Table of Contents

- 1 What electron transition takes the most energy?
- 2 Which transition produces a photon with the longest wavelength?
- 3 Which electronic transition in a hydrogen atom is associated with the smallest emission of energy?
- 4 Which element emits photons of highest energy?
- 5 Which is electron transition requires the most energy?
- 6 What does it mean when an electron undergoes a positive energy change?

## What electron transition takes the most energy?

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.

**Which transition in a hydrogen atom involves the largest change in energy?**

From the above calculations, it is seen that the largest amount of energy will be required for the the transition from n= 1 to n = 2. Hence, the correct option is 1.

**What do larger energy transitions by the electrons give off?**

When the electron changes levels, it decreases energy and the atom emits photons. The photon is emitted with the electron moving from a higher energy level to a lower energy level. The energy of the photon is the exact energy that is lost by the electron moving to its lower energy level.

### Which transition produces a photon with the longest wavelength?

Longest wavelength goes with lowest energy: Thus transition between n = 1 and n = 2 corresponds to the longest wavelength. Likewise, the transition between n = 1 and n = 4 (highest energy) corresponds to the shortest wavelength. 9.

**Which of the following transitions is associated with the largest amount of energy?**

Emission is a transition process from a higher energy level to a lower energy level. The energy in a transition depends on the distance between the energy levels: this means the transition with the greatest distance produces the largest energy.

**Which electron transition is the lowest energy?**

The lowest energy transition is going to be between four and 3. The energies get closer to each other as we increase in the energy levels. So the least amount of energy changes between three and 4. So when it falls from four down to three, that would be the lowest energy emission.

#### Which electronic transition in a hydrogen atom is associated with the smallest emission of energy?

Therefore, the electronic transition that requires the smallest energy to be absorbed by the hydrogen atom is from n = 4 to n = 6.

**Which electron transition in the hydrogen atom releases light at the highest wavelength?**

The transition with the greatest distance is 5p → 1s, which is n = 5 going to n = 1. This means this transition also has the largest energy and frequency. Therefore, the electron transition that produces light of the highest frequency in the hydrogen atom is a. 5p → 1s.

**Which electronic transition would most likely produce red light?**

The lowest energy and longest wavelength photon corresponds to the 3→2 transition and is red. The higher-energy transitions produce shorter wavelengths and the color moves towards the violet end of the spectrum (4→2, blue green; 5→2 and 6→2, violet).

## Which element emits photons of highest energy?

The photons of highest energy will be emitted by gold.

**Which of the following electronic transitions of hydrogen has the highest largest frequency?**

The transition with the greatest distance is 5p → 1s, which is n = 5 going to n = 1. This means this transition also has the largest energy and frequency. The answer is d. 5p → 1s.

**Which of the following electronic transitions of hydrogen has the longest wavelength?**

red light

The red light has the longest wavelength, lowest energy, and lowest frequency.

### Which is electron transition requires the most energy?

The electron transition from n = 1 to n = 2 in hydrogen atom will require largest amount of energy. Was this answer helpful?

**What kind of electron transition emits visible light?**

As this was discovered by a scientist named Theodore Lyman, this kind of electron transition is referred to as the Lyman series. Similarly, any electron transition from n=2 n = 2 emits visible light, and is known as the Balmer series. Electron transition from n=3 n = 3 gives infrared, and this is referred to as the Paschen series.

**When do electrons fall to the 2nd energy level?**

The lines that appear at410 nm, 434 nm, 486 nm, and 656 nm. These electrons are falling to the 2nd energy level from higher ones. This transition to the 2nd energy level is now referred to as the “Balmer Series” of electron transitions. Johan Rydberg use Balmers work to derived an equation for all electron transitions in a hydrogen atom.

#### What does it mean when an electron undergoes a positive energy change?

Obviously, a positive energy change means that the electron absorbs energy, while a negative energy change implies a release of energy from the electron. Note that the formula is the energy per mole, rather than that of a single photon.