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Which of the following statement is not ...

Which of the following statement is not correct from the point of view of molecular orbital ?

A

`Be_(2)` is not ,a stable molecule

B

`He_(2)` is not stable but `He_(2)^(+)` is expected to exist

C

Bond strength of `N_(2)` is maximum amongst th homonuclear diatomic molecules

D

The order of energies of molecular orbitals in `F_(2)` molecules is `pi_(2px)=pi_(2py) lt sigma_(2pz)`

Text Solution

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The correct Answer is:
To determine which statement is not correct from the point of view of molecular orbital theory, we will analyze each statement provided in the question step by step. ### Step 1: Analyze the first statement **Statement:** BE2 is not a stable molecule. **Explanation:** - Beryllium (Be) has an atomic number of 4, meaning it has 4 electrons. For 2 Be atoms, the total number of electrons is 8. - The molecular orbital configuration for Be2 is: - σ1s², σ*1s², σ2s², σ*2s² - The bond order is calculated as: \[ \text{Bond Order} = \frac{(\text{Number of electrons in bonding MOs}) - (\text{Number of electrons in antibonding MOs})}{2} \] Here, we have 4 electrons in bonding orbitals (σ1s², σ2s²) and 4 electrons in antibonding orbitals (σ*1s², σ*2s²). \[ \text{Bond Order} = \frac{4 - 4}{2} = 0 \] - A bond order of 0 indicates that Be2 is not stable. This statement is correct. ### Step 2: Analyze the second statement **Statement:** HE2 is not stable but HE2+ is expected to exist. **Explanation:** - Helium (He) has an atomic number of 2, meaning it has 2 electrons. For 2 He atoms, the total number of electrons is 4. - The molecular orbital configuration for He2 is: - σ1s², σ*1s² - The bond order is: \[ \text{Bond Order} = \frac{(2) - (2)}{2} = 0 \] - Thus, He2 is not stable. - For He2+, one electron is removed, leaving 3 electrons: - The configuration becomes σ1s², σ*1s¹. - The bond order for He2+ is: \[ \text{Bond Order} = \frac{(2) - (1)}{2} = \frac{1}{2} = 0.5 \] - A bond order of 0.5 indicates that He2+ can exist. This statement is also correct. ### Step 3: Analyze the third statement **Statement:** The bond strength of N2 is maximum among the homonuclear diatomic molecules. **Explanation:** - For nitrogen (N), with an atomic number of 7, the total number of electrons for N2 is 14. - The molecular orbital configuration for N2 is: - σ1s², σ*1s², σ2s², σ*2s², π2p_x², π2p_y², σ2p_z² - The bond order is: \[ \text{Bond Order} = \frac{(10) - (4)}{2} = 3 \] - N2 indeed has the highest bond order (and thus bond strength) among homonuclear diatomic molecules. This statement is correct. ### Step 4: Analyze the fourth statement **Statement:** The order of energy of molecular orbitals in F2 is 2Px, 2Py, and then 2Pz. **Explanation:** - For fluorine (F), with an atomic number of 9, the total number of electrons for F2 is 18. - The molecular orbital configuration for F2 is: - σ1s², σ*1s², σ2s², σ*2s², σ2p_z², π2p_x², π2p_y² - In F2, due to the mixing of 2s and 2p orbitals, the order of energy levels is: - σ2p_z has lower energy than π2p_x and π2p_y. - Therefore, the correct order is: - σ2p_z < π2p_x = π2p_y - The statement given is incorrect as it suggests that 2Pz is of higher energy than 2Px and 2Py. ### Conclusion The statement that is not correct from the point of view of molecular orbital theory is the fourth statement regarding the order of energy of molecular orbitals in F2. ---
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Knowledge Check

  • Which of the following statement is not correct from the view point of molecular orbital theory?

    A
    `Be_(2)` is not a stable molecule .
    B
    `He_(2)` is not stable of `N_(2)` is maximum amongst the homonuclear diatomic molecules belonging to the second period .
    C
    Bond strength of `N_(2)` is maximum amongst the homonuclear diatomic molecules belonging to the second period.
    D
    The order of energies of molecular orbitals in `N_(2)` molecule is ` sigma 2s lt sigma^(***) 2s lt sigma2p_(z) lt (pi 2p_(x) = pi 2p_(y)) lt (pi^(***) 2p_(x) = pi^(***) 2p_(y)) lt sigma^(***) 2p_(z)`
  • Which of the following statements is not correct about molecular crystals ?

    A
    They are generally soft and easily compressible
    B
    They are good conductors of electricity as the electrons are delocalised in the bonds
    C
    They have low melting and boiling points
    D
    They consist of polar or non-polar molecules .
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