The oxidation states of copper are 0, +1, +2, +3 and +4, of which +1 and +2 are the common oxidation states. The +3 oxidation state is potassium hexafluorocopper(III) acid, the +4 oxidation state is caesium hexafluorocopper(IV) acid, and the 0 oxidation state, Cu(CO)₂, can be detected by a gas-phase reaction followed by matrix isolation.
Copper is readily corroded by halogens, mutual halides, sulphur and selenium, and vulcanised rubber can blacken copper. Copper does not react with nitrogen tetroxide at room temperature, but in the presence of nitromethane, acetonitrile, ether, or ethyl acetate, copper nitrate is formed:
Cu+2N₂O₄==Cu(NO₃)₂+2NO
Copper metal is soluble in oxidising acids such as nitric acid and insoluble in non-oxidising acids in the absence of an oxidising agent or in the presence of a suitable coordination reagent such as:
Copper is soluble in chloric acid or acidified chlorates:
3Cu + 6H⁺+ ClO³-== 3Cu²⁺+ Cl -+3H₂O
Coordination reaction occurs in the presence of more concentrated chloride ions:
2Cu + 6S==C(NH₂)₂+2 HCl == 2Cu(I) (S=C(NH₂)₂)₃Cl + H₂)
Copper reacts with high-Tc acid radical ions under acidic conditions, reducing the high-Tc acid radical ions to the singlet Tc:
7Cu + 2TcO⁴- + 16H⁺== 2Tc + 7Cu²⁺ + 8H₂O
Copper and ferrous sulphide can undergo a replacement reaction when heated:
2Cu + FeS == Cu₂S + Fe
Copper can react with sulphur trioxide when heated, and there are two main reactions:
4Cu + SO₃== CuS + 3CuO
Cu + SO₃== CuO + SO₂.
When heated, concentrated sulphuric acid can react with copper to form the highly valent metal sulphate {CuSO₄}, which itself is generally reduced to sulphur dioxide.
Cu + 2H₂SO₄ (concentrated) ====CuSO₄ + SO₂↑ + 2H₂O
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