Chemistry: In burning a compound to create a colored flame, was the metal cation Ba2+ in Ba(NO3)2 responsible?

Question

for the effects of the colored flame? or was the anion NO3 responsible? Basically, my question is, which of these two, metal cation or anion was responsible for the colored flame in the process of burning this compound of Ba(NO3)2?

Answer 1

Often the compound is not burned in a flame test. Burning usually means oxidation. A piece of paper placed into a flame will char and then the carbon will combine with oxygen to burn.

The flame in a flame test is used to add energy to a compound. This usually excites electrons which will jump to a higher energy level. When these electrons return to their lower level, they will emit light. This is the color that you see.

When a Barium compound is used, the color you see is usually green. This would be true for Barium nitrate or even Barium chloride. Generally speaking the anions do not excite and give no color.

Answer 2

In general terms, the cation burning is usually what results in a colored flame. However, there are anions that produce the color too.

In the case of your experiment, it was the Barium that resulted in a green flame

What happens is the electron energy levels increase due to the flame, but the electrons then drop down to their original energy level. The photon released when the electron returns to its original state is the color you see. The amount of energy in that color affects which color.

Answer 3

the color depends on the substance being burned and the temp, the shape depends on gravity. Upon reading those posts, my knowledge may be incomplete on the topic, sorry