Would you expect the boiling points to increase or decrease in the following series? Explain.Kr, Ar, Ne

Verified step by step guidance

1. insert step 1> Consider the elements in the series: Krypton (Kr), Argon (Ar), and Neon (Ne). These are all noble gases, which are found in Group 18 of the periodic table.
2. insert step 2> Understand that boiling points are influenced by intermolecular forces. For noble gases, the primary intermolecular force is London dispersion forces, which are weak and arise due to temporary dipoles.
3. insert step 3> Recognize that the strength of London dispersion forces increases with the size and mass of the atoms. Larger atoms have more electrons, which can create stronger temporary dipoles.
4. insert step 4> Compare the atomic sizes and masses: Neon (Ne) is the smallest and lightest, followed by Argon (Ar), and then Krypton (Kr) is the largest and heaviest.
5. insert step 5> Conclude that as you move from Ne to Ar to Kr, the atomic size and mass increase, leading to stronger London dispersion forces and thus higher boiling points. Therefore, you would expect the boiling points to increase in the order Ne < Ar < Kr.

Key Concepts

Noble Gases

Noble gases, such as Krypton (Kr), Argon (Ar), and Neon (Ne), are elements in Group 18 of the periodic table. They are characterized by their full valence electron shells, which make them chemically inert and non-reactive. Understanding their properties is essential for predicting trends in boiling points, as these gases exhibit weak van der Waals forces due to their nonpolar nature.

Boiling Point Trends

The boiling point of a substance is the temperature at which its vapor pressure equals the external pressure, allowing it to transition from liquid to gas. For noble gases, boiling points generally increase with increasing atomic size and mass, as larger atoms have more electrons, leading to stronger London dispersion forces. This trend is crucial for analyzing the boiling points of Kr, Ar, and Ne.

Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion between molecules. In noble gases, the primary intermolecular force is the London dispersion force, which arises from temporary dipoles created by electron movement. The strength of these forces increases with the size and mass of the atoms, influencing the boiling points of the gases in the series, with larger atoms like Kr having higher boiling points than smaller ones like Ne.