Bond order of 1.5 is shown by : [2012]a)O2+b)O2-c)O22+d)O2Correct answer is option 'B'. Can you explain this answer?

Question

Answer

N₂=N+N = 7e⁻+7e⁻ = 14e- which has bond order =3

O₂=8e⁻+8e⁻ = 16e⁻ which has bond order = 2

O₂⁺=8e⁻+8e⁻ - 1e⁻ = 15e⁻ which has bond order= 2.5

O₂⁻ = 8e⁻ +8e⁻ +1e⁻ =17 e⁻ which has bond order=1.5

So option B is correct .

Answer

Option b has 17e- so it has 1.5 bond order
u may remember it by a trick
atom which contain 14e- always have 3 bond order
and after increasing or decreasing no. of electrons bond order also increase or decrease by no. 0.5 respectively..
means if 13e- and 15e- then it has 2.5
and if 12e- and 16e- then it has 2
and so on...

Answer

There are 10 bonding electrons and 7 antibonding electrons
therefore bond order=(no. of bonding -no. of antibonding electrons) /2
so, (nb-nb)/2= (10-7)/2
=3/2=1.5

Answer

When the electrons are 14 the bond order is 3
In O2- electrons=17
So the bond order is 1.5...

Answer

Bond order is a measure of the strength and stability of a covalent bond. It is defined as the half of the difference between the number of bonding and anti-bonding electrons in a molecule. Bond order values can range from 0 to 3.

To determine the bond order of a molecule, we need to first write its molecular orbital diagram. In the molecular orbital diagram, the molecular orbitals are represented by horizontal lines, and the electrons are represented by arrows. The higher the energy level of the molecular orbital, the higher its energy.

In the case of O2, the molecular orbital diagram can be represented as follows:

O2:
σ2s: ↑↓
σ*2s:
σ2p: ↑↓
π2p: ↑↑
π*2p:

In this diagram, the σ2s and σ*2s molecular orbitals are filled with two electrons each, one with spin up and the other with spin down. The σ2p molecular orbital is filled with two electrons, one with spin up and the other with spin down. The π2p molecular orbital is filled with two electrons, both with spin up. Since there are no electrons in the π*2p molecular orbital, it is considered as an anti-bonding orbital.

Now, let's calculate the bond order using the formula:

Bond order = (Number of bonding electrons - Number of anti-bonding electrons) / 2

In the case of O2, the number of bonding electrons is 8 (2 in σ2s, 2 in σ2p, and 4 in π2p), and the number of anti-bonding electrons is 4 (2 in σ*2s and 2 in π*2p). Plugging these values into the formula, we get:

Bond order = (8 - 4) / 2 = 4 / 2 = 2

Therefore, the bond order of O2 is 2, which corresponds to a double bond.

The correct answer is option 'B' (O2).

Answer

B

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