Which of the following elements has the highest first ionization energy?
Element then radius (pm):
X = 105pm
Y = 175pm
Z = 274pm
I think that the answer is "Z-274pm", but I just would like to make sure.
yes, correct.
Z wasn't correct.
Element Z has a larger radius than elements X and Y. Because the outer electrons of element Z are not attracted as tightly to the nucleus as the outer electrons of elements X and Y, we can expect element Z to have a lower first ionization energy than elements X and Y.
would it be: element X then: X=105pm?
Yes, element X has the highest IP1. The largest diameter has the lowest IP and the lowest diameter has the highest IP.
To determine which element has the highest first ionization energy, we need to understand the concept of ionization energy and how it relates to the atomic radius.
Ionization energy refers to the energy required to remove an electron from an atom or ion in the gaseous state. It can be influenced by several factors, including the atomic radius.
Generally, the ionization energy increases as we move across a period from left to right in the periodic table. This is because the atomic radius decreases as we move from left to right, resulting in stronger attraction between the outermost electron and the nucleus. As a result, it becomes more difficult to remove an electron, and the ionization energy increases.
In the given choices, we have elements X, Y, and Z with respective atomic radii of 105pm, 175pm, and 274pm. Since Z has the largest atomic radius (274pm), it means that the outermost electron in Z is farther away from the nucleus compared to the other elements.
As a result, the electron in Z experiences weaker attraction from the nucleus, making it easier to remove. Therefore, Z is expected to have the lowest first ionization energy among the given elements, while X with the smallest atomic radius will have the highest ionization energy.
Hence, your answer is incorrect. The correct answer is "X-105pm," which has the highest first ionization energy.