Reviewer in Chem2 PDF

**Reviewer in Chem2.** - **Kinetic Molecular Theory** is the scientific theory that use to describe the states of matter. Solid, liquid and gas as they transform from one another. - **Kinetic Energy** represents energy in motion/moving. - **Intermolecular forces** attractive forces...

**Reviewer in Chem2.** - **Kinetic Molecular Theory** is the scientific theory that use to describe the states of matter. Solid, liquid and gas as they transform from one another. - **Kinetic Energy** represents energy in motion/moving. - **Intermolecular forces** attractive forces between the molecules.  - the [shapes and volume of solids are definite] particles are closely packed because of **strong attractive forces.** - Their **low kinetic energies** cause them to stay in fixed positions that results in definite shape and volume. - **Johannes Van Der Waal** a Dutch chemist that was named after the intermolecular forces. - **London Dispersion Forces** is the weakest force that exist between non polar molecules. - **Dipole Dipole Forces** attractive forces between polar molecules. - **Ion-dipole forces** exist when polar molecules are attractive to ions. - **Anion** slightly positive hydrogen is attached to chlorine anions. - **Cation** slightly negative oxygen is attached to sodium cations. - **Hydrogen Bond** is a special, strong type of dipole-dipole interaction between hydrogen and polar bond. - **N, O, F** are the only elements that can be bond with hydrogen. **Note:** review all the illustration from this lesson and not all items are included here, so please make sure to visit the PPT that was sent on your LMS and messenger. - **Why ant/insects can float on water?** It is because of the property of liquids brought about by the strength of the attractive forces between the molecules. - **Surface tension** It is the force that cause the molecules on the surface of a liquid to "tighten their hold to one another", creating the effect to a thin membrane on the surface. - **Molecules in the surface**- is being attracted to its neighbors (forming a stronger bonds). There is no force pulling it upward because there is no molecule above. - **Molecules in the interior**- is also attracted to its neighbors. It is more completely surrounded by other molecules. - **Cohesion**- intermolecular attraction between molecules of the **same substance.** - **Adhesion**- intermolecular attraction between molecules of **different substance**. - **Viscosity** Measure of its tendency to resist flowing motion. - **Capillary action** Spontaneous rising of liquid to a narrow tube - **Incompressibility** Water is incompressible because its molecules are very closed to each other that it's very hard to put pressure and bring them even closer. - **Diffusibility** Movement of particles from an area of high concentration to area of lower concentration. - **Evaporation** Indication of the escape of molecules from the surface of the liquid. - **Vapor Pressure** pressure exerted by a vapor over a liquid - **Boiling point** Temperature at which the vapor pressure of a liquid is equal to the external pressure. - **Water** Very remarkable substance with its simple composition and structure - Pure water is an **[odorless and tasteless]** liquid. It has a bluish tint. At standard atmospheric (760 mmHg pressure, its [**freezing point is 0 degree Celsius** and **boiling point is 100 degree Celsius (212 degrees Fahrenheit)**] - **Density** Water molecules started to solidifies. - **Solvent action** Water is known as the **[universal solvent]** because it dissolves more substances than any other common liquids **Note:** remember the examples that was given during discussion. Chapter 3 - If heat is added to a solid & the molecular motion increases sufficiently, the attractive forces are overcome so that the particles are no longer held in fixed positions. They become like liquid particles, **solid melts**. - The temperature at which the solid melts is called the **melting point.** - **Heat of fusion** is the amount of heat energy\ required to change the state of matter from\ solid to liquid. - **Vapor pressure of a solid** it is not common to think of a solid exerting vapor pressure. - The change from solid to gas without passing through the liquid state is called sublimation. - The word ***amorphous*** is a Greek word which means "no form". - **Crystalline,** It is a solid in which the constituent particles have an orderly arrangement, that is, it has regularly arranged structure units with characteristic geometric forms. - **Metallic solid** Are the simplest type of structure since single metallic atoms are the constituent units - **Ionic solid** Crystals in which particles are held together through ionic bond - **Molecular Crystals**, Crystals in which particles are held together through intermolecular forces - **Covalent Network Crystals**, consists of very large numbers of atoms linked by a network of covalent bonds. Chapter 4: - **Phase Change**, change from one state to another without a change in chemical composition. - **Endothermic**, [Takes in energy] from the environment - **Exothermic**, [gives out energy] to the environment. - MELTING POINT temperature at which the solid melts to form the liquid. - FREEZING POINT temperature at which the liquid freezes to form solid. - VAPORIZATION when liquid changes, it will change into gas. - CONDENSATION reverse process of vaporization.\ Process of substance in a gaseous state transforming into a liquid state. - SUBLIMATION transition from solid phase to gas phase without passing through the liquid phase. - DEPOSITION change from gas to solid phase without passing the liquid phase.