States of Matter and Changes

States of Matter

• Solids have closely packed particles held by strong attractive forces, allowing only vibrational movement.
• Liquids consist of loosely packed particles with weaker attractive forces than solids, allowing for more movement.
• Gases contain particles that are not fixed in position due to high kinetic energy, moving randomly in all directions.
• Plasma is an ionized gaseous state, where atoms lose electrons, forming positive ions and negative electrons; examples include ionized neon gas in signs and natural phenomena like auroras.

Gas vs. Vapor

• Gas refers to substances in a gaseous state at room temperature, such as helium, carbon dioxide, air, and ozone.
• Vapor is the gaseous form of substances that are typically solid or liquid at room temperature, encompassing substances like fog, gasoline fumes, and perfume chemicals.

Factors Influencing State Changes

• Matter changes states due to the addition or removal of energy.
• Temperature and pressure can cause phase transitions, like boiling water.

Properties of Matter

• Physical Properties: Observable characteristics not altering the substance's composition, including length, mass, density, and color.
• Chemical Properties: Characteristics displayed when a substance changes composition, such as flammability, acidity, and reactivity.

Intensive vs. Extensive Properties

• Intensive Properties: Do not depend on the sample amount, e.g., boiling point and color.
• Extensive Properties: Depend on the sample amount, e.g., volume and mass.

Changes in Matter

• Physical Change: Alters properties without changing the substance's identity; can be reversible or irreversible.
• Chemical Change: Transforms materials into new substances with different properties.

Classifications of Matter

• Mixtures: Physical combinations of two or more substances without chemical bonding.
• Homogeneous Mixtures: Uniform composition, indistinguishable components, e.g., solutions.
• Heterogeneous Mixtures: Non-uniform composition, distinguishable components, e.g., suspensions and colloids.

Solutions and Components

• Solute: The substance that is being dissolved.
• Solvent: The liquid that dissolves the solute.

Types of Mixtures

• Suspensions: Heterogeneous mixtures with large visible particles that settle over time, e.g., muddy water.
• Colloids: Heterogeneous mixtures with small, suspended particles that do not settle, e.g., milk.
• Coarse Mixtures: Heterogeneous mixtures with easily separable particles, e.g., salads.

Simple Separation Techniques

• Magnetic Separation: Uses a magnet to separate magnetic from non-magnetic substances.
• Filtration: Separates liquids from solids, with solids remaining on the filter and liquids passing through.
• Decantation: Separates immiscible liquids or solids from liquids in suspensions.
• Evaporation: Uses boiling to vaporize the solvent, leaving behind the solute.
• Distillation: Involves boiling a mixture to create vapor, which is then condensed back into liquid, yielding distillates and residues.
• Chromatography: Separates components in a liquid mixture through differential movement.