Green light is emitted when electrons in a substance make a particular energy-level transition. If blue light were instead emitted from the same substance, would it correspond to a greater or lesser change of energy in the atom? and why?

λ (green)≈ 550 nm,

λ (blue) ≈ 450 nm.
λ (green) > λ (blue)
The energy of emitted photon is
ε =h•c/ λ =>
ε(green) < ε(blue).
If blue light was emitted, it corresponds
to a greater change of energy in the atom.

If blue light were emitted instead of green light from the same substance, it would correspond to a greater change of energy in the atom. This is because blue light has a shorter wavelength and higher frequency compared to green light. According to the electromagnetic spectrum, shorter wavelength light corresponds to higher energy photons.

In the case of an atom, the energy level transitions of electrons are specific and discrete. Electrons occupy different energy levels around the atom's nucleus. When an electron undergoes a transition from a higher energy level to a lower one, it emits a photon of light corresponding to the energy difference between the two levels.

Since blue light has a higher energy than green light, it means that the energy difference between the two energy levels of the electron is greater when blue light is emitted. Therefore, the emission of blue light from the same substance corresponds to a greater change of energy in the atom.

To determine whether blue light corresponds to a greater or lesser change of energy in the atom compared to green light, we need to understand the relationship between the energy of light and the energy-level transitions in atoms.

In atoms, electrons occupy different energy levels called electron shells. These shells are quantized, meaning they have specific energy values. When an electron transitions from a higher energy level to a lower energy level, it releases energy in the form of light. The energy of the emitted light corresponds to the energy difference between the two energy levels involved in the transition.

Now, let's consider the scenario where green light is emitted. Green light has a longer wavelength compared to blue light. In the electromagnetic spectrum, longer wavelength light has lower energy, and shorter wavelength light has higher energy.

Given that blue light has a shorter wavelength than green light, it means that blue light carries more energy per photon than green light. Therefore, if blue light were emitted from the same substance, it would correspond to a greater energy-level transition in the atom compared to green light.

In summary, blue light corresponds to a greater change of energy in the atom because it has a higher energy per photon than green light.