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Given below are two statements:

Statement I:	A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II:	As bond order increases, the bond length increases.

1.	Statement I is True but Statement II is False.
2.	Statement I is False but Statement II is True.
3.	Both Statement I and Statement II are True.
4.	Both Statement I and Statement II are False.

Subtopic: M.O.T |

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Q2:

Identify the correct orders against the property mentioned:

A.	$\mathrm{H}_2 \mathrm{O}>\mathrm{NH}_3>\mathrm{CHCl}_3 -\text { }$dipole moment
B.	$\mathrm{XeF}_4>\mathrm{XeO}_3>\mathrm{XeF}_2-\text { }$number of lone pairs on central atom
C.	$\mathrm{O}-\mathrm{H}>\mathrm{C}-\mathrm{H}>\mathrm{N}-\mathrm{O}-\text { }$ bond length
D.	$\mathrm{N}_2>\mathrm{O}_2>\mathrm{H}_2 \text { } -$ bond enthalpy

Choose the correct answer from the options given below:
1. A and C only
2. B and C only
3. A and D only
4. B and D only

Subtopic: M.O.T | Polarity | V.S.E.P.R & V.B.T |

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Q3:

Which one of the following molecules is paramagnetic?

1. $\mathrm{H}_2$
2. $\mathrm{Li}_2$
3. $\mathrm{C_2}$
4. $\mathrm{O}_2$

Subtopic: M.O.T |

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Q4:

Match List-I with List-II:

	List-I (Atom/Molecule)		List-II (Property)
A.	Nitrogen	I.	Paramagnetic
B.	Fluorine molecule	II.	Most reactive element in group 18
C.	Oxygen molecule	III.	Element with highest ionisation enthalpy in group 15
D.	Xenon atom	IV.	Strongest oxidising agent

Identify the correct answer from the option given below:

1.	A- III, B-I, C-IV, D-II	2.	A-I, B-IV, C-III, D-II
3.	A-II, B-IV, C-I, D-II	4.	A-III, B-IV, C-I, D-II

Subtopic: M.O.T |

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Q5:

The correct order of energies of molecular orbitals of N₂ molecule is:

1.	$ \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<$ $\sigma^* 2 s<\left(\pi 2 p_x=\pi 2 p_y\right)<$ $\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma 2 p_z<\sigma^* 2 p_z$
2.	$ \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<\sigma^* 2 s<$ $\left(\pi 2 p_x=\pi 2 p_y\right)< $ $\sigma 2 p_z<\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma^* 2 p_z $
3.	$ \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<\sigma^* 2 s<\sigma 2 p_z<$ $ \left(\pi 2 p_x=\pi 2 p_y\right)<$ $\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma^* 2 p_z $
4.	$ \sigma \text { 1s }<\sigma^* \text { 1s }$ $<\sigma 2 s<\sigma^* 2 s<\sigma 2 p_z< $ $ \sigma^* 2 p_z<\left(\pi 2 p_x=\pi 2 p_y\right)<$ $\left(\pi^* 2 p_x=\pi^* 2 p_y\right) $

Subtopic: M.O.T |

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Q6:

Which one of the following statements is incorrect related to Molecular Orbital Theory?

1.	The $\pi^*$ antibonding molecular orbital has a node between the nuclei.
2.	In the formation of a bonding molecular orbital, the two electron waves of the bonding atoms reinforce each other.
3.	Molecular orbitals obtained from $2P_x$ and $2P_y$ orbitals are symmetrical around the bond axis.
4.	A $\pi-$bonding molecular orbital has larger electron density above and below the internuclear axis.

Subtopic: M.O.T |

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Q7:

Identify the incorrect statement among the following options:

1.	$O^+_2$ ion is diamagnetic.
2.	The bond orders of $O_2^{+},O_2,O^-_2$ and $O_2^{2-}$ are 2.5, 2, 1.5, and 1, respectively.
3.	$C_2$ molecule has four electrons in its two degenerate $\pi $ molecular orbitals.
4.	$H^+_2 $ ion has one electron.

Subtopic: M.O.T |

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Q8:

Which one of the following is the correct order of decreasing bond enthalpies for the given species?
1. $\mathrm {O^{2-}_2>O^-_2>O_2>N_2 }$
2. $\mathrm {N_2>O_2>O^{2-}_2>O^-_2 }$
3. $\mathrm {N_2>O_2>O^-_2>O^{2-}_2 }$
4. $\mathrm {O_2>N_2>O^-_2>O^{2-}_2 }$

Subtopic: M.O.T |

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Q9:

A molecule that cannot exist is:

1.	${Li}_{2}$	2.	$C_{2}$
3.	$O_{2}$	4.	${He}_{2}$

Subtopic: M.O.T |

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Q10:

A diatomic molecule, among the following species, that only has $π$ bonds according to the Molecular Orbital Theory (MOT) is:

1.	Be₂	2.	O₂
3.	N₂	4.	C₂

Subtopic: M.O.T |

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A.	\(\mathrm{H}_2 \mathrm{O}>\mathrm{NH}_3>\mathrm{CHCl}_3 -\text { }\)dipole moment
B.	\(\mathrm{XeF}_4>\mathrm{XeO}_3>\mathrm{XeF}_2-\text { }\)number of lone pairs on central atom
C.	\(\mathrm{O}-\mathrm{H}>\mathrm{C}-\mathrm{H}>\mathrm{N}-\mathrm{O}-\text { }\) bond length
D.	\(\mathrm{N}_2>\mathrm{O}_2>\mathrm{H}_2 \text { } -\) bond enthalpy

1.	\( \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<\) \(\sigma^* 2 s<\left(\pi 2 p_x=\pi 2 p_y\right)<\) \(\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma 2 p_z<\sigma^* 2 p_z\)
2.	\( \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<\sigma^* 2 s<\) \(\left(\pi 2 p_x=\pi 2 p_y\right)< \) \(\sigma 2 p_z<\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma^* 2 p_z \)
3.	\( \sigma \text { 1s }<\sigma^* \text { 1s }<\sigma 2 s<\sigma^* 2 s<\sigma 2 p_z<\) \( \left(\pi 2 p_x=\pi 2 p_y\right)<\) \(\left(\pi^* 2 p_x=\pi^* 2 p_y\right)<\sigma^* 2 p_z \)
4.	\( \sigma \text { 1s }<\sigma^* \text { 1s }\) \(<\sigma 2 s<\sigma^* 2 s<\sigma 2 p_z< \) \( \sigma^* 2 p_z<\left(\pi 2 p_x=\pi 2 p_y\right)<\) \(\left(\pi^* 2 p_x=\pi^* 2 p_y\right) \)

1.	The \(\pi^*\) antibonding molecular orbital has a node between the nuclei.
2.	In the formation of a bonding molecular orbital, the two electron waves of the bonding atoms reinforce each other.
3.	Molecular orbitals obtained from \(2P_x\) and \(2P_y\) orbitals are symmetrical around the bond axis.
4.	A \(\pi-\)bonding molecular orbital has larger electron density above and below the internuclear axis.

1.	\(O^+_2\) ion is diamagnetic.
2.	The bond orders of \(O_2^{+},O_2,O^-_2\) and \(O_2^{2-}\) are 2.5, 2, 1.5, and 1, respectively.
3.	\(C_2\) molecule has four electrons in its two degenerate \(\pi \) molecular orbitals.
4.	\(H^+_2 \) ion has one electron.

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