The problem of the price change of high chemical copper.

I checked the university textbook for you: Inorganic Chemistry (edited by Wuhan University and Ji Da, Third Edition), p820, "Since the energy of the ns electrons of the copper group elements is not much different from the (n-1)d electrons of the sub-shell, when the sum is compared with other elements, not only the ns orbital can participate in bonding, but the (n-1)d electrons can also partially participate in bonding according to different reaction conditions, so they show several oxidation states. That's the chemical explanation.

Cu common positive bivalent, such as copper oxide.

Cuprous oxide is positive monovalent.

Elemental copper is naturally 0.

It is a variable metal.

The valence of an element, in addition to the outermost electrons, is also involved in the orbital electron energy transition. The electrons of the p orbital, the s orbital, the d orbital may transition, looking for relative equilibrium. This is also known as a saturated or semi-saturated state.

You go read about basic inorganic chemistry.

This is related to the electron energy level, which is very complex, involving three orbitals, four forms of transitions, in a word, it is to disperse energy and maintain balance.

Cuprous oxide (copper + 1 valence) can be obtained by reacting with 2-valent copper and aldehydes in aqueous solution, which will be learned from organic matter, copper hydroxide will eventually become cuprous oxide by burning, and cuprous chloride can also be obtained by passing sulfur dioxide into copper chloride solution.

Cuprous oxide. Cuprous chloride is almost insoluble in water.

In aqueous solution, +2 valent copper is more stable than +1 valent copper, and in anhydrous conditions, just the opposite.

2-valent copper is stable at room temperature or in aqueous solution, while +1-valent cuprous is stable at high temperatures, so there is a rule that burning copper hydroxide or copper oxide will eventually turn into cuprous oxide.

The reaction of copper with a weak oxidant is +1 valence, such as cuprous sulfide Cus2

The reaction of copper with a weak oxidant is +2 valence, such as copper chloride CuCl2

When nitric acid is concentrated nitric acid, nitric acid is reduced to nitrogen dioxide:

cu + 4 hno3 = cu(no3)2 + 2 no2↑ +2 h2o

Ionic reaction: Cu + 4 H+ +2 No3- = Cu2+ +2 No2 +2 H2O

When nitric acid is dilute nitric acid, nitric acid is reduced to nitric oxide:

3 cu + 8 hno3 = 3 cu(no3)2+ +2 no↑ +4 h2o

Ion reaction: 3 Cu + 8 H+ +2 No3- = 3 Cu2+ +2 No +4 H2O

The reason for the difference is that concentrated nitric acid has strong oxidizing properties, which can oxidize -5 valence n to the most **+4 valence, while dilute nitric acid is weaker than concentrated nitric acid.

Shanghai elite education teacher replied: NaCl + agno3 = agCl precipitation + nano3, so n(ag) = n(NaCl) =, so the mass fraction of silver =, so the mass fraction of copper =

1.If the anode product is an active electrode (metal before AG), the more active it is, the easier it is to lose electrons, so first the Zn in blister copper is oxidized first, then Fe, in Cu, and finally Ag. In the case of inert electrodes (PT, AU, graphite), it is the loss of electrons from the anion in the solution, in the following order:

S2->I->br->Cl->OH-> oxygenate.

2.The cathode product is directly judged according to the cation discharge sequence: Ag+>Hg2+>Fe3+>Cu2+>H+>Pb2+>Sn2+>Fe2+>Zn2+

Detailed enough

Platinum and gold are two inert electrodes in the electrolytic cell, which do not participate in the electrode reaction and are precipitated.

Other ions are preceded by hydrogen in the sequence of metal activity and cannot be reduced and precipitated in solution, and hydrogen is precipitated first.

AGCl is insoluble in NaOH and HCl

CU is the most oxidizing.

This is a slightly more difficult problem, as monovalent copper ions disproportionate under acidic conditions to form copper ions and copper.

In fact, this question is a special knowledge point, that is, +1 valent copper ions are used as both reducing agents and oxidants here.

This is a disproportionation reaction of monovalent copper ions.

Well, you don't have to think about it. Wait until you've learned about redox reactions in high school. That's all I can tell you.

Iron reacts with acid is +2, and reaction with oxygen depends on the reaction conditions, and the conditions are strong and the valence state is high. Copper at the junior high school level is +2Knowing too much is actually not good for you.

Blister copper at the positive electrode, loses electrons. Blister copper, which is less active than copper, does not discharge, and if discharged, it will be replaced by copper into anode slurry.

If the Zn2+ in the solution, the Fe2+ plasma will precipitate at the cathode and displace the copper.

The metal event order must be used!

This is something I didn't learn in high school, and the reaction is a bit complicated. Participating in the reaction are oxygen, ammonia, copper, and hydrochloric acid. First, ammonium chloride is hydrolyzed into ammonia and hydrochloric acid, and ammonia and copper form chelates, so that copper loses electrons to oxygen, becomes Cu(NH3)22+, and then reacts with hydrochloric acid to generate Cu(NH3)Cl2...

This substance is not very stable. Ammonia gas is easily decomposed by heating. The addition of a substance containing ammonium can be accelerated, and the addition of oxygen can also be accelerated.

Generate [Cu(NH3)4]2+

Tetraammonia copper( ) ion, dark blue.

[Chemistry] compulsory 1 - the reaction of concentrated sulfuric acid with copper.

Ammonium chloride solution is weakly acidic, so it should not be able to react with copper.

Because oxidizing Fe+>Cu2+>H+, it occurs first: 2ag++Fe=2ag++Fe2+ and then occurs: 2Fe3++Fe=3Fe2+0 01mol 0 005mol 0 01mol 005mol 0 01mol Therefore, B is chosen

Nitric acid itself is not oxidizing at all, and only under acidic conditions can it be strongly acidic, to put it bluntly, nitric acid formed by nitrate and hydrogen ions is strongly acidic.

Concentrated nitric acid with strong oxidizing property and dilute nitric acid only have weak oxidizing properties.

aRedox reactions are carried out preferentially.

Oxidizing is ferric iron.