Question

question: 28 of 36 form a 11.0: chemistry on - line test (cd: c) 28 order the elements by increasing first ionization energy. move the labels to the blank boxes to show your answer. lowest 1st ionization energy → highest 1st ionization energy argon, ar magnesium, mg neon, ne silicon, si

Explanation:

Step1: Recall ionization - energy trend

First - ionization energy generally increases across a period and decreases down a group in the periodic table.

Step2: Locate elements in periodic table

Magnesium (Mg) is in Group 2 and Period 3, Silicon (Si) is in Group 14 and Period 3, Argon (Ar) is in Group 18 and Period 3, Neon (Ne) is in Group 18 and Period 2.

Step3: Compare ionization energies

Mg has the lowest first - ionization energy among them as it is in Group 2 and will easily lose its out - ermost electrons. Si has a higher first - ionization energy than Mg as it is to the right of Mg in the same period. Ar has a higher first - ionization energy than Si as it is a noble gas in the same period. Ne has the highest first - ionization energy as it is a noble gas in a higher energy level than Ar but with a smaller atomic radius and a full outer shell.

Answer:

Magnesium, Mg; Silicon, Si; Argon, Ar; Neon, Ne