Questions: The first four ionization energies ( IE₁ through IE₄ ) of a Period 2 element have the following pattern:
Make a reasonable guess about which element this is. Enter its chemical symbol below.
Transcript text: The first four ionization energies ( $\mathrm{IE}_{1}$ through $\mathrm{IE}_{4}$ ) of a Period 2 element have the following pattern:
Make a reasonable guess about which element this is. Enter its chemical symbol below.
Solution
Solution Steps
Step 1: Analyze the ionization energy trend
The ionization energy increases steadily from IE₁ to IE₂ to IE₃ and then a large jump to IE₄. This indicates that the element has 3 valence electrons. Removing the fourth electron requires significantly more energy because it is removing a core electron.
Step 2: Identify the element
Period 2 elements with 3 valence electrons will belong to Group 13 (Boron group), with Boron (B) being in Period 2.