Question:

Given below are two statements:
Statement I: In hydrogen atom, the frequency of radiation emitted when an electron jumps from lower energy orbit \((E_1)\) to higher energy orbit \((E_2)\), is given as \(hf = E_1 – E_2.\)
Statement II: The jumping of electron from higher energy orbit \((E_2)\) to lower energy orbit \((E_1)\) is associated with frequency of radiation given as
\(f=\frac{(E_2−E_1)}{h}\) This condition is Bohr’s frequency condition.
In the light of the above statements, choose the correct answer from the options given below:

Updated On: Jul 8, 2024
  • Both statement I and statement II are true
  • Both statement I and statement II are false
  • Statement I is correct but statement II is false
  • Statement I is incorrect but statement II is true
Hide Solution
collegedunia
Verified By Collegedunia

The Correct Option is D

Solution and Explanation

Radiation is not emitted but absorbed when an electron jumps from low energy to high energy. 

Also, \(E_2 – E_1\) is the energy of photon

\(⇒ E_2 – E_1 = hf\)

\(⇒f=\frac{E_2−E_1}{h}\)

The correct option is (D): Statement I is incorrect but statement II is true

Was this answer helpful?
0
0

Concepts Used:

Bohr's Model of Hydrogen Atom

Niels Bohr introduced the atomic Hydrogen model in 1913. He described it as a positively charged nucleus, comprised of protons and neutrons, surrounded by a negatively charged electron cloud. In the model, electrons orbit the nucleus in atomic shells. The atom is held together by electrostatic forces between the positive nucleus and negative surroundings.

Read More: Bohr's Model of Hydrogen Atom

Bohr's Theory of Hydrogen Atom and Hydrogen-like Atoms

A hydrogen-like atom consists of a tiny positively-charged nucleus and an electron revolving around the nucleus in a stable circular orbit. 

Bohr's Radius: 

If 'e,' 'm,' and 'v' be the charge, mass, and velocity of the electron respectively, 'r' be the radius of the orbit, and Z be the atomic number, the equation for the radii of the permitted orbits is given by r = n2 xr1, where 'n' is the principal quantum number, and r1 is the least allowed radius for a hydrogen atom, known as Bohr's radius having a value of 0.53 Å. 

Limitations of the Bohr Model

The Bohr Model was an important step in the development of atomic theory. However, it has several limitations.

  1. Bohr’s model of the atom failed to explain the Zeeman Effect (effect of magnetic field on the spectra of atoms).
  2. It failed to explain the Stark effect (effect of electric field on the spectra of atoms).
  3. The spectra obtained from larger atoms weren’t explained.
  4. It violates the Heisenberg Uncertainty Principle.