Question

1. arrange the following elements in order from smallest ionization energy to largest ionization energy. periodic table smallest ionization energy → largest ionization energy a b c choices: p ne pd

Explanation:

Step1: Understand ionization energy trends

Ionization energy generally increases across a period and decreases down a group. Noble gases (like Ne) have high ionization energies as they have full - shell electron configurations. Transition metals (like Pd) have relatively lower ionization energies compared to noble gases. Non - metals (like P) have higher ionization energies than metals but lower than noble gases in the same period.

Step2: Analyze the positions of the elements

Pd (palladium) is a transition metal in period 5. P (phosphorus) is a non - metal in period 3. Ne (neon) is a noble gas in period 2. Since Pd is in a lower period (higher atomic number, more shells) compared to P and Ne (for Ne, it has a full shell), Pd has the smallest ionization energy. Ne has the largest ionization energy as it is a noble gas. P has an ionization energy between Pd and Ne.

Answer:

A. Pd, B. P, C. Ne