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Comparison Of Sodium And Valence Electrons

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1a. Sodium has a larger radius than lithium because it has a higher principle quantum number and it’s electrons occupy more subshells. Because sodium and lithium are in the same group they both have 1 valence electron, but sodium has its outermost electron at n=3, and lithium’s outermost electron is at n=2, so sodium will have a larger radius despite effective nuclear charge.
1b. Magnesium has a smaller radius than sodium because it’s valence electrons have a stronger net attraction to the nucleus. Although magnesium and sodium both have a highest principal quantum number of 3, the effective nuclear charge of the valence electrons on magnesium is higher, therefore pulling its electrons closer to the nucleus.

Ionization Energy
2a. Lithium has higher ionization energy than sodium because it’s valence electrons have a smaller average distance from the nucleus. Since Lithium’s valence electron is in n=2 and sodiums is in n=3, lithium’s valence electron will be closer to the nucleus and therefore require more energy to remove. …show more content…

Fluorine has higher ionization energy than boron because fluorine’s valence electrons experience greater attraction to the nucleus. Both boron and fluorine share the same highest principal quantum number, but since fluorine has an effective nuclear charge of 2.2 and boron has an effective nuclear charge of 1.4 it will be harder to remove a valence electron from fluorine.
2c. Oxygen has lower ionization energy than nitrogen because it’s valence electrons are less attracted to the nucleus than those of nitrogen. Both nitrogen and oxygen have valence electrons at n=2, but since oxygen has a lower effective nuclear charge than that of nitrogen it will be easier to remove a valence electron, therefore requiring less energy to ionize

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