Which of the following species is diamagnetic (not paramagnetic): Li, V, Ni, Zn, Fe²+ H Не yen 10 Li Be B Ne 2010 mages 12 sodum 11 13 14 16 16 17 18 Na Mg AI Si s ci Ar tromi 35 19 20 21 22 23 24 27 28 31 32 33 34 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 37 41 42 44 45 47 49 51 52 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe थ 50 12 57-70 71 72 73 14 75 76 77 78 79 81 82 83 84 85 86 Cs Ba Lu Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn 87 89-102 104 105 106 107 108 110 111 112 114 Fr Ra ** Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uuq 57 60 61 SUPVma 62 63 64 65 70 67 "Lanthanide series La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 17 *Actinide series 90 91 92 $4 95 97 98 99 100 101 102 Ac Th Pa Np Pu Am Cm Bk Cf Es Fm Md No Select one: O a. Li O b. V O. Zn Od. Fe2+ O e. Ni
Formal Charges
Formal charges have an important role in organic chemistry since this concept helps us to know whether an atom in a molecule is neutral/bears a positive or negative charge. Even if some molecules are neutral, the atoms within that molecule need not be neutral atoms.
Polarity Of Water
In simple chemical terms, polarity refers to the separation of charges in a chemical species leading into formation of two polar ends which are positively charged end and negatively charged end. Polarity in any molecule occurs due to the differences in the electronegativities of the bonded atoms. Water, as we all know has two hydrogen atoms bonded to an oxygen atom. As oxygen is more electronegative than hydrogen thus, there exists polarity in the bonds which is why water is known as a polar solvent.
Valence Bond Theory Vbt
Valence bond theory (VBT) in simple terms explains how individual atomic orbitals with an unpaired electron each, come close to each other and overlap to form a molecular orbital giving a covalent bond. It gives a quantum mechanical approach to the formation of covalent bonds with the help of wavefunctions using attractive and repulsive energies when two atoms are brought from infinity to their internuclear distance.
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