To determine which statement is best supported by the information in the chart regarding the valence electrons of the atoms, we need to consider the typical behavior of atoms based on their number of valence electrons:
- Atom X has 6 valence electrons. Atoms with 6 valence electrons, like oxygen, tend to gain or share 2 electrons to achieve a full outer shell (8 valence electrons).
- Atom Y has 2 valence electrons. Atoms with 2 valence electrons, like magnesium, typically lose their 2 electrons to achieve a full outer shell.
- Atom Z has 8 valence electrons. Atoms with a full outer shell (8 valence electrons) are generally inert and do not readily donate or accept electrons.
Now, let's evaluate the statements:
- Atom X will donate electrons to Atom Y. - This is unlikely because Atom X needs to gain electrons, not donate them.
- Atom X will accept electrons from Atom Y. - This is supported. Atom Y, with its 2 valence electrons, can donate those electrons to Atom X, allowing Atom X to achieve a full outer shell (8 valence electrons).
- Atom Y will accept electrons from Atom Z. - This is unlikely as Atom Z already has a full outer shell and will not donate electrons to Atom Y.
- Atom Z will donate electrons to Atom X. - This is also unlikely because Atom Z has a full outer shell and is generally inert.
Therefore, the best-supported statement is: Atom X will accept electrons from Atom Y.