CHM2-11_12-Q3-0101-PF-FD-1

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.

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.