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

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54 Terms

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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.

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Intermolecular Forces

The attractive forces between molecules that influence the physical properties of substances.

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Solids

A state of matter characterized by closely packed particles with strong intermolecular forces that restrict their movement to vibrations.

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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.

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Gases

A state of matter where particles are far apart due to weak intermolecular forces, allowing for significant movement and expansion.

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Phase Changes

Transitions between different states of matter (solid, liquid, gas) which occur due to changes in temperature and pressure.

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Melting

The process where a solid becomes a liquid as its temperature increases, causing its molecules to gain kinetic energy and overcome intermolecular forces.

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Vaporization

The process where a liquid turns into a gas, occurring when the liquid's particles gain enough energy to overcome intermolecular attractions.

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Average Kinetic Energy

The energy of motion of the molecules in a substance, which is reflected in the temperature of the substance.

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Macroscopic Properties

Properties of matter that can be observed and measured directly, such as volume, shape, and state.

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Ion-ion interaction

is also known as ionic bonds.

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Ion-ion interaction

is the interaction between two oppositely charged particles.

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Hydrogen bonding

An attractive force that exists when hydrogen is bonded to the most electronegative atoms, namely F, O, or N

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Non polar covalent bonds

are molecules with zero dipole moment due to equally shared electrons between the atoms.

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Polarizability

is the measure of how easy it is to distort the electron distribution of a molecule.

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Ion-dipole interaction

results from the electrostatic attraction of a molecule containing a dipole and an ion.

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Dipole-Dipole interaction

are attractive forces that are a moderately strong type of IMFA and are present in between polar molecules.

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London dispersion forces

are the weakest type of IMFA and are present in between all electrically neutral molecules―polar and nonpolar molecules.

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Surface Tension

is the tendency of a fluid to acquire the least possible surface area.

 

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Cohesion

is the attraction between like molecules,

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Adhesion

is the attraction between unlike molecules.

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Viscosity

is the measure of a fluid’s resistance to flow.

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Vapor pressure

is the pressure exerted by a vapor in equilibrium with its liquid phase in a closed system.

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Solubility

refers to the ability of a substance to dissolve in a given amount of solvent at a specified temperature.

 

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Hydrophilic

Substances or molecules that form interactions with water are also described as

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Hydrophobic

Substances or molecules that repel water are described as

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amphiphatic molecules

Molecules with both hydrophilic and hydrophobic regions are known as

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Boiling

happens when the molecules of a liquid gain enough energy to overcome the intermolecular forces of attraction that hold the molecules together.

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Miscible liquids

If two liquids dissolve or mix together, they are called

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Immiscible

If two liquids do not dissolve or mix together, they are called

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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.

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Phase Changes

Transitions between different states of matter (solid, liquid, gas) that occur due to changes in temperature and pressure.

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Phase

A homogeneous state where a substance has a uniform composition governed by consistent intermolecular forces (IMFs).

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Fundamental Phases of Matter

The three fundamental phases are solid, liquid, and gas.

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Solid

A phase of matter where molecules are tightly packed with restricted movement.

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Liquid

A phase of matter where molecules are loosely packed, allowing some movement.

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Gas

A phase of matter where molecules are far apart and move freely.

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Melting

The process of changing from solid to liquid, resulting in a decrease in molecular order.

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Evaporation

The process of changing from liquid to gas, causing further decrease in molecular order.

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Sublimation

The process of changing from solid to gas, resulting in the maximum decrease in molecular order.

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Endothermic Processes

Processes that absorb heat, such as melting, vaporization, and sublimation.

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Exothermic Processes

Processes that release heat, such as freezing, condensation, and deposition.

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Solution

A homogeneous mixture composed of a solute (less abundant) and a solvent (more abundant).

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Liquid Solutions

Solutions where the solvent is in the liquid phase, e.g., salt in water.

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Solid Solutions

Solutions where the solvent is in the solid phase, e.g., brass.

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Gaseous Solutions

Solutions where the solvent is in the gas phase, e.g., air.

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Unsaturated Solution

A solution with less solute than the solvent’s capacity.

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Saturated Solution

A solution with the maximum amount of solute dissolved at a specific temperature.

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Supersaturated Solution

A solution containing more solute than is normally possible; unstable condition.

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Concentrated Solution

A solution with a high amount of solute, e.g., concentrated sulfuric acid (18M).

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Diluted Solution

A solution with a lower concentration of solute, often prepared by dilution.

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Crystallization

The process of forming a structured solid from a solution.

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Precipitation

The formation of an amorphous solid from a solution.

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Like Dissolves Like Principle

Polar solutes dissolve in polar solvents; nonpolar solutes dissolve in nonpolar solvents.