Quantum mechanics hydrogen atom

In summary, the conversation discusses the energy of a hydrogen atom and how it is affected by quantum mechanics. It is explained that the energy value derived by quantum mechanics is different from what would be expected based on the loss of electrostatic potential energy. The reason for this is because the Schrodinger equation takes into account the kinetic energy of the electron, which is not considered in the comparison to electrostatic potential energy.
  • #1
sharma_satdev
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The hydrogen atom is formed by the combination of proton and electron initially separated by infinite distance therefore energy of hydrogen atom is expected to be equal to loss of electrostatic potential energy but energy value as derived by quantum mechanics is different Why is it so
 
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  • #2
Well, if what you are saying was strictly true, then the atom wouldn't even be in a bound state by conservation of energy arguments. What happens is that the electron releases some of its energy by radiation, and so becomes trapped in one of the energy levels explained by quantum mechanics. Over time, if there is no additional energy put into the system, the electron will eventually emit enough radiation to end up in the "ground state" (the lowest lying quantum state).
 
  • #3
sharma_satdev said:
The hydrogen atom is formed by the combination of proton and electron initially separated by infinite distance therefore energy of hydrogen atom is expected to be equal to loss of electrostatic potential energy but energy value as derived by quantum mechanics is different Why is it so

You are ignoring that in the Schrodinger equation for the hydrogen atom, there is a kinetic energy part as well as the potential energy. Your comparison to the change in electrostatic potential ignores any kinetic energy of the electron.

Zz.
 

1. What is the hydrogen atom in quantum mechanics?

The hydrogen atom in quantum mechanics is a single electron system that is used as a simplified model to study the behavior of atoms. It consists of a positively charged nucleus (proton) and a negatively charged electron orbiting around it.

2. What is the role of quantum mechanics in understanding the hydrogen atom?

Quantum mechanics is used to describe the behavior and properties of the hydrogen atom. It explains how the electron is able to exist in discrete energy levels and how it moves around the nucleus. It also predicts the spectral lines of hydrogen and helps in understanding the stability of the atom.

3. What are energy levels in the hydrogen atom according to quantum mechanics?

Energy levels in the hydrogen atom are the specific quantized states that the electron can occupy. These levels are described by the principal quantum number (n) and represent the energy of the electron in that level. The lowest energy level is called the ground state and higher energy levels are called excited states.

4. How does quantum mechanics explain the spectral lines of hydrogen?

Quantum mechanics explains the spectral lines of hydrogen by considering the discrete energy levels of the electron. When an electron transitions from a higher energy level to a lower one, it emits a photon of specific energy, which corresponds to a specific wavelength of light. This results in the observed spectral lines.

5. What is the significance of the Schrödinger equation in understanding the hydrogen atom?

The Schrödinger equation is the fundamental equation of quantum mechanics and it describes the behavior and properties of the hydrogen atom. It allows for the calculation of the probability of finding the electron at a certain position and time, and it predicts the energy levels and spectral lines of the atom. It is essential in understanding the quantum behavior of the hydrogen atom.

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