Which has greater bond strength between NO and NO+?

Which has greater bond strength between NO and NO+?

As the number of antibonding electrons increases, the N−O bond weakens, having acquired antibonding character (which as the name suggests, goes against making a bond). Thus, the bond strength increases going from NO− to NO+ , and the bond length consequently shortens going from NO− to NO+ .

Which is more stable NO or NO+?

Your NO+ diagram will have one less valence electron and your NO- diagram will have one more valence electron. The stronger bonds will have the higher bond order, greater stability, higher energy and shorter bond. …

What is bond order of NO molecule?

The bond order of NO molecule is 2.

Which of the following species has the shortest bond length NO NO+ NO 2 NO?

NO, NO^(+), NO^(2+),NO^(-) Thus , NO+ has the highest bond order and , therefore, the shortest bond length .

What is the no bond order?

N=O. has a bond order of two, and both N-O bonds have a bond order of one.

Is no molecule stable?

Nitric oxideNitric oxide (NO) is an example of a stable free radical. It does not obey the octet rule on the nitrogen atom. There is persistent radical character on nitrogen because it has an unpaired electron. The two oxygen atoms in this molecule follow the octet rule.

WHY NO molecule is less stable than o2 or n2?

Answer: Since a p-orbital can accommodate a maximum of 6 electrons so we can see Nitrogen has half filled orbital while oxygen has 2 unpaired electrons. “ELEMENTS HAVING HALF FILLED AND FULL FILLED ORBITALS ARE THE MOST STABLE AND HAVE LEAST ENERGY”. So Nitrogen is more stable than oxygen.

Is no stable or unstable?

Nitric oxideNitric oxide (NO) is an example of a stable free radical. It does not obey the octet rule on the nitrogen atom. Each line around the atoms represents a pair of electrons.

How do you know if a molecule is stable or unstable?

A chemical which is stable is unreactive, and a chemical which is unstable is reactive. Reactivity depends on Unequal Distribution of Electrons (UDED) in a chemical species (molecule, atom, ion).

How do you find the bond order no using molecular orbital theory?

The Bond Order Formula can be defined as half of the difference between the number of electrons in bonding orbitals and antibonding orbitals. a = Number of electrons in bonding molecular orbitals. b = Number of electrons in antibonding molecular orbitals. Bond order of NO+ is 3.

How do you calculate bond orders in molecular orbital theory?

In molecular orbital theory, we calculate bond orders by assuming that two electrons in a bonding molecular orbital contribute one net bond and that two electrons in an antibonding molecular orbital cancel the effect of one bond.

What is the bond order of the no molecule?

The bond order means the number of bond present between two atoms . This bond order can be calculated with the help of molecular orbital theory . Now, the total electron of NO molecules is ( 7+8) = 15 . According to molecular orbital theory, the molecular orbital electronic configuration of NO molecule would be ,

What is the molecular orbital electronic configuration of no molecule?

According to molecular orbital theory, the molecular orbital electronic configuration of NO molecule would be , Form the above molecular orbital electronic configuration of NO molecule , it has been found that the number of bonding electron is 10 and the number of anti bonding electron is 5 .

How does the antibonding molecular orbital affect the stability of h2molecules?

Placing an electron in this orbital therefore stabilizes the H2molecule. Since the * antibonding molecular orbital forces the electron to spend most of its time away from the area between the nuclei, placing an electron in this orbital makes the molecule less stable.