Consider these elements: P, Ca, Si, S, Ga. a. Write the electron configuration for each element. b. Arrange the elements in order of decreasing atomic radius. c. Arrange the elements in order of increasing ionization energy. d. Use the electron configurations in part a to explain the differences between your answers to parts b and c.

Verified step by step guidance

1. <b>Step 1:</b> Write the electron configuration for each element. Use the periodic table to determine the number of electrons for each element and fill the orbitals in the order of increasing energy (using the Aufbau principle).
2. <b>Step 2:</b> Arrange the elements in order of decreasing atomic radius. Recall that atomic radius generally decreases across a period from left to right and increases down a group in the periodic table.
3. <b>Step 3:</b> Arrange the elements in order of increasing ionization energy. Remember that ionization energy generally increases across a period from left to right and decreases down a group.
4. <b>Step 4:</b> Compare the electron configurations from Step 1 to explain the differences in atomic radius. Consider the number of electron shells and the effective nuclear charge experienced by the outermost electrons.
5. <b>Step 5:</b> Use the electron configurations to explain the differences in ionization energy. Consider the stability of the electron configuration and the energy required to remove an electron from the outermost shell.