Atoms: The basic building blocks of matter, consisting of protons, neutrons, and electrons.
Elements: Pure substances made of only one kind of atom, listed in the periodic table.
Compounds: Substances formed when two or more elements chemically bond. Example: H₂O (water).
Chemical Equations: Representations of chemical reactions, showing reactants turning into products, e.g., A + B → C.
Mixtures: Combinations of two or more substances that retain their individual properties. Example: Air.
Chromatography: A technique for separating mixtures based on differences in the components’ movement through a medium.
Techniques used to separate components of mixtures, including:
Filtration: Separates solids from liquids.
Evaporation: Removes liquid to leave a solid.
Distillation: A process used to separate mixtures based on differences in boiling points. Used for purifying liquids.
Early models by Democritus and Dalton proposed atoms as indivisible.
Thomson discovered the electron, leading to the “plum pudding” model.
Arrangement of electrons in an atom’s shells, important for understanding chemical bonding and reactivity.
Mendeleev arranged elements by atomic mass; later atomic number became the organizing principle.
Organized by increasing atomic number, revealing periodic trends in properties.
Metals: Typically shiny, conductive, ductile, and malleable. Found on the left side of the periodic table.
Non-Metals: Dull, insulating, and brittle. Located on the right side of the periodic table.
Known as alkali metals (e.g., Li, Na, K), highly reactive and soft, with low melting points.
Known as halogens (e.g., F, Cl, Br), highly reactive non-metals with varying states at room temperature.
Known as noble gases (e.g., He, Ne, Ar), extremely unreactive with complete electron shells, used in neon lights and other applications.