I need help with this chemistry flame test lab discussion question.

"List the metals used in this lab in increasing order of the energy of the light emitted."
We tested BaCl2, CaCl2, CuCl2, FE(NO3)3, KCl, LiCl, NaCl, & Sr(No3)2.
I'm not completely sure how to know the energy of the light emitted. Please help!

The color. E = h*frequency or

E = hc/wavelength. Color goes from violet (about 400 nm wavelength) to red (about 700 nm wavelength). The shorter the wavelength the more energy; the longer the wavelength less less energy.

To determine the increasing order of the energy of light emitted in a flame test lab, you can use the concept of atomic emission spectra and the electromagnetic spectrum.

The energy of light emitted during a flame test is related to the electronic structure of the different metal ions in the compounds being tested. When the metal ions are heated in the flame, the electrons in their atomic or ionic orbitals get excited to higher energy levels. As these excited electrons return to their ground state, they release energy in the form of light.

Generally, the energy of light emitted is directly proportional to the difference in energy between the excited state and ground state of the electrons. This difference in energy corresponds to the specific wavelength or color of light emitted, according to the relationship E=hc/λ, where E is the energy, h is Planck's constant, c is the speed of light, and λ is the wavelength.

In your lab, you observed the colors of the flames produced by different metal ions. While you cannot directly determine the energy of light emitted, you can make an inference about the relative energy levels based on the observed flame colors. Typically, higher energy light (shorter wavelength) corresponds to a bluer color, while lower energy light (longer wavelength) corresponds to a redder or orange color.

Based on this understanding, you can arrange the metals used in your lab in increasing order of the energy of light emitted. Review the observed flame colors for each metal ion and associate them with the wavelength spectrum of visible light. Then, group them in increasing order of energy, from the longest wavelength (lowest energy, red/orange) to the shortest wavelength (highest energy, blue).

For example, let's assume the flame colors observed were:
BaCl2 - Green
CaCl2 - Brick Red
CuCl2 - Green
Fe(NO3)3 - Golden Yellow
KCl - Lilac
LiCl - Crimson Red
NaCl - Intense Yellow
Sr(NO3)2 - Red

Based on the flame colors, we can infer the order of increasing energy of light emitted:
LiCl (Crimson Red) < CaCl2 (Brick Red) < Sr(NO3)2 (Red) < NaCl (Intense Yellow) < Fe(NO3)3 (Golden Yellow) < CuCl2 (Green) < BaCl2 (Green) < KCl (Lilac).

Remember, this inference is based on the assumption that bluer colors correspond to higher energy, and it is important to judge the colors accurately across all trials to ensure the correct ordering.

By understanding the concept of atomic emission spectra and relating it to the observed flame colors, you can determine the increasing order of the energy of light emitted in a flame test lab.