An ion is a charged particle that forms when an atom or molecule loses or gains electrons. This charge imbalance distinguishes ions from neutral atoms or molecules. Understanding ions is fundamental in chemistry.

A cation is an ion that carries a positive charge, formed when an atom loses one or more electrons. This concept is key to understanding ionic bonding and electrostatic interactions.

When an ionic compound dissolves in water, the compound separates into its constituent ions in a process called ionic dissociation. This process is crucial for the conduction of electricity in solutions.

An electrolyte is a substance that dissociates into ions when dissolved in water, enabling the solution to conduct electricity. This behavior is essential in many chemical and biological processes.

An aqueous solution of sodium chloride conducts electricity because it dissociates into sodium and chloride ions. In contrast, pure water and solutions of sugar or ethanol do not produce the free ions needed for conduction.

In forming NaCl, sodium loses one electron and becomes a cation while chlorine gains that electron to become an anion. This transfer of electrons is the basis of ionic bond formation.

Magnesium oxide is composed of magnesium cations (Mg²❺) and oxide anions (O²❻) in a 1:1 ratio, leading to the formula MgO. This balance of charges is essential for creating a neutral compound.

Net ionic equations exclude spectator ions, which do not participate in the actual chemical change. This simplification emphasizes only the species that undergo a transformation during the reaction.

Ion conduction depends on factors such as ion concentration, charge, and temperature, which all affect mobility. The color of the solution, however, does not influence the movement of ions and their conductivity.

The solubility product constant (Ksp) is used to predict whether a precipitate will form in a solution by quantifying an ionic compound's solubility. It helps determine if the ion product exceeds the compound's Ksp, triggering precipitation.

Potassium sulfate dissociates into two potassium ions and one sulfate ion in solution. Correctly identifying the charges on the ions is essential for writing accurate ionic equations.

Calcium chloride dissociates completely into Ca²❺ and Cl❻ ions in water, making it a strong electrolyte. In contrast, compounds like glucose and methane do not ionize in solution.

A precipitate forms when the product of a reaction is insoluble or only slightly soluble in water. This low solubility causes the product to separate out as a solid.

Water's high polarity allows it to interact strongly with ions, effectively separating and stabilizing them. This interaction is the reason water is known as the universal solvent.

Lattice energy is the energy required to overcome the strong electrostatic forces holding ions together in an ionic solid. It is a key factor in determining the stability and melting point of ionic compounds.

To balance the charges, two aluminum ions (2 × +3 = +6) combine with three oxide ions (3 × -2 = -6) to form a neutral compound. This results in the formula Al₂O₃.

Silver nitrate is a strong electrolyte that completely dissociates into Ag❺ and NO₃❻ ions in solution. No intact AgNO₃ molecules remain once it dissolves.

Ionic compounds possess a crystalline lattice where oppositely charged ions are strongly attracted to each other. Overcoming these strong electrostatic forces requires a lot of energy, which contributes to their high melting points.

Barium sulfate (BaSO₄) is known to be insoluble in water and precipitates when barium ions react with sulfate ions. This is in accordance with the solubility rules for ionic compounds.

The mobility of an ion in solution is primarily influenced by its size and charge density. Smaller ions with high charge density interact more strongly with the solvent, which can slow down their movement, whereas factors like molar mass or color are less significant.