Emission Spectrum Uncovered: Discover the Secrets with Plainmath's Expert Help

A bright red star is moving towards Earth. Which of the choices best completes the following statement describing the spectrum of this star? A(n) ___________ spectrum that is _______ relative to an unmoving star.
A. continuous; blueshifted
B. continuous; redshifted
C. emission; redshifted
D.absorption; blueshifted
E. absorption; redshifted

Give the reasons of:
1. In a cavity laser, a beam could be transmitted through the cell without being distorted by the cell wall.
2. The statistical weight for most levels are essentially the in dense material.
3. Homogeneous broading.

If a black body is radiating at ${17}^{\circ <!--\; \circ \; -->}$ C. Calculate the (a) wave length at which maximum energy will be radiated and (b) energy per unit area per second radiated by this black body.

Consider a large number of hydrogen atoms, with electrons all initially in the n = 4 state. (a) How many different wavelengths would be observed in the emission spectrum of these atoms? (b) What is the longest wavelength that could be observed? (c) To which series does the wavelength found in (b) belong?

If the average number of photons emitted by an oscillatory pattern from the surface of a black object is (28-10.2) photon at room temperature.Calculate the following:
1. frequency of patterns emitted by this body.
2. wavelength associated with this emission.
3. within what range of the electromagnetic spectrum is this emission located

What lines would be missing for hydrogen in an absorption spectrum? What wavelengths are missing for hydrogen in an emission spectrum?

Do someone knows the units of the spectra provided here ? It seems obvious enough that it's said nowhere, but even Wikipedia and other sites are quite blurry on this point.
So, is it power (W), radiance($\mathrm{W}/{\mathrm{m}}^2\mathrm{s}\mathrm{r}$), or something else ?

Why can one observe an electronic transition of the 3s state to the 3p state in the emission spectrum of the nitrogen atom, but not in its absorption spectrum?
I know that the selection rules technically don't forbid either one since $\mathrm{\Delta <!--\; \Delta \; -->}\mathrm{\ell <!--\; \ell \; -->}=\pm <!--\; \pm \; -->1$ is permitted.

One of the visible lines in the hydrogen emission spectrum corresponds to the n = 6 to n = 2 electronic transition. What color light is this transition ?

How much does the gravitational redshift change a neutron star emission spectra disturbing so the measurement of its surface temperature?

I need to be able to convert an arbitrary emission spectrum in the visible spectrum range (i.e. for every wavelength between 380 and 780, I have a number between 0 and 1 that represents the "intensity" or dominance of that wavelength), and I need to be able to map any given spectrum into a particular color space (for now I need RGB or CIE-XYZ). Is it possible?
For the spectrum say I have the emission spectrum of a white light, then every wavelength in the spectrum will have an intensity of 1, whereas for a green-bluish light I'd have most of the wavelengths between 500 and 550 with an intensity close to 1, with other wavelengths gradually dropping in intensity. So the first spectrum should be converted to pure white whereas the other one would be converted to a green-bluish color in any color space.
Is there a way to do this?

A line of the Lyman series(nf=1) of the spectrum of hydrogen has a wavelength of 95nm. What was the "upper" quantum state (ni) involved in the associated electron transition?

When sodium is bombarded with electrons accelerated through a potential difference $\mathrm{\Delta <!--\; \Delta \; -->}V$, its x-ray spectrum contains emission peaks at 1.04 keV and 1.07 keV. Find the minimum value of $\mathrm{\Delta <!--\; \Delta \; -->}V$ required to produce both of these peaks.

I learnt that in astrophysical spectroscopy, the emission spectrum of distant stars is used to determine what they're made of. So why is it that our own Sun is emitting the whole spectrum ?

When light hits an atom (I will use a carbon atom for simplicity), if it is not in the absorption and/or emission spectrum of carbon, it will simply pass through without interacting with the atom. Whereas if it is in the absorption or emission spectrum it will be absorbed and either re-emitted or it will decay to become thermal energy.
However, if there are a lot of (carbon)atoms in close proximity (like in a block of coal), the light will (obviously) not pass through it no matter where it is on the visible spectrum. Why does this happen?

The wavelength of emitted radiation when an electron jumps orbits in the Bohr atomic model is given by
1/$\mathrm{\lambda <!--\; \lambda \; -->}$ = $R_H$ ($\frac{1}{n_f^2}$ - $\frac{1}{n_i^2}$) $Z^2$
But that of X-Ray emission is given by
1/$\mathrm{\lambda <!--\; \lambda \; -->}$ = $1.1\times <!--\; \times \; -->{10}^7$ ($\frac{1}{n_f^2}$ - $\frac{1}{n_i^2}$) $(Z-<!--\; -\; -->1{)}^2$
Why is there a difference? Why aren't X-Rays treated like any other emissions?

From my quick investigation, the spectrum is based on the Rydberg formula, and with a small change, would lead to
$\frac{1}{{\mathrm{\lambda <!--\; \lambda \; -->}}_{\mathrm{\mu <!--\; \mu \; -->}}}=\frac{m_{\mathrm{\mu <!--\; \mu \; -->}}}{m_e}\left(R(\frac{1}{n_1^2}-<!--\; -\; -->\frac{1}{n_2^2})\right)$
where $m_{\mathrm{\mu <!--\; \mu \; -->}}$ is the mass of a muon.
So, taking hydrogen as an example, we would observe similar bands, shifted into the x-ray/gamma range.
Is this correct?

I'm writing a program which generates the emission spectrum of an element with atomic number Z. To do this, I have used the equation:
$\frac{1}{\mathrm{\lambda <!--\; \lambda \; -->}}=R_{\mathrm{\infty <!--\; \infty \; -->}}{Z}^2(\frac{1}{n_1^2}-<!--\; -\; -->\frac{1}{n_2^2})$
Where $n_1$ is the number of the original energy level and $n_2$ is the number of the final energy level and where $n_1>n_2$
However, this does not calculate the intensity of the lines. Is there anyway to model the intensity using $n_1$, $n_2$ and/or $Z$, assuming that the brightest line has an intensity of 1?

Hydrogen gas absorbs light of wavelength 103 nm. Afterward, what wavelengths are seen in the emission spectrum?