rank the following elements according to their ionization energy.\n| element | ionization energy…

rank the following elements according to their ionization energy.\n| element | ionization energy |\n|--|--|--|\n| phosphorus | (choose one) |\n| bismuth | (choose one) |\n| argon | (choose one) |\n| thallium | (choose one) |

rank the following elements according to their ionization energy.\n| element | ionization energy |\n|--|--|--|\n| phosphorus | (choose one) |\n| bismuth | (choose one) |\n| argon | (choose one) |\n| thallium | (choose one) |

Answer

Explanation:

Step1: Recall ionization - energy trend

Ionization energy generally increases across a period and decreases down a group in the periodic table.

Step2: Locate elements in periodic table

Phosphorus (P) is in Group 15, Period 3; Bismuth (Bi) is in Group 15, Period 6; Argon (Ar) is in Group 18, Period 3; Thallium (Tl) is in Group 13, Period 6.

Step3: Analyze based on trends

Argon is a noble - gas with a stable electron configuration, so it has a high ionization energy. Phosphorus is to the left of argon in the same period, so argon > phosphorus. Bismuth and thallium are in the sixth period. Bismuth is to the right of thallium in the periodic table, so bismuth > thallium. Also, elements in lower periods generally have higher ionization energies than those in higher periods (for non - noble - gas comparisons in the same group or across a period). So, phosphorus > bismuth and phosphorus > thallium.

Answer:

argon > phosphorus > bismuth > thallium