Draw all possible resonance structures for SO2, SO,, and SO. Use the resonance structures to solve the problems below. (a) Arrange these species in order of increasing S-O bond length (shortest bond first). O S03²- O SO O SO O SO2 O SO2 O SO O So;²- O SO2 (b) Match each species with the number of covalent bonds predicted by Lewis structures to exist between an S atom and an O atom bonded to this S atom. (Hint: Average the number of bonds between S and an attached oxygen atom in a particular position using all of your resonance structures for the species that you are working on.) So: -Select-v bonds between S and 0. SO,:-Select--- ♥ bonds between S and 0. Select-v bonds between S and O. (c) Match each species with the correct formal charge on the central S atom. So: -Select-v charge on S. SO2: -Select-v charge on S. So,²:Select- charge on S. (d) Match each species with the average formal charge on an outside oxygen atom predicted by Lewis structures. So: -Select-v average charge on outside O atom. Select-vaverage charge on outside O atom. SO2: SO3: -Select-- ♥ average charge on outside O atom.
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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