S1.1.pdf (Part 1) PDF - Introduction to the Particulate Nature of Matter

S1.1.pdf (Part 1) Structure 1.1: Introduction to the Part iculate Nature of Matter 1.1.1: The Composition of Matter Elements: The fundamental building blocks of matter, unable to be broken down into simpler substances through chemical means. (Str ucture 1.1.1) Compounds: Formed by the chemical b...

S1.1.pdf (Part 1) Structure 1.1: Introduction to the Part iculate Nature of Matter 1.1.1: The Composition of Matter Elements: The fundamental building blocks of matter, unable to be broken down into simpler substances through chemical means. (Str ucture 1.1.1) Compounds: Formed by the chemical bonding of two or more differ ent elements in a fixed ratio. (Structure 1.1.1) Mixtures: Combinations of elements or compounds not chemically bonded, present in variable ratios, and separable by physical metho ds. (Structure 1.1.1) 1.1.2: The Kinetic Molecular Theory Model: Explains the physical properties of matter (solids, liquids, and gases) and changes of state. (Structure 1.1.2) States of Matter: Determined by the interactions between particles. (Structure 1.1.2) Solid: Fixed volume and shape, particles vibrate in fixed positions. (Structure 1.1.2) Liquid: Fixed volume but no fixed shape, particles vibrate, rotate, a nd move around. (Structure 1.1.2) Gas: No fixed volume or shape, particles move rapidly and are far apart. (Structure 1.1.2) Changes of State: Occur when substances absorb or release energ y. (Structure 1.1.2) Melting: Solid to liquid, endothermic process. (Structure 1.1.2) Freezing: Liquid to solid, exothermic process. (Structure 1.1.2) Vaporization: Liquid to gas, endothermic process. (Structure 1.1.2) Condensation: Gas to liquid, exothermic process. (Structure 1.1.2) Sublimation: Solid to gas, endothermic process. (Structure 1.1.2) Deposition: Gas to solid, exothermic process. (Structure 1.1.2) 1.1.3: Temperature and Kinetic Energy Temperature: A measure of the average kinetic energy ($Ę$) of part icles. (Structure 1.1.3) Kelvin Scale: The base unit of temperature measurement in the Inte rnational System of Units (SI). (Structure 1.1.3)  Heating Curve: Shows the relationship between temperature and en ergy input for a substance. (Structure 1.1.3) Plateaus: Indicate changes of state where energy is used to overc ome intermolecular forces rather than increase temperature. (Stru cture 1.1.3) Matter and Energy Matter: Anything that occupies space and has mass. (Structure 1.1) Energy: Anything that exists but does not have the properties of mat ter. (Structure 1.1) Conservation of Mass and Energy: In chemical reactions, mass and energy are conserved, meaning they are not created or destroyed, b ut transformed from one form to another. (Structure 1.1) Einstein's Equation: $E = mc^2$ demonstrates the interconversion o f mass and energy. (Structure 1.1) Approximation: In chemistry, the energy changes in chemical rea ctions are relatively small compared to the speed of light, making t he mass change negligible. (Structure 1.1) Non-Newtonian Fluids Viscosity: A measure of a fluid's resistance to flow. (Structure 1.1.2) Non-Newtonian Fluids: Substances whose viscosity changes depen ding on the force applied. (Structure 1.1.2) Example: Maize starch slime, which hardens when tapped but flow s smoothly when stirred slowly. (Structure 1.1.2) Summary Table State of Intermolecul Volume Shape Particle Movement Matter ar Forces Vibrate in fixed posit Solid Fixed Fixed Strong ions No fixed Vibrate, rotate, and Weaker than Liquid Fixed shape move around solids No fixed volum No fixed Move rapidly and ar Gas Negligible e or shape shape e far apart Notes continue on Page 2, Select the next page from the sidebar