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Hello,
I just started learning this topic today after reviewing electronegavity. The kaplan book says a typical galvanic cell consists of a Zn half cell and a Cu half cell, where Cu is the cathode and Zn is the anode. The reactions are:
Zn(s)->Zn2+(aq)+2e (anode)
Cu(2+)(aq)+2e->Cu(s) (cathode)
I got confused here. According to the Periodic Table, isn't Zn the MORE electronegative one? Since electronegativity increases from left to right. That would mean Zn should be the cathode (accept electrons) and Cu should be the anode, which is not the case. Clearly, the "default" arrangement of Zn anode and Cu cathode is more favorable since the galvanic cell is spontaneous. But why is this the case? Would it still be spontaneous if the Cu becomes the anode instead? How do you determine the spontaneity of this particular reaction?
Thanks in advance to anyone who can help me out 🙂
Cherry
I just started learning this topic today after reviewing electronegavity. The kaplan book says a typical galvanic cell consists of a Zn half cell and a Cu half cell, where Cu is the cathode and Zn is the anode. The reactions are:
Zn(s)->Zn2+(aq)+2e (anode)
Cu(2+)(aq)+2e->Cu(s) (cathode)
I got confused here. According to the Periodic Table, isn't Zn the MORE electronegative one? Since electronegativity increases from left to right. That would mean Zn should be the cathode (accept electrons) and Cu should be the anode, which is not the case. Clearly, the "default" arrangement of Zn anode and Cu cathode is more favorable since the galvanic cell is spontaneous. But why is this the case? Would it still be spontaneous if the Cu becomes the anode instead? How do you determine the spontaneity of this particular reaction?
Thanks in advance to anyone who can help me out 🙂
Cherry