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It is, of course, the same as that given previously in Figure 3.3.1 3.3. 1 for P1 P 1, but now plotted from the nucleus in both directions. This completes the description of the most stable state of the hydrogen atom, the state for which \ ( n = 1\).
- 7.3: The Atomic Spectrum of Hydrogen - Chemistry LibreTexts
Because a hydrogen atom with its one electron in this orbit...
- 1.8: The Bohr Theory of the Hydrogen Atom - Chemistry LibreTexts
Let us assume that we are able to place the electron in...
- 7.3: The Atomic Spectrum of Hydrogen - Chemistry LibreTexts
Because a hydrogen atom with its one electron in this orbit has the lowest possible energy, this is the ground state (the most stable arrangement of electrons for an element or a compound), the most stable arrangement for a hydrogen atom.
This diagram is for the hydrogen-atom electrons, showing a transition between two orbits having energies \(E_{4}\) and \(E_{2}\). Bohr was clever enough to find a way to calculate the electron orbital energies in hydrogen.
Let us assume that we are able to place the electron in Bohr's hydrogen atom into an energy state \(E_n\) for \(n>1\), i.e. one of its so-called excited states. The electron will rapidly return to its lowest energy state, known as the ground state and, in doing so, emit light.
An electron remains bound in the hydrogen atom as long as its energy is negative. An electron that orbits the nucleus in the first Bohr orbit, closest to the nucleus, is in the ground state, where its energy has the smallest value. In the ground state, the electron is most strongly bound to the nucleus and its energy is given by Equation \ref{6 ...
An electron remains bound in the hydrogen atom as long as its energy is negative. An electron that orbits the nucleus in the first Bohr orbit, closest to the nucleus, is in the ground state, where its energy has the smallest value. In the ground state, the electron is most strongly bound to the nucleus and its energy is given by Equation 6.46.
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 \(n\) denotes the principal quantum number: \[E_n=-\frac{1312}{n^2}\text{ kJ/mol}.\]
