## Astronomy: Chapter 8 Flashcards

Which electron energy level transition corresponds to a hydrogen atom absorbing a visible light photon that has a wavelength of 656 nanometers? The electron makes the transition from energy level 2 to energy level 3. You research the star Sirius and find that its spectral lines are blue-shifted. What does this tell you about Sirius?

## Bohr's model of hydrogen (article)

Bohr’s model of hydrogen is based on the nonclassical assumption that electrons travel in specific shells, or orbits, around the nucleus. Bohr’s model calculated the following energies for an electron in the shell, n n : E (n)=-\dfrac {1} {n^2} \cdot 13.6\,\text {eV} E (n) = −n21 ⋅13.6eV.

## Energy Level and Transition of Electrons

Imgur The energy of the electron of a monoelectronic atom depends only on which shell the electron orbits in. The energy level of the electron of a hydrogen atom is given by the following formula, where n n denotes the principal quantum number: E_n=-\frac {1312} {n^2}\text { kJ/mol}. E n = − n21312 kJ/mol.

## 6.3: Line Spectra and the Bohr Model

Figure \(\PageIndex{6}\): Absorption and Emission Spectra. Absorption of light by a hydrogen atom. (a) When a hydrogen atom absorbs a photon of light, an electron is excited to an orbit that has a higher energy and larger value of n. (b) Images of the emission and absorption spectra of hydrogen are shown here. (CC BY-NC-SA 3.0; anonymous).

## 6.4 Bohr’s Model of the Hydrogen Atom

When an atom absorbs a photon, the electron makes a transition to a higher-energy orbit. When an atom emits a photon, the electron transits to a lower-energy orbit. Electron transitions with the simultaneous photon absorption or photon emission take place instantaneously. The allowed electron transitions satisfy the second quantization condition:.

## Lesson Explainer: Electron Energy Level Transitions

The conversion between the two is 1 = 1. 6 × 1 0. e V J Every element has its own amount of energy for its shells, but this explainer will exclusively use the energy levels of hydrogen. The diagram below shows the energy levels, 𝑛, and corresponding electron binding energies of a hydrogen atom.

## 5.7: Spectral Lines of Atomic Hydrogen

The energy that is gained by the atom is equal to the difference in energy between the two energy levels. When the atom relaxes back to a lower energy state, it releases energy that is again equal to the difference in energy of the two orbits (see below). Figure 5.7.2 5.7. 2: Bohr model of the atom: electron is shown transitioning from the n.

## Emission spectrum of hydrogen (video)

In a hydrogen atom, why would an electron fall back to any energy level other than the n=1, since there are no other electrons stopping it from falling there? • ( 30 votes) Flag Just Keith 9 years ago The electron can only have specific states, nothing in between.

## Energy level diagrams and the hydrogen atom

The photon emitted in the n=4 to n=2 transition The photon emitted in the n=3 to n=2 transition The smaller the energy the longer the wavelength. The photon has a smaller energy for the n=3 to n=2 transition. In the hydrogen atom, with Z = 1, the energy of the emitted photon can be found using: E = (13.6 eV) [1/n f 2 – 1/n i 2] Atoms can also.

## Transitions Hydrogen Energy Levels

The formula defining the energy levels of a Hydrogen atom are given by the equation: E = -E0/n2, where E0 = 13.6 eV ( 1 eV = 1.602×10-19 Joules) and n = 1,2,3… and so on. The energy is expressed as a negative number because it takes that much energy to unbind (ionize) the electron from the nucleus. It is common convention to say an unbound.