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How many electrons occupy the bonding mo...

How many electrons occupy the bonding molecular orbitals of a C:N triple bond?

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Define bonding molecular orbital.

How many electrons are present in anti bonding molecular orbitals of O_(2) ,molecule

Knowledge Check

  • Assertion(A) - Fluorine molecule has bond order one. Reason(R)-The number of electrons in antibonding molecular orbital is two less than that of bonding molecular orbitals.

    A
    Both A and R true and R is the correct explanation of A
    B
    Both A and R true and R is not a correct explanation of A
    C
    A is true but R is false
    D
    A is false but R is true

  • Assertion: The bond order of helium molecule is always zero. Reason: The number of electrons in bonding molecular orbital and antibonding molecular orbital is equal.

    A
    If both assertion and reason are true and the reason is the correct explanation of the assertion
    B
    if both assertion and reason are true but reason is not the correct explanation of the assertion
    C
    if assertion is true but reason is false
    D
    if the assertion and reason both are false

  • The molecular orbital with the lowest eenrgy is filled first. Thus sigma (1s) is filled first where as 'sigma^(*)(2p) isfilled in thelast, also the maximum number of electron in bonding and antibonding molecular orbitals are according to Pauli and Hund's rule. As an electron in an antibonding molecular orbital cancels out the stability introduced by the electron in a bonding molecular orbital, it means that in order for bonding of atoms to occur there should be an excess of bonding electron sover antibonding electrons. In case where the number of bonding and antibonding electrons are equal, no bond will be formed between the atoms. With the help of above discussion, we can define easily bond order, relative bond length, relative stability and magnetic properties for a molecule. In an antibonding molecular orbital, there is a line between the two probability contours of hydrogen atoms. This is called

    A
    Antinode
    B
    Nodal plane
    C
    A plane where electron charge density is maximum
    D
    A and C both are correct

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    What will happen to the bond order if the electron is added ot bonding molecular orbital ?

    Chemical Bonding - Molecular Orbital Theory

    The total number of electrons in all bonding molecular orbitals of O _(2) ^(2-) is ........... (Round off to the nearest integer)

    The molecular orbital with the lowest eenrgy is filled first. Thus sigma (1s) is filled first where as 'sigma^(*)(2p) isfilled in thelast, also the maximum number of electron in bonding and antibonding molecular orbitals are according to Pauli and Hund's rule. As an electron in an antibonding molecular orbital cancels out the stability introduced by the electron in a bonding molecular orbital, it means that in order for bonding of atoms to occur there should be an excess of bonding electron sover antibonding electrons. In case where the number of bonding and antibonding electrons are equal, no bond will be formed between the atoms. With the help of above discussion, we can define easily bond order, relative bond length, relative stability and magnetic properties for a molecule. According to MOT which statement is correct about Boron molecule ?

    The molecular orbital with the lowest eenrgy is filled first. Thus sigma (1s) is filled first where as 'sigma^(*)(2p) isfilled in thelast, also the maximum number of electron in bonding and antibonding molecular orbitals are according to Pauli and Hund's rule. As an electron in an antibonding molecular orbital cancels out the stability introduced by the electron in a bonding molecular orbital, it means that in order for bonding of atoms to occur there should be an excess of bonding electron sover antibonding electrons. In case where the number of bonding and antibonding electrons are equal, no bond will be formed between the atoms. With the help of above discussion, we can define easily bond order, relative bond length, relative stability and magnetic properties for a molecule. Which of the following are paramagnetic in nature ?

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