In fact it isn't. Copper (II) ions are stable wrt copper (i) ions. Although this is apparently contradictory to the electronic structure. This anomaly has been attributed to the Jahn-Teller effect which is the lengthening of the axial ligand bonds in a transition metal complex.
2006-07-05 10:10:58
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answer #1
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answered by Anonymous
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Copper has 29 protons and 29 electrons. If it gains one (Cu+1) then it will have 30 electrons which gives it a full d orbital. If it gained 2 then it would want to lose one and be very unstable until it does.
2006-07-05 03:53:55
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answer #2
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answered by b 3
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Cu(I) has a stable electron configuration i.e. the electrons occupy the valence shell completely.
Cu(II) has one electron short of a complete valence shell.
2006-07-05 03:40:53
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answer #3
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answered by Als 2
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ok when an atom goes positive it doesn't gain electrons it looses them. Cu1 has more protons than electrons so they come in close and the arrangement becomes more stable
2006-07-05 04:38:53
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answer #4
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answered by shiara_blade 6
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The outer electrons are closer to the nucleus and so harder to lose which makes cu(I) more stable
2006-07-05 03:24:23
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answer #5
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answered by Invictus 2
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maybe lack of ionization energy required to break off the other electron.
2006-07-05 14:48:50
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answer #6
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answered by Lawrence Boyer,edinboro univ, pa 2
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kevster is correct.
I couldn't answer because I couldn't think of a good reason. My inorganic is a little weak, it seems.
2006-07-05 14:06:09
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answer #7
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answered by niuchemist 6
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