Question

question 8. which of the following elements have a higher ionization energy than aluminum (al)? select all that apply. chlorine (cl) silicon (si) sodium (na) boron (b) calcium (ca) nitrogen (n)

Explanation:

Step1: Recall ionization energy trends

Ionization energy generally increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. Aluminum (Al) is in period 3, group 13.

Step2: Analyze each element

• Chlorine (Cl): Period 3, group 17. Right of Al in same period. Ionization energy increases across period, so Cl > Al.
• Silicon (Si): Period 3, group 14. Right of Al in same period. Ionization energy increases across period, so Si > Al.
• Sodium (Na): Period 3, group 1. Left of Al in same period. Ionization energy decreases left to right, so Na < Al.
• Boron (B): Period 2, group 13. Above Al in same group. Ionization energy increases up a group, so B > Al.
• Calcium (Ca): Period 4, group 2. Below and left of Al. Ionization energy lower (down group and left in period), so Ca < Al.
• Nitrogen (N): Period 2, group 15. Above and right of Al's group. Ionization energy higher (up group, right in period), so N > Al.

Answer:

A. Chlorine (Cl), B. Silicon (Si), D. Boron (B), F. Nitrogen (N)