Part B Write the electron configuration for each atom on your own; then complete

Question

Part B Write the electron configuration for each atom on your own; then complete the sentences to explain the trends in ionization energy Match the words in the left column to the appropriate blanks in the sentences on the right. Reset Help zero The third ionization energy of manganese is greater than that of both chromium and iron This is best explained by noting that Mn2+ has unpaired and one set(s) of paired electrons in its 3d orbitals, while Cr2+ has 0 unpaired and set(s) of paired electrons in its 3d orbitals three and Fe2+ has its 3d orbitals. Therefore, the larger Z value of Mn explains why it has a larger third ionization energy than larger third ionization energy than unpaired and set(s) of paired electrons in four five , while electron repulsion explains why it has a smaller greater The second ionization energy of oxygen is greater than the first ionization energy of fluorine This trend is best explained by noting that O has unpaired and set(s) of paired electrons in its 2p orbitals, while F has unpaired and have a removing an electron from a 2p orbital of F requires less energy than removing an electron from a 2p orbital of O set(s) of paired electrons in its 2p orbitals. Paired electrons electrostatic repulsion than unpaired electrons; therefore

Explanation / Answer

Mn+2 has 5 unpaired electrons in 3d orbital zero paired electron pairs.

While Cr+2 has 4 unpaired electrons and zero paired electrons

Ionization energy of Mn is Larger than Crystal and due to electron repulsions, ionization energy is larger than Cr+2.

O+ has 3 unpaired electrons and zero sets of paired electrons while F has one unpaired electron and two sets of paired electrons.

Paired electrons have smaller electrostatic repulsions than unpaired electrons.

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