Matter and Its Classification

Matter and Classification

• Matter comprises particles that dictate its observable characteristics and reactivity.
• Strength, thermal conductivity, and electrical conductivity are key properties.
• Matter can be brittle, malleable, or ductile.
• Matter is magnetic or non-magnetic.
• Density is important and based on lead/aluminum.
• Melting and boiling points determine matter.
• Mixtures have properties.
• Heterogeneous mixtures have properties.
• Homogeneous mixtures have properties.
• Examples of heterogeneous and homogeneous mixtures exist.
• Microscopic and symbolic representations are key for elements, compounds, and mixtures.
• An element has a definition.
• A compound has a definition.
• Pure substances have definitions.
• Substances are classified as pure, compounds, or elements.
• Purity criteria can be devised, using melting and boiling points or chromatography.
• Compound names are derived from their constituent elements.
• Cation and anion tables are important.
• Naming compounds uses their formulas.
• Formulae are made from given names.
• Suffixes like -ide, -ite, and -ate have meanings.
• Prefixes di-, tri- etc., have meanings.

Metals, Metalloids, and Non-Metals

• Substances are classified as metals, metalloids, or non-metals based on properties.
• Metals and non-metals are located on the periodic table.
• Metalloids are generally non-metallic.
• Non-metals are classified by their properties.
• Metalloids increase conductivity with temperature.
• Metalloids feature increasing conductivity with increasing temperature which is the reverse of metals, examples include silicon and graphite.
• Metalloids are located on the periodic table.

Electrical/Thermal Conductors and Magnetic Materials

• Materials are electrical conductors, semiconductors, and insulators.
• Examples of each type of materials.
• Common appliances use properties of conductors, insulators, and semiconductors.
• Test and classify thermal conductors and insulators.
• Examples include thermal conductors and insulators.
• Materials are classified as magnetic and non-magnetic.
• There are examples of magnetic and non-magnetic materials.
• Magnets are used in speakers, telephones, electric motors, and compasses.

States of Matter

• Physical state classifies matter, linking to the kinetic-molecular theory and intermolecular forces.
• Matter exists as solids, liquids, gases, and solutions.
• Verify nature of matter with diffusion and Brownian motion.
• The three states of matter should be listed and characterized.
• Freezing, melting, and boiling points are key.
• Identify a substance's state at a given temperature.
• Define melting, evaporation, freezing, sublimation, and condensation.
• Demonstrate state changes.
• Describe matter states using kinetic molecular theory and particles.

Atomic Structure: The Atom

• Matter comprises atoms.
• Atomic theory is important.
• The periodic table organizes elements by atomic number, showing element periodicity.
• The world is made of element combinations from the periodic table.

Models, Mass, Structure, Isotopes, Configuration

• Match discoveries/hypotheses to following atom descriptions.
• This starts from Greek atom suggestions to radioactivity discovery, Rutherford's experiment, and Bohr model.
• Identify atomic model contributions.
• Models show atomic structure.
• Estimate atom mass and diameter.
• Atoms are mostly empty space; the nucleus occupies little space, which becomes indicated by alpha-particle scattering experiments.
• The concept of relative atomic mass should be described and used.
• Atomic number should be defined, and its value given.
• The number of protons are in an atom of an element.
• Neutral atoms have electrons.
• Removing electrons alters atom neutrality.
• Determine charge using electrons added/removed.
• Neutrons are calculated.
• Isotopes have calculated mass numbers.
• Define isotope.
• Calculate element atomic mass using isotope percentages.
• Represent atoms (nuclides) using notation X.
• Electronic arrangements for atoms should be given (up to Z=20) with diagrams and spectroscopic notation.
• Atomic orbitals and the shapes of the s- and p-orbitals are important.
• Hund's rule and Pauli's Exclusion Principle are important.

Periodic Table

• The periodic table shows elements by number and property periodicity.
• Understanding the periodic table is important in Chemistry.
• Knowledge of periodic property trends is needed.
• Understand PT element arrangement by atomic number.
• Understand PT as element organization.
• Define the element's group and period on the PT.
• The electronic structure links to element position on the PT.
• Periodicity for elements Li to Ar encompasses density, boiling/melting points, atomic radius, and formulae.
• This includes periodicity in halide and oxide formulae, and ionization energy.
• Periodicity influences electron-affinity and electronegativity.
• Define radius, ionization energy, electron affinity, and electronegativity.
• Group 1, 2, 17 and 18 feature electronic arrangements and chemical properties.
• The reactivity differences in groups 1, 2, and 17 must be described.
• Chemical properties of unfamiliar elements in the specified groups can be predicted.
• Metals are found on the periodic table.
• Nonmetals are found on the periodic table.
• Transition metals are found on the periodic table.