Cu 2+ is blue. Cu2O is reddish; CuO is black, I think.
The colour of silver metal in water is whiteThe colour of copper nitrate in water is blue (due to the Cu++ ion).
The metallic ion in the solution is likely copper(II) ion (Cu^2+). This is based on its blue color in a flame test, which gives a blue-green flame, and the formation of a blue precipitate when sodium hydroxide is added, indicating the presence of Cu(OH)2.
Copper can have a +1 charge, known as cuprous ion, and a +2 charge, known as cupric ion. These charges depend on the oxidation state of copper in a compound.
The oxidation state of the cupric ion in copper tartarate is +2. Copper (II) ion, or cupric ion, has an oxidation state of +2 due to the loss of 2 electrons. In the case of copper tartarate, the ligand (tartarate) does not affect the oxidation state of the central copper ion.
The charge on the copper ion in CuF2 is +2. This is because fluorine typically has a charge of -1, and there are two fluorine atoms in the compound which balances out the charge of the copper ion.
Flame colours depend on just the metal ion. All copper compounds give the same colour, green.
The ion responsible for the blue color in many compounds is usually copper(II) ion (Cu2+). Copper(II) compounds often appear blue due to the absorption of certain wavelengths of light in the visible spectrum associated with the ion's electronic structure.
Anhydrous copper(II) sulphate is white. When added to water, it forms a solution of CuSO4(aq) which is blue because of the Cu2+ ion, which is itself a transition metal ion.
The colour of silver metal in water is whiteThe colour of copper nitrate in water is blue (due to the Cu++ ion).
The metallic ion in the solution is likely copper(II) ion (Cu^2+). This is based on its blue color in a flame test, which gives a blue-green flame, and the formation of a blue precipitate when sodium hydroxide is added, indicating the presence of Cu(OH)2.
Copper and carbonate ions form copper carbonate. In practice, copper carbonate usually contains hydroxide ions as well.
The metallic ion in copper II chloride is copper (Cu2+).
In copper sulfate (CuSO4), the polyatomic ion is SO4^2-, which is covalently bonded. The copper ion (Cu) is not part of the polyatomic ion and is ionically bonded to the sulfate ion.
Copper can have a +1 charge, known as cuprous ion, and a +2 charge, known as cupric ion. These charges depend on the oxidation state of copper in a compound.
When copper combines with oxygen to form copper (II) oxide, the charge of the copper ion is +2. This is because in copper (II) oxide, each copper ion has lost two electrons to oxygen atoms, resulting in a +2 charge.
The oxidation state of the cupric ion in copper tartarate is +2. Copper (II) ion, or cupric ion, has an oxidation state of +2 due to the loss of 2 electrons. In the case of copper tartarate, the ligand (tartarate) does not affect the oxidation state of the central copper ion.
The charge on the copper ion in Cu3P is +1. This is because the overall charge for the compound Cu3P is 0, and since there are three copper ions present, each copper ion must have a charge of +1 to balance the -3 charge of the phosphorus ion.