What happens to the molecule when the electron was promoted to the antibonding orbital?

What happens to the molecule when the electron was promoted to the antibonding orbital?

If one of the bonding electrons absorbs a photon that has just the right amount of energy (the energy difference between the bonding and antibonding orbital) it will be promoted and move into the destabilized antibonding orbital – causing the bond between the atoms to break.

What would be the bond order of an H2 molecule in its ground state?

For H2, bond order = 1/2 (2-0) = 1, which means H2has only one bond.

What is more stable H2 or H2+?

In H2- ion one electron is present in anti bonding orbital due to which destabilizing effect is more and thus the stability is less than that of H2+ ion.

What happens when electrons move from the excited state to the ground state?

When an atom is in an excited state, the electron can drop all the way to the ground state in one go, or stop on the way in an intermediate level. Electrons do not stay in excited states for very long – they soon return to their ground states, emitting a photon with the same energy as the one that was absorbed.

What is the bond order of H2+?

As seen in lecture and in the course reader page 15 of ch 4, H2+ has a bond order of (1/2). I have learned that single bonds are weakest but are the longest whereas for example, a double bond is stronger than a single bond but shorter.

What is bond order of O2?

O2 has two unpaired electrons in its π* orbitals, and a bond order of 2.

What is bond order H2+?

The number of electrons present in hydrogen is 2. In one electron is removed so, the number of electrons is 1. Thus the number of bonding electrons is one and the number of antibonding electrons is 0. Thus bond order of is 0.5.

What is the bond order in H2 +?

Bond order of H2+ : H2+ means that the molecule of hydrogen loses its one electron. The H2+ molecule ion will have the electronic configuration [ (σ1s)1 ]. For H2+ , bond order = 1/2 (1 – 0)=1/2 σ bond.

Why is H2 a stable molecule?

H2 is stable since all electrons of the molecule can be put into the bonding molecular orbital. O H2 is stable since all electrons of the molecule can be put into the anti-bonding molecular orbital.

Why is H2 so unstable?

Atoms of hydrogen have a single proton in their center and a single electron in the lowest energy level. This is a very unstable arrangement, and hydrogen gas undergoes a variety of reactions so as to reach a stable electron configuration where its energy level is either empty of electrons, or filled with electrons.

What is the bonding energy of H2+?

Thus, H 2+ should exist as a stable molecule. The calculated bonding energy is 1.77 eV. This is a quite satisfying result; from experiments we get 2.77 eV. Therefore, we are now able to calculate approximate energy curves for molecules and compare the results with experimental data.

Is H2 more stable when two protons are closer together?

Here although separated H & H^- are more stable than two separated H atoms & an electron, it turns out that it is not more stable than H2 & a free-electron when two protons are closer together.

What is the bond order of (H2)- in the gas phase?

(H2)+ is stable in the gas phase with a bond order of 0.5. However, it is reactive and will rapidly attract an electron to form H2 gas. (H2)- has a bond order of 0.5 as well, but you are adding an electron to the antibonding orbital, which is unfavourable. How you can fight against the country’s gas crisis.

What happens when you add two electrons to a molecule of H2?

If you put in two electrons, they go to the bonding orbital and you obtain the regular H2 molecule. Adding another electron, this would go in the antibonding orbital but, since there would be two bonding electrons and an antibonding one, the H2(-) molecule could still exist.