Physical and Chemical Properties of Matter

• Properties describe an object or substance's appearance, texture, and interactions.
• Physical and chemical properties are the two types of properties.

Physical Properties

• There are two types: intensive and extensive.
• Intensive properties do not depend on the amount of matter in a sample, examples are the senses.
• Extensive properties depend on the amount of matter in a sample, examples of this are measurement.

Intensive Properties

• Include color, odor, luster, malleability, ductility, conductivity, hardness, brittleness, durability, texture, boiling point, melting point, and density.
• Color refers to the pigment of a substance.
• Odor is detected by the sense of smell.
• Luster is the ability to reflect light.
• Malleability is the ability to be hammered into sheets.
• Ductility is the ability to be stretched into thin wires.
• Conductivity describes conducting electricity or heat.
• Hardness is the resistance to scratching.
• Brittleness is the ability to break or shatter easily.
• Durability is the ability to resist corrosion.
• Texture describes how a substance feels when touched.
• Density refers to mass per unit of volume.

Chemical Properties

• Include flammability, combustibility, and light sensitivity.
• Flammable liquids burn at normal working temperatures.
• Combustible liquids need heat to ignite.
• Light sensitivity is the ability of a substance to change in the presence of visible light.

Extensive Properties

• Include mass, weight, and length.
• Mass measures the amount of matter in an object.
• Weight measures the force of gravity on an object.
• Length measures the extent of something along its greater dimension.

Phases of Matter

• Matter has volume and mass.
• Volume is the space taken up by an object.
• Mass is the amount of matter in an object.
• Matter is made up of atoms.
• Kinetic energy pertains to the energy of motion.
• Temperature relates to kinetic energy, resulting in movement.

Solid Phase

• Solids have a definite volume and shape at a given temperature.
• Molecules are closely packed.
• Solids have high density.
• Arrangement is compact and well-organized.
• Molecular force is strong.
• Solids exhibit vibrational motion.

Liquid Phase

• Liquids have a definite volume, but their shape depends on the container.
• Arrangement is disorganized.
• There are few gaps/spaces between molecules.
• Molecular force is weak.
• Movement is loose.

Gas Phase

• Gases have no definite volume.
• Shape conforms to the container.
• Molecular force is weak.
• Molecules are spread apart.
• Movement is free.

Plasma Phase

• Plasma is an electrically charged gas.

Change in Matter

• Physical change alters the form of matter but not its chemical identity.
• Phase describes the existing physical state of matter.
• Temperature increase excites particles, increasing their movement.
• Changes occur when a substance contains sufficient energy due to temperature or pressure.

Phase Changes

• Solid to liquid is melting.
• Liquid to gas is evaporation.
• Gas to liquid is condensation.
• Liquid to solid is freezing.
• Gas to solid is deposition.
• Solid to gas is sublimation.

Chemical Change

• A substance changes into a new one with different composition, altering the chemical properties.
• Submicroscopic models help visualize properties.
• Monatomic molecules have one atom and lack covalent bonds.
• Diatomic molecules consist of two atoms of the same or different elements.

Types of Matter

• Matter is categorized into pure substances and mixtures.

Pure substances

• Have a definite and constant composition, such as salt or sugar.
• A compound is composed of two or more elements in a specific ratio.

Mixtures

• Mixtures are physical combinations of pure substances with no definite composition.
• Homogeneous mixtures (solutions) are uniform, like water.
• Heterogeneous mixtures are non-uniform with visually distinguishable components.

Atoms

• Atoms are the building blocks of matter.
• Consist of a nucleus, neutrons, protons, and electrons.

Subatomic Particles

• Neutrons have no charge and were discovered by James Chadwick in 1932.
• Protons have a positive charge and were discovered by Ernest Rutherford in 1911.
• Electrons have a negative charge and were discovered by J.J. Thompson in 1897.
• Positive and negative charges attract, while like charges repel.

Atomic Models

• Democritus (15th century B.C.) proposed indivisible particles called "atomos".
• John Dalton (1808) proposed the solid sphere model for the atom.
• Thomson (1903) proposed the plum pudding model.
• Rutherford (1911) proposed the nuclear model.
• Bohr (1913) proposed the planetary model.
• Schrödinger (1926) proposed the quantum model.

Periodic Table History

• Johann Dobereiner (1829) created "The Law of Triads".
• John Newlands (1866) created "The Law of Octaves".
• Dmitri Mendeleev (1869) is known as the father of the periodic table and arranged elements by increasing atomic mass.
• Henry Moseley (1913) discovered that atoms have a unique number of protons, arranging the table by increasing atomic number.
• Glenn Seaborg (1940) discovered plutonium and other transuranic elements.

Modern Periodic Table

• Elements are arranged by increasing atomic number.
• Each element has a unique symbol.
• Horizontal rows are called periods.
• Vertical columns are called groups/families.

Categories of Elements

• Metals
• Nonmetals
• Metalloids

Properties of Metals

• Good conductors of heat and electricity.
• Shiny.
• Ductile.
• Malleable.
• Metals chemically react with water, resulting in corrosion.

Properties of Non-metals

• Poor conductors of heat and electricity.
• Not ductile or malleable.
• Solid nonmetals are brittle and break easily.
• Dull.
• Many are gases.

Periodic Table Blocks

• S and P blocks are representative elements.
• D and F blocks are transition elements.

Families of Elements

• Hydrogen (all alone).
• Alkali Metals (Group 1): Industrial chemicals.
• Alkaline Earth Metals (Group 2): High melting point.
• Transition Metals (Groups 3-12): Good conductors.
• Boron Family (Group 13): Metalloids and metals.
• Carbon Group (Group 14): Basis of life.
• Nitrogen Group (Group 15): Fertilizer.
• Oxygen Group (Group 16): Photosynthesis.
• Halogens (Group 17): Varying appearance.
• Noble Gases (Group 18): Found in the atmosphere.