Using the MO diagram of #"NO"#, calculate the bond order
2017年8月29日 · To obtain the bond order, look at the molecular orbitals formed and decide whether they are bonding or antibonding. BO = 1 2 (bonding e− − antibonding e−) = 1 2 [(2 + 2 + 2 + 2) − (2 + 1)] = 2.5. And this should make sense because NO+ is isoelectronic with CO, which has a bond order of 3. With one additional electron in an antibonding ...
What is the electron configuration of nitrogen monoxide?
2017年8月8日 · So, the molecular electron configuration would be written in a similar manner as the atomic counterpart, but using molecular orbitals instead. We obtain: (σ1s)2(σ* 1s)2(σ2s)2(σ* 2s)2(π2px)2(π2py)2(σ2pz)2(π* 2px)1. Or, another way to write this is in the notation seen in the MO diagram, with KKσ indicating the filled σ1s and σ* 1s ...
By writing molecular orbital configuration for NO,CO,O2 molecules ...
2018年3月18日 · "O"_2 is well-known to be paramagnetic, and it is one of the successes of molecular orbital theory. You can see that "CO" is not (as it has zero unpaired electrons), but "NO" is (it has one unpaired electron). Well, the MO diagram for "O"_2 is: The bond order is already calculated in the diagram.
Draw the diagrams for "NO"_2^-, "NO"_2^+, and "NO"_2. The
2018年2月9日 · You've seen the molecular orbital (MO) diagram of "CO"_2: "CO"_2 and "NO"_2^+ are isoelectronic and thus have the same electron configuration. Thus, simply add one or two electrons into the 2b_(3u) and 2b_(2u) to get "NO"_2 and "NO"_2^-, respectively. Nitrogen atom has 2p atomic orbitals lower by "2.52 eV", and 2s atomic orbitals lower by "6.13 eV" than with carbon atom. That makes the HOMO ...
What are nonbonding molecular orbitals? + Example - Socratic
2014年4月13日 · A non-bonding orbital (NBMO) is a molecular orbital for which the addition or removal of an electron does not change the energy of the molecule. Molecular orbitals come from the linear combination of atomic orbitals. In a simple diatomic molecule such as HF, F has more electrons than H. The s orbital of H can overlap with the 2p_z orbital of fluorine to form a bonding σ and an antibonding σ ...
What is the molecular orbital diagram for B_2? - Socratic
2015年1月27日 · Before we can draw a molecular orbital diagram for B₂, we must find the in-phase and out-of-phase overlap combinations for boron's atomic orbitals. Then we rank them in order of increasing energy. We can ignore the 1s orbitals, because they do not contain the valence electrons. Each boron atom has one 2s and three 2p valence orbitals. The 2s orbitals will overlap to form 2sσ and 2sσ ...
Order by bond length? #"NO"#, #"NO"^(+)#, #"NO"^(-)# - Socratic
2017年9月17日 · 1 Answer. The bond strength increases going from NO− to NO+, and the bond length consequently shortens going from NO− to NO+. rNO− N−O> rNO N−O> rNO+ N−O. To start with, O2 is (roughly) isoelectronic with NO−[*], and O2 has two π* antibonding electrons, as you should know from its MO diagram from your textbook. Thus, so does NO−.
How to draw a BN molecular orbital diagram? - Socratic
2017年12月11日 · This is the general MO diagram you need to fill with the valence electrons of BN. Boron has 3 valence electrons, and nitrogen has 5 valence electrons, this makes 8 electrons. You have to start filling the orbitals from those with lowest energy to those with higher energy. So, 2 electrons on σ2s. , two electrons on σ∗2s, two electrons on σ2p.
Molecular Orbital Theory - Chemistry - Socratic
2014年3月22日 · Molecular Orbital (MO) theory better explains the properties of more complex molecules. MO theory explains the partial bonds of NO₃⁻ without using resonance. This makes MO theory more useful for the description of extended π systems. Also, in benzene the six p electrons are in three molecular π orbitals around the ring.
Why is O2 paramagnetic? - Socratic
2016年9月25日 · The correct explanation comes from Molecular Orbital theory. The atomic orbitals of the #"O"# atoms overlap to form the σ and π orbitals of the #"O"_2# molecule as shown in the diagram above. We add the 12 valence electrons according to the Aufbau principle. The last two electrons go into separate, degenerate π orbitals, according to Hund's ...