Question

rank the following atoms in order of increasing ionization energy, from lowest to highest: p, ne, f, s, si

Explanation:

Step1: Recall ionization energy trends

Ionization energy generally increases across a period (left - to - right) and decreases down a group. Noble gases (like Ne) have very high ionization energies due to their stable electron configurations.

Step2: Analyze the positions of the elements

• Si is in group 14, period 3.
• P is in group 15, period 3.
• S is in group 16, period 3.
• F is in group 17, period 2.
• Ne is a noble gas (group 18, period 2).
• Among Si, P, and S (same period), ionization energy: \(Si
• F is in period 2, has a higher ionization energy than Si, P, and S (smaller atomic radius, more protons relative to electron shells).
• Ne is a noble gas with a full valence shell, so it has a very high ionization energy.

Answer:

\(Si < P < S < F < Ne\)