Skip to content
Login Register

#photon absorption

6 public questions tagged with this topic.

Bohr Model Energy Levels and Hydrogen Spectrum

Which of the following statements is correct about the absorption process in a hydrogen atom?

**Hydrogen transitions** example n=3→n=1 ΔE=13.6(1-1/9)=12.09 eV, photon 12.09 eV, λ=1240/12.09≈102.6 nm Lyman series, n=3→n=2 ΔE=1.89 eV Balmer visible Hα 656 nm. Absorption photon energy must match difference, if atom in n=2 absorbs 1.89 eV jumps to n=3, if absorbs 12.75 eV from ground 1→4 because -13.6+12.75=-0.85 eV = -13.6/16. Absorption occurs when an electron jumps to a higher energy level by absorbing a photon matching the energy difference between levels. Using E_n = -13.6/n² eV, r_n = n² a₀, L = n h/2π, R = R₀ A^¹/³, BE = Δm c² and 1 u = 931.5 MeV, evaluation yields Electron jumps to

Ref: NCERT > Physics Book > Atoms and Nuclei > Bohr Model Energy Levels and Hydrogen Spectrum

View Details
Atomic Models - Rutherford, Thomson and Bohr

A photon of energy 10.2 eV is absorbed by a hydrogen atom in the ground state. To which energy level does the electron j

**Bohr's stationary orbits** defined by angular momentum quantization L = n ħ, ħ = h/2π, n=1 ground state, electron in these orbits does not radiate despite acceleration, contrary to classical EM theory which predicts atom collapse due to energy loss via radiation, Bohr postulates to explain observed stability and discrete spectra. E₁ = -13.6 eV . E_n = E₁ + 10.2 = -13.6 + 10.2 = -3.4 eV . -3.4 = -(13.6/n²) ⇒ n² = 4 ⇒ n = 2 . Using E_n = -13.6/n² eV, r_n = n² a₀, L = n h/2π, R = R₀ A^¹/³, BE = Δm c² and 1 u

Ref: NCERT > Physics Book > Atoms and Nuclei > Atomic Models - Rutherford, Thomson and Bohr

View Details
Bohr Model Energy Levels and Hydrogen Spectrum

A hydrogen atom absorbs a photon of energy 12.75 eV from the ground state. To which energy level does it jump? (Use \( E

**Excitation** energy required to go from n=1 to n=3 is 12.09 eV, from ground to n=∞ ionization 13.6 eV, state n=∞ means ionized, electron free with zero energy, highest level reached by electron beam energy determines which levels can be excited, e.g., 11 eV beam from ground can reach n=2 (10.2 eV) but not n=3 (12.09 eV), so max n=2. E₁ = -13.6 eV . E_n = -13.6 + 12.75 = -0.85 eV . -0.85 = -(13.6/n²) ⇒ n² = 16 ⇒ n = 4 . Using E_n = -13.6/n² eV, r_n = n² a₀, L = n h/2π, R = R₀ A^¹/³, BE =

Ref: NCERT > Physics Book > Atoms and Nuclei > Bohr Model Energy Levels and Hydrogen Spectrum

View Details
Bohr Model Energy Levels and Hydrogen Spectrum

A hydrogen atom absorbs a photon of energy 1.89 eV from the \( n = 2 \) state. To which energy level does it jump? (Use

**Bohr energy levels** E_n = -13.6/n² eV for hydrogen, negative indicating bound state, total energy = -13.6 eV ground state n=1, -3.4 eV n=2, -1.51 eV n=3, etc., photon energy for transition n_i → n_f is ΔE =13.6(1/n_f² -1/n_i²) eV, wavelength λ = hc/ΔE, h=6.6×10⁻³⁴ J·s, c=3×10⁸ m/s. Emission line spectrum characterized by discrete wavelengths because energy levels discrete. E₂ = -3.4 eV . E_n = -3.4 + 1.89 = -1.51 eV . -1.51 = -(13.6/n²) ⇒ n² = 9 ⇒ n = 3 . Using E_n = -13.6/n² eV, r_n = n² a₀, L = n h/2π, R = R₀ A^¹/³, BE = Δm

Ref: NCERT > Physics Book > Atoms and Nuclei > Bohr Model Energy Levels and Hydrogen Spectrum

View Details