ANTH 010 Lecture Notes - Lecture 17: Alkali Metal, Acid Strength, Lewis Acids And Bases
13 Aug 2020
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A. bronsted acid: anything that that donates a proton. B. bronsted base: anything that accepts a proton. A. lewis acid: anything that accepts a pair of electrons. B. lewis base: anything that donates a pair of electrons. A. alkali metal cations (li+, na+, k+, rb+, cs+, fr+) Heavier alkaline earth metal cations (ca2+, sr2+, ba2+, ra2+) Strong = smaller cation, higher charge = less stable = wants an electron more. Lewis acids are not necessarily all bronsted or arrhenius acids. Three factors determine i f a compound will release i ts" proton: strength, polarity and stability. Strength of the bond holding the hydrogen to the molecule. A. hf is the most polar (good) but also the strongest (bad) A. hcl is acidic while ch (methane) is not. A. hf is the most polar (good), but f is the smallest (bad) and thus the most unstable (bad) A. polarity: increasing electronegative oxygens increases polarity.
