The solubility rules were used to determine which reactant was aqueous and which one was a solid. The solid is the precipitate formed in the reaction. The formation of the precipitate indicates that a chemical reaction occurred. If no precipitate formed the reaction would be labeled with DNR, which stands for does not react. The solubility rules states which elements are soluble or insoluble, including the exceptions for each rule. For example at station one, barium chloride reacted with silver nitrate yielding to barium nitrate and silver chloride. Barium nitrate is aqueous because all nitrates are soluble. Silver chloride is the precipitate because all chlorides expect silver and a few others are soluble, since silver is an exception silver chloride is insoluble. To determine which reactant out of the chemical reactions the solubility rules provided the guideline necessary to figure out which reactant is the precipitate. The reactions in this equation were all of the same type of chemical reaction. They were double replacement reactions which is the two products are interchanged to formed two new compounds on the reactant side. Intermolecular forces have heavy influence over solubility. Intermolecular forces are between molecules and are weak forces of attraction. There are four intermolecular forces including hydrogen bonding, dipole-dipole forces, dipole-induced dipole forces, and london dispersion forces. Hydrogen bonding is the strongest and occurs when one hydrogen molecule is attracted to another molecule. Next is dipole- dipole forces which occurs between polar molecules. After that is dipole- induced dipole, it is weaker than dipole-dipole because its occurs between a polar and a nonpolar molecule. The weakest intermolecular force is london dispersion forces because it is only temporary
The solubility rules were used to determine which reactant was aqueous and which one was a solid. The solid is the precipitate formed in the reaction. The formation of the precipitate indicates that a chemical reaction occurred. If no precipitate formed the reaction would be labeled with DNR, which stands for does not react. The solubility rules states which elements are soluble or insoluble, including the exceptions for each rule. For example at station one, barium chloride reacted with silver nitrate yielding to barium nitrate and silver chloride. Barium nitrate is aqueous because all nitrates are soluble. Silver chloride is the precipitate because all chlorides expect silver and a few others are soluble, since silver is an exception silver chloride is insoluble. To determine which reactant out of the chemical reactions the solubility rules provided the guideline necessary to figure out which reactant is the precipitate. The reactions in this equation were all of the same type of chemical reaction. They were double replacement reactions which is the two products are interchanged to formed two new compounds on the reactant side. Intermolecular forces have heavy influence over solubility. Intermolecular forces are between molecules and are weak forces of attraction. There are four intermolecular forces including hydrogen bonding, dipole-dipole forces, dipole-induced dipole forces, and london dispersion forces. Hydrogen bonding is the strongest and occurs when one hydrogen molecule is attracted to another molecule. Next is dipole- dipole forces which occurs between polar molecules. After that is dipole- induced dipole, it is weaker than dipole-dipole because its occurs between a polar and a nonpolar molecule. The weakest intermolecular force is london dispersion forces because it is only temporary