Which of the following best describes the relationship between metallic character and ionization energy across the periodic table?

• A. Metallic character increases as ionization energy decreases.
• B. Metallic character and ionization energy are unrelated.
• C. Metallic character increases as ionization energy increases.
• D. Metallic character decreases as ionization energy decreases.

Answer: (A)

Verified step by step guidance

1. Understand the definition of metallic character: Metallic character refers to how readily an atom can lose electrons to form positive ions (cations). Metals tend to lose electrons easily, so higher metallic character means atoms lose electrons more readily.
2. Recall the definition of ionization energy: Ionization energy is the amount of energy required to remove an electron from a gaseous atom or ion. A high ionization energy means it is difficult to remove an electron, while a low ionization energy means it is easier.
3. Analyze the relationship: Since metallic character involves losing electrons easily, atoms with low ionization energy (which require less energy to remove an electron) will have higher metallic character.
4. Consider periodic trends: Moving from left to right across a period, ionization energy generally increases and metallic character decreases. Moving down a group, ionization energy decreases and metallic character increases.
5. Conclude the relationship: Therefore, metallic character increases as ionization energy decreases, showing an inverse relationship between these two properties across the periodic table.