What is the Evidence for quantized electronic energy levels?

What is the Evidence for quantized electronic energy levels?

The hydrogen spectrum is an important piece of evidence showing that the electronic structure of the atom is quantized. When an electric discharge is passed through a gaseous hydrogen molecule, the hydrogen atoms in the molecule dissociate.

What does it mean when energy levels are quantized?

1. Quantized energy means that the electrons can possess only certain discrete energy values; values between those quantized values are not permitted.

What would an emission spectrum look like if quantized energy levels in an atom did not exist?

If atomic energy levels were not quantized, the light would be white (all energies). Stimulated emission: • external photon causes electron jump to lower level • a photon is emitted • the original photon is not absorbed!

What is difference between emission spectrum and absorption spectrum?

The main difference between emission and absorption spectra is that an emission spectrum has different coloured lines in the spectrum, whereas an absorption spectrum has dark-coloured lines in the spectrum.

What are the evidence of quantization?

Originally Answered: What is some evidence of quantization and electronic energy level? The evidence is that the atomic spectra consist of distinct lines rather than continuum. If electronic energy levels were continuous, the atomic spectra would have shown continuous emission/absorption.

How does an emission spectrum work?

Thus, emission spectra are produced by thin gases in which the atoms do not experience many collisions (because of the low density). The emission lines correspond to photons of discrete energies that are emitted when excited atomic states in the gas make transitions back to lower-lying levels.

What is emission spectrum in chemistry?

The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an atom or molecule making a transition from a high energy state to a lower energy state.

What is the connection between the absorption and emission spectrum?

Emission lines refer to the fact that glowing hot gas emits lines of light, whereas absorption lines refer to the tendency of cool atmospheric gas to absorb the same lines of light. When light passes through gas in the atmosphere some of the light at particular wavelengths is scattered resulting in darker bands.

How does an absorption spectrum work?

An absorption spectrum occurs when light passes through a cold, dilute gas and atoms in the gas absorb at characteristic frequencies; since the re-emitted light is unlikely to be emitted in the same direction as the absorbed photon, this gives rise to dark lines (absence of light) in the spectrum.

What do we mean when we say that energy levels are quantized in atoms quizlet?

What do we mean when we say that energy levels are quantized in atoms? We mean that the electrons can have only discrete values of electrical potential energy in atoms.

Which part of the light spectrum has the highest energy?

Further, from the diagram, we could see that the photons emitted have very close (dare I say converging) wavelength, which is toward the low end of the wavelength, aka, has higher energy.

Can electrons give off photons at arbitrary energy levels?

If electrons could give off arbitrary photons as they change to arbitrary energy levels, there would by no spiked at all. Just a continuous emmision range. And a continuous range of energy states for the electron. Sure, if a continuous steam of photons at different energies is emitted, electrons might still have discrete energy levels.

Do electrons have discrete or continuous energy levels?

Sure, if a continuous steam of photons at different energies is emitted, electrons might still have discrete energy levels. Photon A plus B could be any two values such that they equal energy level C, a continuous range. But if only discrete photon energy levels are emitted, you can’t get to any arbitrary energy level for the electron.

Why can only certain wavelengths of light be emitted from hydrogen atoms?

Such an electron will emit photons of certain wavelength as they return to their level of origin. Hence, there should only be certain wavelengths of light emitted, since the change in energy from different energy levels is constant (nearly) in such a hydrogen atom.