Matter: Properties, Kinetic Theory & Classification

• Lessons provide foundational knowlege of matter, it's properties, and classification based on composition and energy interactions
• The documents cover nomenclature of ionic compounds and methods of separating mixtures

Lesson 1: Properties of Matter

• Matter occupies space and has mass
• Properties of matter include Physical and Chemical

Physical Properties

• Physical properties are observable without changing the substance

Chemical Properties

• Chemical properties are observed when a substance transforms (reactivity or combustibility)

Extensive Properties

• Extensive properties depend on the amount of matter (mass, volume)

Intensive Properties

• Intensive properties depend on the type of matter (color, solubility, temperature)
• Heat transfer affects molecular kinetic energy, increasing motion, and temperature

Lesson 2: Kinetic Theory of Matter

• All matter consists of particles in constant motion within kinetic molecular theory
• Energy and spacing determine the state of matter

States of Matter

• Solid particles vibrate, have high potential energy, and low kinetic energy
• Liquid particles move in straight-line motion and have medium kinetic energy
• Gas particles have rotational, vibrational, and translational motion with the highest kinetic energy

Phase Changes

• Heat energy changes kinetic energy and particle spacing
• Temperature remains constant during phase changes like melting and boiling

Physical Changes

• Physical changes include heat of fusion and heat of vaporization

Chemical Changes

• Chemical changes include heat of combustion and heat of formation

Lesson 3: Classification of Matter

• Matter has mass and volume

Pure Substances

• Elements are made of one type of atom (oxygen, carbon)
• Compounds are made of different atoms chemically bonded (water)

Mixtures

• Mixtures are physical combinations of substances

Homogenous Mixtures

• Homogenous mixtures have uniform composition (saltwater)

Heterogenous Mixtures

• Heterogenous mixtures have non-uniform composition (salad, colloids, suspensions)

Types of Compounds

• Organic compounds are carbon-based
• Inorganic compounds lack carbon-hydrogen bonds
• Ionic compounds contain charged ions
• Molecular compounds are formed by covalent bonds

Ionic Compounds

• Students should express ionic compounds in words or formulas (Lesson 5a, Page 1)
• Binary ionic compounds consist of one cation and one anion
• The metal is named first, and the non-metal's suffix changes to "ide" (chlorine to chloride)
• Chemical formulas have the metal symbol first, followed by the non-metal
• Subscripts balance the charges to achieve a net charge of zero

Multivalent Ionic Compounds

• Multivalent ionic compounds form more than one stable ion and follow similar naming rules
• Polyatomic ions retain their suffix
• Hydrates are compounds with chemically bound water molecules

Separating Mixtures

• Students should select appropriate methods for separating mixture components (Lesson 4, Page 1)
• Methods are mechanical or non-mechanical
• Mechanical includes decantation, filtration, centrifugation
• Non-mechanical includes chromatography, distillation

Mechanical Methods

• Mechanical methods include density separation techniques (decantation and centrifugation) for solid particles that pass through filters

Chromatography

• Chromatography separates based on solubility
• Types of chromatography: paper and thin-layer

Distillation

• Distillation purifies liquids based on boiling point differences
• Includes simple and fractional distillation

Froth Flotation

• Froth flotation separates hydrophobic components from hydrophilic, used in mining

Exercises and Assignments

• Activities for practical understanding and group assignments regarding methods of separation are included in both lessons

Vocabulary

• Ionic compound," "filtration," "chromatography," and others are key vocabulary

Polytomic and Multivalent Ions

• Students will differentiate between univalent, polyatomic, and multivalent ions
• Polyatomic ions consist of multiple atoms and can be represented as Lewis Structures
• Naming conventions include suffixes like "ate" and "ite," and prefixes "hypo" and "hyper"
• Nomenclature rules for cations and anions are covered with emphasis on understanding structure
• Common examples of polyatomic ions: ammonium (NH4+), nitrate (NO3-), nitrite (NO2-), carbonate (CO32-), sulfate (SO42-), sulfite (SO32-), and phosphate (PO43-)
• Some transition metals form ions with more than one charge (Fe2+ and Fe3+)
• Denoted in naming (iron (III) chloride)
• Oxyanions consist of a central element bonded to several oxygen atoms

Nomenclature of Compounds

• Students will represent molecular compounds in words or formulas

Nomenclature of Ionic Compounds

• Includes rules for naming ionic compounds
• Includes the replacement of suffixes for certain non-metals (fluorine to fluoride)
• Includes the use of prefixes to indicate the number of atoms

Nomenclature of Covalent Compounds

• Presents rules for naming covalent compounds
• The order of naming is based on the chemical formula and the use of Greek prefixes

Writing Formulas

• Lesson provides formula writing examples
• Discusses the IUPAC system for naming complex covalent compounds, such as glucose (C6H12O6)

Activites

• Activities help practice compound naming

• Examples: chemicals bingo and chemistry jeopardy

• Lessons provide understanding of ion composition and nomenclature

• Provides the rules governing naming of both ionic and covalent compounds

Explore matter's fundamental properties, including physical, chemical, extensive, and intensive characteristics. Understand the kinetic theory, detailing particle motion and energy interactions. Learn about classifying matter based on composition and energy dynamics.