# Atomic physics questions and answers

Recent questions in Atomic Physics
Sappeycuii 2022-05-14

### Energy vs wavelength relation is given by, $E\left(eV\right)=\frac{1241}{nm}$. Energy of H-atom in the ground state is -13.6eV as form the relation $E\left(eV\right)=-13.6\frac{{Z}_{eff}^{2}}{{n}^{2}}\left(eV\right)$. Find that in which transition on hydrogen atom is the wavelength 486.1 nm produced? To which seriesdoes it belong ?

spazzter08dyk2n 2022-05-14

### 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 $\mathrm{\Delta }\ell =±1$ is permitted.

Annabel Sullivan 2022-05-14

### What is the smallest-wavelength line in the Balmer series? Is it in the visible part of the spectrum?

Carina Valenzuela 2022-05-14

### 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 ?

quorums15lep 2022-05-13

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

Alisa Durham 2022-05-13

### 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?

Carley Haley 2022-05-13

### 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?

Waylon Mcbride 2022-05-13

### For the hydrogen atom, the Balmer Series is the series of line spectra produced when an election falls from any higher energy level and has n=2 as its final energy state. The longest wavelength is the Balmer Series is 656.7 nm. what was the initial principal energy level (n) associated with this photon.Will the energy value in the trasnistion be the geatest or smalles in the entie Balmer Series?

Leon Robinson 2022-05-13

### Calculate the longest wavelength of the hydrogen Balmer series using the Bohr model of the atom.

anniferathonniz8km 2022-05-10

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

quorums15lep 2022-05-10

### The first member of Balmer series of hydrogen atom has a wavelength of 6561 Å. Find wavelength of the second member of the Balmer series (in nm)

Autumn Pham 2022-05-10

### 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 ?

garcialdaria2zky1 2022-05-09

### Calculate the two longest wavelength of the Balmer series of triply ionized berillium (Z=4)

anniferathonniz8km 2022-05-08

### 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?

Amappyaccon22j7e 2022-05-08

### Which has a larger frequency the 4th line of Balmer series or the 4th line of the Lyman series ?Provide an explanation

Flakqfqbq 2022-05-08

### What electron transitions account for the Balmer series?

Lexi Chandler 2022-05-08

### The wavelength of emitted radiation when an electron jumps orbits in the Bohr atomic model is given by1/$\lambda$ = ${R}_{H}$ ($\frac{1}{{n}_{f}^{2}}$ - $\frac{1}{{n}_{i}^{2}}$) ${Z}^{2}$But that of X-Ray emission is given by1/$\lambda$ = $1.1×{10}^{7}$ ($\frac{1}{{n}_{f}^{2}}$ - $\frac{1}{{n}_{i}^{2}}$) $\left(Z-1{\right)}^{2}$Why is there a difference? Why aren't X-Rays treated like any other emissions?

hisyhauttaq84w 2022-05-08