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Because that's the way physics works. There really isn't a "why".
It's kind of like asking why there are negative numbers. There just are.
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∙ 13y ago
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What is the difference between bonding and anti bonding molecular orbital?
Electrons in a bonding orbital have lower energy levels than the average energy of a valence electrons in the isolated atoms between which the orbital is formed. Antibonding orbitals do not meet this criterion, so that anitbonding orbitals can be stable only in conjunction with bonding orbitals, whereas bonding orbitals can be formed without any accompanying antibonding orbitals.The molecular orbitals which is formed by the addition of atomic orbitals is called bonding molecular orbitals.The molecular orbitals which is formed by the subtraction of atomic orbitals is called antibonding molecular orbitals.
Why py and pz cannot form bonding and anti bonding molecular orbital?
Standard PY and PZ cannot form bonding and anti bonding molecular oribitals due to their structural differences. Depending on the composition of the bonds, most atoms and molecules can create orbitals.
Which chemical bond most likely stores the most energy?
C=c Double carbon-carbon bond
What happens when electron shells of two atoms overlap?
A hybrid is created when two atomic orbitals overlap. Further, "hybridization is a theoretical process involving the combination of atomic orbitals to create a new set of orbitals that take part in covalent bonding."
Why Be2 does not exist according to mo theory?
According to the molecular orbital theory, Beryllium containes 4 electrons and two orbitals. However, when two atoms combine, they produce four orbitals and eight electrons. Therefore, for every bond formed, there will be an anti-bond created.
What is the difference between bonding and anti bonding molecular orbital?
Electrons in a bonding orbital have lower energy levels than the average energy of a valence electrons in the isolated atoms between which the orbital is formed. Antibonding orbitals do not meet this criterion, so that anitbonding orbitals can be stable only in conjunction with bonding orbitals, whereas bonding orbitals can be formed without any accompanying antibonding orbitals.The molecular orbitals which is formed by the addition of atomic orbitals is called bonding molecular orbitals.The molecular orbitals which is formed by the subtraction of atomic orbitals is called antibonding molecular orbitals.
What species have no electrons in anti bonding 2p molecular orbitals?
f2
Why py and pz cannot form bonding and anti bonding molecular orbital?
Standard PY and PZ cannot form bonding and anti bonding molecular oribitals due to their structural differences. Depending on the composition of the bonds, most atoms and molecules can create orbitals.
What are the postulates of molecular orbit theory?
Molecular Orbital Theory (MOT):•Basic idea of MOT is that atomic orbitals of individual atoms combine toform molecular orbitals. Electrons in molecule are present in themolecular orbitals which are associated with several nuclei.•The molecular orbital formed by the addition of atomic orbitals is calledthe bonding molecular orbital (s ).•The molecular orbital formed by the subtraction of atomic orbital is calledanti-bonding molecular orbital (s*).•The sigma (s ) molecular orbitals are symmetrical around the bond-axiswhile pi (p ) molecular orbitals are not symmetrical.•Sequence of energy levels of molecular orbitals changes for diatomicmolecules like Li2, Be2, B2, C2, N2 is 1s < *1s < 2s< *2s < ( 2px = 2py)
How many anti bonding orbitals are there in an O2 molecule?
there are two
Which chemical bond most likely stores the most energy?
C=c Double carbon-carbon bond
Why nitrogen is diamagnetic while contains unpaired electrons?
If you are going by the electron configuration of nitrogen then the unpaired electrons in the 2p shell would indicate that it is paramagnetic. However experiments show that it is diamagnetic. You must remember that nitrogen is a diatomic element and as such is found as N2. The molecular orbital theory explains how there are no unpaired electrons in the bonds between the two N atoms. The 1s and 2s molecular orbitals are completely filled and all of the bonding 2p orbitals are also filled. There are no electrons in the any of the 2p anti-bonding orbitals. Seeing a molecular orbital diagram for N2 will clarify what i mean.
What happens when electron shells of two atoms overlap?
A hybrid is created when two atomic orbitals overlap. Further, "hybridization is a theoretical process involving the combination of atomic orbitals to create a new set of orbitals that take part in covalent bonding."
Why Be2 does not exist according to mo theory?
According to the molecular orbital theory, Beryllium containes 4 electrons and two orbitals. However, when two atoms combine, they produce four orbitals and eight electrons. Therefore, for every bond formed, there will be an anti-bond created.
Why does co forms numerable metal complexes?
Carbon monoxide forms complexes called carbonyls. The carbon monoxide bonds via the carbon atom. A full molecular orbital treatment shows that there is a pair of electrons on the carbon that can be donated to the metal forming a sigma bond; There are filled d orbitals on the metal that "back donate" into empty anti-bonding molecular orbitals on the CO. This is a push me pull you synergistic effect.
Is oxygen paramagnetic?
Oxygen, O2 is paramagnetic indicating 2 unpaired electrons, howver simple bonding schemes for O2 with its 12 electrons would predict that they would all be paired. A molecular orbital treatment of O2 shows that there are two degenerate (equal energy) anti-bonding pi orbitals that each holds one electron.
Are alkali metals softer or harder than other metals?
The softness of alkali metals has to do with metallic bonding in terms of bonding and anti bonding orbitals. In molecular orbitals, there are the s, p, d orbitals with corresponding anti-bonding orbitals. For alkali metals, the s orbital is only partially filled. This means that the bonds between each atom are weak because only a cloud of s-orbital electrons are holding them together. As we move right across the periodic table the strength of metals reach a maximum at about group 7-8. This is because at this point anti-bonding and bonding orbitals are both partially filled and this maximizes the amount of unpaired electrons that participate in the electron cloud that holds metallic bonds together. As we proceed further right (toward Au) the bonds become weaker because the bonding and anti-bonding orbitals begin to fill and pair up. This means these electrons do not participate in the electron cloud of metallic bonding. Thus a weaker bond (softer metal) is formed.
