General Chemistry II Reviewer PDF

🧪GENERAL CHEMISTRY 2nd Semester, 3rd Quarter | S.Y. ‘24—’25 | Ms. Angela Mendoza | Gabi and Chai values​ point ​...

🧪GENERAL CHEMISTRY 2nd Semester, 3rd Quarter | S.Y. ‘24—’25 | Ms. Angela Mendoza | Gabi and Chai values​ point ​ - centipoise 1 (cP) = 0.001 Pa-s V. PHYSICAL PROPERTIES OF LIQUIDS AND THE INTERMOLECULAR FORCES VI. AMORPHOUS AND CRYSTALLINE SOLIDS #3 Vapor Pressure​ ​ - equilibrium pressure of vapor above its #1 Surface Tension - measure of elastic force in the liquid or solid state​ surface of a liquid​ ​ - at equilibrium, evaporation rate = VI.A. CLASSES OF SOLIDS ​ *Surfactants - increases spreading and condensation rate​ penetrating properties by lowering surface tension ​ - molecules in vapor pressure collide with A.​ CRYSTALLINE SOLIDS the walls and lid of container, causing pressure​ - evaporation = condensation​ (1)​ Composed of a large number of small COHESIVE & ADHESIVE FORCES - *Equilibrium Vapor Pressure is exerted by gas​ crystals with a definite geometrical - high vapor pressure, high temperature shape. a.​ COHESIVE ​ (molecules have enough kinetic energy to (2)​ Rigid and incompressible - between molecules and liquid​ overcome IMF)​ (3)​ Long-range order of particles with a - less attraction - VP is inversely proportional to IMF, repeated arrangement. Dipole-dipole, Pressure (4)​ Considered as true solids b.​ ADHESIVE​ - the stronger the IMF are, the greater the (5)​ Has a definite heat of fusion. - between molecules and surface of another amount of energy. (6)​ Has a sharp melting point. substance​ (a)​ Transition immediately to liquid - greater attraction #4 Molar Heat of Vaporization ​ upon reaching it. ​ ​ - energy required to vaporize 1 mole of a ​ MENISCUS FORMATION - formed from liquid to given temperature​ cohesive and adhesive forces, ​ ​ - high intermolecular attraction, high VI.A.I PROPERTIES OF CRYSTALLINE SOLIDS ​ 1) Concave up​ energy, high heat of vaporization​ ​ 2) Convex down​ ​ *energy is required to free molecules from liquid phase​ 1.​ Unit cell: the basic repeating unit of crystalline ​ - measured at atm solids #2 Viscosity ​ 2.​ Atoms or molecules at lattice points are ​ - liquid resistance to flow​ identically arranged. ​ - inversely proportional to temperature​ #5 Boiling Point​ ​ - temperature when VP = External 3.​ In most metals, lattice points are occupied by ​ directly proportional to strong IMF​ atoms. ​ directly proportional to large and complex ​ Pressure​ ​ - normal BP: temp at which liquid converts 4.​ Crystalline solids often show a plane of ​ - SI unit is pascal-second (Pa-s) for smaller symmetry in their structure. to gas at 1 atm​ ​ - higher rate of evaporation, higher boiling 5.​ Stable crystal structure due to intermolecular b.​ LIQUID​ forces. (1)​ Lack well-defined shape and regular - occurs at moderate temperature and pressure​ 6.​ Well-defined order structure in three dimensions. atomic arrangement. - center of the graph 7.​ Geometric shape net attractive intermolecular (2)​ Fake solids. Pseudo-solids. Or c.​ VAPOUR/GAS​ forces. supercooled liquids. - occurs at high temperature and low pressure (3)​ Molden and blown into various shapes, behaving like crystals at a certain BOUNDARIES temperature. VI.A.II CRYSTALS (4)​ Glass is the most versatile example of ​ At boundaries is a line wherein in combination an amorphous solid. of pressure and temperature, the phases beside ​ IONIC CRYSTALS (5)​ Shatters irregularly. each other are at equilibrium ○​ Composed of charged ions. (6)​ No sharp melting points. ○​ Hard with high melting points due to (7)​ Wide range temperature. a.​ RED/FIRST LINE​ strong electrostatic force. (8)​ Might contain impurity. - divides solid and gas phase​ ○​ Poor electrical conductors in solid form, (9)​ Weak intermolecular forces. - sublimation and deposition but good conductor when melted. b.​ GREEN/SECOND LINE​ ○​ Brittle due to breakage of attractive - divides solid and liquid​ forces. - melting and freezing c.​ BLUE/LAST LINE​ ​ METALLIC CRYSTALS VII. PHASE DIAGRAM - divides liquid and solid​ ○​ Held by electrostatic forces. - evaporation and condensation ○​ Good conductors ○​ High melting points. Phase Diagram ○​ Lustrous (shiny) - represents the: POINTS 1)​ conditions in which a particular state is ​ MOLECULAR CRYSTALS stable 2)​ physical states of a substance under a.​ Triple Point​ ○​ Lattice points occupied by molecules. - both the temperature and pressure of the three ○​ Intermolecular forces: London different conditions of temperature and pressure phases coexist in equilibrium Dispersion forces and Hydrogen bond b.​ Critical Point​ forces. 3)​ Y-axis: pressure, X-axis: temperature - point wherein the phase of liquid and gaseous ○​ Weak intermolecular forces. phases merge together into a single phase​ REGIONS - beyond this point is known as supercritical ​ COVALENT CRYSTALS fluid which possesses properties of both and ○​ Strong intermolecular forces. a.​ SOLID​ where liquid and gas are indistinguishable ○​ Poor electrical conductors. - occurs when temperature is low and pressure ○​ Can be made into one type of atom. is high​ ○​ Very high melting points. - found on the left side of the graph​ - this is where phase changes start B.​ AMORPHOUS SOLIDS