Emission spectra of isoelectronic species

[sakabato93]

Do isoelectronic species have identical emission spectra? Bohr atom's are defined as chemical species that contain only one electron, and all Bohr atoms' energy levels can be defined with the following equation:

En= (-2.178e-18)/n^2

Since this is true for ALL Bohr atoms (H, He+, Li2+ etc.), does this mean all isoelectronic species have identical emission spectra? If so, that implies emission spectra only describe electronic structure, not necessarily the identity of the species, right?

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[AureatEagle]

Do isoelectronic species have identical emission spectra? Bohr atom's are defined as chemical species that contain only one electron, and all Bohr atoms' energy levels can be defined with the following equation:

En= (-2.178e-18)/n^2

Since this is true for ALL Bohr atoms (H, He+, Li2+ etc.), does this mean all isoelectronic species have identical emission spectra? If so, that implies emission spectra only describe electronic structure, not necessarily the identity of the species, right?

No. You're using the simplified version of the atom's energy levels that applies ONLY to hydrogen.

The REAL equation for the energy levels in a Bohr atom is the same equation multiplied by a factor of Z^2, where Z is the atom number of the atom. Thus, for hydrogen, Z^2 = 1, and the term is invisible. But for all other Bohr atoms, the factor of Z^2 is not 1 (e.g. for He+ it'd be 2^2 = 4), and the energy levels would be different.

 

[sakabato93]

No. You're using the simplified version of the atom's energy levels that applies ONLY to hydrogen.

The REAL equation for the energy levels in a Bohr atom is the same equation multiplied by a factor of Z^2, where Z is the atom number of the atom. Thus, for hydrogen, Z^2 = 1, and the term is invisible. But for all other Bohr atoms, the factor of Z^2 is not 1 (e.g. for He+ it'd be 2^2 = 4), and the energy levels would be different.

Gotcha! I appreciate the help!