313719
What is the bond order of \(\mathrm{O}_{2}\) molecule?
1 2.0
2 1.5
3 1
4 3.5
Explanation:
The electronic configuration of \(\mathrm{O}_{2}\) is \(\sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{2} \sigma 2 \mathrm{p}_{\mathrm{z}}{ }^{2} \pi 2 \mathrm{p}_{\mathrm{x}}{ }^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}{ }^{2} \pi^{*} 2 \mathrm{p}_{\mathrm{x}}{ }^{1}\) \(=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}{ }^{1}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}=\dfrac{10-6}{2}=2\)
MHTCET - 2022
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313720
As per molecular orbital theory, bond order of \({\mathrm{\mathrm{Li}_{2}}}\) is \({\mathrm{x}}\) and bond order of \({\rm{Li}}_2^ - \) is \({\mathrm{y}}\). The value of \({\mathrm{(\mathrm{x}-\mathrm{y})}}\) is ____.
1 1
2 0.5
3 2
4 3
Explanation:
\(\mathrm{Li}_{2} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}\)\(=\dfrac{4-2}{2}=1\)\(\,\,\) \(\therefore \quad x=1\)\(\mathrm{Li}_{2}^{-} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{1}\) Bond order \(=\dfrac{4-3}{2}=\dfrac{1}{2}=0.5\)\(\therefore y=0.5\)\(\therefore(x-y)=(1-0.5)=0.5\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313721
The incorrect statement among the following is
1 In \({{\rm{C}}_{\rm{2}}}\), there is a double bond and both the bonds are \({\rm{\pi - bonds}}\)
2 Bond order of \({\rm{CO}}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{O}}^{\rm{ + }}}\) are respectively 3.0 and 3.5
3 \({\rm{CO,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}\,\,{\rm{and}}\,\,{{\rm{N}}_{\rm{2}}}\) all have the same bond order value
4 The B.O of \({\rm{CO = 2,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}{\rm{ = 2}}{\rm{.5}}\,\,{\rm{\& }}\,\,{{\rm{N}}_{\rm{2}}}{\rm{ = 3}}\)
Explanation:
Conceptual Questions
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313722
Assertion : \(\mathrm{O}_{2}\) is paramagnetic. Reason : It has one unpaired electron.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Oxygen has two unpaired electrons in its antibonding \(\pi 2 \mathrm{p}\) molecular orbitals making it paramagnetic. So the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313734
The bond length of \({\rm{H}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\,\,{\rm{and}}\,\,{{\rm{H}}_{\rm{2}}}\) are in the order
B.O. of \({\rm{H}}_{\rm{2}}^{\rm{ + }}\) is 0.5, \({\rm{H}}_{\rm{2}}^{\rm{ - }}\) is 0.5 and B.O. of \({{\rm{H}}_{\rm{2}}}\) is 1. \({\rm{H}}_{\rm{2}}^{\rm{ + }}\,\,{\rm{and}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\) have same bond order. However in \({\rm{H}}_{\rm{2}}^{\rm{ - }}\), the \({{\rm{3}}^{{\rm{rd}}}}\) electron is entering an ABMO, making it less stable than the former. So, Greater the B.O., shorter the bond and species is more stable.
313719
What is the bond order of \(\mathrm{O}_{2}\) molecule?
1 2.0
2 1.5
3 1
4 3.5
Explanation:
The electronic configuration of \(\mathrm{O}_{2}\) is \(\sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{2} \sigma 2 \mathrm{p}_{\mathrm{z}}{ }^{2} \pi 2 \mathrm{p}_{\mathrm{x}}{ }^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}{ }^{2} \pi^{*} 2 \mathrm{p}_{\mathrm{x}}{ }^{1}\) \(=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}{ }^{1}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}=\dfrac{10-6}{2}=2\)
MHTCET - 2022
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313720
As per molecular orbital theory, bond order of \({\mathrm{\mathrm{Li}_{2}}}\) is \({\mathrm{x}}\) and bond order of \({\rm{Li}}_2^ - \) is \({\mathrm{y}}\). The value of \({\mathrm{(\mathrm{x}-\mathrm{y})}}\) is ____.
1 1
2 0.5
3 2
4 3
Explanation:
\(\mathrm{Li}_{2} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}\)\(=\dfrac{4-2}{2}=1\)\(\,\,\) \(\therefore \quad x=1\)\(\mathrm{Li}_{2}^{-} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{1}\) Bond order \(=\dfrac{4-3}{2}=\dfrac{1}{2}=0.5\)\(\therefore y=0.5\)\(\therefore(x-y)=(1-0.5)=0.5\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313721
The incorrect statement among the following is
1 In \({{\rm{C}}_{\rm{2}}}\), there is a double bond and both the bonds are \({\rm{\pi - bonds}}\)
2 Bond order of \({\rm{CO}}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{O}}^{\rm{ + }}}\) are respectively 3.0 and 3.5
3 \({\rm{CO,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}\,\,{\rm{and}}\,\,{{\rm{N}}_{\rm{2}}}\) all have the same bond order value
4 The B.O of \({\rm{CO = 2,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}{\rm{ = 2}}{\rm{.5}}\,\,{\rm{\& }}\,\,{{\rm{N}}_{\rm{2}}}{\rm{ = 3}}\)
Explanation:
Conceptual Questions
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313722
Assertion : \(\mathrm{O}_{2}\) is paramagnetic. Reason : It has one unpaired electron.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Oxygen has two unpaired electrons in its antibonding \(\pi 2 \mathrm{p}\) molecular orbitals making it paramagnetic. So the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313734
The bond length of \({\rm{H}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\,\,{\rm{and}}\,\,{{\rm{H}}_{\rm{2}}}\) are in the order
B.O. of \({\rm{H}}_{\rm{2}}^{\rm{ + }}\) is 0.5, \({\rm{H}}_{\rm{2}}^{\rm{ - }}\) is 0.5 and B.O. of \({{\rm{H}}_{\rm{2}}}\) is 1. \({\rm{H}}_{\rm{2}}^{\rm{ + }}\,\,{\rm{and}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\) have same bond order. However in \({\rm{H}}_{\rm{2}}^{\rm{ - }}\), the \({{\rm{3}}^{{\rm{rd}}}}\) electron is entering an ABMO, making it less stable than the former. So, Greater the B.O., shorter the bond and species is more stable.
313719
What is the bond order of \(\mathrm{O}_{2}\) molecule?
1 2.0
2 1.5
3 1
4 3.5
Explanation:
The electronic configuration of \(\mathrm{O}_{2}\) is \(\sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{2} \sigma 2 \mathrm{p}_{\mathrm{z}}{ }^{2} \pi 2 \mathrm{p}_{\mathrm{x}}{ }^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}{ }^{2} \pi^{*} 2 \mathrm{p}_{\mathrm{x}}{ }^{1}\) \(=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}{ }^{1}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}=\dfrac{10-6}{2}=2\)
MHTCET - 2022
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313720
As per molecular orbital theory, bond order of \({\mathrm{\mathrm{Li}_{2}}}\) is \({\mathrm{x}}\) and bond order of \({\rm{Li}}_2^ - \) is \({\mathrm{y}}\). The value of \({\mathrm{(\mathrm{x}-\mathrm{y})}}\) is ____.
1 1
2 0.5
3 2
4 3
Explanation:
\(\mathrm{Li}_{2} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}\)\(=\dfrac{4-2}{2}=1\)\(\,\,\) \(\therefore \quad x=1\)\(\mathrm{Li}_{2}^{-} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{1}\) Bond order \(=\dfrac{4-3}{2}=\dfrac{1}{2}=0.5\)\(\therefore y=0.5\)\(\therefore(x-y)=(1-0.5)=0.5\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313721
The incorrect statement among the following is
1 In \({{\rm{C}}_{\rm{2}}}\), there is a double bond and both the bonds are \({\rm{\pi - bonds}}\)
2 Bond order of \({\rm{CO}}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{O}}^{\rm{ + }}}\) are respectively 3.0 and 3.5
3 \({\rm{CO,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}\,\,{\rm{and}}\,\,{{\rm{N}}_{\rm{2}}}\) all have the same bond order value
4 The B.O of \({\rm{CO = 2,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}{\rm{ = 2}}{\rm{.5}}\,\,{\rm{\& }}\,\,{{\rm{N}}_{\rm{2}}}{\rm{ = 3}}\)
Explanation:
Conceptual Questions
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313722
Assertion : \(\mathrm{O}_{2}\) is paramagnetic. Reason : It has one unpaired electron.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Oxygen has two unpaired electrons in its antibonding \(\pi 2 \mathrm{p}\) molecular orbitals making it paramagnetic. So the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313734
The bond length of \({\rm{H}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\,\,{\rm{and}}\,\,{{\rm{H}}_{\rm{2}}}\) are in the order
B.O. of \({\rm{H}}_{\rm{2}}^{\rm{ + }}\) is 0.5, \({\rm{H}}_{\rm{2}}^{\rm{ - }}\) is 0.5 and B.O. of \({{\rm{H}}_{\rm{2}}}\) is 1. \({\rm{H}}_{\rm{2}}^{\rm{ + }}\,\,{\rm{and}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\) have same bond order. However in \({\rm{H}}_{\rm{2}}^{\rm{ - }}\), the \({{\rm{3}}^{{\rm{rd}}}}\) electron is entering an ABMO, making it less stable than the former. So, Greater the B.O., shorter the bond and species is more stable.
313719
What is the bond order of \(\mathrm{O}_{2}\) molecule?
1 2.0
2 1.5
3 1
4 3.5
Explanation:
The electronic configuration of \(\mathrm{O}_{2}\) is \(\sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{2} \sigma 2 \mathrm{p}_{\mathrm{z}}{ }^{2} \pi 2 \mathrm{p}_{\mathrm{x}}{ }^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}{ }^{2} \pi^{*} 2 \mathrm{p}_{\mathrm{x}}{ }^{1}\) \(=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}{ }^{1}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}=\dfrac{10-6}{2}=2\)
MHTCET - 2022
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313720
As per molecular orbital theory, bond order of \({\mathrm{\mathrm{Li}_{2}}}\) is \({\mathrm{x}}\) and bond order of \({\rm{Li}}_2^ - \) is \({\mathrm{y}}\). The value of \({\mathrm{(\mathrm{x}-\mathrm{y})}}\) is ____.
1 1
2 0.5
3 2
4 3
Explanation:
\(\mathrm{Li}_{2} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}\)\(=\dfrac{4-2}{2}=1\)\(\,\,\) \(\therefore \quad x=1\)\(\mathrm{Li}_{2}^{-} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{1}\) Bond order \(=\dfrac{4-3}{2}=\dfrac{1}{2}=0.5\)\(\therefore y=0.5\)\(\therefore(x-y)=(1-0.5)=0.5\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313721
The incorrect statement among the following is
1 In \({{\rm{C}}_{\rm{2}}}\), there is a double bond and both the bonds are \({\rm{\pi - bonds}}\)
2 Bond order of \({\rm{CO}}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{O}}^{\rm{ + }}}\) are respectively 3.0 and 3.5
3 \({\rm{CO,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}\,\,{\rm{and}}\,\,{{\rm{N}}_{\rm{2}}}\) all have the same bond order value
4 The B.O of \({\rm{CO = 2,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}{\rm{ = 2}}{\rm{.5}}\,\,{\rm{\& }}\,\,{{\rm{N}}_{\rm{2}}}{\rm{ = 3}}\)
Explanation:
Conceptual Questions
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313722
Assertion : \(\mathrm{O}_{2}\) is paramagnetic. Reason : It has one unpaired electron.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Oxygen has two unpaired electrons in its antibonding \(\pi 2 \mathrm{p}\) molecular orbitals making it paramagnetic. So the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313734
The bond length of \({\rm{H}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\,\,{\rm{and}}\,\,{{\rm{H}}_{\rm{2}}}\) are in the order
B.O. of \({\rm{H}}_{\rm{2}}^{\rm{ + }}\) is 0.5, \({\rm{H}}_{\rm{2}}^{\rm{ - }}\) is 0.5 and B.O. of \({{\rm{H}}_{\rm{2}}}\) is 1. \({\rm{H}}_{\rm{2}}^{\rm{ + }}\,\,{\rm{and}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\) have same bond order. However in \({\rm{H}}_{\rm{2}}^{\rm{ - }}\), the \({{\rm{3}}^{{\rm{rd}}}}\) electron is entering an ABMO, making it less stable than the former. So, Greater the B.O., shorter the bond and species is more stable.
313719
What is the bond order of \(\mathrm{O}_{2}\) molecule?
1 2.0
2 1.5
3 1
4 3.5
Explanation:
The electronic configuration of \(\mathrm{O}_{2}\) is \(\sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{2} \sigma 2 \mathrm{p}_{\mathrm{z}}{ }^{2} \pi 2 \mathrm{p}_{\mathrm{x}}{ }^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}{ }^{2} \pi^{*} 2 \mathrm{p}_{\mathrm{x}}{ }^{1}\) \(=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}{ }^{1}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}=\dfrac{10-6}{2}=2\)
MHTCET - 2022
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313720
As per molecular orbital theory, bond order of \({\mathrm{\mathrm{Li}_{2}}}\) is \({\mathrm{x}}\) and bond order of \({\rm{Li}}_2^ - \) is \({\mathrm{y}}\). The value of \({\mathrm{(\mathrm{x}-\mathrm{y})}}\) is ____.
1 1
2 0.5
3 2
4 3
Explanation:
\(\mathrm{Li}_{2} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2}\) Bond order \(=\dfrac{\mathrm{N}_{\mathrm{b}}-\mathrm{N}_{\mathrm{a}}}{2}\)\(=\dfrac{4-2}{2}=1\)\(\,\,\) \(\therefore \quad x=1\)\(\mathrm{Li}_{2}^{-} \Rightarrow \sigma 1 \mathrm{~s}^{2} \sigma^{*} 1 \mathrm{~s}^{2} \sigma 2 \mathrm{~s}^{2} \sigma^{*} 2 \mathrm{~s}^{1}\) Bond order \(=\dfrac{4-3}{2}=\dfrac{1}{2}=0.5\)\(\therefore y=0.5\)\(\therefore(x-y)=(1-0.5)=0.5\)
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313721
The incorrect statement among the following is
1 In \({{\rm{C}}_{\rm{2}}}\), there is a double bond and both the bonds are \({\rm{\pi - bonds}}\)
2 Bond order of \({\rm{CO}}\,\,{\rm{and}}\,\,{\rm{C}}{{\rm{O}}^{\rm{ + }}}\) are respectively 3.0 and 3.5
3 \({\rm{CO,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}\,\,{\rm{and}}\,\,{{\rm{N}}_{\rm{2}}}\) all have the same bond order value
4 The B.O of \({\rm{CO = 2,}}\,\,{\rm{N}}{{\rm{O}}^{\rm{ + }}}{\rm{ = 2}}{\rm{.5}}\,\,{\rm{\& }}\,\,{{\rm{N}}_{\rm{2}}}{\rm{ = 3}}\)
Explanation:
Conceptual Questions
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313722
Assertion : \(\mathrm{O}_{2}\) is paramagnetic. Reason : It has one unpaired electron.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Oxygen has two unpaired electrons in its antibonding \(\pi 2 \mathrm{p}\) molecular orbitals making it paramagnetic. So the option (3) is correct.
CHXI04:CHEMICAL BONDING AND MOLECULAR STRUCTURE
313734
The bond length of \({\rm{H}}_{\rm{2}}^{\rm{ + }}{\rm{,}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\,\,{\rm{and}}\,\,{{\rm{H}}_{\rm{2}}}\) are in the order
B.O. of \({\rm{H}}_{\rm{2}}^{\rm{ + }}\) is 0.5, \({\rm{H}}_{\rm{2}}^{\rm{ - }}\) is 0.5 and B.O. of \({{\rm{H}}_{\rm{2}}}\) is 1. \({\rm{H}}_{\rm{2}}^{\rm{ + }}\,\,{\rm{and}}\,\,{\rm{H}}_{\rm{2}}^{\rm{ - }}\) have same bond order. However in \({\rm{H}}_{\rm{2}}^{\rm{ - }}\), the \({{\rm{3}}^{{\rm{rd}}}}\) electron is entering an ABMO, making it less stable than the former. So, Greater the B.O., shorter the bond and species is more stable.
