CHEM FINAL

Significant Figures

Important for accurate measurements and calculations in scientific experiments, signifying the precision of a measurement.

Density

Defined as mass per unit volume, crucial for identifying substances and understanding their properties.

Chemical Changes

Alter the composition of substances and involve chemical reactions, such as combustion.

Physical Changes

Affect the form of a substance without changing its composition, like melting ice.

Mixtures

Consist of two or more substances combined physically, retaining their individual properties.

Dimensional Analysis

A technique used to convert units from one system to another, ensuring calculations maintain dimensional consistency.

Atomic Symbols

Represent elements uniquely; consist of one or two letters, essential for understanding chemical formulas.

Grams to Moles

Conversion essential for stoichiometry, enabling calculation of reactants and products in chemical reactions.

Periodic Table

Includes groups, periods, and individual elements characterized by atomic number and electron configuration.

Energy and Wavelength Relationship

Explains that energy of electromagnetic radiation is inversely proportional to wavelength.

Hydrogen Electronic Transitions

Involve absorption or emission of photons as electrons move between energy levels in hydrogen atoms.

Allowed Quantum Numbers

Describe electron orbitals through four quantum numbers that indicate energy levels, shape, orientation, and spin.

Periodic Trends

Signify how elements interact and form compounds including electronegativity and ionization energy.

Ground State Electron Configurations

Describe the arrangement of electrons in an atom at its lowest energy state.

Type 1 and Type 2 Metals

Naming conventions based on oxidation states; Type 1 have fixed charges, Type 2 have variable charges.

Polyatomic Ions

Composed of multiple atoms bonded covalently that carry a charge.

Lewis Structures

Diagrams representing the bonding between atoms in a molecule and the lone pairs of electrons.

Molecular Polarity

Determination of polarity based on electronegativity differences and molecular shape.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals.

Limiting Reagent

The reactant that is fully consumed in a reaction, determining the maximum yield of products.

Strong Acids

Include common strong acids like HCl and HNO₃; understanding their properties is essential.

Redox Reactions

Involve the transfer of electrons between species.

Molarity

A measure of concentration given by M = moles of solute/liters of solution.

Hess’ Law

States that total enthalpy change of a reaction is the sum of enthalpy changes of individual steps.

Gas Laws

Describe the relationships between pressure, volume, number of moles, and temperature.

urms

The root mean square speed of gas molecules, calculated using urms = sqrt(3RT/M).

Phase Changes

Understanding the transitions between solid, liquid, and gas phases.

Phase Diagram

Graphical representation depicting the state of a substance under varying temperature and pressure.