Boiling Points of CS2, KCl, and H2O Compounds

Which compounds have increasing boiling points?

Based on the data, which compounds are listed in order of increasing boiling points: CS2, KCl, or H2O?

The compounds listed in order of increasing boiling points are CS2 < KCl < H2O.

Carbon disulfide (CS2) has the lowest boiling point as it is a nonpolar molecule with weak intermolecular forces. KCl (potassium chloride) has a higher boiling point due to strong ionic bonds between potassium and chloride ions. Water (H2O) has the highest boiling point because of its polar nature, which allows for extensive hydrogen bonding between water molecules. Hydrogen bonding is a strong intermolecular force, resulting in a higher boiling point compared to CS2 and KCl. Therefore, the order of increasing boiling points is CS2 < KCl < H2O.

In this data, we are comparing the boiling points of carbon disulfide (CS2), potassium chloride (KCl), and water (H2O). Boiling point is a physical property that indicates the temperature at which a substance changes from a liquid to a gas. The boiling point of a compound is influenced by its molecular structure and the strength of intermolecular forces present.

CS2 has the lowest boiling point among the three compounds listed. This is because CS2 is a nonpolar molecule composed of carbon and sulfur atoms bonded by a covalent bond. The intermolecular forces in CS2 are weak Van der Waals forces, resulting in a low boiling point.

KCl, on the other hand, is an ionic compound consisting of potassium ions (K+) and chloride ions (Cl-). Ionic compounds like KCl have strong electrostatic attractions between the positively and negatively charged ions, leading to higher boiling points compared to covalent compounds like CS2.

H2O, or water, has the highest boiling point among the three compounds. This is due to the presence of hydrogen bonding in water molecules. Hydrogen bonding is a strong intermolecular force that occurs between the partially positive hydrogen atoms of one molecule and the partially negative oxygen atoms of another molecule. The presence of hydrogen bonding in water results in a higher boiling point compared to CS2 and KCl.

Understanding the factors that influence boiling points can provide insights into the physical properties and behavior of different compounds. It is important to consider molecular structure, intermolecular forces, and chemical interactions when comparing the boiling points of substances.