States and Properties of Matter

States of Matter

• Solid:

  • Definite shape and volume.
  • Particles are closely packed in a fixed arrangement.

• Liquid:

  • Definite volume but no definite shape.
  • Particles are close but can move past one another, allowing flow.

• Gas:

  • No definite shape or volume; expands to fill its container.
  • Particles are far apart and move freely.

• Plasma:

  • Ionized gas with free electrons and ions; conducts electricity.
  • Found in stars, including the sun.

Properties of Matter

• Physical Properties:

  • Characteristics that can be observed or measured without changing the substance (e.g., color, density, melting point).

• Chemical Properties:

  • Characteristics that describe how a substance reacts with others (e.g., flammability, reactivity).

• Intensive Properties:

  • Independent of the amount of substance (e.g., density, boiling point).

• Extensive Properties:

  • Dependent on the amount of substance present (e.g., mass, volume).

Change of State

• Melting:

  • Transition from solid to liquid; occurs at the melting point.

• Freezing:

  • Transition from liquid to solid; occurs at the freezing point.

• Vaporization:

  • Transition from liquid to gas; can occur via evaporation or boiling.

• Condensation:

  • Transition from gas to liquid; occurs when gas cools.

• Sublimation:

  • Transition from solid to gas without becoming liquid (e.g., dry ice).

• Deposition:

  • Transition from gas to solid without becoming liquid (e.g., frost formation).

Atomic Structure

• Atoms: The basic unit of matter; consists of protons, neutrons, and electrons.

• Nucleus:

  • Central part of an atom containing protons (positively charged) and neutrons (neutral).

• Electrons:

  • Negatively charged particles that orbit the nucleus in electron shells.

• Isotopes:

  • Atoms of the same element with different numbers of neutrons; affects atomic mass.

• Ions:

  • Charged atoms formed by the loss (cations) or gain (anions) of electrons.

Matter Conservation

• Law of Conservation of Mass:

  • Mass is neither created nor destroyed in a chemical reaction; the total mass of reactants equals the total mass of products.

• Energy Conservation:

  • Energy in a closed system is conserved; it can change forms (e.g., potential to kinetic) but cannot be created or destroyed.

• Implications:

  • Understanding conservation helps predict outcomes in chemical reactions and physical changes.

States of Matter

• Solid: Defined by a definite shape and volume, with closely packed particles in a fixed arrangement.
• Liquid: Has a definite volume, but takes the shape of its container; particles are close yet able to move past one another, enabling flow.
• Gas: Lacks definite shape and volume, expanding to fill available space; particles are far apart and in constant, free motion.
• Plasma: An ionized state of matter consisting of free electrons and ions; highly conductive and primarily found in stars, including the sun.

Properties of Matter

• Physical Properties: Observable or measurable characteristics that do not alter the substance (e.g., color, density, melting point).
• Chemical Properties: Characteristics indicating how a substance interacts with other substances (e.g., flammability, reactivity).
• Intensive Properties: Independent of the amount of matter, such as density and boiling point.
• Extensive Properties: Dependent on the quantity of matter, including mass and volume.

Change of State

• Melting: The process where a solid transitions to a liquid at a specific temperature known as the melting point.
• Freezing: The conversion of a liquid to a solid, occurring at the freezing point.
• Vaporization: The change from liquid to gas through either evaporation or boiling.
• Condensation: The transition from gas to liquid, typically due to cooling.
• Sublimation: Direct transition from solid to gas without passing through the liquid state, exemplified by dry ice.
• Deposition: The process where gas converts directly to solid, as seen in frost formation.

Atomic Structure

• Atoms: Fundamental units of matter, comprising protons, neutrons, and electrons.
• Nucleus: The atom's core, containing protons (positively charged) and neutrons (neutral).
• Electrons: Negatively charged particles orbiting the nucleus, arranged in electron shells.
• Isotopes: Variants of the same element possessing different neutron counts, affecting atomic mass.
• Ions: Charged species that result from electron loss (cations) or gain (anions).

Matter Conservation

• Law of Conservation of Mass: Asserts that mass remains constant during chemical reactions; the mass of products equals that of reactants.
• Energy Conservation: States that energy within a closed system remains constant, transforming between forms but not created or destroyed.
• Implications: Knowledge of conservation principles is crucial for predicting the results of chemical reactions and physical changes.