Table of Contents

- 1 What is the wavelength of light associated with the n 3 to n 1 electron transition?
- 2 What is the wavelength of light emitted when the electron falls from n 5 to n 3?
- 3 What is the wavelength of the photons emitted by hydrogen atoms when they undergo n 5 to n 4 transitions?
- 4 Which transition shown below will require the absorption of the shortest wavelength photon?
- 5 What is N in Balmer equation?
- 6 What is the wavelength of a photon emitted during?
- 7 How does the Bohr model explain the spectrum of the hydrogen atom?

## What is the wavelength of light associated with the n 3 to n 1 electron transition?

Electron Transition | Energy (J) | Wavelength (nm) |
---|---|---|

Lyman Series ( to n=1) | ||

n=2 to n=1 | 1.632 x 10 -18 | 122 |

n=3 to n=1 | 1.93 x 10-18 | 103 |

n=4 to n=1 | 2.04 x 10-18 | 97.3 |

### What is the wavelength of light emitted when the electron falls from n 5 to n 3?

We’re going to use the Balmer Equation which relates wavelengths to a photon’s electronic transitions. The wavelength of the light emitted when an electron falls from n = 5 to n = 3 is 1.2819 x 10-6 m or 1281.9 nm.

#### What is the wavelength of the photons emitted by hydrogen atoms when they undergo n 5 to n 4 transitions?

The wavelength of the light emitted is 434 nm.

**What is the wavelength of the photon that has been released?**

The wavelength λ of the photon is 9.74×10-8 m.

**What is the wavelength of the emitted or absorbed photon?**

Only a photon with an energy of exactly 10.2 eV can be absorbed or emitted when the electron jumps between the n = 1 and n = 2 energy levels. l = hc/E. A photon with an energy of 10.2 eV has a wavelength of 1.21 x 10-7 m, in the ultraviolet part of the spectrum.

## Which transition shown below will require the absorption of the shortest wavelength photon?

This means that the transition that gives the shortest wavelength has the largest frequency, energy, and distance. Choice D, n = 3 to n = 1, will produce the shortest wavelength since the distance between the energy levels is the greatest. The answer is D. n = 3 to n = 1.

### What is N in Balmer equation?

The Balmer series is characterized by the electron transitioning from n ≥ 3 to n = 2, where n refers to the radial quantum number or principal quantum number of the electron. The transitions are named sequentially by Greek letter: n = 3 to n = 2 is called H-α, 4 to 2 is H-β, 5 to 2 is H-γ, and 6 to 2 is H-δ.

#### What is the wavelength of a photon emitted during?

What is the wavelength, in nm, of a photon emitted during a transition from the n = 5 state to the n = 2 state in the hydrogen atom? This should be a transition in the so called “Balmer Series”:

**What are the colors in the emission spectrum of hydrogen?**

Wavelength Color 656.2 red 486.1 blue-green 434.0 blue-violet 410.1 violet Four more series of lines were discovered in the emission spectrum of hydrogen by searching the infrared spectrum at longer wave-lengths and the ultraviolet spectrum at shorter wavelengths.

**When does hydrogen atom fall into a lower energy orbit?**

According to the Bohr model, the wavelength of the light emitted by a hydrogen atom when the electron falls from a high energy (n = 4) orbit into a lower energy (n = 2) orbit. Substituting the appropriate values of RH, n1, and n2 into the equation shown above gives the following result.

## How does the Bohr model explain the spectrum of the hydrogen atom?

Niels Bohr proposed a model for the hydrogen atom that explained the spectrum of the The Bohr modelwas based on the following assumptions. The electron in a hydrogen atom travels around the nucleus in a circular orbit. The energy of the electron in an orbit is proportional to its distance from the nucleus.