CHE-2201 Lecture Notes - Lecture 3: Conjugate Acid, Formal Charge, Equilibrium Constant
Document Summary
Bronsted-lowry acid: a base accepts a proton. Bronsted-lowry base: an acid gives up a proton. All acid/base reactions occur in one step - the acid cannot lose its proton without the base take it. Quantitative strength analysis: using numerical data to compare how strong acids are. Ka is the equilibrium constant for the reaction between an acid and water. The stronger the acid the weaker its conjugate base. With the relevant pka values, you can predict which direction an acid/base equilibrium will favor. Qualitative analysis: compare structural stability to determine which is a stronger acid. The more effectively a reaction product can stabilize its formal charge, the more the equilibrium will favor that product. The more effectively a conjugate base can stabilize its negative charge, the stronger the acid. Factors that affect the stability of a negative formal charge (ario): The type of atom that carries that charge. More electronegative atoms are better at stabilizing negative charge.
