Balmer is well renowned for his research on the hydrogen spectral series. The part of the hydrogen emission spectrum that corresponds to electron transitions from higher orbicular states n>2 to the energy level with principal quantum number n=2 is a series of spectral lines known as the Balmer series. And the Balmer series consists of a sequence of spectral emissions in both ultraviolet and visible regions of the electromagnetic spectrum.

1. Balmer series
By
Jayam chemistry learners
P R E S E N T A T I O N

2. HISTORY HISTORY OF THE BALMER SERIES
In 1666, Sir Isaac Newton used this atomic emission
phenomenon to study the different colors of
sunlight. He used a prism to disperse the sunlight
into individual wavelengths. Then Newton kept a
screen to display the solar emission lines. To which
he named it a spectrum.
Since the 1550s, in the smelting of ores, the flame
color served as a qualitative application to
identify the chemical substances. Because each
chemical element imparts its characteristic color
to the flame when heated.
In 1885, Jakob Balmer discovered an empirical
equation to calculate the wavelengths of hydrogen
emission lines in the visible region of the hydrogen
spectrum. And it is termed the Balmer formula.

3. OVERVIEW
OVERVIEW OF THE BALMER SERIES
Balmer is well renowned for his research on the
hydrogen spectral series. The part of the
hydrogen emission spectrum that corresponds
to electron transitions from higher orbicular
states n>2 to the energy level with principal
quantum number n=2 is a series of spectral lines
known as the Balmer series. And the Balmer
series consists of a sequence of spectral
emissions in both ultraviolet and visible regions
of the electromagnetic spectrum.
With the suggestion of Eduard Hagenbach, he
utilized Angstrom’s measurements on solar
emissions to find a formula for the visible
spectral lines of hydrogen. It was popularly
known as the Balmer formula. And it computes
the wavelengths of the hydrogen emission lines
in the visible region.

4. HYDROGEN VISIBLE SPECTRUM
HYDROGEN
VISIBLE
SPECTRUM
In the visible zone, we observe four spectral lines
at wavelengths 656nm, 486nm, 434nm, and 410nm
correspond to electron transitions from energy
levels such as 3 to 2, 4 to 2, 5 to 2, 6 to 2 giving
characteristic red, aqua, blue and violet colored
emissions in the hydrogen spectrum. This portion
of the Balmer series is also known as the visible
hydrogen spectrum.
Out of these four spectral emissions, we observe
an intense spectral line during the electron
movement from the third energy level to the
second level. It is a bright red spectral line in the
emission spectra of hydrogen or the ionization
nebula.

5. VISIBLE
BALMER
SPECTRUM
VISIBLE BALMER SPECTRUM
These transitions are also
referred to sequentially by
Greek letters. The electron
transition from the third
stationary orbit to the second
is known as Hydrogen-alpha or
H-α. And Hydrogen beta refers
to the electron movement
from the fourth main energy
level to the second level. The
hydrogen gamma spectral line
is due to electron transference
from the fifth stationary
configuration to its early level.
Finally, the hydrogen delta
spectral line occurs by the
electron transition from the
sixth orbit to the ground state
n=2.

6. UV
BALMER
SPECTRUM UV BALMER SPECTRUM
From the spectral studies, Balmer found that
a single wavelength has relation to every
spectral line in the visible region of the
hydrogen spectrum. And that wavelength is
364.5 nm. Hence, it is also known as the
Balmer break.
The electron transitions from the principal
quantum number n>6 to the Balmer series
ground state n=2 emit spectral lines in the
ultraviolet region of the electromagnetic
spectrum. Further, Balmer colleagues Wilhelm
Vogel and William Huggins confirmed these
spectral emissions in the white stars.

7. ULTRAVIOLET
BALMER
SPECTRUM
UV BALMER SPECTRUM
The spectral line formed due
to the electron transition from
the static configuration n=7 to
the normal state n=2 is known
as hydrogen epsilon. The
hydrogen zeta emission line is
due to the electron transition
from top energy level n=8 to
the ground state n=2 at a
wavelength of about 389 nm.
Similarly, the electron
movement from n=9 to n=2
results in a spectral line
named hydrogen eta. Finally,
the spectral emission that
results from n=∞ to the Balmer
series ground state n=2 at
364.5 nm is the series limit of
the Balmer series.

8. THE
BALMER
FORMULA THE BALMER FORMULA
In 1888, the physicist Johannes Rydberg
generalized the Balmer formula with the
necessary modifications. The Rydberg formula
helps to calculate the wavelengths of all
spectral lines that occur in the hydrogen
spectrum with the help of an empirical fitting
parameter known as the Rydberg constant.
From the history of the Balmer series, we can
understand that physicists' experiments on
the atomic emission spectrum started in the
1550s. But they lacked an empirical formula to
imagine the wavelengths of spectral lines of
an element. In 1885, the Balmer equation was
the first empirical formula discovered to
estimate the wavelengths of spectral
emissions in the hydrogen spectrum.

9. THE
WAVELENGTH
OF
BALMER
SERIES
THE MAXIMUM &
MINIMUM WAVELENGTHS
The maximum wavelength for the Balmer
series is 656 nm, and the minimum wavelength
is 364.5 nm. Hence, the limits of the Balmer
series are 656 nm and 364.5 nm.
The electron transitions from n ≥3 to n=2
result in the emergence of a sequence of
spectral lines in the Balmer series of the
hydrogen spectrum. Consequently, the n1 and
n2 values of the Balmer series vary from 2 to
infinity.

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