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Topic: Balmer series

	Balmer series
		A series of emission or absorption lines in the visible part of the hydrogen spectrum that is due to transitions between the second (or first excited) state and higher energy states of the hydrogen atom.
		The transition from the third level to the second level yields the red H-alpha emission line at 6563 Å; H-beta is in the green part of the spectrum at 4861 Å, H-gamma is in the violet (as are higher members of the series) at 4342 Å, and H-delta at 4101 Å.
		The Balmer jump is the relatively abrupt decrease in a continuous spectrum at about 3650 Å caused by hydrogen absorption lines in the Balmer series crowding to their series limit.
	www.daviddarling.info /encyclopedia/B/Balmer_series.html (206 words)

	Johann Jakob Balmer - Wikipedia, the free encyclopedia
		Johann Jakob Balmer (May 1, 1825 – March 12, 1898) was a Swiss mathematician and an honorary physicist.
		Balmer then used this formula to predict the wavelength for m = 7, and a colleague at the university was able to confirm a match to a high degree of accuracy.
		Balmer lines and Balmer series are named after him.
	en.wikipedia.org /wiki/Johann_Jakob_Balmer (332 words)

	Balmer Series: Free Encyclopedia Articles at Questia.com Online Library
		Balmer was awarded the 1983 Sidney E. Mead...religious community after 1664 issued in a series of disputes about clerical salaries over...Calendar of State Papers, Colonial Series: American and West Indes, 1700 (London...
		Randall Balmer, an evangelical who has written a series of influential studies of the...fundamentalist doctrine, the Left Behind series is unreconstructed and proud...evil is the moral heart of the series, and the utter lack of ambiguity...
		The series of spectral lines for which n f =1 is known as the Lyman series; that for n f =2 is the Balmer series; that for n f =3 is the Paschen series; that for n f =4 is the Brackett series; and that for n f =5 is the Pfund...
	www.questia.com /library/encyclopedia/balmer-series.jsp?l=B&p=1 (1382 words)

	Balmer (Site not responding. Last check: )
		However, despite being a mathematics teacher and lecturer all his life, Balmer is best remembered for his work on spectral series and his formula, given in 1885, for the wavelengths of the spectral lines of the hydrogen atom.
		It is surprising to realise that Balmer was sixty years old when he wrote the paper for which he is famous on the spectral lines of the hydrogen atom and that he was seventy-two when he wrote his only other work on this topic.
		The major contribution which Balmer made, however, depended much more on his mathematical skills than on his understanding of physics, for he produced a formula which gave the wavelengths of the observed lines produced by the hydrogen atom without giving any physical explanation.
	www-history.mcs.st-and.ac.uk /history/Mathematicians/Balmer.html (592 words)

	BIGS, physics: Spectral series of hydrogen
		From the Lyman series to the Brackett series, it can be seen that the energy applied forces the hydrogen electrons to a higher energy level by a quantum leap.
		The Balmer series becomes visible if the electron first falls to an excited state with the principal quantum number of n = 2 before returning to its initial state.
		The lines of the Balmer series (n = 2) are located in the visible range of the spectrum.
	www.bigs.de /en/shop/htm/termsch01.html (638 words)

	Atomic Absorption and Emission Spectra
		Thus, for example, the Balmer Series involves transitions starting (for absorption) or ending (for emission) with the first excited state of hydrogen, while the Lyman Series involves transitions that start or end with the ground state of hydrogen; the adjacent image illustrates the atomic transitions that produce these two series in emission.
		Because of the details of hydrogen's atomic structure, the Balmer Series is in the visible spectrum and the Lyman Series is in the the UV.
		Thus the longest wavelength Balmer transition is designated H with a subscript alpha, the second longest H with a subscript beta, and so on.
	csep10.phys.utk.edu /astr162/lect/light/absorption.html (408 words)

	Ch 445 Rydberg Analysis
		The independent variable is the reciprocal of the quantum numbers, with the lowest or series "ground" state implied to be one less than that of the lowest "excited" state of the series.
		The extent to which the spectral series deviates from that of a one electron atom is reflected in the apparent nuclear charge and in the ionization energy from the lowest state in the spectral series.
		Calculate and record in separate tables for each spectral series the energies of all the levels in the series, using the regression-derived dissociation energies and the ground state energy of the lithium atom.
	www.sou.edu /chem/ch445/rydberg.htm (1115 words)

	Brackett (1922) on his series
		Balmer series might be attributed to increasing the probability of transitions between the orbits of higher quantum numbers.
		It should be noticed that the higher members of the Paschen series occur in a region readily studied by photographic methods, plates hypersensitized by means of dicyanin being sensitive to 1.0 µ.
		The first two lines of a new series have been observed at wave-lengths 4.05 ±.03 µ and 2.63 ±.02 µ, due, according to Bohr's theory, to an electron falling into the fourth from the fifth and sixth rings of the hydrogen atom.
	dbhs.wvusd.k12.ca.us /webdocs/Chem-History/Brackett-1922/Brackett-1922.html (1916 words)

	The Balmer Relationship (Site not responding. Last check: )
		In 1890, Balmer's formula was revised by Johannes Robert Rydberg (1854-1919) to be expressed in wave numbers (1/lambda).
		It was not until after 1908 that improvements in spectroscopy allowed other series of lines to be actually found in the infrared and ultraviolet region of the electromagnetic spectrum.
		Example Calculation: Using Balmer's original formula, calculate the wavelength of the wavelength of the line Balmer predicted at the edge of the violet.
	gemini.tntech.edu /~tfurtsch/scihist/balmer.htm (334 words)

	Bohr's atom model
		For example for the first Balmer line (n = 3) the length of the light wave is equal 6563 angstroms, for n = 4 it is equal 4861, for n = 5 it is equal 4341 and for n = 6 it is equal 4102.
		The Pachen spectral series - placed in infra-red - is described by the first formula but n' is equal 3 here, and n is equal 4 or bigger.
		The Brackett spectral series - placed in infra-red - is described by the first formula but n' is equal 4 here, and n is equal 5 or bigger.
	library.thinkquest.org /19662/low/eng/model-bohr.html (1463 words)

	The Balmer Formula
		At the time, Balmer was nearly 60 years old and taught mathematics and calligraphy at a high school for girls as well as giving classes at the University of Basle.
		Balmer was very interested in mathematical and physical ratios and was probably thrilled he could express the wavelengths of the hydrogen spectrum using integers.
		Balmer was devoted to numerology and was interested in things like how many sheep were in a flock or the number of steps of a Pyramid.
	dbhs.wvusd.k12.ca.us /webdocs/Electrons/Balmer-Formula.html (844 words)

	Balmer spectral series: teaching notes
		Balmer reported observations by several researchers of ultraviolet lines in the hydrogen spectrum that matched the five predicted lines of the n=2 series quite well (i.e., the five wavelengths sought here in exercise 2)--although not quite so well as the four lines in the visible range.
		This series of hydrogen lines is now known as the Balmer series.
		Balmer's speculation that there were other series of spectral lines for hydrogen was also correct; however, his extended formula (used here in exercise 3) did not quite predict their wavelengths correctly.
	web.lemoyne.edu /~giunta/classicalcs/balmernote.html (257 words)

	Atomic Spectra (Lab 5) Hydrogen
		Emission or absorption processes in hydrogen occur in multiple series, which are sequences of lines corresponding to atomic transitions, each ending or beginning with the same energy level in hydrogen.
		Thus, for example, the Balmer Series involves transitions starting (for absorption) or ending (for emission) with the first excited state of hydrogen, while the Lyman Series involves transitions that start or end with the ground state of hydrogen.
		Because of the wide range of energy gaps in hydrogen's atomic structure, the Balmer Series is in the visible spectrum and the Lyman Series is in the the UV.
	www.unm.edu /~astro1/101lab/lab5/lab5_E.html (194 words)

	ChemLab - Chemistry 6 - Week 3 - Chemistry
		For example, transitions in the Lyman series, which appear in the UV region of the spectrum, all terminate at the ground electronic state of the hydrogen atom.
		Balmer's equation was simply an empirical fit to the observed emission frequencies, without any basis in theory.
		Thus, the lowest energy line (which is the longest wavelength line) in the Balmer series appears in the red portion of the visible spectrum.
	www.dartmouth.edu /~chemlab/chem6/hspect/full_text/chemistry.html (2521 words)

	HSC Online
		Bohr's findings are generally presented as a series of electron jumps from the 6th, 5th, 4th and 3rd electron orbital to the 2nd electron orbital out from the nucleus of the hydrogen atom to produce the four visible emission lines in the spectrum of hydrogen.
		Note the Balmer equation applies to orbital movements that result in wavelengths in the infrared and UV portions of the electromagnetic spectrum although the work of Balmer involved only the four visible spectral lines of the hydrogen spectrum.
		The Paschen series involves the movement of electrons from the 6th, 5th and 4th orbital to the 3rd orbital for example.
	hsc.csu.edu.au /physics/options/quanta_quarks/3004/phy981.html (1720 words)

	radiating
		The Balmer series is characterized by the electron transitioning from n ≥ 3 to n = 2, where n refers to the radial quantum number or principal quantum number of the electron.
		The Balmer series is particularly useful in astronomy because the Balmer lines appear in numerous stellar objects due to the abundance of hydrogen in the universe.
		Astrophysicists are able to use the Balmer lines to help determine the age of stars because younger stars are composed almost entirely of hydrogen, while older stars have greater quantities of heavier elements due to nuclear fusion.
	www.experiencefestival.com /radiating (390 words)

	Johann Jacob Balmer
		At first it appears that these four coefficients do not form a regular series; but if we multiply the numerators in the second and the fourth terms by 4 a consistent regularity is evident and the coefficients have for numerators the numbers 3
		For n = 1 we obtain the series 4/3, 9/8, 16/15, 25/24, and so on, for n = 2 the series 9/5, 16/12, 25/21, 36/32, 49/45, 64/60, 81/77, 100/96, and so on.
		In this second series the second term is already in the first series but in a reduced form.
	web.lemoyne.edu /~giunta/balmer.html (1120 words)

	[No title]
		The simplest example is pure Hydrogen gas which shows series of absorption or emission lines, some in visible light (the Balmer series), some in the UV (the Lyman series), IR (the Brackett series) and so on.
		The observed series of spectral lines are now explained as transitions to a given energy level.
		For Hydrogen, the Lyman series is all transitions to the ground state, the Balmer series is all transitions to the first excited state, and so on.
	www.ifa.hawaii.edu /~acowie/class99b/class_14.html (1582 words)

	Chemical Sciences: Line Spectrum of Hydrogen
		In the visible range, a series of lines is observed at the following wavelengths (in nm): 656.279, 486.133, 434.047, 410.174, 397.007, 388.905, 383.539, and 379.790.
		Additional series of lines were later discovered for hydrogen in the ultraviolet region of the spectrum (Lyman series, 1908) and in the infrared region of the spectrum (Paschen series, Brackett series, and Pfund series).
		In this equation k is the integer 1 (Lyman), 2 (Balmer), 3 (Paschen), 4 (Brackett), 5 (Pfund),...
	www.psigate.ac.uk /newsite/reference/plambeck/chem1/p01214.htm (1360 words)

	Balmer deuterium lines detected for the first time
		In 1997 and 1999 a team including researchers from the "Institut d'astrophysique de Paris" (Paris Institute of Astrophysics) detected visible deuterium lines belonging to the "Balmer series" using the Canada-France-Hawaii Telescope (CFHT).
		Observation of Balmer lines, which are in the visible spectrum, allows measurements from Earth-bound telescopes.
		Subsequent measurements from the VLT detected a dozen deuterium lines from the Orion Nebula and other nebulae, and confirmed the existence of the Balmer series.
	www.cnrs.fr /Cnrspresse/n388/html/en388a03.htm (350 words)

	Atomic Spectra
		The first mathematical formulation of the hydrogen series was given in 1885 by Johann Balmer, a high school teacher in Basel, Switzerland.
		The first successful explanation of the Balmer (as well as other) series was made by the Danish physicist, Niels Bohr.
		Bohr developed a theory which attempted to explain the Balmer series, as well as other observed series, and the Rydberg equation.
	www.sonoma.edu /chemistry/chem115A/atomicspectra.html (1029 words)

	The laws list: B
		The form of Bode's law (that is, a roughly geometric series) is not surprising, considering our theories on the formation of solar systems, but its particular formulation is thought of as coincidental.
		The distance corresponding the mean distance of an electron from the nucleus in the ground state of the hydrogen atom.
		The series which describes the emission spectrum of hydrogen when the electron is jumping to the fourth orbital.
	www.alcyone.com /max/physics/laws/b.html (774 words)

	Lecture 8: The Hydrogen Atom
		In 1890 Johannes Robert Rydberg generalized Balmer's formula to cover other hydrogen spectral lines (and also introduced the concept of the wave number, which is the reciprical of the wavelength).
		The various hydrogen spectral "series" are defined by their ending (bottom) level, e.g.
		There are names for series where the electron goes to levels 3, 4, 5, or 6 that are respectively called the Paschen, Brackett, Pfund and Humphreys series.
	instruct1.cit.cornell.edu /courses/astro101/lectures/lec08.htm (991 words)

	MIT Spectroscopy Lab - History
		Regularities among lines of the simpler spectra were noted, and several attempts were made to represent a series of lines as harmonics of one or more vibrations, all without success.
		Finally in 1885, J.J. Balmer showed that the wavelengths of the visible spectral lines of atomic hydrogen, now known as the Balmer series, could be represented by the simple mathematical formula,
		Equally important, the Bohr model presented a concept of the origin of spectra in which the frequency of a spectral line could be interpreted as a difference between energy levels, and a series of spectral lines as differences between one fixed energy level and a group of levels.
	web.mit.edu /spectroscopy/history/history-quantum.html (1322 words)

	(Q-3) Atomic Energy Levels
		It suggested that an electromagnetic wave gave up its energy in definite portions ("photons"), and the size of such portions was proportional to the frequency ν of an electromagnetic wave (ν is the Greek letter "nu"; the letter "f" is also used sometimes).
		Examining the Balmer formula and also the Ritz combination principle (further below), Bohr suggested that atoms could exist (even briefly) only in certain energy levels, and light was emitted only when an atom descended from some higher energy level to a lower one.
		In 1908 Ritz found that Balmer's formula was just one prominent example of a more widespread phenomenon, in "line spectra" emitted by hot gas.
	www.phy6.org /stargaze/Q3.htm (1120 words)

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