Home
Class 11
CHEMISTRY
The bond length the species O(2), O(2)^(...

The bond length the species `O_(2), O_(2)^(+) and O_(2)^(-)` are in the order of

A

`O_(2)^(+) gt O_(2) gt O_(2)^(-)`

B

`O_(2)^(+) gt O_(2)^(-) gt O_(2)`

C

`O_(2) gt O_(2)^(+) gt O_(2)^(-)`

D

`O_(2)^(-) gt O_(2) gt O_(2)^(+)`

Text Solution

AI Generated Solution

The correct Answer is:
To determine the bond lengths of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \), we will use the concept that bond order is inversely proportional to bond length. This means that a higher bond order corresponds to a shorter bond length, while a lower bond order corresponds to a longer bond length. ### Step-by-Step Solution: 1. **Determine the Bond Order for Each Species:** - For \( O_2 \): - The bond order is calculated as follows: \[ \text{Bond Order} = \frac{(N_b - N_a)}{2} \] where \( N_b \) is the number of bonding electrons and \( N_a \) is the number of antibonding electrons. For \( O_2 \), there are 12 bonding electrons and 4 antibonding electrons, so: \[ \text{Bond Order of } O_2 = \frac{(12 - 4)}{2} = 4 \] However, the bond order is typically simplified to 2 for \( O_2 \) in molecular orbital theory. - For \( O_2^+ \): - Removing one electron from \( O_2 \) (which is in a bonding orbital) gives us a bond order of: \[ \text{Bond Order of } O_2^+ = \frac{(11 - 4)}{2} = 3.5 \] This is typically simplified to 2.5. - For \( O_2^- \): - Adding one electron to \( O_2 \) (which goes into an antibonding orbital) gives us a bond order of: \[ \text{Bond Order of } O_2^- = \frac{(12 - 5)}{2} = 3.5 \] This is typically simplified to 1.5. 2. **List the Bond Orders:** - \( O_2 \): Bond Order = 2 - \( O_2^+ \): Bond Order = 2.5 - \( O_2^- \): Bond Order = 1.5 3. **Determine the Order of Bond Lengths:** - Since bond order is inversely proportional to bond length: - Higher bond order means shorter bond length. - Therefore, the order of bond lengths from longest to shortest is: - \( O_2^- \) (lowest bond order, longest bond length) - \( O_2 \) (medium bond order) - \( O_2^+ \) (highest bond order, shortest bond length) 4. **Final Order of Bond Lengths:** - The bond lengths are in the order: \[ O_2^- > O_2 > O_2^+ \] ### Conclusion: The bond lengths of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \) are in the order of: \[ O_2^- > O_2 > O_2^+ \]
To determine the bond lengths of the species \( O_2 \), \( O_2^+ \), and \( O_2^- \), we will use the concept that bond order is inversely proportional to bond length. This means that a higher bond order corresponds to a shorter bond length, while a lower bond order corresponds to a longer bond length. ### Step-by-Step Solution: 1. **Determine the Bond Order for Each Species:** - For \( O_2 \): - The bond order is calculated as follows: \[ ...
Promotional Banner

Similar Questions

Explore conceptually related problems

The bond order in the species O_2, O_(2)^(+) and O_(2)^(-) follows the order

Bond order of O_(2),O_(2)^(+),O_(2)^(-) and O_(2)^(2-) is in order

Write the molecular orbital configuration O_(2),O_(2)^(-)and O_(2)^(2-) Arrange them in increasing order of (i) Bond order (ii) Bond dissociation energy

Which out of O_(2)^(-)and O_(2)^(2-) has higher bond order and why ?

Compare the relative stability of the following species and indicate their magnetic properties : O_(2) , O_(2)^(+) ,O_(2)^(-) ( susperoxide ) ,O_(2)^(2-) (peroxide )

Consider the isoelectronic species, Na^(+),Mg^(2+),F^(-) and O^(2-) . The correct order of increasing length of their radii is:

The H - O - O bond angle in H_(2)O_(2) (g) is

The correct order of O - O bond length in O_(2)H_(2)O_(2) and O_(3) is

Using molecular orbital theory predict the correct decreasing bond order of the following species 1. O_(2)^(+) 2. O_(2)^(-) 3. O_(2)^(2-) 4. O_(2)^(2+)