Consider the bicarbonate ion, HCO3-. 1. First, draw the complete Lewis dot structure for it. Since there is no way to type these structures into Blackboard, please show your work by writing it on the provided answer sheet. You do not have to type anything here (for this part), but be sure to submit your answer sheet as soon as possible after completing the exam. 2. By each polar bond in the previous part, draw a vector showing the dipole moment. 3. Finally, if the overall structure has a dipole moment, draw an additional vector indicating the direction. Please circle that vector to distinguish it from the ones marking the bonds. Hint: you may need to redraw your structure with proper VSEPR shape first.
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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