GENCHEM

• Gases consist of particles moving randomly at high speeds.
• Increasing temperature leads to increased average kinetic energy of gas particles.
• Both temperature and mass of gas particles influence the average kinetic energy of gas particles.
• As volume increases, pressure decreases due to increased collisions.
• Increased temperature leads to increased collisions between gas particles and the container walls.
• Hydrogen bonds are most likely to be observed in ethanol.
• London dispersion forces occur between nonpolar molecules.
• Iodine (I2) molecules experience London dispersion forces.
• The strength of hydrogen bonding depends primarily on the electronegativity difference between atoms.
• Boiling point is likely different between substances exhibiting and not exhibiting hydrogen bonding.
• Polar functional groups increase solubility in water due to stronger interactions.
• Substances with strong hydrogen bonding have a higher boiling point.
• Liquids with significantly higher viscosity likely have stronger intermolecular forces, such as hydrogen bonding.
• Unsaturated bonds weaken intermolecular forces.
• Asymmetrical structures are more likely to exhibit dipole-dipole interactions.
• Boiling point defines the temperature at which a liquid changes into a gas.
• Surface tension causes the curvature observed in water droplets on a surface.
• Evaporation is the conversion of a liquid into its vapor phase at the surface.
• Vapor pressure is exerted by a vapor in equilibrium with its liquid phase.
• Water is likely to have higher surface tension.
• Liquids typically evaporate more rapidly at higher temperatures.
• The rate of evaporation depends on temperature and surface area.
• Liquids with lower boiling points at the same pressure have higher vapor pressures.
• Substances with higher surface tension likely have stronger intermolecular forces.
• Crystalline solids have a well-defined and ordered arrangement of particles.
• Amorphous solids lack a well-defined melting point.
• Amorphous solids have a random arrangement of particles.
• Crystalline solids exhibit definite geometric shapes.
• Crystalline solids are more likely to have a sharp and distinct melting point.
• Amorphous solids lack a characteristic geometric shape and tend to flow.
• Crystalline solids have long-range order.
• Amorphous solids have a random arrangement of particles.
• Amorphous solids lack a distinct melting point compared to crystalline solids.
• Amorphous solids are preferred for producing optical lenses due to their transparency and lack of long-range order.