Why nitrogen has higher electron bond dissociation energy?

Why nitrogen has higher electron bond dissociation energy?

The nitrogen molecule links two atoms by a triple bond ( one Sigma and two pi) whereas oxygen has only a double bond. The bond energy is directly proportional to bond order, so since there are more bonds in nitrogen, it will possess more energy and has a higher dissociation energy.

Does N2 or N2 have greater bond dissociation energy than N2+?

N2 has greater bond energy than N2^+ but O2 has tower bond dissociation energy then O2^+ .

Why is N2+ bond order less than N2?

When N2 changes to N2+, the electron is removed from the bonding molecular orbital while when O2 changes to O2+, the electron is removed from antibonding molecular orbital. This is the reason why the bond order of N2 is greater than N2+ but the bond order of O2 is less than that of O2+.

Which has greater bond energy N2+ or N2?

(a) Both N2+ and N2− has almost same bond energy, though N2− is slightly less stable and hence it has less bond energy than N2+ due to the presence of greater number of electrons in the antibonding molecular orbitals.

Why does N2 has greater dissociation energy than N2+ whereas O2 has lower dissociation energy than O2+?

According to Molecular orbital theory: N2 have 6 more electrons in a bonding atomic orbital so it’s bond order is 3, whereas N2+ has only 5 in bonding so it’s bond order is 2.5. Bond dissociation energy is directly proportional to Bond order of a molecule so N2 has more bond dissociation energy.

Why N2 has greater dissociation energy than N2+ while O2 has lower dissociation energy than O2+ explain with the help of molecular orbital theory?

Chemical Bonding and Molecular Structure. Show that N2 molecule has a greater bond dissociation energy than N-2 where O2 has lower bond dissociation energy than O+2. The bond dissociation energy is directly proportional to bond order such that, greater the bond order, greater is the bond dissociation energy.

Is bond length in N2+ is less than N2?

N2- has 5e- in antibonding while N2+ has 4. So, N2+ will make a stronger bond and will have a shorter bond length.

Do you expect the bond in the N2+ ion to be stronger or weaker than the bond in the N2 molecule?

Thus, the bond is stronger and shorter than in O2. no unpaired electrons, so N2 is diamagnetic. Both N2+ and N2 – have 5 net bonding electrons and so both have weaker bonds than N2.

Why is N2+ more stable than N2?

N2 has highest bond order of 3 compared to N2+ which is 2.5, hence N2 it is more stable than N2+.

How does bond energy varies from N to N Why?

Foe the energy we need to determines the Bond order for which we need to do the electronic configuration of both the molecules by the MOT. We know the Molecule having the hind bond order will be having the high bond energy. Therefore, Bond energy of the N₂ will be more than N₂⁺.

Is N2+ A bond order?

The MO method for N2+ gives the bond order equal to 2.5. But first, we look at the diagram of molecular orbitals for N2 (the bond order for the nitrogen molecule is 3). That is, the bond order for N2+ is 2.5.

Does N2 have a stronger bond than O2?

There are two unpaired electrons in the 2pπ* orbitals, thus O2 is paramagnetic. Electron configuration — 2sσ2 2sσ*2 2pσ2 2pπ4 2pπ*1 There are 5 net bonding electrons (bond order of 2.5). Thus, the bond is stronger and shorter than in O2. no unpaired electrons, so N2 is diamagnetic.

Why does N2 have more bond energy than N2+?

N2 have 6 more electrons in a bonding atomic orbital so it’s bond order is 3, whereas N2+ has only 5 in bonding so it’s bond order is 2.5. Bond dissociation energy is directly proportional to Bond order of a molecule so N2 has more bond dissociation energy. AMMusani. Between N2 and N2+, which has less bond energy and why? N2+ has less bond energy.

What is the bond order of N2 molecule?

From the above electronic configuration of N2 molecule , the total number of bonding electron is 10 and the number of anti bonding electron is 4 . Therefore, the bond order of N2 molecule is 3 . Which has more bond length between O2 and N2?

Why is N2 diamagnetic but O2 is diamagnetic?

Thus, the bond is stronger and shorter than in O2. no unpaired electrons, so N2 is diamagnetic. Both N2+ and N2 – have 5 net bonding electrons and so both have weaker bonds than N2.

Which is more stable N2+ or O2+?

N2+ is more stable since N has to lose 5 electrons so as to be stable and oxygen has to lose 6 so as to gain stability. Thus oxygen remains with 4 if it loses 2 and nitrogen remains with 3 on losing 2. Thus N2+ is more stable since it is closer to stability than O2+.