A compound consisting of small atomic mass is more likely to require a higher ionization energy to remove an electron.

Here's why:

* Smaller atomic radius: Atoms with smaller atomic masses generally have smaller atomic radii. This means the electrons are closer to the nucleus, experiencing a stronger electrostatic attraction.

* Stronger nuclear pull: The smaller distance between the nucleus and electrons leads to a stronger attractive force from the nucleus. This makes it more difficult to remove an electron.

* Higher ionization energy: Ionization energy is the energy required to remove an electron from a gaseous atom or ion. Because of the strong attraction, more energy is needed to overcome the force holding the electron in place, resulting in a higher ionization energy.

Example:

Helium (He) has a very small atomic mass and a very high ionization energy compared to larger atoms like potassium (K).

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