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- https://chem.libretexts.org/Courses/Nassau_Community_College/Principles_of_Chemistry/10%3A_Solids_and_Liquids/10.02%3A_Intermolecular_ForcesAll substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F at...All substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F atoms experience hydrogen bonding. The preferred phase of a substance depends on the strength of the intermolecular force and the energy of the particles.
- https://chem.libretexts.org/Courses/Lubbock_Christian_University/LCU%3A_CHE_1305_-_Introductory_Chemistry/11%3A_Energy/11.6%3A_Phase_ChangesFusion, vaporization, and sublimation are endothermic processes, whereas freezing, condensation, and deposition are exothermic processes. Changes of state are examples of phase changes, or phase trans...Fusion, vaporization, and sublimation are endothermic processes, whereas freezing, condensation, and deposition are exothermic processes. Changes of state are examples of phase changes, or phase transitions. All phase changes are accompanied by changes in the energy of a system. Changes from a more-ordered state to a less-ordered state (such as a liquid to a gas) are endothermic. Changes from a less-ordered state to a more-ordered state (such as a liquid to a solid) are always exothermic.
- https://chem.libretexts.org/Courses/University_of_Missouri/MU%3A__1330H_(Keller)/11%3A_Liquids_and_Intermolecular_Forces/11.4%3A_Phase_ChangesFusion, vaporization, and sublimation are endothermic processes, whereas freezing, condensation, and deposition are exothermic processes. Changes of state are examples of phase changes, or phase trans...Fusion, vaporization, and sublimation are endothermic processes, whereas freezing, condensation, and deposition are exothermic processes. Changes of state are examples of phase changes, or phase transitions. All phase changes are accompanied by changes in the energy of a system. Changes from a more-ordered state to a less-ordered state (such as a liquid to a gas) are endothermic. Changes from a less-ordered state to a more-ordered state (such as a liquid to a solid) are always exothermic.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Beginning_Chemistry_(Ball)/10%3A_Solids_and_Liquids/10.02%3A_Intermolecular_ForcesAll substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F at...All substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F atoms experience hydrogen bonding. The preferred phase of a substance depends on the strength of the intermolecular force and the energy of the particles.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_I/08%3A_State_Changes_and_Thermodynamics/8.03%3A_Phase_TransitionsPhase transitions are processes that convert matter from one physical state into another. There are six phase transitions between the three phases of matter. Melting, vaporization, and sublimation are...Phase transitions are processes that convert matter from one physical state into another. There are six phase transitions between the three phases of matter. Melting, vaporization, and sublimation are all endothermic processes, requiring an input of heat to overcome intermolecular attractions. The reciprocal transitions of freezing, condensation, and deposition are all exothermic processes, involving heat as intermolecular attractive forces are established or strengthened.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Beginning_Chemistry_(Ball)/10%3A_Solids_and_Liquids/10.03%3A_Phase_Transitions_-_Melting_Boiling_and_SublimingPhase changes can occur between any two phases of matter. All phase changes occur with a simultaneous change in energy. All phase changes are isothermal.
- https://chem.libretexts.org/Courses/Colorado_State_University_Pueblo/Elementary_Concepts_in_Physics_and_Chemistry/04%3A_Chapter_4_-_Molecules_Bonding_and_Forces/4.07%3A_Intermolecular_ForcesAll substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F at...All substances experience dispersion forces between their particles. Substances that are polar experience dipole-dipole interactions. Substances with covalent bonds between an H atom and N, O, or F atoms experience hydrogen bonding. The preferred phase of a substance depends on the strength of the intermolecular force and the energy of the particles.
- https://chem.libretexts.org/Courses/Louisville_Collegiate_School/General_Chemistry/LibreTexts_Louisville_Collegiate_School_Chapters_10%3A_Liquids_and_Solids/LibreTexts%2F%2FLouisville_Collegiate_School%2F%2FChapters%2F%2F10%3A_Liquids_and_Solids%2F%2F10.3%3A_Phase_TransitionsPhase transitions are processes that convert matter from one physical state into another. There are six phase transitions between the three phases of matter. Melting, vaporization, and sublimation are...Phase transitions are processes that convert matter from one physical state into another. There are six phase transitions between the three phases of matter. Melting, vaporization, and sublimation are all endothermic processes, requiring an input of heat to overcome intermolecular attractions. The reciprocal transitions of freezing, condensation, and deposition are all exothermic processes, involving heat as intermolecular attractive forces are established or strengthened.
- https://chem.libretexts.org/Courses/Fullerton_College/Beginning_Chemistry_(Chan)/10%3A_Solids_and_Liquids/10.03%3A_Phase_Transitions_-_Melting_Boiling_and_SublimingPhase changes can occur between any two phases of matter. All phase changes occur with a simultaneous change in energy. All phase changes are isothermal.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(Fleming)/08%3A_Phase_Equilibrium/8.05%3A_The_Clausius-Clapeyron_EquationThe page discusses the derivation and application of the Clausius-Clapeyron equation for phase equilibria involving gas phases, focusing on vaporization. It explains the equation's construction, assum...The page discusses the derivation and application of the Clausius-Clapeyron equation for phase equilibria involving gas phases, focusing on vaporization. It explains the equation's construction, assumptions (e.g., treating vapor as an ideal gas), and integration. An example problem uses known temperature and vapor pressure conditions to find the enthalpy of vaporization (ΔHvap).
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Thermodynamics/Energies_and_Potentials/Enthalpy/Heat_of_SublimationThe molar heat (or enthalpy) of sublimation is the amount of energy that must be added to a mole of solid at constant pressure to turn it directly into a gas (without passing through the liquid phase)...The molar heat (or enthalpy) of sublimation is the amount of energy that must be added to a mole of solid at constant pressure to turn it directly into a gas (without passing through the liquid phase). Sublimation requires all the forces are broken between the molecules (or other species, such as ions) in the solid as the solid is converted into a gas
