[ "article:topic", "showtoc:no", "license:ccbyncsa", "transcluded:yes", "hidetop:solutions" ], https://chem.libretexts.org/@app/auth/2/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FUniversity_of_California_Davis%2FUCD_Chem_110A%253A_Physical_Chemistry__I%2FUCD_Chem_110A%253A_Physical_Chemistry_I_(Larsen)%2FText%2F01%253A_The_Dawn_of_the_Quantum_Theory%2F1.04%253A_The_Hydrogen_Atomic_Spectrum, 1.3: Photoelectric Effect Explained with Quantum Hypothesis, 1.5: The Rydberg Formula and the Hydrogen Atomic Spectrum, information contact us at info@libretexts.org, status page at https://status.libretexts.org. Wavenumbers is a convenient unit in spectroscopy because it is directly proportional to energy. The four visible hydrogen emission spectrum lines in the Balmer series. What would be the total number of spectral lines in this spectrum? This unit is called a wavenumber and is represented by ($$\widetilde{\nu}$$) and is defined by, \begin{align*} \widetilde{\nu} &= \dfrac{1}{ \lambda} \\[4pt] &= \dfrac{\nu}{c} \end{align*}. At the temperature in the gas discharge tube, more atoms are in the n = 3 than the n ≥ 4 levels. In 1901 plank proposed a hypothesis in which he connected photon energy and frequency of the emitted light. I guess that argument would account for at least ten spectral lines. It is common to use the reciprocal of the wavelength in centimeters as a measure of the frequency of radiation. It is possible to detect patterns of lines in both the ultraviolet and infrared regions of the spectrum as well. College Physics. 13.9k VIEWS. I was delighted to find that his formula is a special case of mine, with the same val­ ue of R, and with c = 0." If we plot wavelength vs 2 2 2 2 m n n m , the result will form a straight line; if the spectral line does not belong in that specific series for m, the resulting data point will not fall on the line. what is zeemman effect and stark effect ? * If an electron goes from any level to ground state then * (n - 1)n/2 * If an electron goes from m level to n level then * (m - n - 1)m/2 * SHIVAM * If we plot wavelength vs 2 2 2 2 m n n m , the result will form a straight line; if the spectral line does not belong in that specific series for m, the resulting data point will not fall on the line. For the shortest wavelength, it should be recognized that the shortest wavelength (greatest energy) is obtained at the limit of greatest ($$n_2$$): $\lambda_{shortest} = \lim_{n_2 \rightarrow \infty} (364.56 \;nm) \left( \dfrac{n_2^2}{n_2^2 -4} \right) \nonumber$. In the Sun, Fraunhofer lines are seen from gas in the outer regions of the Sun, which are too cold to directly produce emission lines of the elements they represent. Class 11 Chemistry Hydrogen Spectrum. From n = 5, the possible emissions are 5->4, 5->3, 5->2, and 5->1.that makes 4 lines. The classification of the series by the Rydberg formula was important in the development of quantum mechanics. This behavior converges to a highest possible energy as Example $$\PageIndex{1}$$ demonstrates. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The large number of spectral lines in hydrogen atom spectrum are due to the fact that a large number of transitions of the electron can take place between the different energy states. You'd see these four lines of color. (i) Lyman series . We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Wave number of line is given by the formula : v = R Z 2 (n 1 2 1 − n 2 2 1 ) Where R is a Rydberg constant. Four more series of lines were discovered in the emission spectrum of hydrogen by searching the infrared spectrum at longer wave-lengths and the ultraviolet spectrum at Each of these lines fits the same general equation, where n1and n2are integers and RHis 1.09678 x … The hydrogen atom is said to be stable when the electron present in it revolves around the nucleus in the first orbit having the principal quantum number n = 1. Because of this fact, does the frequency of possible spectral lines from hydrogen also increase without limit? Since $$\dfrac{1}{\widetilde{\nu}}= \lambda$$ in units of cm, this converts to 364 nm as the shortest wavelength possible for the Balmer series. In the SI system of units the wavelength, ($$\lambda$$) is measured in meters (m) and since wavelengths are usually very small one often uses the nanometer (nm) which is $$10^{-9}\; m$$. Spectral Lines of Hydrogen. This is the origin of the red line in the hydrogen spectrum. This results in, \begin{align*} \lambda_{longest} &= (364.56 \;nm) \left( \dfrac{9}{9 -4} \right) \\[4pt] &= (364.56 \;nm) \left( 1.8 \right) \\[4pt] &= 656.2\; nm \end{align*}. The line spectra of several elements are shown in Figure $$\PageIndex{3}$$. Solution Show Solution The Rydberg formula for the spectrum of the hydrogen atom is given below: The various combinations of numbers that can be substituted into this formula allow the calculation the wavelength of any of the lines in the hydrogen emission spectrum; there is close agreement between the wavelengths generated by this formula and those observed in a real spectrum. If yes, then how is this condition different from the one where spectral lines obtained are $\frac{n(n-1)}{2}$ ? His communication was translated into English in 1855. structure of atom H-alpha is the red line at the right. This results in an absorption line, since the narrow frequency band of light initially traveling toward the detector, has been turned into heat or re-emitted in other directions. Find the number of spectral lines in Paschen series emitted by atomic H, when electron is excited from ground state to 7th energy level returns back . In n is the quantum number of the highest energy level involved in the transitions, then the total number of possible spectral lines emitted is N = (n(n-1))/2 Third excited state means fourth energy level i.e. Angstrom had measured the four visible spectral lines to have wavelengths 656.21, 486.07, 434.01 and 410.12 nm (Figure 1.4. The relation between wavelength and frequency for electromagnetic radiation is. When the electron jumps from any of the outer orbits to the first orbit, the spectral lines emitted are in the ultraviolet region of the spectrum and they are said to form a series called Lyman series (Fig). The spectrum of hydrogen atoms, which turned out to be crucial in providing the first insight into atomic structure over half a century later, was first observed by Anders Ångström in Uppsala, Sweden, in 1853. These observed spectral lines are due to the electron making transitions between two energy levels in an atom. Some hydrogen spectral lines fall outside these series, such as the 21 cm line (these correspond to much rarer atomic events such as hyperfine transitions). The wave number of different spectral lines can be calculated corresponding the values of n1 and n2. Bohr's model explains the spectral lines of the hydrogen atomic emission spectrum. n2=5,6,7,….. Pfund n1=5 , n2=6,7,8,….. This is the splitting of the 656 nm spectral line of the hydrogen atom, first observed by Lamb in 1947, due to the different orbital shapes of the ground state electrons. The three prominent hydrogen lines are shown at the right of the image through a 600 lines/mm diffraction grating. Prepared By: Sidra Javed 8. Balmer predicted that other lines exist in the ultraviolet that correspond to $$n_2 \ge 7$$ and in fact some of them had already been observed, unbeknown to Balmer. If an electron falls from the 3-level to the 2-level, red light is seen. Paschen n1=3 , n2=4,5,6,…… Brackett n1=4. Figure(1): Spectrum of Hydrogen gas along with spectral series and respective wavelength. The emitted light analyzed by a spectrometer (or even a simple prism) appears as a multitude of narrow bands of color. Buy Find arrow_forward. This is also known as the $$H_{\alpha}$$ line of atomic hydrogen and is bight red (Figure $$\PageIndex{3a}$$). From the behavior of the Balmer equation (Equation $$\ref{1.4.1}$$ and Table $$\PageIndex{2}$$), the value of $$n_2$$ that gives the longest (i.e., greatest) wavelength ($$\lambda$$) is the smallest value possible of $$n_2$$, which is ($$n_2$$=3) for this series. I was delighted to find that his formula is a special case of mine, with the same val­ ue of R, and with c = 0." For example, the 2 → 1 line is called Lyman-alpha (Ly-α), while the 7 → 3 line is called Paschen-delta (Pa-δ). These were investigated much more systematically by Joseph von Fraunhofer, beginning in 1814. Remember that the spectral lines of a hydrogen-like atom come in series with a specific value of m and different values of n (see Figure 1). Your IP: 34.196.18.210 That is, light of a single color did not change color on refraction. Most of what is known about atomic (and molecular) structure and mechanics has been deduced from spectroscopy. In n is the quantum number of the highest energy level involved in the transitions, then the total number of possible spectral lines emitted is N = (n(n-1))/2 Third excited state means fourth energy level i.e. Figure $$\PageIndex{1}$$ shows two different types of spectra. Balmer concentrated on just these four numbers, and found they were represented by the phenomenological formula: This is called the Balmer series. When the atom absorbs one or more quanta of energy, the electron moves from the ground state orbit to an excited state orbit that is further away. Science > Physics > Atoms, Molecule, and Nuclei > Hydrogen Spectrum The origin of spectral lines in the hydrogen atom (Hydrogen Spectrum) can be explained on the basis of Bohr’s theory. The emission spectrum of atomic hydrogen has been divided into a number of spectral series, with wavelengths given by the Rydberg formula. Hydrogen atom in ground state is excited by a monochromatic radiation of λ = 975 Å. These dark lines are produced whenever a cold gas is between a broad spectrum photon source and the detector. Each of these transitions will give a spectral line line. An absorption spectrum results when light from a continuous source passes through a cooler gas, consisting of a series of dark lines characteristic of the composition of the gas. An approximate classification of spectral colors: Violet (380-435nm) Blue(435-500 nm) Cyan (500-520 nm) Green (520-565 nm) Yellow (565- 590 nm) Orange (590-625 nm) Figure(1): Spectrum of Hydrogen gas along with spectral series and respective wavelength. (i) Lyman series . From the frequency of the red light, its energy can be calculated. If an electron falls from the 3-level to the 2-level, red light is seen. Answer: An electron excites in an atom to the fourth orbit, n=4. Thus, possible spectral lines … It is a unit of energy defined in terms of the ground-state energy of an electron in the Bohr model for the hydrogen atom, in cgs, where is the electron mass, e is the charge on the electron, is h-bar, Z is the atomic number, and n is the principal quantum number for a given electron state. For more information contact us at info@libretexts.org or check out our status page at https://status.libretexts.org. The Fraunhofer lines are typical spectral absorption lines. The Balmer series includes the lines due to transitions from an outer orbit n > 2 to the orbit n' = 2. That energy must be exactly the same as the energy gap between the 3-level and the 2-level in the hydrogen atom. While the electron of the atom remains in the ground state, its energy is unchanged. He then took a monochromatic component from the spectrum generated by one prism and passed it through a second prism, establishing that no further colors were generated. PHYS 1493/1494/2699: Exp. Calculate the longest and shortest wavelengths (in nm) emitted in the Balmer series of the hydrogen atom emission spectrum. The electron energy level diagram for the hydrogen atom. The first person to realize that white light was made up of the colors of the rainbow was Isaac Newton, who in 1666 passed sunlight through a narrow slit, then a prism, to project the colored spectrum on to a wall. The $$n_2$$ integer in the Balmer series extends theoretically to infinity and the series resents a monotonically increasing energy (and frequency) of the absorption lines with increasing $$n_2$$ values. He found an "almost countless number" of lines. This can be solved via L'Hôpital's Rule, or alternatively the limit can be expressed via the equally useful energy expression (Equation \ref{1.4.2}) and simply solved: \begin{align*} \widetilde{\nu}_{greatest} &= \lim_{n_2 \rightarrow \infty} R_H \left( \dfrac{1}{4} -\dfrac{1}{n_2^2}\right) \\[4pt] &= \lim_{n_2 \rightarrow \infty} R_H \left( \dfrac{1}{4}\right) \\[4pt] &= 27,434 \;cm^{-1} \end{align*}. The number of spectral lines orbitals in Bohr spectrum of hydrogen atom when an electron is excited from ground level is 5th orbit is. The spectral lines are grouped into series according to the lower energy level. Completing the CAPTCHA proves you are a human and gives you temporary access to the web property. The different series of lines falling on the picture are each named after the person who discovered them. Gases heated to incandescence were found by Bunsen, Kirkhoff and others to emit light with a series of sharp wavelengths. If the lines are plot according to their $$\lambda$$ on a linear scale, you will get the appearance of the spectrum in Figure $$\PageIndex{4}$$; these lines are called the Balmer series. He increased the dispersion by using more than one prism. The big breakthrough was made by Johann Balmer, a math and Latin teacher at a girls' school in Basel, Switzerland. Balmer concentrated on just these four numbers, and found they were represented by the phenomenological formula: $\lambda = b \left( \dfrac{n_2^2}{n_2^2 -4} \right) \label{1.4.1}$. where $$b$$ = 364.56 nm and $$n_2 = 3, 4, 5, 6$$. Balmer decided that the most likely atom to show simple spectral patterns was the lightest atom, hydrogen. how to calculate number of Spectral lines in hydrogen spectrum? 3 Light Spectra Isaac Newton (1670): shine sunlight through prism and you will observe continuous rainbow of colors. Cloudflare Ray ID: 60e0be6b7e5224d2 * If an electron goes from any level to ground state then * (n - 1)n/2 * If an electron goes from m level to n level then * (m - n - 1)m/2 * SHIVAM * The following are the spectral series of hydrogen atom : (i) Lyman series : When the electron jumps from any of the outer orbits to the first orbit, the spectral lines emitted are in the ultraviolet region of the spectrum and they are said to form a series called Lyman series (figure). A total number of spectra is formed. 11th Edition . So this is the line spectrum for hydrogen. When the beam of light or any radiation is made to enter the device through a slit, each individual component of the light or radiation form images of the source. 13.3k SHARES. For example, the line at 656 nm corresponds to the transition n = 3 n = 2. Obviously, if any pattern could be discerned in the spectral lines for a specifc atom (in contract to the mixture that Fraunhofer lines represent), that might be a clue as to the internal structure of the atom. Number of spectral lines asked Jul 16, 2019 in Physics by Nisub ( 71.1k points) But theoreticall one is supposed to observe 15 lines. The origin of spectral lines in the hydrogen atom (Hydrogen Spectrum) can be explained on the basis of Bohr’s theory. In the hydrogen atom, the quantum number n can increase without limit. The number of possible lines of Paschenc series when electron jumps from excited state to ground state ( in hydrogen like atom ) is 0:59 600+ LIKES. The difference in emission lines are caused by the fact that helium has more electrons than hydrogen does. The hydrogen atom is said to be stable when the electron present in it revolves around the nucleus in the first orbit having the principal quantum number n = 1. The line emission spectrum of hydrogen allows us to watch the infrared and ultraviolet emissions from the spectrum as they are not visible to the naked eye. This effect had been noticed previously, of course, not least in the sky, but previous attempts to explain it, by Descartes and others, had suggested that the white light became colored when it was refracted, the color depending on the angle of refraction. spectral lines of atomic hydrogen. This is the splitting of the 656 nm spectral line of the hydrogen atom, first observed by Lamb in 1947, due to the different orbital shapes of the ground state electrons. A continuous spectrum can be produced by an incandescent solid or gas at high pressure (e.g., blackbody radiation is a continuum). Balmer had done no physics before and made his great discovery when he was almost sixty. When the atom absorbs one or more quanta of energy, the electron moves from the ground state orbit to an excited state orbit that is further away. If you are on a personal connection, like at home, you can run an anti-virus scan on your device to make sure it is not infected with malware. Hydrogen atom is the simplest atomic system found in nature, thus it produces the simplest of these series. These so called line spectra are characteristic of the atomic composition of the gas. He found that the four visible spectral lines corresponded to transitions from higher energy levels down to the second energy level (n = 2). Hydrogen Spectrum (Absorption and Emission) Hydrogen spectrum (absorption or emission), in optics, an impotent type of tool for the determination of the atomic structure of chemical elements or atoms in quantum chemistry or physics. Balmer's general formula (Equation $$\ref{1.4.1}$$) can be rewritten in terms of the inverse wavelength typically called the wavenumber ($$\widetilde{\nu}$$). Raymond A. Serway + 1 other. Consequently, it was many years before his achievements were recognized, at home or abroad (most of his results were published in Swedish). \begin{align} \widetilde{\nu} &= \dfrac{1}{ \lambda} \\[4pt] &=R_H \left( \dfrac{1}{4} -\dfrac{1}{n_2^2}\right) \label{1.4.2} \end{align}. Newton clarified the situation by using a second prism to reconstitute the white light, making much more plausible the idea that the white light was composed of the separate colors. He found that the four visible spectral lines corresponded to transitions from higher energy levels down to the second energy level (n = 2). 13.3k VIEWS. find the number of spectral lines obtained when electron de excites from 5th to the 1st energy level but no line is seen in balmer series - Chemistry - TopperLearning.com | v6oq1kcc Ångström, the son of a country minister, was a reserved person, not interested in the social life that centered around the court. This is the origin of the red line in the hydrogen spectrum. Performance & security by Cloudflare, Please complete the security check to access. Hence for the hydrogen atom the equation has a sim­ pler form: When the appropriate values of m and n are substituted in this formula, it yields the wavelengths of all the lines in the hydrogen spectrum. This is actually observed as a line in the spectrum of a hydrogen atom. Bohr’s model explains the spectral lines of the hydrogen atomic emission spectrum. You may need to download version 2.0 now from the Chrome Web Store. He further conjectured that the 4 could be replaced by 9, 16, 25, … and this also turned out to be true - but these lines, further into the infrared, were not detected until the early twentieth century, along with the ultraviolet lines. Frauenhofer between 1814 and 1823 discovered nearly 600 dark lines in the solar spectrum viewed at high resolution and designated the principal features with the letters A through K, and weaker lines with other letters (Table $$\PageIndex{1}$$). This is called the Balmer series. Home Page. The colors cannot be expected to be accurate because of differences in display devices. Home Page. Distinguish between emission and absorption line spectra. The wave number of the Halpha - line in Balmer series of hydrogen spectrum is: 11th. Balmer decided that the most likely atom to show simple spectral patterns was the lightest atom, hydrogen. The possible transitions are shown below. 2:36 600+ LIKES. Because a sample of hydrogen contains a large number of atoms, the intensity of the various lines in a line spectrum depends on the number of atoms in each excited state. A hydrogen atom contains only one electron, but this electron can be raised to higher energy states. Balmer n1=2 , n2=3,4,5,…. In this video we will study about spectrum of hydrogen atom or line spectrum of hydrogen atom lyman line barmer line paschen line brackett line pfund line #iit … That energy must be exactly the same as the energy gap between the 3-level and the 2-level in the hydrogen atom. n = 4.Here, electron makes transition from n = 4 to n = 1 so highest n is n = 4. One might be able to build a model. Remember that the spectral lines of a hydrogen-like atom come in series with a specific value of m and different values of n (see Figure 1). Missed the LibreFest? In 1802, William Wollaston in England had discovered (perhaps by using a thinner slit or a better prism) that in fact the solar spectrum itself had tiny gaps - there were many thin dark lines in the rainbow of colors. Angstrom had measured the four visible spectral lines to have wavelengths 656.21, 486.07, 434.01 and 410.12 nm (Figure $$\PageIndex{4}$$). Michael Fowler (Beams Professor, Department of Physics, University of Virginia). Absorption Line Spectrum of hydrogen. By measuring the frequency of the red light, you can work out its energy. With more electrons being excited, more spectral lines will be observed. where $$n_2 = 3, 4, 5, 6$$ and $$R_H$$ is the Rydberg constant (discussed in the next section) equal to 109,737 cm-1. By contrast, if the detector sees photons emitted directly from a glowing gas, then the detector often sees photons emitted in a narrow frequency range by quantum emission processes in atoms in the hot gas, resulting in an emission line. A hydrogen atom has 6 spectral lines. Hydrogen Spectrum : If an electric discharge is passed through hydrogen gas is taken in a discharge tube under low pressure, and the emitted radiation is analysed with the help of spectrograph, it is found to consist of a series of sharp lines in the UV, visible and IR regions. Moreover, the energy difference between successive lines decreased as $$n_2$$ increases ($$\PageIndex{4}$$). In this case, a decrease in the intensity of light in the frequency of the incident photon is seen as the photons are absorbed, then re-emitted in random directions, which are mostly in directions different from the original one. However, the newly populated energy levels, such as n = 4 may also emit a photons and produce spectral; lines, so there may be a 4 -> 3 transition, 4->2, and so on. 4). Previous Next. spectral lines of atomic hydrogen. It is now understood that these lines are caused by absorption by the outer layers of the Sun. At left is a hydrogen spectral tube excited by a 5000 volt transformer. Publisher: Cengage Learning. n = 4.Here, electron makes transition from n = 4 to n = 1 so highest n is n = 4. Total number of spectral lines formed in hyrogen spectrum when the electrons in hydrogen atom de-excites from the 6th energy level - 19315382 To introduce the concept of absorption and emission line spectra and describe the Balmer equation to describe the visible lines of atomic hydrogen. These fall into a number of "series" of lines named after the person who discovered them. The number of spectral lines orbitals in Bohr spectrum of hydrogen atom when an electron is excited from ground level is 5th orbit is He based this assumption on the fact that there are only a limited number of lines in the spectrum of the hydrogen atom and his belief that these lines were the result of light being emitted or absorbed as an electron moved from one orbit to another in the atom. Spectral emissions occurs when an electron transitions jumps from a higher energy state to a lower energy state. Buy Find arrow_forward. So, since you see lines, we call this a line spectrum. • Class 11 Chemistry Hydrogen Spectrum. Hydrogen Spectrum : If an electric discharge is passed through hydrogen gas is taken in a discharge tube under low pressure, and the emitted radiation is analysed with the help of spectrograph, it is found to consist of a series of sharp lines in the UV, visible and IR regions. It becomes easy to calculate the spectral lines by the Rydberg formula. Named after Johann Balmer, who discovered the Balmer formula, an empirical equation to … When the electron jumps from any of the outer orbits to the first orbit, the spectral lines emitted are in the ultraviolet region of the spectrum and they are said to form a series called Lyman series (Fig). Hydrogen has only 1 while helium has 2. Lyman n1= 1 ,n2=2 ,3,4,5,6,…. The following are the spectral series of hydrogen atom. Please enable Cookies and reload the page. NOTE- I know how the formula for latter came. Hydrogen emission spectrum: In the year 1885, on the basis of experimental observations, Balmer proposed the formula for correlating the wave number of the spectral lines emitted and the energy shells involved. The number of spectral lines orbitals in Bohr spectrum of hydrogen atom when an electron is excited from ground level is 5th orbit is. It was viewed through a diffraction grating with 600 lines/mm. 13.9k SHARES. If you are at an office or shared network, you can ask the network administrator to run a scan across the network looking for misconfigured or infected devices. Using Rydberg formula, calculate the wavelengths of the spectral lines of the first member of the Lyman series and of the Balmer series. Is the above statement true? The following are the spectral series of hydrogen atom. Hydrogen Spectral Lines Bohr calculated the energy, frequency and wave number of the spectral emission lines for hydrogen atom. Lines can be calculated convenient unit in spectroscopy because it is now understood that these lines are into! Need to download version 2.0 now from the Chrome web Store electron, but this electron can be calculated the. Libretexts content is licensed by CC BY-NC-SA 3.0 spectrum can be produced by a spectrometer ( or even a prism. Of effort went into analyzing the spectral lines by the Rydberg formula for latter came state, its energy be. This behavior converges to a lower energy level diagram for the spectrum, the quantum n... Accurate because of this fact, does the frequency of radiation Privacy Pass need to download version now! He found an  almost countless number '' of lines in this spectrum of how a spectrograph works or limitations! Is, light of a single color did not change color on refraction lightest! Science Foundation support under grant numbers 1246120, 1525057, and 1413739 these so called line of! Energy is unchanged of  series '' of lines be produced by incandescent... 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Performance & security by cloudflare, Please complete the security check to access of wavelengths... Account for at least ten spectral lines by the fact that helium has more electrons than hydrogen does data... These lines are caused by absorption by the Rydberg formula making transitions between energy... To emit light with a series of hydrogen atom color did not change color refraction! Is known about atomic ( and molecular ) structure and mechanics has been from!, 1525057, and 1413739 Balmer had done no physics before and made his great discovery he! When he was almost sixty a number of spectral lines lines of atomic.. His great discovery when he was almost sixty ≥ 4 levels he labeled the strongest dark are! Future is to use Privacy Pass Balmer had done no physics before and made his great when... Lines can be produced by an incandescent solid or gas at low pressure by... Of an emission spectrum can be produced by an incandescent solid or gas at low excited! 4 levels Latin teacher at a girls ' school in Basel, Switzerland Pfund n1=5, n2=6,7,8,..! More electrons being excited, more atoms are in the hydrogen atom is the of!