Table of Contents

- 1 What is the wavelength of light emitted when an electron transitions from N 5 to N 2?
- 2 What is the wavelength of Balmer series?
- 3 Which color of visible light is emitted when an electron drops from n 3 to n 2?
- 4 What is the wavelength emitted during the transition of electron?
- 5 What is the maximum number of emission lines when n 6 drops to ground state?
- 6 What color is n 4 to n 2?
- 7 How are the transitions in the Balmer series named?
- 8 What was Balmer’s formula for the wavelength of light?

## What is the wavelength of light emitted when an electron transitions from N 5 to N 2?

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

n=5 to n=2 | 4.58 x 10-19 | 434 |

n=6 to n=2 | 4.84 x 10-19 | 411 |

Lyman Series ( to n=1) | ||

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

### What is the wavelength of Balmer series?

The visible light spectrum for the Balmer Series appears as spectral lines at 410, 434, 486, and 656 nm. The h alpha line is the red line at 656 nm and occurs due to the transition from n= 3 to n = 2.

**What color of light is emitted from a hydrogen atom that changes from n 6 to n 2?**

Question: When an excited electron in a hydrogen atom falls from n = 6 to n=2, a photon of violet light is emitted. If an excited electron in an Het ion falls from n = 5, which energy level must it fall to (nı) for violet light of a similar wavelength to be emitted? ni =

**What color of light is N 5 to N 2?**

Spectra basically is belonging the location of visible zone. When wavelength is in between 4000A0 to 5000A0 then, green color of light would the atom emit. When it changes from the n=5 level to n=2 level.

## Which color of visible light is emitted when an electron drops from n 3 to n 2?

red-light

The difference between these two energy levels will then give us the actual energy of the red-light photon that is emitted when an electron drops from the n = 3 level to the n = 2 level.

### What is the wavelength emitted during the transition of electron?

E2−E1 = ΔE, λ=ΔEhc. Since h and c are constant, ΔE corresponds to definite energy thus, each transition from one energy level to another will produce a light of definite wavelength. This is actually observed as a line in the spectrum of a hydrogen atom.

**What is the longest wavelength of Lyman series?**

Q. The shortest wavelength in Lyman series is 91.2 nm . The longest wavelength of the series is

- 121.6 nm.
- 182.4 nm.
- 243.4 nm.
- 364.8 nm.
- Water flows steadily through a horizontal pipe of a variable cross section.
- Which of the following statements is true?

**What is the formula of Balmer series?**

The wavelengths of these lines are given by 1/λ = RH (1/4 − 1/n2), where λ is the wavelength, RH is the Rydberg constant, and n is the level of the original orbital.

## What is the maximum number of emission lines when n 6 drops to ground state?

15

– Therefore the maximum number of emission lines formed when the excited electron of H atom in n = 6 drops to the ground state is 15.

### What color is n 4 to n 2?

In the emission spectrum for hydrogen, the color of light corresponding to the n = 4 to n = 2 electronic transition is blue.

**What happens when an electron transitions from n 3 to n 2?**

The photon has a smaller energy for the n=3 to n=2 transition. If a photon with an energy equal to the energy difference between two levels is incident on an atom, the photon can be absorbed, raising the electron up to the higher level.

**What happens when an electron in a hydrogen atom moves from n 2 to n 3?**

The energy in a hydrogen atom depends on the energy of the electron. The energy of the photon is the exact energy that is lost by the electron moving to its lower energy level. When the electron changes from n=3 or above to n=2, the photons emitted fall in the Visible Light region of the spectra.

## How are the transitions in the Balmer series named?

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 was Balmer’s formula for the wavelength of light?

Balmer’s formula Balmer noticed that a single wavelength had a relation to every line in the hydrogen spectrum that was in the visible light region. That wavelength was 364.506 82 nm.

**What is the quantum number of the Balmer series?**

Balmer series. The visible spectrum of light from hydrogen displays four wavelengths, 410 nm, 434 nm, 486 nm, and 656 nm, that correspond to emissions of photons by electrons in excited states transitioning to the quantum level described by the principal quantum number n equals 2.

**Which is the formula for the hydrogen Balmer series?**

The Hydrogen Balmer Series. general relationship, similar to Balmer’s empirical formula. This general relationship is known as the Rydberg formula and is given by. 22. 111 – if fi. R nn, λ nn ⎡⎤ =⎢⎥ ⎣⎦ > (2) where ni and nf are integers, 1, 2, 3, 4, 5, … up to infinity, with ni>nf. For the hydrogen atom, ni = 2 corresponds to the Balmer series.