How can standard electrode potentials be used to gauge a half-reaction's tendency to gain electrons?

a) The more positive the standard electrode potential, the greater the tendency to undergo reduction, thereby gaining electrons.

b) more negative the standard electrode potential, the greater is the tendency to participate in spontaneous reactions.

c) The individual standard electrode potentials do not indicate anything about tendency to gain electrons. The cell potential of the entire cell does.

d) Standard electrode potentials are neither positive nor negative, since we define the standard hydrogen electrode as having a potential of zero.