This can be explained by simple electronegativity nh3

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Unformatted text preview: HO O HO HO H wrong O H wrong O H correct Factors affecting acidity/basicity: The main factor in deciding acidity or basicity is stability. If you are unsure, draw the molecule’s conjugate acid or base and ask yourself if you have gained or lost stability. If a molecule is stable without the proton attached, chances are that proton is an acidic proton. If the molecule is unstable when you remove the proton, chances are that proton was not acidic. There are numerous effects to consider. Element Effect: Look at the element attached to the proton in question As you go across the periodic table, protons attached to the elements are more acidic. HF is more acidic than H’s attached to oxygens, which are more acidic than H’s attached to nitrogens, which are more acidic than H’s attached to carbons. This can be explained by simple electronegativity. NH3 CH4 H2O HF HCl Increasing acidity HBr Increasing acidity HI As you go down a row, the inherent acidity increases. HI more acidic than HBr which is more acidic than HCl which is more acidic than HF. This is not explained by electronegativity. As you go down a periodic table, the atom sizes get bigger. Bigger atoms can handle negative charge better than smaller atoms. F- is small. I- is big. They both have the same charge, but I- has a much smaller charge per surface area than F- . Thus, I- is more stable and HI is more acidic. Charge Effect: This one is the easiest to understand. When in atom has a positive formal charge,...
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