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Molecular orbital theory as developed b...

Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength.
Which of the following combination does ot give `sigma` MO (assume Z - axis as internuclear axis)

A

`2p_(x)+2p_(x)`

B

`2p_(z)+2s`

C

`2s+2s`

D

`2p_(z)+2p_(z)`

Text Solution

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The correct Answer is:
To solve the question regarding which combination does not give a sigma molecular orbital, we will analyze the combinations of atomic orbitals based on their overlapping characteristics. ### Step-by-Step Solution: 1. **Understanding Sigma and Pi Molecular Orbitals**: - Sigma (σ) molecular orbitals are formed by the head-on (end-to-end) overlapping of atomic orbitals along the internuclear axis. - Pi (π) molecular orbitals are formed by the side-to-side overlapping of atomic orbitals. 2. **Identifying the Combinations**: - We need to evaluate the given combinations of atomic orbitals to determine which one does not yield a sigma molecular orbital. 3. **Analyzing Each Combination**: - **Combination 1: 2Px and 2Px**: - The 2Px orbitals overlap side-to-side because they are oriented along the x-axis. Therefore, this combination does not form a sigma molecular orbital. - **Combination 2: 2Pz and 2s**: - The 2Pz orbital (which is oriented along the z-axis) can overlap head-on with the spherical 2s orbital. This combination will form a sigma molecular orbital. - **Combination 3: 2H2s**: - Similar to the previous case, the 2s orbitals can overlap head-on, thus forming a sigma molecular orbital. - **Combination 4: 2Pz and 2Pz**: - The 2Pz orbitals overlap head-on along the z-axis, which allows for the formation of a sigma molecular orbital. 4. **Conclusion**: - From the analysis, the combination that does not give a sigma molecular orbital is **2Px and 2Px**. ### Final Answer: The combination that does not give a sigma molecular orbital is **2Px and 2Px**.
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Knowledge Check

  • Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength. Which of the following is expected to have largest bond length?

    A
    `O_(2)`
    B
    `O_(2)^(+)`
    C
    `O_(2)^(-)`
    D
    `O_(2)^(2-)`

  • Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength. Which one of the following does not have single electron in a bonding molecular orbital?

    A
    `CN`
    B
    `B_(2)`
    C
    `NO`
    D
    `N_(2)^(+)`

  • Molecular orbital theory as developed by Hund and Mulliken concerns with the formation of molecular orbitals formed by linear combination of atomic orbitals. The electrons are present in these molecular orbitals. The molecular orbitals are filled. The molecular orbital configuration helps us to calculate bond order which gives information about the number of bonds present between atoms. The bond order is related to bond length and bond strength. Which of the following will have maximum number of electrons in antibonding MOs?

    A
    `N_(2)^(+)`
    B
    `O_(2)^(+)`
    C
    `F_(2)`
    D
    `Be_(2)`

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    Molecular orbitals are formed by the overlap of atomic orbitals. Two atomic orbitals combine to form two molecular orbitals called bonding and antibonding MO s . The molecular orbitals are filled with electrons following the same rules as followed for filling of atomic orbitals. The molecular orbitals electronic configurations help us to calculate bond order when which give important information about bond strength and bond length. Why does Be_(2) molecule not exist?

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