Which best explains why an Al 3+ ion is smaller than an Al atom?

In forming the Al^3+ ion (Al 3+ seems to be a typographical error for Al^3+), the aluminum atom loses electrons from its outermost energy level. This loss of electrons reduces the electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus, resulting in a decrease in the atomic radius.

Which best explains why an Al 3+ ion is smaller than an Al atom?

In forming the Al^3+ ion (Al 3+ seems to be a typographical error for Al^3+), the aluminum atom loses electrons from its outermost energy level. This loss of electrons reduces the electron-electron repulsion and allows the remaining electrons to be pulled closer to the nucleus, resulting in a decrease in the atomic radius.

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Which Best Explains Why an Al³⁺ Ion Is Smaller Than

Question 26

Multiple Choice

Which best explains why an Al³⁺ ion is smaller than an Al atom?

A) In forming the Al³⁺ ion,the Al atom loses the electrons in its outermost energy level,causing a decrease in the atomic radius.
B) In forming the Al³⁺ ion,the Al atom gains three protons and the resulting net positive charge keeps the electrons more strongly attracted to the nucleus,reducing the radius.
C) The Al³⁺ ion contains more electrons than the Al atom,which results in a greater attraction for the nucleus and a smaller atomic radius.
D) In forming the Al³⁺ ion,the Al atom adds electrons into a higher energy level,causing a decrease in the atomic radius.
E) There are more protons in an Al³⁺ ion than there are in an Al atom.

Correct Answer: