Question

The electron in a hydrogen atom transitions from the n = 2 energy level to the n = 5 energy level. What is the energy absorbed or liberated in this process? Let Planck’s constant h = 4.136 × 10⁻¹⁵ eV • s, the speed of light c = 3.00 × 10⁸ m/s, and the Rydberg constant R = 1.097 × 10⁷ m⁻¹.

6.11 eV is liberated.

2.86 eV is absorbed.

3.55 eV is absorbed.

2.86 eV is liberated.

A hypothetical atom has two excited states that produce a line spectrum that consists of three bands. The bands correspond to photons of energy 0.25 eV, 0.50 eV, and 0.75 eV. Which could be the energy levels of the excited states of the atom?

	0.75 eV and 1.00 eV above the ground state
	0.25 eV and 0.75 eV above the ground state
	0.25 eV and 0.50 eV above the ground state
	0.50 eV and 1.00 eV above the ground state

Answer 1

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