What is the maximum number of emission lines when the excited electron of a H atom in n = 6 drops to the ground state?
Solution and Explanation
When the excited electron of an H atom in n= 6 drops to the ground state, the following transitions are possible:
Hence, a total number of (5 + 4 + 3 + 2 + 1) 15 lines will be obtained in the emission spectrum.
The number of spectral lines produced when an electron in the nth level drops down to the ground state is given by \(\frac {n(n - 1)}{2}\).
Given, n= 6
Number of spectral lines = \(\frac {6(6-1)}{2}\) = 15
Top Questions on Developments Leading to the Bohr’s Model of Atom
- Using s, p, d notations, describe the orbital with the following quantum numbers.
- n=1, l=0
- n = 3, l=1
- n = 4, l =2
- n=4, l=3
- CBSE Class XI
- Chemistry
- Developments Leading to the Bohr’s Model of Atom
- Yellow light emitted from a sodium lamp has a wavelength (λ) of 580 nm. Calculate the frequency (ν) and wavenumber (v) of the yellow light
- CBSE Class XI
- Chemistry
- Developments Leading to the Bohr’s Model of Atom
- What is the energy in joules, required to shift the electron of the hydrogen atom from the first Bohr orbit to the fifth Bohr orbit and what is the wavelength of the light emitted when the electron returns to the ground state ? The ground state electron energy is –2.18×10–11 ergs.
- CBSE Class XI
- Chemistry
- Developments Leading to the Bohr’s Model of Atom
- Calculate the wavenumber for the longest wavelength transition in the Balmer series of atomic hydrogen.
- CBSE Class XI
- Chemistry
- Developments Leading to the Bohr’s Model of Atom
- The energy associated with the first orbit in the hydrogen atom is –2.18×10–18 J atom–1. What is the energy associated with the fifth orbit ?
- Calculate the radius of Bohr’s fifth orbit for hydrogen atom.
- CBSE Class XI
- Chemistry
- Developments Leading to the Bohr’s Model of Atom
Questions Asked in CBSE Class XI exam
- Find the sum to indicated number of terms in each of the geometric progressions in 1, – a, \(a^2\), –\(a^3\), ... n terms (if a ≠ – 1).
- CBSE Class XI
- geometric progression
- Find n if n-1P3: nP3 = 1: 9.
- CBSE Class XI
- Permutations
- Give a brief description of the principles of the following techniques taking an example in each case.(a) Crystallisation (b) Distillation (c) Chromatography.
- CBSE Class XI
- Organic Chemistry- Some Basic Principles and Techniques
- Three reasons why the author’s grandmother was disturbed when he started going to the city school.
- CBSE Class XI
- The Portrait of a lady
- Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in \(C_2H_4\) and \(C_2H_2\) molecules.
- CBSE Class XI
- Bond Parameters
Concepts Used:
Atomic Spectra
The emission spectrum of a chemical element or chemical compound is the spectrum of frequencies of electromagnetic radiation emitted due to an electron making a transition from a high energy state to a lower energy state. The photon energy of the emitted photon is equal to the energy difference between the two states.
Read More: Atomic Spectra
Spectral Series of Hydrogen Atom
Rydberg Formula:
The Rydberg formula is the mathematical formula to compute the wavelength of light.
\[\frac{1}{\lambda} = RZ^2(\frac{1}{n_1^2}-\frac{1}{n_2^2})\]Where,
R is the Rydberg constant (1.09737*107 m-1)
Z is the atomic number
n is the upper energy level
n’ is the lower energy level
λ is the wavelength of light
Spectral series of single-electron atoms like hydrogen have Z = 1.
Uses of Atomic Spectroscopy:
- It is used for identifying the spectral lines of materials used in metallurgy.
- It is used in pharmaceutical industries to find the traces of materials used.
- It can be used to study multidimensional elements.