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 Mn has unpaired and set(s) one of paired electrons in its 3d orbitals, while Cr has unpaired and two set(s) of paired electrons in its 3d orbitals and Fe2+ has unpaired and three set(s) of paired electrons in its 3d orbitals. Therefore, the larger Z value of Mn four explains why it has a larger third ionization energy than while electron repulsion five explains why it has a larger third ionization energy than smaller The second ionization energy of axygen is greater than the first ionization energy of fluorine This trend is best explained by noting that O has set(s) of paired electrons in its 2p orbitals, while Fhas set(s) of paired electrons in its 2p orbitals. Paired electrons have a greater unpaired and Cr unpaired and Fe electrostatic repulsion than unpaired electrons; therefore, removing an electron from a 2p orbital of Frequires less energy than removing an electron from a 2p orbital of O
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 Mn has unpaired and set(s) one of paired electrons in its 3d orbitals, while Cr has unpaired and two set(s) of paired electrons in its 3d orbitals and Fe2+ has unpaired and three set(s) of paired electrons in its 3d orbitals. Therefore, the larger Z value of Mn four explains why it has a larger third ionization energy than while electron repulsion five explains why it has a larger third ionization energy than smaller The second ionization energy of axygen is greater than the first ionization energy of fluorine This trend is best explained by noting that O has set(s) of paired electrons in its 2p orbitals, while Fhas set(s) of paired electrons in its 2p orbitals. Paired electrons have a greater unpaired and Cr unpaired and Fe electrostatic repulsion than unpaired electrons; therefore, removing an electron from a 2p orbital of Frequires less energy than removing an electron from a 2p orbital of O
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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Transcribed Image Text:Part B
Write the electron configuration for each atonm 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 Mn has
unpaired and
set(s)
one
of paired electrons in its 3d orbitals, while Crt has
unpaired and
two
set(s) of paired electrons in its 3d orbitals and Fe2 has
unpaired and
three
set(s) of paired electrons in its 3d orbitals. Therefore, the larger Z value of Mn
four
explains why it has a larger third ionization energy than
while electron repulsion
five
explains why it has a larger third ionization energy than
smaller
The second ionization energy of oxygen is greater than the first ionization energy of fluorine.
greater
This trend is best explained by noting that O has
unpaired and
Cr
set(s) of paired electrons in its 2p orbitals, while F has
unpaired and
Fe
set(s) of paired electrons in its 2p orbitals. Paired electrons have a
electrostatic
repulsion than unpaired electrons; therefore, removing an electron from a 2p orbital of F requires less
energy than removing an electron from a 2p orbital of O
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