Question

In general, as you move across a period (from left to right), how does the ionization energy change?

o decreases randomly
o changes
o stays the same
o increases

Answer 1

In general, as you move across a period from left to right on the periodic table, the ionization energy increases. Option D is correct.

Step-by-step explanation:

The ionization energy generally increases as you move across a period from left to right on the periodic table.

This is because the atomic size decreases and the electrostatic interactions between the nucleus and valence electrons increase, making it harder to remove electrons.

For example, elements on the left side of the periodic table have lower ionization energies because their valence electrons are farther from the nucleus and experience less pull, while elements on the right side have higher ionization energies because their valence electrons are closer to the nucleus and experience stronger attraction.

As you move across a period from left to right, the ionization energy generally increases. This increase in ionization energy is due to the greater nuclear charge as you move across the period.

With more protons in the nucleus, the attraction between the nucleus and the valence electrons is stronger, making it more difficult to remove an electron. The atomic size decreases and the electrostatic interactions between the nucleus and valence electrons increase, which in turn raises the energy required to remove an electron.