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Which homonuclear diatomic molecule besi...

Which homonuclear diatomic molecule besides `O_(2)` is paramagnetic?

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To determine which homonuclear diatomic molecule besides O₂ is paramagnetic, we need to analyze the electron configurations of various homonuclear diatomic molecules and identify those with unpaired electrons. ### Step-by-Step Solution: 1. **Understanding Paramagnetism**: - Paramagnetic substances have unpaired electrons in their molecular orbitals. This means that when we fill the molecular orbitals, if any electrons are left unpaired, the molecule is paramagnetic. 2. **Analyzing O₂**: ...
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Explore conceptually related problems

A diatomic molecules has

Which diatomic molecule of second period basides O_(2) should be paramagnetic ? .

For a homonuclear diatomic molecule the energy of sigma_(2s) orbital is

O_2 molecule is paramagnetic in

There are five species P, Q, R, S and T. Spectroscopical analysis shows that P,Q and R are homonuclear diatomic species and have their bond order 2.4, 1.5 and 2.5 respectively and rest two species S and T are heteronuclear diatomic species and have bond order 3 and 2 respectively. All homonuclear diatomic species are paramagnetic and all heteronuclear species are diamagnetic in nature. P, R , S and T are monocovalent positive ion and Q is monovalent negative ion: Q. The correct statement is :

There are five species P, Q, R, S and T. Spectroscopical analysis shows that P,Q and R are homonuclear diatomic species and have their bond order 2.5, 1.5 and 2.5 respectively and rest two species S and T are heteronuclear diatomic species and have bond order 3 and 2 respectively. All homonuclear diatomic species are paramagnetic and all heteronuclear species are diamagnetic in nature. P, R , S and T are monocovalent positive ion and Q is monovalent negative ion: Q. The incorrect statements is :

There are five species P, Q, R, S and T. Spectroscopical analysis shows that P,Q and R are homonuclear diatomic species and have their bond order 2.5, 1.5 and 2.5 respectively and rest two species S and T are heteronuclear diatomic species and have bond order 3 and 2 respectively. All homonuclear diatomic species are paramagnetic and all heteronuclear species are diamagnetic in nature. P, R , S and T are monocovalent positive ion and Q is monovalent negative ion: Q. According to given information the incorrect match is :

MODERN PUBLICATION-CHEMICAL BONDING AND MOLECULAR STRUCTURE-HIGHER ORDER THINKING SKILLS
  1. Explain why melting point of NaCl is higher than that of AlCl(3).

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  2. Silver halides have law solubilities in water as compared to alkali me...

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  3. Which homonuclear diatomic molecule besides O(2) is paramagnetic?

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  4. Distinguish between antibonding and nonbonding orbitals.

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  5. Anhydrous AlCl(3) is covalent but AlCl(3). 6H(2)O is ionic in nature. ...

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  6. Cu^(+) and Na^(+) are of same size but CuCl is insoluble while NaCl is...

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  7. The geometry of I(3)^(-) is

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  8. The type of bonds present in NH(4)Cl are

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  9. Which one has high boiling point and why? Ethyl alcohol or dimethyl ...

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  10. XeF(2) molecule is linear molecule but it is sp^(3)d hybridized. Why?

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  11. Bonds presents in CuSO(4) .5H(2)O is

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  12. The following are aresome statement about oxides of VA group element ...

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  13. The bond order in O2^-ion is

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  14. Explain, why o-hydroxybenzaldehyde is a liquid at room temperature whi...

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  15. A gaseous compound of nitrogen and oxygen is paramagnetic in nature. W...

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  16. Draw three possible geometrical structures of PBr(2)Cl(3) and predict ...

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  17. Bond angle in PH(4)^(+) is higher than that in PH(3).Why ?

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  18. Why does PCl(5) exist as [PCl(4)]^(+)[PCl(6)]^(-) in the crystalline s...

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  19. Explain the observations that the bond length in N^(+) is 0.02Å larger...

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  20. IF molecular axis is X then which of the following overlapping will f...

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