Paramagnetic: characteristic of unpaired electrons in an atom/ion, attracted into a magnetic field. Step 3: Look for unpaired electrons. If an atom has one or more unpaired electrons, the magnetic dipoles of the unpaired electrons will line up with an applied magnetic field. 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! There is one unpaired electron. Answer: Aluminum (Al) is a Paramagnetic. 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). This is relatively weaker than paramagnetism of materials with unpaired magnetic moments anchored on fixed atoms. Their paramagnetism comes from the spin of conduction electrons, so is strongly limited by the Pauli exclusion principle ("Pauli paramagnetism"). The actual molar mass of your unknown solid is exactly three times larger than the value you determined experimentally. Step 4: Determine whether the substance is paramagnetic or diamagnetic The substance will be paramagnetic. Paramagnetic or Diamagnetic. Thus, NaCl is diamagnetic, because all spins are paired in Na⁺ and in Cl⁻. Step 2: Draw the valence orbitals. Fe, Cr, Cl-, Rb+, Sc+, Ag+, Ar. Therefore, it is not a magnetic molecule. (make sure to take into account the charge) Then slowly fill in the orbitals and check if the end result has unpaired electrons. For Cl atoms, the electron configuration is 3s 2 3p 5. (2) Be^- :[He] 2s^1; one unpe⁻ : paramagnetic. Its MOLECULAR ORBITAL ELECTRONIC CONFIGURATION shows that it has all electrons paired, so it is DIAMAGNETIC. The metals I mentioned above all have both diamagnetic and paramagnetic contributions. Therefore, Ni 2+ undergoes sp 3 hybridization to make bonds with Cl-ligands in tetrahedral geometry. *Response times vary by subject and question complexity. Ignore the core electrons and focus on the valence electrons only. Q: A chemist adds 0.30 L of a 0.865 mol/L iron(II) bromide (FeBr,) solution to a reaction flask. 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. ? Almost all main group compounds (ns np valence electrons) are diamagnetic. As there are unpaired electrons in the d-orbitals, NiCl 4 2-is paramagnetic and is referred to as a high spin complex. Diamagnetic has no unpaired e-, while paramagnetic does. All of the electrons in its molecular orbitals are paired up. Median response time is 34 minutes and may be longer for new subjects. 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