Question

size trends
ionic radius
consider your knowledge about the
behavior of atoms forming ions and ionic
radius trends.
i. the radius of all ions are smaller than
their original atoms due to a change in the
number of electrons.
ii. the radius of cations are smaller than
their original atoms due to the loss of
electrons from the furthest energy level.
iii. the radius of anions are larger than
their original atoms due to the loss of
protons from the nucleus.
iv. the ionic radius trend is generally
increasing in size from left to right on the
periodic table.
which statement is true regarding ionic
radius?
statement i
statement ii
statement iv
statement iii
skip

Explanation:

• Statement I is false: anions (negatively charged ions) gain electrons, so their radius is larger than the original atom, not smaller.
• Statement II is true: cations lose electrons, often from the outermost energy level, reducing electron cloud size and making the cation radius smaller than the parent atom.
• Statement III is false: anions form by gaining electrons, not losing protons; the increased electron-electron repulsion expands the electron cloud, increasing radius.
• Statement IV is false: ionic radius generally decreases from left to right across a period for isoelectronic ions, as nuclear charge increases while electron count stays the same.

Answer:

Statement II