The ground state magnetic property of B_{2} a | vedclass

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(A) According to molecular orbital theory,the electronic configuration for $B_{2}$ ($10$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{

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$B_{2}$ paramagnetic and $C_{2}$ diamagnetic

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(A) According to molecular orbital theory,the electronic configuration for $B_{2}$ ($10$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \pi 2p_{x}^{1} = \pi 2p_{y}^{1}$.Since it contains two unpaired electrons,$B_{2}$ is paramagnetic.The electronic configuration for $C_{2}$ ($12$ electrons) is: $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \pi 2p_{x}^{2} = \pi 2p_{y}^{2}$.Since all electrons are paired,$C_{2}$ is diamagnetic.

The ground state magnetic property of $B_{2}$ and $C_{2}$ molecules will be

Similar Questions

Compare the relative stability of the following species and indicate the magnetic properties: $O_2$,$O_2^+$,$O_2^-$ (superoxide),and $O_2^{2-}$ (peroxide).

Match the following molecules/ions in List-$I$ with their respective bond orders in List-$II$:
| List-$I$ (Molecules/ions) | List-$II$ (Bond order) |
| :--- | :--- |
| $A. N_2^+$ | $I. 1.0$ |
| $B. CO$ | $II. 1.5$ |
| $C. O_2$ | $III. 2.0$ |
| $D. O_2^-$ | $IV. 2.5$ |
| | $V. 3.0$ |

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