**Use molecular orbital theory to complete the ground state electron configuration for each of the molecules.****Molecule | Ground state electron configuration**The table consists of molecules (NF, NF⁺, NF⁻) alongside their molecular orbital electron configurations. Each row provides empty boxes for electrons corresponding to the following molecular orbitals: - \( ( \sigma_{1s} ) \)- \( ( \sigma_{1s}^* ) \)- \( ( \sigma_{2s} ) \)- \( ( \sigma_{2s}^* ) \)- \( ( \pi_{2p} ) \)- \( ( \sigma_{2p} ) \)- \( ( \pi_{2p}^* ) \)Each orbital is represented by dashed boxes where electrons are to be filled indicating their position in the respective molecular orbitals. There are three different molecular species indicated:- **NF:** Consists of eight boxes laid out, corresponding to each molecular orbital. - **NF⁺:** Similar layout with eight boxes for each orbital. - **NF⁻:** Again, eight boxes for electrons, correlating to the indicated orbitals.To complete the electron configurations, one would fill these boxes according to the molecular orbital theory rules, using arrows to represent electrons.

Use molecular orbital theory to complete the ground state electron configuration for each of the molecules. Ground state electron configuration Molecule IT2p (025) (025 T2p NF (01s) TT2 NF+ 02p (T2p*) (02s T2P NF- (01s) 1s

Use molecular orbital theory to complete the ground state electron configuration for each of the molecules. Ground state electron configuration Molecule IT2p (025) (025 T2p NF (01s) TT2 NF+ 02p (T2p*) (02s T2P NF- (01s) 1s

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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