Chemistry Chapter: Nature of Reactants

Ionic compound reactions are typically faster than covalent compound reactions because ionic compounds are composed of charged particles that react immediately when mixed, while covalent compounds require breaking bonds, which takes time.

Increasing the surface area of a solid reactant increases the reaction rate by increasing the number of collisions between reactants.

The rate of a reaction depends on the frequency of collisions between reactant particles.

Reaction between ions occurring immediately upon mixing.

Reaction between molecules requiring energy to break bonds.

The ratio of product concentrations to reactant concentrations at equilibrium. It indicates whether products or reactants are favored.

The equilibrium constant ($K_c$) is greater than 1. This indicates that at equilibrium, the concentration of products is higher than the concentration of reactants. Therefore, the reaction favors the formation of products.

The equilibrium constant ($K_c$) is less than 1. This indicates that at equilibrium, the concentration of reactants is higher than the concentration of products. Therefore, the reaction favors the formation of reactants.

Solid substances do not appear in the equilibrium constant expression because their concentrations remain constant during the reaction.

Changing the stoichiometric coefficients in a balanced chemical equation changes the equilibrium constant. For example, doubling the coefficients squares the $K_c$ value.

A reaction that can proceed in both forward and reverse directions. Both the formation of products and the reformation of reactants are possible.

A reaction that proceeds to completion (essentially, all reactants are consumed) because the forward rate is much faster than the reverse rate.

The process where a sparingly soluble salt dissolves to a small extent, producing ions in solution. This results in an equilibrium between the solid salt and its ions in solution.

For a reaction to occur, reactant molecules must collide with sufficient energy and correct orientation.

Increasing reactant concentration increases the rate of reaction by increasing the frequency of collisions.

The rate of a reaction is proportional to the product of reactant concentrations, each raised to its stoichiometric coefficient.

The equilibrium constant (Kc) is calculated as the product of product concentrations divided by the product of reactant concentrations, each raised to their stoichiometric coefficients.