramagnetic or Diamagnetic ? (2) Be^- :[He] 2s^1; one unpe⁻ : paramagnetic. For Cl atoms, the electron configuration is 3s 2 3p 5. *Response times vary by subject and question complexity. Therefore, Ni 2+ undergoes sp 3 hybridization to make bonds with Cl-ligands in tetrahedral geometry. Answer: Aluminum (Al) is a Paramagnetic. Fe, Cr, Cl-, Rb+, Sc+, Ag+, Ar. Step 2: Draw the valence orbitals. The magnetic moments cancel, and the substance is diamagnetic. Almost all main group compounds (ns np valence electrons) are diamagnetic. ? Add up the amount bonding valence electrons it has. The actual molar mass of your unknown solid is exactly three times larger than the value you determined experimentally. diamagnetic: all the electrons are paired. The Cl2 molecule is diamagnetic. Ignore the core electrons and focus on the valence electrons only. Diamagnetic has no unpaired e-, while paramagnetic does. The substance will be paramagnetic. Step 3: Look for unpaired electrons. (make sure to take into account the charge) Then slowly fill in the orbitals and check if the end result has unpaired electrons. Therefore, it is not a magnetic molecule. Diamagnetic characteristic of an atom/ion where electrons are paired. Paramagnetic 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! Its MOLECULAR ORBITAL ELECTRONIC CONFIGURATION shows that it has all electrons paired, so it is DIAMAGNETIC. Obtain the electron configuration of the element from Wikipedia and add and subtract electrons to give the appropriate io (1) Cl^- : [Ne]3s^2 3p^6 ; all electrons paired: diamagnetic. The metals I mentioned above all have both diamagnetic and paramagnetic contributions. Paramagnetic or Diamagnetic. Paramagnetic: characteristic of unpaired electrons in an atom/ion, attracted into a magnetic field. 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