An element with the symbol Z has the electron configuration 2.8.6. Which species is this elrment most likely to form?

A. The ion Z 2+
B. The ion Z 6+
C. The compound H subscript 2 Z
D. The compound Z subscript 6 F

Which ionization requires the most energy?
A. Na--> Na superscript + plus one electron
B. Na superscript + -----> Na superscript 2+ plus one electron
C. Mg---> Mg superscript + plus one electron
D. Mg superscript + -----> Mg superscript 2+ plus one electron

For 2.8.6 we would expect

1s2 2s2 2p6 3s2 3p4 which puts the element in group 16 (or VI) it probably is S. It could form +6 but is more likely to form -2 so H2Z is what I would pick.
It might also form ZF6 (but not Z6F) but H2S is still the most probable.

Would #2 make sense to go with B?

A. The ion Z 2+: Well, it seems like this element just wants to get rid of those surplus electrons, like cleaning out the closet. It's saying, "I don't need these extra electrons, let me be light and carefree." So, it's most likely to form the ion Z 2+.

D. The compound Z subscript 6 F: Ah, the element Z seems to have a sweet tooth for fluorine (F). They're like peanut butter and jelly, but instead, it's Z and F. It's most likely to form the compound Z subscript 6 F.

Now, as for the ionization that requires the most energy:

B. Na superscript + -----> Na superscript 2+ plus one electron: Imagine you're trying to pry open a jar that's super tight. It takes a lot of effort and energy to get that lid off. In the same way, removing an electron from a 2+ ion of sodium (Na) would require the most energy.

So, the answer is B. Na superscript + -----> Na superscript 2+ plus one electron. That electron is sticking tight, like glue!

An element with the electron configuration 2.8.6 means that it has 2 electrons in the first energy level, 8 electrons in the second energy level, and 6 electrons in the third energy level.

Based on this configuration, the element is most likely to form the ion Z 2+ because it can lose two electrons from the outermost energy level (third energy level) to achieve a stable electron configuration.

Therefore, the correct answer is:
A. The ion Z 2+.

For the second question, we are looking for the ionization that requires the most energy.

Ionization refers to the removal of an electron from an atom or ion. Generally, it requires more energy to remove an electron from an atom that has a smaller atomic radius and a greater nuclear charge.

Comparing the given options:
A. Na --> Na superscript + plus one electron
B. Na superscript + -----> Na superscript 2+ plus one electron
C. Mg---> Mg superscript + plus one electron
D. Mg superscript + -----> Mg superscript 2+ plus one electron

Among these options, the ionization that requires the most energy is:

B. Na superscript + -----> Na superscript 2+ plus one electron.

This is because the second ionization of sodium (Na superscript 2+) involves removing an electron from a cation that already has a positive charge. As the positive charge increases, it becomes harder to remove another electron, thus requiring more energy.

So, the correct answer is:
B. Na superscript + -----> Na superscript 2+ plus one electron.

To determine the most likely species that the element with the symbol Z will form and the ionization that requires the most energy, we can analyze the electron configuration and ionization patterns.

In the electron configuration 2.8.6, Z has 2 electrons in the first energy level (2s subshell), 8 electrons in the second energy level (2p subshell), and 6 electrons in the third energy level (3s subshell).

Based on the electron configuration, the element Z is most likely to form the ion Z2+. This means it loses 2 electrons to attain the electron configuration of the noble gas that precedes it in the periodic table. Losing 2 electrons will leave the element with the electron configuration 2.8, which matches the electron configuration of the noble gas.

Now let's consider the ionization energies of the given options:

A. Na to Na+ + e- : This corresponds to the removal of one electron from a sodium atom to form a sodium ion with a positive charge.
B. Na+ to Na2+ + e- : This corresponds to the removal of an additional electron from a sodium ion already carrying a positive charge.
C. Mg to Mg+ + e- : This corresponds to the removal of one electron from a magnesium atom to form a magnesium ion with a positive charge.
D. Mg+ to Mg2+ + e- : This corresponds to the removal of an additional electron from a magnesium ion already carrying a positive charge.

In general, removing electrons from an atom or ion requires increasing amounts of energy as each electron is closer to the nucleus and more strongly attracted. Therefore, the option that requires the most energy is D. Mg+ to Mg2+ + e- because it involves the removal of an additional electron from a positively charged ion.

To summarize:
- The element Z is most likely to form the ion Z2+ based on its electron configuration.
- The ionization that requires the most energy is D. Mg+ to Mg2+ + e-, corresponding to the removal of an additional electron from a positively charged ion.

A. The ion Z2+