## Which transition would give light the shortest wavelength?

When an electron absorbs sufficient energy and becomes excited, it would jump to a higher level. The diagram below shows how much energy is required when an electron goes from 1 shell to another. Therefore, the electronic transition would give the light of the shortest wavelength is 3.

## Which transition in a hydrogen atom would emit the shortest wavelength of light?

Choice D, n = 3 to n = 1, will produce the shortest wavelength since the distance between the energy levels is the greatest.

## Which of the following transitions of an electron in hydrogen atom emits of the lowest wavelength?

The transition n2=∞ to n1=2 emits radiation of the lowest wavelength. This transition corresponds to maximum energy of emitted radiation. It is equal to the ionization energy and corresponds to the energy required when an electron is completely removed from ground state of hydrogen atom.

## Which type of electromagnetic radiation is lowest in energy?

Red has the lowest energy and violet the highest. Beyond red and violet are many other kinds of light our human eyes can’t see, much like there are sounds our ears can’t hear. On one end of the electromagnetic spectrum are radio waves, which have wavelengths billions of times longer than those of visible light.

## Why is a shorter wavelength of light emitted?

The energy difference between n=3 and n=2 is greatest because the energy differences get closer together with increasing n. The greater the energy difference results in an emitted photon of greater energy and therefore shorter wavelength.

## Which transition has the longest wavelength?

2 transitionn=3ton=2 transition corresponds to the longest wavelength transition.

## Which transition has the highest energy?

Fig 1: Energy levels of electronic transitions 1 shows the energy requirements for different electronic transitions. 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.

## What is the transition of electrons in a hydrogen atom?

The Rydberg formula explains the different energies of transition that occur between energy levels. When an electron moves from a higher energy level to a lower one, a photon is emitted. The Hydrogen atom can emit different wavelengths of light depending on the initial and final energy levels of the transition.

## Which one of the following transitions of an electron in hydrogen atom emits radiation of the largest wavelength?

Higher the value of the principle quantum number to which electron is jumping, longer will be the wavelength. So, n = 6, p = 8 transition produces longest wavelength.

## Are shorter wavelengths stronger?

We usually measure this as the number of wavelength cycles that pass per second. The units for this measurement are Hertz (hz). That means that longer wavelengths have a lower frequency. Conclusion: a longer wavelength means a lower frequency, and a shorter wavelength means a higher frequency!

## Which is transition would emit the shortest wavelength?

And since n=3 to n=1 has a higher energy emitted than from n=2 to n=1, the one with the higher energy emitted would have the shorter wavelength as Wavlength and Energy are inversely related. Light is emitted when an electron jumps from higher orbit to lower orbit.

## What is the wavelength of light emitted when the electron?

What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2? λ = 4.86×10−5cm= 486×10−9m = 486nm.

## Which is one of the following electron transitions between energy levels?

The electron transitions between first and fourth energy levels (n4 →n1) in the hydrogen atom produces the line of shortest wavelength in hydrogen spectrum. Among the given transitions, the energy difference for the transition n4

## Where does the light emission of an electron fall?

For this reason, the light emission by the fall of the energy level of an electron can be categorized into several groups. If an electron falls from any n=1, n = 1, then the wavelength calculated using the Rydberg formula gives values ranging from 91 nm to 121 nm, which all fall under the domain of ultraviolet.