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Use molecular orbital theory to complete this table

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Use molecular orbital theory to complete this table. Molecule Ground state electron configuration Bond order Number 700 Number NF (s) (02s)(()(2 Number NF( () (02()2)(T2) Drag a number into each of the blank boxes above. Classify these species according to their magnetic properties. Diamagnetic Paramagnetic NF NF NF

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According to the molecular orbital theory, the filling of molecular orbitals by electrons follows the ascending energy order:

$\sigma _{1s} < \sigma^* _{1s} < \sigma _{2s} < \sigma^* _{2s} < \pi _{2py} = \pi _{2pz} < \sigma _{2px} < \pi^* _{2py}=\pi^* _{2pz}< \sigma ^*_{2px}$

In every molecular orbital, we can place two electrons as a maximum. The orbitals signed with an asterisk are the non-bonding orbitals, and those that have not the asterisk are the bonding orbitals

GROUND ELECTRON STATE FOR NF MOLECULE:

To complete the ground state electron configuRAtion of NF molecule, we have to calculate first the number of electrons in the molecule from the atomic number of N and F:

For N atom:

$Z_{(N)} = 7 \;\;\rightarrow 7 e^-$

For F atom:

$Z_{(F)} = 9 \;\;\rightarrow 9 e^-$

The total number of electrons to place in the molecular orbitals is:

$\#e^-=7e^-+9e^-$

$\#e^-=16e^-$

In the ground state electron configuration of NF molecule we have:

$(\sigma _{1s})^2 (\sigma^* _{1s})^2 (\sigma _{2s})^2 (\sigma^* _{2s})^2 (\pi _{2p})^4 (\sigma _{2p})^2 (\pi^* _{2p})^2$

In the last orbital we can place four electrons( in π^*_2py and π^*_2pz orbitals), but we have only two, they are occuping differents orbitals and these are unpaired, as a consequence:

NF MOLECULE IS PARAMAGNETIC

The bond order is given by the equation:

$Bond order12)ebonding bonding non bonding$

The number of bonding electrons is directly obtained from the sum of electrons in bonding orbitals. The number of non bonding electrons is directly obtained from the sum of electrons in non bonding orbitals. For NF molecule in its ground state electron configuration we have:

$10e bonding$

$non bonding$

The bond order is:

$Bond order = (1/2)(10-6)$

$Bond\;order=2$

GROUND ELECTRON STATE FOR NF⁺ ION:

To complete the ground state electron configuration of NF⁺ ion, we have to take into account the lack of one electron respect to the total number of electrons in NF molecule, then the total number of electrons to place in the molecular orbitals is:

$\#e^-=16e^--1e^-$

$\#e^-=15e^-$

In the ground state electron configuration of NF⁺ ion we have:

$(\sigma _{1s})^2 (\sigma^* _{1s})^2 (\sigma _{2s})^2 (\sigma^* _{2s})^2 (\pi _{2p})^4 (\sigma _{2p})^2 (\pi^* _{2p})^1$

With an unpaired electron:

NF⁺ ION IS PARAMAGNETIC

The bond order is given by the equation:

$Bond order12)ebonding bonding non bonding$

The number of bonding electrons is directly obtained from the sum of electrons in bonding orbitals. The number of non bonding electrons is directly obtained from the sum of electrons in non bonding orbitals. For NF⁺ ion in its ground state electron configuration we have:

$10e bonding$

$e^-_{non\;bonding}=5e^-$

The bond order is:

$Bond\;order=(1/2)(10-5)$

$Bond\;order=2.5$

GROUND ELECTRON STATE FOR NF^- ION:

To complete the ground state electron configuartion of NF^- ion, we have to take into account the excess of one electron respect to the total number of electrons in NF molecule, then, the total number of electrons to place in the molecular orbitals is:

$\#e^-=16e^-+1e^-$

$\#e^-=17e^-$

In the ground state electron configuration of NF^- ion we have:

$(\sigma _{1s})^2 (\sigma^* _{1s})^2 (\sigma _{2s})^2 (\sigma^* _{2s})^2 (\pi _{2p})^4 (\sigma _{2p})^2 (\pi^* _{2p})^3$

With an unpaired electron:

NF^- ION IS PARAMAGNETIC

The bond order is given by the equation:

$Bond order12)ebonding bonding non bonding$

The number of bonding electrons is directly obtained from the sum of electrons in bonding orbitals. The number of non bonding electrons is directly obtained from the sum of electrons in non bonding orbitals. For NF^- ion in its ground state electron configuration we have:

$10e bonding$

$e^-_{non\;bonding}=7e^-$