The Balmer series refers to the spectral lines of hydrogen, associated to the emission of photons when an electron in the hydrogen atom jumps from a level $n \geq 3$ to the level $n=2$ .

The wavelength associated to each spectral line of the Balmer series is given by:

$\frac{1}{\lambda}=R_H (\frac{1}{2^2}-\frac{1}{n^2})$

where $R_H$ is the Rydberg constant for hydrogen, and where $n$ is the initial level of the electron that jumps to the level n = 2.

The first few spectral lines associated to this series are withing the visible part of the electromagnetic spectrum, and their wavelengths are:

656 nm (red, corresponding to the transition $3 \rightarrow 2$ )

486 nm (green, $4 \rightarrow 2$ )

434 nm (blue, $5 \rightarrow 2$ )

410 nm (violet, $6 \rightarrow 2$ )

All the following lines lie in the ultraviolet part of the spectrum. The limit of the Balmer series, corresponding to the transition $\infty \rightarrow 2$ , is at 364.6 nm.

4 0

3 years ago

Which statement is true about the element shown here? A) This element tends to gain electrons to become stable. B) This element

cestrela7 [59]

ITS C

This element tends to lose 2 electrons to become a 2+ ion, is the correct statement regarding the element calcium. Calcium has 2 electrons in its outer shell and it is easier to lose them than it is to gain enough to become stable. When stable it has 2 more protons than electrons forming a 2+ ion.

8 0

3 years ago

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