Final answer:
Magnesium and boron, though different elements, share the property of having a filled s subshell in their electron configuration. Magnesium has a [Ne]3s² configuration while boron is [He]2s² 2p¹, both showing completed s orbitals as their outermost shells.
Step-by-step explanation:
The question is inquiring about what 24 grams of magnesium (Mg) and 10 grams of boron (B) have in common. While these two elements differ in many ways, one similarity they share is that the atoms of both elements have a filled s subshell outside their filled inner shells: magnesium, a member of the alkaline earth metals, has an electron configuration of [Ne]3s², while boron, a member of the group 13 elements, has an electron configuration of [He]2s² 2p¹. This means that despite their differences in atomic number and properties, both elements have completed s orbitals as their outermost electron shell configuration.