Why do ions have different colors in a flame test?

Answer 1

When a metallic ion is heated in a flame test, the heat (energy) causes an electron to be exicted to a higher energy state. When this electron returns to a lower energy state, energy is emitted as visible light. Depending on how much energy is released when the electron returns from the higher to lower energy state will determine what color the flame will be.

Answer 2

When a metallic ion is heated in a flame test, the heat (energy) causes an electron to be exicted to a higher energy state. When this electron returns to a lower energy state, energy is emitted as visible light. Depending on how much energy is released when the electron returns from the higher to lower energy state will determine what color the flame will be.

Answer 3

You can tell that it is the cation which is causing the flame colour because all compounds of Sodium will give a yellow/orange colour regard less of the anion. All compounds of Copper give a blue/green colour regardless of the anion.

If the anion was producing the flame colour then all nitrates would be the same colour but they are not - sodium nitrate gives an orange and copper nitrate a green/blue colour because of the anions not the cations.

Answer 4

The loosely held electrons of a metal are easily excited in the flame of a lab burner.

Answer 5

When a metallic ion is heated it goes into an excited state. Whn the metallic ion goes back to its ground state it emits the energy in form of light.

Answer 6

Because each solution contains the nonmetal chlorine. The solutions are all salts with a common nonmetal.

Answer 7

because they absorb and emit different amount or energies.