Question

instructions: in each question, list the elements from least to greatest ionization energy:

1. strontium (sr), magnesium (mg), beryllium (be)
2. germanium (ge), arsenic (as), selenium (se)
3. antimony (sb), sulfur (s), cadmium (cd)

Explanation:

4) Strontium (Sr), Magnesium (Mg), Beryllium (Be)

Step1: Analyze the group trend

Ionization energy decreases down a group. These elements are in Group 2. Sr is below Mg, and Mg is below Be.

5) Germanium (Ge), Arsenic (As), Selenium (Se)

Step1: Analyze the period trend

In a period (they are in Period 4), ionization energy generally increases from left to right. Ge is to the left of As, and As is to the left of Se.

6) Antimony (Sb), Sulfur (S), Cadmium (Cd)

Step1: Consider period and group

Sb (Period 5, Group 15), S (Period 3, Group 16), Cd (Period 5, Group 12). S has a higher ionization energy than Sb (higher period for Sb). Cd has a lower ionization energy than Sb (metallic character: Cd is more metallic than Sb in the same period).

Answer:

1. \(Sr
2. \(Ge
3. \(Cd