Skip to main content
Pearson+ LogoPearson+ Logo
Ch.8 - Periodic Properties of the Elements
All textbooksTro 4th EditionCh.8 - Periodic Properties of the ElementsProblem 103
Previous problem
Next problem
Chapter 8, Problem 103

The lightest noble gases, such as helium and neon, are completely inert—they do not form any chemical compounds whatsoever. In contrast, the heavier noble gases do form a limited number of compounds. Explain this difference in terms of trends in fundamental periodic properties.

Verified step by step guidance
1
<insert step 1> The noble gases are located in Group 18 of the periodic table and are known for their lack of reactivity due to having a complete valence electron shell.>
<insert step 2> Helium and neon, the lightest noble gases, have very high ionization energies and small atomic radii, making it difficult for them to participate in chemical bonding.>
<insert step 3> As you move down the group from helium to heavier noble gases like xenon and radon, the atomic size increases, and the ionization energy decreases.>
<insert step 4> The decrease in ionization energy and increase in atomic size for heavier noble gases make it easier for them to form compounds, as they can more readily share or transfer electrons.>
<insert step 5> Additionally, the presence of d and f orbitals in heavier noble gases allows for expanded valence shells, facilitating the formation of compounds under certain conditions.>
Previous problem
Next problem
Related Practice
Open Question
Consider these elements: N, Mg, O, F, Al. 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.
Open Question
Explain why atomic radius decreases as you move to the right across a period for main-group elements but not for transition elements.
Open Question
Explain why vanadium (radius = 134 pm) and copper (radius = 128 pm) have nearly identical atomic radii, even though the atomic number of copper is about 25% higher than that of vanadium. Predict the relative densities of these two metals. Look up the densities in a reference book, periodic table, or on the Internet to check if your predictions are correct.
Open Question
Why does the lightest halogen, which is also the most chemically reactive, exhibit a decrease in reactivity as you move down the column of halogens in the periodic table? Explain this trend in terms of periodic properties.
Open Question
What are the general outer electron configurations (nsx npy) for groups 6A and 7A in the periodic table? The electron affinity of each group 7A element is more negative than that of each corresponding group 6A element. Use the electron configurations to explain why this is so.
Open Question
Why is the electron affinity of each group 5A element more positive than that of each corresponding group 4A element? Use the outer electron configurations for these columns to suggest a reason for this observation.