Why aren't acid-base reactions considered redox reactions, even though they involve the transfer of hydrogen atoms?

  Acid/base and precipitation reactions almost always are NOT redox reactions. For redox to have happened, the number of electrons that an element has must change (i.e. its oxidation state must change). ... But the hydrogen ion never "has" any electron throughout the process and remains in a +1 oxidation state.

Explanation:

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alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.