Question

Calculate The Frequency Of The Light Emitted When An Electron In A Hydrogen Atom Makes Each Of The Following Transitions. A. N=4→N=3 B. N=5→N=1 C. N=5→N=4 D. N=6→N=5 *** Express The Frequency In Inverse Seconds ***

Calculate the frequency of the light emitted when an electron in a hydrogen atom makes each of the following transitions.
a. n=4→n=3
b. n=5→n=1
c. n=5→n=4
d. n=6→n=5
*** Express the frequency in inverse seconds ***

Answer 1

The frequency of light emitted in hydrogen atom transitions can be calculated using the formula Frequency = (E_initial - E_final) / Planck's constant. Substituting the energy values for each level, the frequencies can be calculated for the given transitions.

Step-by-step explanation:

When an electron in a hydrogen atom undergoes a transition from one energy level to another, it emits a photon of light with a specific frequency. The frequency of the light emitted can be calculated using the formula:

Frequency = (E_initial - E_final) / Planck's constant

Where E_initial is the energy of the initial level and E_final is the energy of the final level. Planck's constant is a fundamental constant in physics and is approximately equal to 6.626 x 10^-34 J s.

Using this formula, we can calculate the frequency of the light emitted for each of the given transitions:

1. a. N=4→N=3: Frequency = (E_4 - E_3) / Planck's constant
2. b. N=5→N=1: Frequency = (E_5 - E_1) / Planck's constant
3. c. N=5→N=4: Frequency = (E_5 - E_4) / Planck's constant
4. d. N=6→N=5: Frequency = (E_6 - E_5) / Planck's constant

Substituting the energy values for each level from the given information, we can calculate the frequencies.