# Question

The figure below represents part of the emission spectrum for a one- electron ion in the gas phase. All the lines result from electronic transitions from excited states to the n = 3 state.

a. What electronic transitions correspond to lines A and B?

b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.

a. What electronic transitions correspond to lines A and B?

b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.

## Answer to relevant Questions

Explain the photoelectric effect. The following numbers are the ratios of second ionization energy to first ionization energy: Na: 9.2 P: 1.8 Mg: 2.0 S: 2.3 Al: 3.1 Cl: 1.8 Si: 2.0 Ar: 1.8 Explain these relative numbers. Without looking at data in the text, sketch a qualitative graph of the third ionization energy versus atomic number for the elements Na through Ar, and explain your graph. Assume that a hydrogen atom’s electron has been excited to the n = 5 level. How many different wavelengths of light can be emitted as this excited atom loses energy? The Heisenberg uncertainty principle can be expressed in the form where E represents energy and t represents time. Show that the units for this form are the same as the units for the form used in this chapter:Post your question

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