What is the molecular orbital configuration of C2?

1 σ and 2 π bonds.

What is the bond order of C2 − C 2 −?

The bond order of C2 is 2. B.In vapour phase, C2 molecule is diamagnetic. C. Double bond in C2 molecule consists of both π- bonds because of the presence of 4 electrons in two π – molecular orbitals.

Is C2 − C 2 − paramagnetic or diamagnetic?

Since C2 has no unpaired electrons, it is diamagnetic.

What is the bond order of CN?

For the above question, $CN^{-}$ has a total of 14 electrons which include 6 of carbon atoms and 7 of nitrogen atoms and it has a one extra electron due to the negative charge on the compound. Therefore, the bond order of cyanide is 3.

How do you write Mo configuration?


  1. Find the valence electron configuration of each atom in the molecule.
  2. Decide if the molecule is homonuclear of heteronuclear.
  3. Fill molecular orbitals using energy and bonding properties of the overlapping atomic orbitals.
  4. Use the diagram to predict properties of the molecule.

Which is more stable C2+ or C2?

Re: C2+ C2- Therefore, the 8 electrons would fill up both outer orbitals, the s and p orbitals, while for C2- it would only fill up the 1s orbital and have 2 electrons in the 2s orbital. Therefore, C2- has a stronger bond as it is more stable and harder to pull an electron away from it.

What is the effect of the process C2 C 2+ E on the bond order of C2?

Answer Expert Verified. Highest bond order means highest bond energy and shortest bond length. So, the highest bond order with highest bond energy and the shortest bond length is found in C2-. So, the order starting with the highest bond order is = C2- > C2 > C2+.

What is the bond order of n2 2?

2, 2.5 and 3 respectively.

Is CN diamagnetic or paramagnetic?

CN is paramagnetic with bond order 3, CN− is diamagnetic with bond order 5/2. D.

Is C2+ diamagnetic or paramagnetic?

Write molecular orbital configuration of c2+ predict magnetic behaviour and calculate its bond order. The C2 molecule is diamagnetic because all electrons are paired there are no unpaired electrons.

What is the bond length of CN?

Similar to carbon–carbon bonds, these bonds can form stable double bonds, as in imines, and triple bonds such as nitriles. Bond lengths range from 147.9 pm for simple amines to 147.5 pm for C-N= compounds such as nitromethane to 135.2 pm for partial double bonds in pyridine to 115.8 pm for triple bonds as in nitriles.

What is the orbital configuration of C N +?

The molecular orbital configuration of C N + is K K σ(2s)2, σ∗(2s)2, π(2px. ​. )2, π(2py. ​. )2 . Bond order is 2. All the electrons are paired and ion is diamagnetic.

What kind of molecular orbital does cyanide have?

Clearly, Cyanide (CN) lies in a hetero-nuclear diatomic molecular orbital as it contains two different atoms. Also, using the Molecular orbital diagram of CN we can also find its bond order which helps us to predict its bond length and stability as well.

Which is the lowest energy orbital of C _ 2?

The lowest energy unoccupied molecular orbital is 2p_ (sigma), so that is where the extra electron will be added. The electron configuration of the neutral “C”_2 molecule is — I’ll use the notation given to you in the diagram

How does the molecular orbital diagram explain bond order?

CN molecular orbital diagram (MO) and its bond order Molecular orbital theory explain the placement of electrons in a molecule. Generally, two types of bonding are formed by the combination of atomic orbitals. 1.