Chemistry · Periodic trends in properties of elements: atomic and ionic radii, ionization enthalpy, electron gain enthalpy, valence, oxidation states and chemical reactivity
has lower ionization potential than that of because:
\( A l \) has lower ionization potential than that of \( M g \) because:
- A. \( A l \) atom is bigger than \( M g \) atom
- B. \( M g \) atom is bigger than \( A l \) atom
- C. all electrons in \( M g \) are paired, but those of \( A l \) are not
- D. all belongs to a higher group
Step-by-step solution
Magnesium has a filled 3s subshell (all electrons paired), which gives it extra stability due to exchange energy. Removing an electron from Mg disrupts this stable configuration, resulting in a higher ionization enthalpy. Aluminum has one unpaired electron in the 3p orbital, which is easier to remove because it is less tightly bound and does not require breaking a fully filled subshell.
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