Why is a shorter wavelength of light emitted when an electron falls from N 4 to N 1?

Why is a shorter wavelength of light emitted when an electron falls from N 4 to N 1?

Therefore, from n=4 to n=1, higher energy is emitted, higher energy means higher frequency which means shorter wavelength.

What is the shortest wavelength photon it can emit?

The transition from the highest to the lowest energy levels would involve the greatest energy change and thus the shortest wavelength, x nm. An atom emits yellow light when an electron makes the transition from the n = 5 to the n = 1 level.

Which transition has minimum wavelength?

– Therefore, n = 3 to n = 1 transition will have the least wavelength.

Which electronic transition has the largest wavelength?

Longest wavelength goes with lowest energy: Thus transition between n = 1 and n = 2 corresponds to the longest wavelength. Likewise, the transition between n = 1 and n = 4 (highest energy) corresponds to the shortest wavelength.

What is the wavelength of third line of Balmer series?

434 nm

Which of the following would show a greater wavelength?

Answer. In this order the third compound has longest wavelength. Because considering the large conjugated systems the peak wavelength of absorption tends to be shifted towards the long wavelength region. Absorption peaks tend to be larger so the wave length is largest in this case when comparing with other cases.

Which of the following electron transition will emit the highest frequency of light?

The transition with the greatest distance is 5p → 1s, which is n = 5 going to n = 1. This means this transition also has the largest energy and frequency. The answer is d. 5p → 1s.

Which transition will have the highest energy?

The energy requirement order for excitation for different transitions is as follows. n→∏* transition requires lowest energy while σ→σ* requires highest amount of energy.

Which one of the following transition of an electron in hydrogen atom emits radiation of lowest wavelength?

The transition n2=∞ to n1=2 emits radiation of the lowest wavelength. This transition corresponds to maximum energy of emitted radiation.

In which of the following DD electron transition requires the radiation of minimum wavelength?

Answer. Answer: n₄ to n₁ will have the minimum wavelength.

Which one of the following transitions of an electron in a hydrogen atom will emit maximum energy?

Maximum energy is liberated for transition En→E1 and minimum energy for En→En−1 so n3 → n1 transitions in hydrogen atoms emit photons of highest frequency (energy).

Which transition of electron in the hydrogen atom emits maximum energy?

Maximum energy is liberated for transition En​→E1​ and minimum energy for En​→En−1​ so n3​ → n1​ transitions in hydrogen atoms emit photons of highest frequency (energy).

What is the transition of electrons in a hydrogen atom?

The electron energy level diagram for the hydrogen atom. He found that the four visible spectral lines corresponded to transitions from higher energy levels down to the second energy level (n = 2). This is called the Balmer series.

What is the maximum energy liberated due to Balmer series transition?

For the Balmer series hc/λmax = 13.6 eV(¼ – 1/9) (n = 3 –> n = 2). For the Lyman series: hc/λmax = 13.6 eV(1/1 – ¼) (n = 2 –> n = 1). λmax(Balmer)/λmax(Lyman) = (1/1 – ¼) /(¼ – 1/9) = 27/5.

On what factor potential of hydrogen atom depends on?

The wavefunctions for the hydrogen atom depend upon the three variables r, θ, and φ and the three quantum numbers n, l, and ml. The variables give the position of the electron relative to the proton in spherical coordinates.

How do the four quantum numbers signify the state of an electron in a hydrogen atom?

To completely describe an electron in an atom, four quantum numbers are needed: energy (n), angular momentum (ℓ), magnetic moment (mℓ), and spin (ms). The first quantum number describes the electron shell, or energy level, of an atom.