Why do we see the characteristic colour of a metal ion when a salt of that metal ion is introduced in the flame? Why is it that all metal ions do not give the flame test?
996we have a flame colour when an electron of the metal receiving energy from the flame jumps to an excited level and returning to the ground level emits an electromagnetic radiation. But to have a colour the energy of that radiation must be in the limit of the visible spectra. A great number of transition metals have such levels of energy which fulfill this requirement. But , it is not sure that ALL metals have this requirement. So the majority does but not all.
383Flame colours are produced from the movement of the electrons in the metal ions. When the electrons are heated, the electrons gain energy and can jump into any of the empty orbitals at higher levels. Each of these jumps released specific amount of energy as light energy, and each jump corresponds to a particular colour.
Soumyabrata Mondal sorry
Bitan Chakraborty Electronic jump to higher levels require ABSORPTION of energy, whereas to see a colour, energy is to be emitted. So jump to higher level donot correspond to the visible light.
Also the 2nd part of my question remains to be answered.