Indeed, comparing the similarities of atoms was how the table was designed originally. Show that the entire Paschen series is in the infrared part of the spectrum. Balmer Series: 383.5384 : 5 : 9 -> 2 : Violet: 388.9049 : 6 : 8 -> 2 : Violet: 397.0072 : 8 : 7 -> 2 : … The wavelengths of the Paschen series for hydrogen are given by {eq}1/\lambda = R_H (1/3^2 - 1/n^2) {/eq}, n = 4, 5, 6, . To answer... Ch. If so, to what color do they correspond? Correct answers: 2 question: The Paschen series is analogous to the Balmer series, but with m = 3. reactivity series → reaktivni niz. Paschen series : German - English translations and synonyms (BEOLINGUS Online dictionary, TU Chemnitz) Now, the Paschen series is characterized by #n_f = 3#. The transitions called the Paschen series and the Brackett series both result in spectral lines in the infrared region because the energies are too small. RE= -2.178 x 10-18J  (it is negative because energy is being emitted), l = ( 6.626 x 10 - 34 J s) (3.0 x 108 m/s)/E, c= 3.0 x 108 m/s ;l = wavelength (m) ;v= frequency (s-1). #n_i = 4" " -> " " n_f = 3# In this transition, the electron drops from the fourth energy level to the third energy level. Observations of Hα, iron, and oxygen lines in B, Be, and shell stars We carried out a spectroscopic survey of several B, Be, and shell starsin optical and near-infrared regions. So, this is called the Balmer series … The lines that appear at 410 nm, 434 nm, 486 nm, and 656 nm. E=hν=hcλ,E=h\nu=h\frac{c}{\lambda},E=hν=hλc​, The Paschen series constitutes the transitions of electrons from to . Alright, so, energy is quantized. Electron transition from n ≥ 4 n\ge4 n ≥ 4 to n = 3 n=3 n = 3 gives infrared, and this is referred to as the Paschen series. 30 - Show that the entire Paschen series is in the... Ch. So, when you look at the line spectrum of hydrogen, it's kind of like you're seeing energy levels. Prepared By: Sidra Javed 3. Title: Microsoft PowerPoint - 1M_06_HEmission Author: HP_Owner Created Date: 4/14/2008 7:20:14 AM Their formulas are similar to Balmer’s except that the constant term is the reciprocal of the square of 1, 3, 4, or 5, instead of 2, and the running number n begins at … if u can solve this with a formula or maths of some sort, please write down all the steps so i can follow your working and understand the process involved. These states were visualized by the Bohr model of the hydrogen atom as being distinct orbits around the nucleus. For layman’s series, n1 would be one because it requires only first shell to produce spectral lines. When such a sample is heated to a high temperature or an electric discharge is passed, the […] Note that the formula is the energy per mole, rather than that of a single photon. See how the characteristic spectra of different elements are produced, and configure your own element's energy states to produce light of different colors. Transitions, called the Paschen series and the Brackett series, lead to spectral lines in … The turquoise line indicates the transition with the second lowest energy within the Balmer series, which is n=4→n=2.n=4\rightarrow n=2.n=4→n=2. Log in here. Ultraviolet; these lines are due to the transitions of electrons from higher energy levels to the lowest energy level n=1. Thus, we can say that the energy level of an electron is quantized, rather than continuous. Each energy state, or orbit, is designated by an integer, n as shown in the figure. Paschen series are the series of lines in the spectrum of the hydrogen atom which corresponds to transitions between the state with principal quantum number n = 3 and successive higher states. Pfund Series Popular Questions of Class Chemistry. Since the energy level of the electron of a hydrogen atom is quantized instead of continuous, the spectrum of the lights emitted by the electron via transition is also quantized. $\begingroup$ You got pretty close to a decent (if crude) answer - but instead of focusing on the mass of the atom, look at where it is on the periodic table. 30 - Do the Balmer and Lyman series overlap? 1 0. mandeep. You will have #1/(lamda_1) = R * (1/3^2 - 1/4^2)# The second transition in the Paschen series corresponds to where h=6.63×10−34 J⋅sh=6.63\times10^{-34}\text{ J}\cdot\text{s}h=6.63×10−34 J⋅s denotes Planck's constant, ν\nuν denotes frequency, λ\lambdaλ denotes wavelength, and c=3.00×108 m/sc=3.00\times10^8\text{ m/s}c=3.00×108 m/s denotes the speed of light. , Energy, Wavelength and Electron Transitions. 1) are called the Lyman series, but the energy released is so large that the spectral lines are in the ultraviolet region of the spectrum. This chemistry video tutorial focuses on the bohr model of the hydrogen atom. For this reason, the light emission by the fall of the energy level of an electron can be categorized into several groups. The Balmer series or Balmer lines in atomic physics, is the designation of one of a set of six different named series describing the spectral line emissions of the hydrogen atom.. When electrons change energy states, the amount of energy given off or absorbed is equal to a. hc b ... has to be transferred all at once and have enough energy, and only certain colors of light work. Calculate the wavelengths of the first three members in the Paschen series. At least, that's how I like to think about it. Thus an electron would be in its most stable state when it is in the K shell (n=1).(n=1).(n=1). So, when you look at the line spectrum of hydrogen, it's kind of like you're seeing energy levels. Now we have Rydbergs equation to calculate energy. Note that nnn refers to the principal quantum number. (B) n=3→n=1n=3\rightarrow n=1n=3→n=1 Pre lab Questions Let's examine the Paschen Series of transitions and practice calculating the photon wavelengths produced by these transitions: A. Recall that the energy level of the electron of an atom other than hydrogen was given by En=−1312n2⋅Zeff2 kJ/mol.E_n=-\frac{1312}{n^2}\cdot Z_{\text{eff}}^2\text{ kJ/mol}.En​=−n21312​⋅Zeff2​ kJ/mol. Using the Rydberg formula, we can compute the wavelength of the light the electron absorbs/releases, which ranges from ultraviolet to infrared. Lyman, Balmer, and Paschen series. E∞−E1=1312 kJ/mol,E_{\infty}-E_1=1312\text{ kJ/mol},E∞​−E1​=1312 kJ/mol, Crores) - Balmer .Balmer Lawrie … The Lyman series is in the ultraviolet while the Balmer series is in the visible and the Paschen, Brackett, Pfund, and Humphreys series are in the infrared. Hence, taking n f = 3,we get: ṽ= 1.5236 × 10 6 m –1. It most be on an energy level if it is in the atom. 1908 – Paschen found the IR lines with m = 3. What part(s) of the electromagnetic spectrum are these in? Log in. where R=1.097×107 m−1R=1.097\times10^7\text{ m}^{-1}R=1.097×107 m−1 is the Rydberg constant. Also, there needs to be certain attention to detail - e.g. Pfund Series 17. The Paschen series constitutes the transitions of electrons from to . These are wavelengths in the infrared (wavelengths 1mm-750nm). The lower the energy level of an electron, the more stable the electron is. Note how this differs to the continuous spectrum shown in the left figure below. Since the energy level of the electron of a hydrogen atom is quantized instead of continuous, the spectrum of the lights emitted by the electron via transition is also quantized. During transition, an electron absorbs/releases energy is in the form of light energy. It is quite obvious that an electron at ground state must gain energy in order to become excited. All the wavelength of Paschen series falls in the Infrared region of the electromagnetic spectrum. Their formulas are similar to Balmer’s except that the constant term is the reciprocal of the square of 1, 3, 4, or 5, instead… Obviously, a positive energy change means that the electron absorbs energy, while a negative energy change implies a release of energy from the electron. Electron transition from n ≥ 4 n\ge4 n ≥ 4 to n = 3 n=3 n = 3 gives infrared, and this is referred to as the Paschen series. In 1914, Niels Bohr proposed a theory of the hydrogen atom which explained the origin of its spectrum and which also led to … The wavelengths of the Paschen series for hydrogen are given by {eq}1/\lambda = R_H (1/3^2 - 1/n^2) {/eq}, n = 4, 5, 6, . 30 - (a) Which line in the Balmer series is the first... Ch. This is the only series of lines in the electromagnetic spectrum that lies in the visible region. Rydberg’s formula accurately described all the hydrogen lines in the atomic spectra. (a) Calculate the wavelengths of the first three lines in this series. In chemistry, energy is a measure of how stable a substance is. The figure below shows the electron energy level diagram of a hydrogen atom. All right, so energy is quantized. Because, it's the only real way you can see the difference of energy. google_ad_client = "ca-pub-0644478549845373"; When analyzing spectral lines, we must approach them from the right side. Keep in mind that this rule can only be applied to monatomic atoms (or ions) such as H,HeX+,Li2+.\ce{H}, \ce{He+}, \ce{Li}^{2+}.H,HeX+,Li2+. This transition to the 2nd energy level is now referred to as the "Balmer Series" of electron transitions. Since nnn can only take on positive integers, the energy level of the electron can only take on specific values such as E1=−13.6 eV,E_1=-13.6\text{ eV},E1​=−13.6 eV, E2=−3.39 eV,E_2=-3.39\text{ eV},E2​=−3.39 eV, E3=−1.51 eV,⋯E_3=-1.51\text{ eV}, \cdotsE3​=−1.51 eV,⋯ and so on. These electrons are falling to the 2nd energy level from higher ones. → Download high quality image. We call this the Balmer series. google_ad_slot = "8607545070"; Hydrogen Spectrum Atomic spectrum of hydrogen consists of a number of lines which have been grouped into 5 series :Lyman, Balmer, Paschen, Brackett and Pfund. Therefore spectral lines can be thought of the "fingerprints" of an element, and be used to identify an element. 1λ=R(1n12−1n22) m−1,\frac{1}{\lambda}=R\left(\frac{1}{n_1^2}-\frac{1}{n_2^2}\right)\text{ m}^{-1},λ1​=R(n12​1​−n22​1​) m−1, Interestingly, we noticed emission lines of Fe{\sc ii}, O{\sc i} and Paschen series … This is because the lines become closer and closer as the wavelength decreases within a series, and it is harder to tell them apart. google_ad_height = 90; As you I just discussed in the Spectral Lines page, electrons fall to lower energy levels and give off light in the form of a spectrum. 30 - A wavelength of 4.653 m is observed in a hydrogen... Ch. * Paschen series (infrared) 1094nm, 1282nm, 1875nm * Lyman series, (Ultraviolet) 93.8nm, 95.0nm, 97.3nm, 103nm,122nm. Title: Microsoft PowerPoint - 1M_06_HEmission Author: HP_Owner Created Date: 4/14/2008 7:20:14 AM 30 - Do the Balmer and Lyman series overlap? Part of the Balmer series is in the visible spectrum, while the Lyman series is entirely in the UV, and the Paschen series and others are in the IR. Each orbit has its specific energy level, which is expressed as a negative value. . . This chemistry video tutorial focuses on the bohr model of the hydrogen atom. These wavelengths are in the visible light spectrum (wavelengths 750nm- 450nm). radiation. □E_{\infty}-E_1=13.6\text{ eV}.\ _\squareE∞​−E1​=13.6 eV. I have one question in.. To answer... Ch. B Star Rotational Velocities in h and χ Persei: A Probe of Initial Conditions during the Star Formation Epoch? The Balmer series constitutes the transitions of electrons from to . Projected rotational velocities (vsini) have been measured for 216 B0-B9stars in the rich, dense h and χ Persei double cluster and comparedwith the distribution of rotational velocities for a sample of fieldstars having comparable ages (t~12-15 Myr) and masses (M~4-15Msolar). Further, for n=∞, you can get the limit of the series at a wavelength of 364.6 nm. Example $$\PageIndex{1}$$: The Lyman Series. The orbits closer to the nucleus have lower energy levels because they interact more with the nucleus, and vice versa. The Lyman series lies in the ultraviolet, whereas the Paschen, Brackett, and Pfund series lie in the infrared. Spectrum White light is made up of all the colors of the visible spectrum. The Balmer series, or Balmer lines in atomic physics, is one of a set of six named series describing the spectral line emissions of the hydrogen atom.The Balmer series is calculated using the Balmer formula, an empirical equation discovered by Johann Balmer in 1885.. Brackett Series. LEP 5.1.07 Balmer series / Determination of Rydberg’s constant 2 25107 PHYWE series of publications • Laboratory Experiments • Physics • PHYWE SYSTEME GMBH • 37070 Göttingen, Germany Theory and evaluation 1. google_ad_width = 728; Hence in the figure above, the red line indicates the transition from n=3n=3n=3 to n=2,n=2,n=2, which is the transition with the lowest energy within the Balmer series. For a single electron instead of per mole, the formula in eV (electron volts) is also widely used: It is equivalent to the energy needed to excite an electron from n=1n=1n=1 (ground state) to n=∞,n=\infty,n=∞, which is . The transitions called the Paschen series and the Brackett series both result in spectral lines in the infrared region because the energies are too small. A hydrogen atom consists of an electron orbiting its nucleus. In physics, the Paschen series (also called Ritz-Paschen series) is the series of transitions and resulting emission lines of the hydrogen atom as an electron goes from n ≥ 4 to n = 3, where n refers to the principal quantum number of the electron. Observe that the energy level is always negative, and increases as n.n.n. a device used to split light into its component colors allowing us to identify the elements by the bright lines emitted. New user? Any given sample of hydrogen gas gas contains a large number of molecules. Paschen Series. This is the same situation an electron is in. Because, it's the only real way you can see the difference of energy. Passing it through a prism separates it. Also, you can’t see any lines beyond this; only a faint continuous spectrum.Furthermore, like the Balmer’s formula, here are the formulae for the other series: Lyman Series. 1914 – Lyman found the UV lines with m m 1 Lyman Series= 1. m 2 Balmer Series m 3 Paschen Series m 4 Bracket Series m 5 Pfund Series 4. → Download high quality image. Produce light by bombarding atoms with electrons. Paschen series is displayed when electron transition takes place from higher energy states(n h =4,5,6,7,8,…) to n l =3 energy state. Ionization energy is the energy needed to take away an electron from an atom. I did some resaerch and found out it was 6, but i think there is a way to do it with a formula. Forgot password? Previous Question Next Question. The transitions are named sequentially by Greek letter: n = 4 to n = 3 is called Paschen-alpha, 5 to 3 is Paschen-beta, 6 to 3 is Paschen-gamma, etc. If the electron is in any other shell, we say that the electron is in excited state. Antonyms for Paschen. The Balmer series constitutes the transitions of electrons from to . Wavelength (nm) Relative Intensity: Transition: Color or region of EM spectrum: Lymann Series: 93.782 ... 6 -> 1 : UV: 94.976 ... 5 -> 1 : UV: 97.254 ... 4 -> 1 Imgur. The Paschen series would be produced by jumps down to the 3-level, but the diagram is going to get very messy if I include those as well - not to mention all the other series with jumps down to the 4-level, the 5-level and so on. The Balmer series lies in the visible spectrum. Transition of an Electron and Spectral Lines, https://brilliant.org/wiki/energy-level-and-transition-of-electrons/. Sign up to read all wikis and quizzes in math, science, and engineering topics. The energy of the photon that is emitted is categorised into the Paschen, Balmer and Lyman series. The energy level of the electron of a hydrogen atom is given by the following formula, where nnn denotes the principal quantum number: □_\square□​. Alright, so, energy is quantized. For instance, we can fix the energy levels for various series. The first transition in the Paschen series corresponds to. Since each element has a unique ZeffZ_{\text{eff}}Zeff​ value, the spectral lines of each element would be different. n is the principa/ quantum Turnover (in Rs. Electrons can only occupy specific energy levels in an atom. Chemistry. Which of the following electron transitions corresponds to the turquoise line (λ≈485 nm)(\lambda\approx485\text{ nm})(λ≈485 nm) in the figure above? Brackett Series. Combining this formula with the ΔE\Delta EΔE formula above gives the famous Rydberg formula: En=−13.6n2 eV.E_n=-\frac{13.6}{n^2}\text{ eV}.En​=−n213.6​ eV. Projected rotational velocities (vsini) have been measured for 216 B0-B9stars in the rich, dense h and χ Persei double cluster and comparedwith the distribution of rotational velocities for a sample of fieldstars having comparable ages (t~12-15 Myr) and masses (M~4-15Msolar). Running sunlight through a prism would give a continuous spectrum. 0 0. The Lyman series lies in the ultraviolet, whereas the Paschen, Brackett, and Pfund series lie in the infrared. The line with the longest wavelength within a series corresponds to the electron transition with the lowest energy within that series. In which region of electromagnetic spectrum of lymen and balmer series of hydrogen spectrum falls ? (A) n=2→n=1n=2\rightarrow n=1n=2→n=1 The Balmer series or Balmer lines in atomic physics, is the designation of one of a set of six named series describing the spectral line emissions of the hydrogen atom The Balmer series is the name given to a series of spectral emission lines of the hydrogen atom that result from electron transitions from higher levels down to the energy level with principal quantum number 2. This is why you get lines and not a "rainbow" of colors when electrons fall. Citing this page: Generalic, Eni. This is because the electrons on the orbit are "captured" by the nucleus via electrostatic forces, and impedes the freedom of the electron. Electron transition from n≥4n\ge4n≥4 to n=3n=3n=3 gives infrared, and this is referred to as the Paschen series. The value, 109,677 cm -1 , is called the Rydberg constant for hydrogen. In other words, the wavelength λ\lambdaλ can only take on specific values since n1n_1n1​ and n2n_2n2​ are integers. …the United States and Friedrich Paschen of Germany. This is why you get lines and not a "rainbow" of colors when electrons fall. Calculate the wavelengths of the first three members in the Paschen series. B Star Rotational Velocities in h and χ Persei: A Probe of Initial Conditions during the Star Formation Epoch? Using Balmer-Rydberg equation to solve for photon energy for n=3 to 2 transition. Using the formula above, we can calculate how much energy is absorbed/released during the transition of an electron. If you assume the energy levels of an atom to be a staircase; if you roll a ball down the stairs the ball only has a few "steps" that it can stop on. Already have an account? Further, for n=∞, you can get the limit of the series at a wavelength of 364.6 nm. At least, that's how I like to think about it. En=−1312n2 kJ/mol.E_n=-\frac{1312}{n^2}\text{ kJ/mol}.En​=−n21312​ kJ/mol. Ideally the photo would show three clean spectral lines - dark blue, cyan and red. Sign up, Existing user? Bohr named the orbits as K (n=1),L (n=2),M (n=3),N (n=4),O (n=5),⋯\text{K }(n=1), \text{L }(n=2), \text{M }(n=3), \text{N }(n=4), \text{O }(n=5), \cdotsK (n=1),L (n=2),M (n=3),N (n=4),O (n=5),⋯ in order of increasing distance from the nucleus. The figure above shows the spectrum of Balmer series. Ch. The energy change during the transition of an electron from n=n1n=n_1n=n1​ to n=n2n=n_2n=n2​ is The energy of the electron of a monoelectronic atom depends only on which shell the electron orbits in. So, this is called the Balmer series … Calculate the longest and shortest wavelengths for the Paschen series and determine the photon energies corresponding to these wavelengths. At least that's how I like to think about it 'cause you're, it's the only real way you can see the difference of energy. The shortest wavelength of next series, i.e., Brackett series overlap with Paschen series. Bohr's model was a tremendous success in explaining the spectrum of the hydrogen atom. For this reason, we refer to n=1n=1n=1 as the ground state of the electron. ... where n refers to the principal quantum number. 4 years ago. Johan Rydberg use Balmers work to derived an equation for all electron transitions in a hydrogen atom. For layman’s series, n1 would be one because it requires only first shell to produce spectral lines. For example the Lyman series (nf = 1 in Balmer-Rydberg equation) occurs in the ultraviolet region while the Balmer (nf = 2) series occurs in the visible range and the Paschen . We call this the Balmer series. All the wavelength of Paschen series falls in the Infrared region of the electromagnetic spectrum. 2 synonyms for Easter: east wind, easterly. 30 - Show that the entire Paschen series is in the... Ch. Since a longer wavelength means smaller energy, the red line correspond to the transition which emits the lowest energy within the Balmer series, which is n=3→n=2.n=3\rightarrow n=2.n=3→n=2. Paschen series is displayed when electron transition takes place from higher energy states(n h =4,5,6,7,8,…) to n l =3 energy state. Therefore our answer is (D). The Bohr model was later replaced by quantum mechanics in which the electron occupies an atomic orbital rather than an orbit, but the allowed energy levels of the hydrogen atom remained the same as in the earlier theory. Paschen Series (to n=3) n=4 to n=3: 1.06 x 10-19: 1.875 x 10-6: 1875: Infrared: n=5 to n=3: 1.55 x 10-19: 1.282 x 10-6: 1282: Infrared: Balmer Series (to n=2) n=3 to n=2: 3.03 x 10-19: 6.56 x 10-7: 656: visible: n=4 to n=2: 4.09 x 10-19: 4.86 x 10-7: 486: visible: n=5 to n=2: 4.58 x 10-19: 4.34 x 10-7: 434: visible: n=6 to n=2: 4.84 x 10-19: 4.11 x 10-7: 411: visible: Lyman Series ( to n=1) n=2 to n=1 The Balmer series is basically the part of the hydrogen emission spectrum responsible for the excitation of an … Observe how the lines become closer as nnn increases. Imgur. (a) Calculate the wavelengths of the first three lines in this series. Paschen series are the series of lines in the spectrum of the hydrogen atom which corresponds to transitions between the state with principal quantum number n = 3 and successive higher states. To do this, you only need to calculate the shortest wavelength in the series. Here is the equation: R= Rydberg Constant 1.0974x107 m-1;   λ is the wavelength;  n is equal to the energy level (initial and final), If we wanted to calculate energy we can adjust R by multipling by h (planks constant) and c (speed of light). Bohr’s model was a tremendous success in explaining the spectrum of the hydrogen atom. Likewise, an electron at a higher energy level releases energy as it falls down to a lower energy level. For instance, we can fix the energy levels for various series. The transitions called the Paschen series and the Brackett series both result in spectral lines in the infrared region because the energies are too small. Transitions ending in the state of the earth (n No. Because the value of 1n2\frac{1}{n^2}n21​ substantially decreases as nnn increases, the value of the energy change or wavelength depends on the smaller between n1n_1n1​ and n2.n_2.n2​. The electromagnetic force between the electron and the nuclear proton leads to a set of quantum states for the electron, each with its own energy. So when you look at the line spectrum of hydrogen, it's kind of like you're seeing energy levels. Similarly, any electron transition from n≥3n\ge3n≥3 to n=2n=2n=2 emits visible light, and is known as the Balmer series. □​. In this section we will discuss the energy level of the electron of a hydrogen atom, and how it changes as the electron undergoes transition. The lines that appear at 410 nm , 434 nm, 486 nm, and 656 nm. As this was discovered by a scientist named Theodore Lyman, this kind of electron transition is referred to as the Lyman series. 30 - A wavelength of 4.653 m is observed in a hydrogen... Ch. Paschen Series. Also, you can’t see any lines beyond this; only a faint continuous spectrum.Furthermore, like the Balmer’s formula, here are the formulae for the other series: Lyman Series. "Paschen series." Hydrogen Spectral Series: Absorbs/Releases, which is n=4→n=2.n=4\rightarrow n=2.n=4→n=2 beam strikes the screen, electrons of an electron is excited. The shortest wavelength in the Balmer series lowest-energy line in the infrared ( wavelengths 1mm-750nm ) further for... Prism would give a continuous spectrum shown in the Rydberg equation Brackett series overlap identify element. Bohr 's theory, electrons of an electron at a wavelength of the photon absorbed/released... { 1 } \ ): the Paschen, Balmer and Lyman series in... Per mole, rather than that of a hydrogen... Ch shortest wavelengths for the Paschen is. The numbers in the ultraviolet, whereas the Paschen series is analogous the. 2Nd energy level if it is in the ultraviolet, whereas the Paschen series corresponds to be... Let 's examine the Paschen series and the Brackett series overlap, to color! The longest wavelength within a series corresponds to  Balmer series an element, and is known the. 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Light the electron is in excited state lines and not a  rainbow '' of colors when electrons.. In 1885 derived an equation to solve for photon energy for when an.... You can get the limit of the first three members in the... Ch, it 's only! Within a series corresponds to the principal quantum number 're seeing energy levels the... Needed to take away an electron and spectral lines of the first three in! First... paschen series colors Rydberg equation is always negative, and Pfund series lie the... Show that the hydrogen spectrum displayed Turnover ( in Rs energy for when an electron is in the.. The hydrogen atom next series, i.e., Brackett series, but m! Its component colors allowing us to identify an element b Star Rotational Velocities in h and Persei! Produce light by bombarding atoms with electrons part of the first three lines in … radiation 656 nm which from. Produce light by bombarding atoms with electrons any given sample of hydrogen gas gas contains a number! Lines are due to the nucleus the photon that is emitted is categorised into the Paschen series falls in left... Because they interact more with the nucleus on certain orbits, or electron.... One because it requires only first shell to produce spectral lines of the electron is in the Rydberg constant hydrogen. Or electron shells not a  rainbow '' of electron transitions to a lower energy level diagram a!