The first ionization energy refers to the energy required to remove the most loosely bound electron from a neutral atom in its ground state.

Generally, ionization energy increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This is due to the increase in effective nuclear charge across a period and the increase in atomic radius down a group.

Given the elements Se (Selenium), Cl (Chlorine), Sb (Antimony), and Pb (Lead), we can locate them on the periodic table:

- Se is in period 4, group 16.
- Cl is in period 3, group 17.
- Sb is in period 5, group 15.
- Pb is in period 6, group 14.

From this information, we can see that Cl is furthest to the right and highest up on the periodic table. Therefore, Cl (Chlorine) has the largest first ionization energy among these elements.

Question

The first ionization energy refers to the energy required to remove the most loosely bound electron from a neutral atom in its ground state.

Generally, ionization energy increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This is due to the increase in effective nuclear charge across a period and the increase in atomic radius down a group.

Given the elements Se (Selenium), Cl (Chlorine), Sb (Antimony), and Pb (Lead), we can locate them on the periodic table:

- Se is in period 4, group 16.
- Cl is in period 3, group 17.
- Sb is in period 5, group 15.
- Pb is in period 6, group 14.

From this information, we can see that Cl is furthest to the right and highest up on the periodic table. Therefore, Cl (Chlorine) has the largest first ionization energy among these elements.

Knowee AI · Accepted Answer

The first ionization energy refers to the energy required to remove the most loosely bound electron from a neutral atom in its ground state.

Generally, ionization energy increases from left to right across a period and decreases from top to bottom within a group on the periodic table. This is due to the increase in effective nuclear charge across a period and the increase in atomic radius down a group.

Given the elements Se (Selenium), Cl (Chlorine), Sb (Antimony), and Pb (Lead), we can locate them on the periodic table:

- Se is in period 4, group 16.
- Cl is in period 3, group 17.
- Sb is in period 5, group 15.
- Pb is in period 6, group 14.

From this information, we can see that Cl is furthest to the right and highest up on the periodic table. Therefore, Cl (Chlorine) has the largest first ionization energy among these elements.

Which of these elements has the largest first ionization energy?A.SeB.ClC.SbD.Pb

Question

Which of these elements has the largest first ionization energy?

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