Which of these trends increase as you move from left to right on the Periodic Table? Select all that apply....

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Which of these trends increase as you move from left to right on the Periodic Table? Select all that apply. ionization energy electronegativity electron affinity activity series of metals atomic radii

CramX · Accepted Answer

Step 1: : Ionization energy generally increases as you move from left to right across a period in the Periodic Table.. This is because the valence electrons are in the same energy level and are farther from the nucleus, making them easier to remove. As you move to the right, the number of protons in the nucleus increases, causing a greater attraction to the electrons and thus increasing the ionization energy. Step 2: : Electronegativity also tends to increase from left to right across a period.. Electronegativity is a measure of an element's ability to attract electrons in a covalent bond. Similar to ionization energy, this is due to the increased nuclear attraction as you move to the right in a period. Step 3: : Electron affinity, however, does not have a consistent trend across a period.. Electron affinity is the energy change when an electron is added to a neutral atom to form a negative ion. The trend in electron affinity is not straightforward because it depends on the electron configuration of the atom and the resulting stability of the ion. Step 4: : The activity series of metals does not directly relate to the Periodic Table's layout.. The activity series is a list of metals arranged in order of their relative reactivity, from most reactive to least reactive. It does not have a consistent trend from left to right on the Periodic Table. Step 5: : Atomic radii generally decrease as you move from left to right across a period.. This is due to the increased nuclear charge, which pulls the electrons closer to the nucleus and reduces the atomic radius. Final Answer: - Ionization energy increases. - Electronegativity increases. - Electron affinity does not have a consistent trend. - The activity series of metals does not apply. - Atomic radii decrease.

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Step 1:
: Ionization energy generally increases as you move from left to right across a period in the Periodic Table.

Step 2:
: Electronegativity also tends to increase from left to right across a period.

Step 3:
: Electron affinity, however, does not have a consistent trend across a period.

Step 4:
: The activity series of metals does not directly relate to the Periodic Table's layout.

Step 5:
: Atomic radii generally decrease as you move from left to right across a period.

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Step 1:: Ionization energy generally increases as you move from left to right across a period in the Periodic Table.

Step 2:: Electronegativity also tends to increase from left to right across a period.

Step 3:: Electron affinity, however, does not have a consistent trend across a period.

Step 4:: The activity series of metals does not directly relate to the Periodic Table's layout.

Step 5:: Atomic radii generally decrease as you move from left to right across a period.