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Kinetic Molecular Theory
A theory that explains the properties of matter in terms of the motions of its particles and the interactions between those particles.
Intermolecular Forces
The attractive forces between molecules that influence the physical properties of substances.
Solids
A state of matter characterized by closely packed particles with strong intermolecular forces that restrict their movement to vibrations.
Liquids
A state of matter where the particles are less tightly packed than in solids, allowing them to move past each other but still remain in close proximity.
Gases
A state of matter where particles are far apart due to weak intermolecular forces, allowing for significant movement and expansion.
Phase Changes
Transitions between different states of matter (solid, liquid, gas) which occur due to changes in temperature and pressure.
Melting
The process where a solid becomes a liquid as its temperature increases, causing its molecules to gain kinetic energy and overcome intermolecular forces.
Vaporization
The process where a liquid turns into a gas, occurring when the liquid's particles gain enough energy to overcome intermolecular attractions.
Average Kinetic Energy
The energy of motion of the molecules in a substance, which is reflected in the temperature of the substance.
Macroscopic Properties
Properties of matter that can be observed and measured directly, such as volume, shape, and state.
Ion-ion interaction
is also known as ionic bonds.
Ion-ion interaction
is the interaction between two oppositely charged particles.
Hydrogen bonding
An attractive force that exists when hydrogen is bonded to the most electronegative atoms, namely F, O, or N
Non polar covalent bonds
are molecules with zero dipole moment due to equally shared electrons between the atoms.
Polarizability
is the measure of how easy it is to distort the electron distribution of a molecule.
Ion-dipole interaction
results from the electrostatic attraction of a molecule containing a dipole and an ion.
Dipole-Dipole interaction
are attractive forces that are a moderately strong type of IMFA and are present in between polar molecules.
London dispersion forces
are the weakest type of IMFA and are present in between all electrically neutral molecules―polar and nonpolar molecules.
Surface Tension
is the tendency of a fluid to acquire the least possible surface area.
Cohesion
is the attraction between like molecules,
Adhesion
is the attraction between unlike molecules.
Viscosity
is the measure of a fluid’s resistance to flow.
Vapor pressure
is the pressure exerted by a vapor in equilibrium with its liquid phase in a closed system.
Solubility
refers to the ability of a substance to dissolve in a given amount of solvent at a specified temperature.
Hydrophilic
Substances or molecules that form interactions with water are also described as
Hydrophobic
Substances or molecules that repel water are described as
amphiphatic molecules
Molecules with both hydrophilic and hydrophobic regions are known as
Boiling
happens when the molecules of a liquid gain enough energy to overcome the intermolecular forces of attraction that hold the molecules together.
Miscible liquids
If two liquids dissolve or mix together, they are called
Immiscible
If two liquids do not dissolve or mix together, they are called
Enthalpy of vaporization
is the amount of energy that must be added to a liquid substance, to transform a quantity of that substance into a gas.
Phase Changes
Transitions between different states of matter (solid, liquid, gas) that occur due to changes in temperature and pressure.
Phase
A homogeneous state where a substance has a uniform composition governed by consistent intermolecular forces (IMFs).
Fundamental Phases of Matter
The three fundamental phases are solid, liquid, and gas.
Solid
A phase of matter where molecules are tightly packed with restricted movement.
Liquid
A phase of matter where molecules are loosely packed, allowing some movement.
Gas
A phase of matter where molecules are far apart and move freely.
Melting
The process of changing from solid to liquid, resulting in a decrease in molecular order.
Evaporation
The process of changing from liquid to gas, causing further decrease in molecular order.
Sublimation
The process of changing from solid to gas, resulting in the maximum decrease in molecular order.
Endothermic Processes
Processes that absorb heat, such as melting, vaporization, and sublimation.
Exothermic Processes
Processes that release heat, such as freezing, condensation, and deposition.
Solution
A homogeneous mixture composed of a solute (less abundant) and a solvent (more abundant).
Liquid Solutions
Solutions where the solvent is in the liquid phase, e.g., salt in water.
Solid Solutions
Solutions where the solvent is in the solid phase, e.g., brass.
Gaseous Solutions
Solutions where the solvent is in the gas phase, e.g., air.
Unsaturated Solution
A solution with less solute than the solvent’s capacity.
Saturated Solution
A solution with the maximum amount of solute dissolved at a specific temperature.
Supersaturated Solution
A solution containing more solute than is normally possible; unstable condition.
Concentrated Solution
A solution with a high amount of solute, e.g., concentrated sulfuric acid (18M).
Diluted Solution
A solution with a lower concentration of solute, often prepared by dilution.
Crystallization
The process of forming a structured solid from a solution.
Precipitation
The formation of an amorphous solid from a solution.
Like Dissolves Like Principle
Polar solutes dissolve in polar solvents; nonpolar solutes dissolve in nonpolar solvents.
