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.
Draw the Lewis structure of acetic acid, CH3CO2H, clearly indicating all non-bonding pairs of electrons.
Even though nitrogen and phosphorus have the same number of valence electrons, nitrogen can only bond to chlorine four times forming NCl4+ but phosphorus can bond with chlorine five times forming PCl5. Explain.
Draw all the isomers of C4H9Br, using bond-line formulas.
Draw the Lewis structure of the nitrite ion, NO2–, clearly indicating resonance contributors as well as non-bonding pairs of electrons and formal charges, as relevant.
Nitromethane is a polar molecule but contains 2 equal polar covalent bonds. Briefly explain why and draw a relevant 3-dimensional structure to show the overall dipole moment of the molecule.
Draw all isomers of C6H12O that are
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