Chemistry Class Nomenclature and Bonding

Naming compounds: A systematic way of assigning names to chemical compounds, based on their chemical composition, helps to identify and understand their properties
IUPAC (International Union of Pure and Applied Chemistry): The organization responsible for setting the standards for chemical nomenclature
Organic and inorganic compounds: Have different naming conventions due to the vast diversity of organic structures
Prefixes and suffixes: Help indicate the number of atoms, type of functional groups, and the presence of multiple bonds

Chemical bonds: The forces that hold atoms together in molecules and compounds
Electrostatic forces: The fundamental basis for chemical bonding, attractive and repulsive forces between electrically charged particles
Electronegativity: The relative ability of an atom in a molecule to attract electrons in a covalent bond

Ionic bonding: Electrostatic attraction between oppositely charged ions, typically formed between metals and nonmetals
Covalent bonding: Sharing of electrons between atoms, typically formed between nonmetals
Metallic bonding: A unique type of bonding found in metals, involving a "sea" of delocalized electrons shared by all atoms

Polar covalent bonds: Unequal sharing of electrons in a covalent bond, creating a partial positive and partial negative charge
Non-polar covalent bonds: Equal sharing of electrons, resulting in no net charge separation
Polar molecule: Molecules with a net dipole moment, arising from the arrangement of multiple polar bonds or lone pairs of electrons
Non-polar molecule: Molecules with no net dipole moment, either due to the absence of polar bonds or a symmetrical arrangement of polar bonds

Weak forces: Attractive forces between molecules, weaker than chemical bonds, but play a crucial role in many chemical and physical properties
Van der Waals forces: Dipole-dipole interactions, London dispersion forces, and induced dipole forces
Hydrogen bonding: A special type of dipole-dipole interaction involving a hydrogen atom bonded to a highly electronegative atom like oxygen or nitrogen

Ionic compounds: High melting and boiling points, good conductors of electricity in molten or dissolved states, generally soluble in polar solvents
Polar covalent compounds: Intermediate melting and boiling points, vary in conductivity depending on the specific compound, generally soluble in other polar solvents
Non-polar covalent compounds: Low melting and boiling points, poor conductors of electricity, generally soluble in other non-polar solvents

Chemical equations: Symbolic representation of chemical reactions, showing the reactants, products, and stoichiometry
Reactants: Substances that are consumed during the reaction
Products: Substances that are formed during the reaction
Coefficients: Whole numbers used to balance the number of atoms on each side of the equation

Conservation of mass: A fundamental principle in chemistry, stating that mass is neither created nor destroyed in chemical reactions
Balancing coefficients: Ensuring that the number of atoms of each element is equal on both sides of the equation
Trial and error method: Commonly used to balance equations, adjusting coefficients until the number of atoms of each element is balanced

Synthesis reaction: Two or more reactants combine to form a single product
Decomposition reaction: A single reactant breaks down into two or more products
Single displacement reaction: An element reacts with a compound, replacing one of the elements in the compound
Double displacement reaction: Two reactants exchange ions to form two new products
Combustion reaction: A substance reacts rapidly with oxygen, producing heat and light
Neutralization reaction: An acid reacts with a base to form salt and water

Understanding reaction types: helps anticipate the products of chemical reactions
Solubility rules: Help predict the formation of precipitates in double displacement reactions
Activity series: Predicts the outcome of single displacement reactions