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Ghella [55]
3 years ago
13

Among the elements of the main group, the general trend in the first ionization energy moving across a period is not followed be

tween group 2 and group 13. Which best explains these exceptions?
The ionization energy decreases because the full s orbital shields the electron entering the p orbital.
The ionization energy increases because the full s orbital shields the electron entering the p orbital.
The ionization energy decreases because the stability of the half-full p subshell is increased.
The ionization energy increases because the stability of the half-full p subshell is increased.
Chemistry
2 answers:
Maru [420]3 years ago
8 0

Group 2 and group 13 do not follow these rules because in their case, s orbitals block electrons from going into the p orbital. So A is the answer.

Radda [10]3 years ago
5 0
<span>The Ionization energy decreases because the full s orbital shields the electron entering the p orbital. This is known as "shielding", When each new electron experiences attraction from the nucleus and repulsion forces from the S orbitals, the net force on outer shell electrons is significantly smaller. Therefore, ionization energy decreases during these groups.</span>
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Thus 85.0  g of H_2O will be required and 2 steps are required to get the answer.

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3 years ago
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