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Molecular orbitals are formed by the ove...

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 are `H_(2)^(+)` ions more stable than `H_(2)^(-)` ions, though they have the same bond order?

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To understand why the \( H_2^+ \) ion is more stable than the \( H_2^- \) ion, even though they have the same bond order, we need to analyze their electronic configurations and the implications of bonding and antibonding molecular orbitals. ### Step-by-Step Solution: 1. **Identify the Molecular Orbitals**: - For hydrogen molecules, the molecular orbitals formed are: - **Bonding Molecular Orbital (σ1s)**: Lower energy, stabilizes the molecule. - **Antibonding Molecular Orbital (σ*1s)**: Higher energy, destabilizes the molecule. ...
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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?

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. Which has smaller bond length No or NO^(+) ?

Knowledge Check

  • The strength of bonds by overlapping of atomic orbitals is in order

    A
    `s - s gt s - p gt p - p`
    B
    `s - s gt s - p gt s - p`
    C
    `s - p gt s - s gt p - p`
    D
    `p - p gt s - s gt s - p`

  • The strength of bonds formed by overlapping of atomic orbitals is in the order:

    A
    `s-s gt s-p gt p-p`
    B
    `s-s lt p-p lt s-p`
    C
    `s-p lt s-s lt p-p`
    D
    `p-p lt s-s lt s-p`

  • Comprehension given below is followed by some multiple choice question, Each question has one correct options. Choose the correct option. Molecular orbitals are formed by the overlap of atomic orbitals. Two atomic orbitals combine to form two molecular orbitals called bonding molecular orbital (BMO) and anti-bonding molecular orbital (ABMO). Energy of anti-bonding orbital is raised above the parent atomic orbitals that have combined and hte energy of the bonding orbital is lowered than the parent atomic orbitals. energies of various molecular orbitals for elements hydrogen to nitrogen increase in the order sigma1s lt sigma^(star)1s lt sigma^(star)2s lt ((pi2p_(x))=(pi2p_(y))) lt sigma2p_(z) lt (pi^(star)2p_(x) = pi^(star)2p_(y)) lt sigma^(star)2p_(z) and For oxygen and fluorine order of enregy of molecules orbitals is given below. sigma1s lt sigma^(star)1s lt sigma2s lt sigma^(star)2s lt sigmap_(z) lt (pi2p_(x) ~~ pi2p_(y)) lt (pi^(star)2p_(x)~~ pi^(star)2py) lt sigma^(star)2p_(z) Different atomic orbitalsof one atom combine with those atoms orbitals of the second atom which have comparable energies and proper orientation. Further, if the overlapping is head on, the molecular orbital is called sigma, sigma andif the overlap is lateral, the molecular orbital is called pi, pi . The molecular orbitals are filled with electrons according to the same rules as followed for filling of atomic orbitals. However, the order for filling is not the same for all molecules or their ions. Bond order is one of the most important parameters to compare the strength of bonds. 67) Which of the following pair is expected to have the same bonod order?

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

    • Similar Questions

    Explore conceptually related problems

    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. Which out oof O_(2)^(+) and O_(2)^(-) is more stable?

    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. Considering Z - axis as internuclear axis, which one of the following will be for sigma antibonding MO? (i) 2p_(y)+2p_(y)" "2p_(x)-2p_(y) (iii) 2s+2p_(z)" "(iv) 2p_(z)-2p_(z)

    How is bonding molecular orbitals in a molecule of hydrogen different from its antibonding molecular orbital ?

    The strength of bonds formed by overlapping of atomic orbitals is in the order .

    Molecular orbitals are formed by the overlap of atomic orbitals. Two atomic called bonding molecular orbital (BMO) and anti - bonding molecular orbital (ABMO). Energy of anti - bonding molecular orbital (BMO) and anti - bonding molecular orbital ABMO). Energy of anti - bonding orbitals is raised above the parent atomic orbitals that have combined and the energy of the bonding orbital is lowered than the parent atomic orbitals. Energies of various molecular orbitals for elements hydrogen to nitrogen increase in the order : sigma1slt sigma^(**)1s lt sigma2sltsigma^(**)2slt(pi2p_(x)~~pi2p_(y))ltsigma2p_(z)lt(pi^(**)p2p_(x)~~pi^(**)2p_(y))ltsigma^(**)2p_(z) and for oxygen and fluorine order of energy of molecular orbitals is given as : sigma1s lt sigma^(**)1slt sigma2sltsigma^(**)2sltsigma2p_(z)lt(pi2p_(x)~=2pi2p_(y))lt(pi^(**)2p_(x)~=pi^(**)2p_(y))ltsigma^(**)2p_(z). Different atomic orbitals of one atom combine with those atomic orbitals of the second atom which have comparable energies and proper orientation. Further, if the overlapping is head on, the molecular orbital is called 'sigma', (sigma) and if the overlap is lateral, the molecular orbital is called 'pi', (pi) . The molecular orbitals are filled with electrons according to the same rules as followed for filling of atomic orbitals. However, the order for filling is not the same for all moleculas or their ions. Bond order is one of hte most important parameters to compare the strength of bonds. Which of the following pair is expected to have the same bond order?

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