Acetic acid (shown below) has a K, that is much smaller,1.8x10*. Why is chloroacetic acid a stronger acid than acetic acid? The chlorine atom withdraw electrons, ultimately from the O atoms making them positive which then repel H". The chlorine atom in chloroacetic acid is very electronegative, withdrawing electrons from the rest of the molecule ultimately making the O-H bond weaker. This statement is not true, acetic acid is a stronger acid than chloroacetic acid.
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
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