compare the structure of the atoms of two different elements like cooper and iron
Why does the colour of copper sulphate solution change when an iron nail is dipped in it? When an iron nail is placed in a copper sulphate solution, iron displaces copper from copper sulphate solution forming iron sulphate, which is green in colour. Therefore, the blue colour of copper sulphate solution fades and green colour appears.
Contacting the iron powder with an aqueous solution of copper (II) salts will produce a copper coating on iron powder: Iron is higher in the electromotive series than copper and therefore will displace copper from the solution, resulting in copper-coated iron and dissolved iron cations. When all of the surface of the iron powder has been coated with copper, the iron will stop reacting because it no longer has access to the copper ions in solution, the access of the iron being blocked by the layer of copper coating the remaining iron powder.
iron + copper sulphate ''goes to'' iron sulphate + copper
The iron will displace the copper as it is more reactive. here's the equation: iron + copper sulphate = iron sulphate +copper
When an iron nail is dipped in the copper sulfate solution then iron displaces copper from the copper sulfate because iron is more reactive than copper.
The iron is a more active metal than copper, so the iron atoms in the nail replace the copper atoms in the copper sulphate solution, so it becomes iron sulfate. The copper atoms will start to build on the iron nail, as well.
No. Copper and Iron are both elements and are made up of atoms of the pure element.
Yes, atoms of copper and iron can generally form stable bonds with transition elements. Copper and iron are both transition elements themselves and can form stable bonds with other transition elements. The stability of the bonds will depend on factors such as the electronegativity and bonding properties of the specific elements involved.
Iron is a more active metal than copper, so it replaces/displaces the copper in the copper sulfate, forming iron sulfate and copper. So the hole in the iron pot is where the iron atoms came from. This is called a single replacement/displacement reaction.
3 types, Cu (Copper), Fe (Iron) and S(Sulfur)
63.55g or 63.55 grams
Why does the colour of copper sulphate solution change when an iron nail is dipped in it? When an iron nail is placed in a copper sulphate solution, iron displaces copper from copper sulphate solution forming iron sulphate, which is green in colour. Therefore, the blue colour of copper sulphate solution fades and green colour appears.
Because iron is more reactive than copper. If iron displaces copper, that releases energy (enthalpy). If copper were to displace iron, that would require energy to be used. This is less favourable and , averaged over the huge number of molecules, atoms and ions in the solution, the more energy producing reaction is vastly preferred. Hence, iron put into copper sulphate solution gets coated in copper and the solution slowly loses its blue colour. But if you put copper metal in iron sulphate solution, nothing noticable occurs.
You need to know what elements the coin is made up of (ie. what percent is iron and what percent is copper). You'd then need to weigh the coin out. If you wanted to know how many iron atoms there are, then you'd calculate how much iron there is and convert that to moles and then to atoms using avogadro's number.
The number of atoms in a given mass of metal may be calculated by dividing the mass by the gram atomic mass, then multiplying by Avogadro's Number. The gram atomic masses of iron and copper are 55.847 and 63.546 respectively. Since Avogadro's Number is constant, the required mass m of copper atoms can be found from the equation m/63.546 = 235/63.546, or m = 235 X (63.456/55.847), or 267 grams of copper, to the justified number of significant digits.
It may seem like the iron rusts, but it doesn't. The chemical formula for copper sulfate is CuSO4, or, 1 copper atom, 1 sulfur atom, and 4 oxygen atoms to each molecule. When the iron is placed in the solution of copper sulfate, it replaces the copper in the solution, turning copper sulfate into iron sulfate (FeSO4) and pure copper collects on the iron. This can be proved by removing the copper and seeing that the iron has lost a lot of its mass, as in, it lost mass to the copper sulfate. The iron (steel wool) takes on a pinkish color which is metallic copper deposited when the solution forms iron sulfate.
Iron atoms.