Complete the Lewis structures for COCI2 and SOCI2 using the skeletal structure shown below, being sure to follow the procedure for minimizing the sum of the absolute values for the formal charges, where the octet rule need not be followed. Based on the complete structures, which statement below is true? [aid Hint: Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons. O The NOCI₂* exhibits both residual formal charges and resonance hybrids, while the BrOCI₂ exhibits formal charges but no resonance hybrids. O No answer text provided. The NOC₂ exhibits both formal charges and resonance hybrids, while the BrOCI₂ exhibits resonance hybrids but no formal charges. O At least one atom in each molecule exhibits formal charges, and the molecules have no resonance hybrids. O The BrOCl₂ exhibits both formal charges and resonance hybrids, while the POCI₂* exhibits resonance hybrids but no formal charges. O The NOC₂ exhibits formal charges but no resonance hybrids, while the BrOCI₂* exhibits both formal charges and resonance hybrids. O The BrOCl₂ exhibits formal charges but no resonance hybrids, while the NOCI₂* exhibits resonance hybrids but no formal charges.
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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