The iodide ions reduce the Cu(II) to Cu(I) and the iodide is oxidised to iodine. The iodine formed reacts with potassium ions in the reaction mixture to give potassium triiodide. So, you will get a precipitate of white copper (I) iodide in a brown solution of potassium triiodide.

Answer: The reaction of copper sulfate in aqueous state and potassium iodide in solid state produces cuprous iodide as a precipitate, liberates iodine gas and forms potassium sulfate in aqueous state.

Potassium iodate is often used as a reference material to standardize a sodium thiosulfate solution which is a familiar titrant for redox titrations. In the standardization, iodine (triiodide) liberated by potassium iodate in an acidic potassium iodide solution is titrated with a sodium thiosulfate solution.

Explanation: The reduction of Cu2+ to Cu+ occurs as the result of the oxidation of I- to I2. The I2 combines with iodide ion to produce the dark brown triodide ion, I3-. The excess iodide ion also causes the reduced copper to precipitate as white cuprous iodide, CuI.

Copper sulphate on treatment with potassium iodide precipitates cuprous iodide (CuI), liberates iodine gas and also forms potassium sulphate.

The simple reaction Copper(II) ions oxidise iodide ions to iodine, and in the process are themselves reduced to copper(I) iodide. Note: If you need to, you can find out more about oxidation states by following this link.

Cu(OH)2 + 2 HCl → CuCl2 + 2 H2O – Balanced equation | Chemical Equations online!

The reaction between CuSO4 and NaOH is a double displacement reaction that forms Na2SO4 and Cu(OH)2. Copper (II) hydroxide will precipitate from the solution and appears as a pale blue solid. This compound has several uses and can be extracted from the solution.

Stability depends on the hydration energy (enthalpy) of the ions when they bond to the water molecules. The Cu2+ ion has a greater charge density than Cu+ ion and thus forms much stronger bonds releasing more energy.

Copper(2+) is an ion of copper carrying a double positive charge. It has a role as a cofactor. It is a divalent metal cation, a copper cation and a monoatomic dication….4.3Related Element.

Explanation: It’s an energy balance. Donating additional valence electrons to make higher oxidation states costs energy. In the case of copper it usually works for donating one 3d electrons plus the 4s electron for +2 , but getting to +3 is too much.

Cu+1 is more stable than Cu+2 due to fully filled d10 electronic configuration. However Cu+2 is more stable than Cu+1 in aqueous solution as hydration enthalpy overpowers the second ionization enthalpy of Copper.

In an aqueous solution, a Cu2+ ion is more stable than a Cu+ ion due to the fact that the Cu2+ ion has a high negative value of hydration enthalpy. Means that more energy is released when Cu2+ is dissolved in water than in the case of Cu+. Hence it’s more stable.

Since the energies of the 4s and the 3d electrons in copper is nearly identical, it is also possible to remove both 4s electrons( instead of moving it to a d orbital. This makes the cupric or Cu(II) 2+ ion.

Fe3+ is more stable than Fe2+. In Fe3+ ions, there are five 3d half-filled orbitals and is more symmetrical than Fe2+. Whereas in Fe2+ ion there are four 3d half-filled orbitals and one orbital is filled.

Explanation: The outermost electrons in 4s2 are readily given out to Chlorine. But it requires a further catalyst or oxidant like Oxygen or H2O2 etc, to give out an unpaired 3d^6 electron from d orbitals. In general , Ferric compounds are more stable as compared to Ferrous Fe compounds.

The Fe 3+ ion more stable than Fe 2+ ion because due to his electronic configuration i.e the electronic configuration of Fe 3+ has half filled last orbital and we know that half or fulled filled orbitals are most stable and here Fe 2+ has not half or full-filled orbital so Fe 3+ ion more stable than Fe 2+ ion.

The reason why fe3+ is more stable than fe2+ is because, in fe2+ there are 6 electrons in d orbital as compared to 5 electrons in the case of fe3+. Since 10 electrons make fully filled d orbital (most stable) , the 5 electrons in fe3+ makes the d orbital half filled and therefore is more stable compared to fe2+.

Ferric ion

In chemistry, iron(III) refers to the element iron in its +3 oxidation state. In ionic compounds (salts), such an atom may occur as a separate cation (positive ion) denoted by Fe3+. Iron is almost always encountered in the oxidation states 0 (as in the metal), +2, or +3.

This article has been rated as Mid-importance on the project’s importance scale….hydrated ions.

Iron is almost always encountered in the oxidation states 0 (as in the metal), +2, or +3. Solid iron(II) salts are relatively stable in air, but in the presence of air and water they tend to oxidize to iron(III) salts that include hydroxide (HO−) or oxide (O2−) anions.

1s2 2s2 2p6 3s2 3p6 4s2 3d6. When Fe loses 3 electrons, it will lose 1 electron from 4s orbital and 2 electrons from 3d orbital. Hence you can decide the required configuration.

Iron has 26 electrons, thus it can be written as [Ar]3d64s2. An orbital is considered stable when it is half-filled or fully filled. Thus for the case of 4s, the maximum number of electrons it can contain is 2, and thus the 4s is fully filled, as indicated by the superscript ‘2’.

The difference between Fe2+ and Fe3+ is the Fe2+ has a pale green colour and turns violet when water is added to it. While Fe3+ forms blood-red when it reacts with thiocyanate ions. Fe2+ has paramagnetic properties whereas Fe3+ has diamagnetic properties.

A transition metal is one that forms one or more stable ions which have incompletely filled d orbitals. On the basis of this definition, scandium and zinc do not count as transition metals – even though they are members of the d block. The zinc ion has full d levels and does not meet the definition either.

Fe

Iron, one of the most abundant elements on Earth, helped give rise to entire civilizations and is the key ingredient in steel, without which many of our modern structures would not be standing. The story of iron’s origins is astronomical, and it begins with the element being born from the explosion of stars.

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