**8.21×10−7m**is the shortest wavelength in the Paschen series of spectral lines.

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- Calculation:
- ∴ λL = 18750 Å
- The longest wavelength in the Paschen series is 18750 Å.

Paschen series is displayed when electron transition takes place from higher energy states(nh=4,5,6,7,8,…) to nl=3 energy state. All the wavelength of Paschen series falls in the **Infrared region** of the electromagnetic spectrum. The shortest wavelength of next series, i.e., Brackett series overlap with Paschen series.

The wavelength of the series limit of the Paschen series is **820.1 nm**.

The constant R is known as the **Rydberg constant**, after Johannes Robert Rydberg, a Swedish physicist, and, in the case of hydrogen, has a value of 109,737.31 reciprocal centimetres.

Question: The wavelengths of the Paschen series for hydrogen are given by **1/λ=RH(1/32−1/n2) 1 / λ = R H ( 1 / 3 2 − 1 / n 2 )** , n = 4, 5, 6, . . .

The shortest wavelength of the light emitted is when **the electron jumps from Infinity to 3**. For Li²⁺, λ = 9/R × 3² m. = 81/R m. This is the Required Answer.

For longest wavelength in Paschen series, n1 = 3 & n2 = 4. Hence, longest wavelength in Paschen series is **18752 A°**.

n | λ, air (nm) |
---|---|

4 | 1875 |

5 | 1282 |

6 | 1094 |

7 | 1005 |

Sol. For the third member of Paschen series n = 3, n, = 6 E, -E, = 2.18×109 D or E,-E, = **2.18×10-18 = 0.1817×10-18**.

The series limit for the Paschen series of hydrogen spectrum occurs at **8205.8Å**.

ANSWER↓ Wavelength of the first line of Paschen series is **`- (R = 109700 cm^-1`)**.

Determine the wavelength of the second line of the Paschen series for hydrogen. 1λ=(1.097×10-3Å-1)(132-152) or **λ=12,820Å**.

The wavelength of the Paschen series is **(820-1870) nm**. – We need to arrange the wavelengths of the first lines of Lyman, Balmer and Paschen series in increasing order and from the data above mentioned the answer comes out to be [{{lambda }_{L}},{{lambda }_{P}},{{lambda }_{B}}] in ascending order respectively.

In hydrogen spectrum, the shortest wavelength in Balmer series is **the ‘lambda ‘** .

Explanation: Just put value of 1/RH = **912 Angstroms** to get value of maximum wavelength.

**6557A˚**

The Paschen series in the hydrogen emission spectrum is formed by **electron transitions from ni>3 to nf=3**.

It is one of the hydrogen line series, such as the Lyman series and Balmer series and is named after Friedrich Paschen. Lines: **4 -> 3: 1875 nm**.

The wavelength (λ) **that is associated with an object in relation to its momentum and mass** is known as de Broglie wavelength. A particle’s de Broglie wavelength is usually inversely proportional to its force.

Answer: the Brackett Series for the emission spectra of hydrogen the final destination of a dropping electron from a higher orbit is n=4 . The third line of Brackett series is formed **when electron drops from n=7 to n=4**. The released wavelength lies in the Infra Red region of the spectrum.

n23Wavelength (nm)**121.56701****102.57220**

The value of the Rydberg constant R∞ is **10,973,731.56816 per metre**. When used in this form in the mathematical description of series of spectral lines, the result is the number of waves per unit length, or the wavenumbers.

Definition of series limit : the position (as of a wavelength, wave number, or frequency) in an atomic line spectrum toward which the series progresses in the ultraviolet direction and which though there is no line at this point corresponds to **the limiting value of photon energy characteristic of the series**.

The second line in Paschen series is obtained when the electron makes transition from. If you are seeing this message, that means **JavaScript has been disabled on your browser**, please enable JS to make this app work.

The wavelength of the second line of Balmer series in the hydrogen spectrum is **4861 A** .

When an electron drops from n = 2 to n = 1, **it emits a photon of ultraviolet light**. The step from the second energy level to the third is much smaller. It takes only 1.89 eV of energy for this jump.