General chem maam joy uwu baka

 KINETIC MOLECULAR THEORY

explains the properties of solids and liquids in terms of intermolecular forces of attraction and the kinetic energy of the individual particles.

INTERMOLECULAR FORCES

pull the particles together while kinetic energy keeps the particles at a distance and moving around

Kinetic energy

is dependent on the temperature of the substance.

All matter is made up of tiny particles.

These particles are in constant motion.

The speed of particle is proportional  to temperature. Increased temperature means greater speed.

Solids, liquids, and gases differ in distances between particles, in the freedom of motion of particles, and in the extent to which the particles interact.

4 FACTS ABOUT PARTICLES

LIQUIDS

have definite volume but no definite shape

they take the shape of the container

very difficult to compress

slightly expand when heated

weakly attracted to each other; break their interaction easily

move more freely than those is solids; slide past one another

move faster when heated

SOLIDS

definite volume and shape

do not flow

virtually incompressible

expand when heated

strongly attracted to each other

vibrate in fixed positions

vibrate faster when heated

GAS

assumes volume and shape of container

easy to compress

Heat of Vaporization

the amount of heat required to vaporize one mole of substance at its boiling point.

Intermolecular forces

are attractive forces between molecules or particles in the solid or liquid states

relatively weaker than the forces within the molecules forming bonds (intramolecular)

Intramolecular forces

hold atoms together in a molecule

van der Waals forces.

The intermolecular forces of attraction in a pure substance are collectively known as?

Dipole-dipole

Hydrogen bonding

Ion-dipole

London dispersion

Dipole-induced dipole force

5 VAN DER WAALS FOCRES

Dipole-dipole

exists between polar molecules. One end of a dipole attracts the oppositely charged end of the other dipole

HYDROGEN BONDING

special and very strong type of dipole-dipole force that exists between hydrogen atom bound to small and highly electronegative non-metal atom

HYDROGEN BONDING

occurs in polar molecules containing H and any of highly electronegative elements, in particular Nitrogen, Fluorine, and oxygen.

Ion- Dipole Force

acts between an ion and a polar molecule

Ion- Dipole Force

explains the solubility of ionic compounds in water, which is polar molecule

Ion- Dipole Force

ions and the oppositely charged ends of the polar water molecules overcome the attraction between ions themselves. Each ion becomes separated and water molecules cluster around it

London Dispersion Forces

weakest type of intermolecular force

London Dispersion Forces

when two non-polar molecules approach each other, an instantaneous dipole moment forms

London Dispersion Forces

sometimes called an induced dipole-induced dipole attraction

Instantaneous Dipole Moment

when two non-polar molecules approach each other, what moment forms?

Dipole-Induced Dipole Forces

interaction between Polar and nonpolar molecules

Liquids

do not have a simple or regular structure, but many of their properties can be explained qualitatively by viewing them at the particulate level

Liquid

a state of matter with definite volume, low density, takes the shape of its container, whose particles are close together and incompressible.

Surface tension

Capillary Action

Viscosity

Vapor Pressure

Boiling Point

Heat of Vaporization

GENERAL PROPERTIES OF LQUIDS

Surface Tension

The measure of the elastic force in the surface of a liquid

Surface Tension

The amount of energy required to stretch or increase the surface of a liquid by a unit area

Surface Tension

Manifested as some sort of skin on the surface of a liquid or in a drop of liquid

Capillary Action

Tendency of a liquid to rise in narrow tubes or be drawn into small openings such as those between grains of a rock

Capillary Action

Also known as capillarity

COHESION attraction between like molecules. ADHESION attraction between unlike molecules

Two types of forces involved in Capillary Action

COHESION , ADHESION

__________ attraction between like molecules. __________ attraction between unlike molecules

convex, concave

When the cohesive forces between the liquid molecules are greater than the adhesive forces between the liquid and the walls of the container, the surface of the liquid is ______

When the cohesive forces between the liquid molecules are lesser than the adhesive forces between the liquid and the walls of the container, the surface of the liquid is _______

Viscosity (oil, honey)

Resistance of a liquid to flow

Viscosity

Referred to as the thickness or thinness of a liquid

higher

The stronger the intermolecular force, the ________ is the liquid’s viscosity

Vapor Pressure

Pressure exerted by its vapor when in equilibrium with liquid or soild

Boiling Point

The temperature at which its vapor pressure is equal to the external or atmospheric pressure

False, raises

TRUE OR FALSE

Increasing the temperature of a liquid LOWERS the kinetic energy of its molecules, until such point where the energy of the particle movement exceeds the intermolecular forces that hold them together.

True

TRUE OR FALSE

The greater intermolecular force, the higher the energy needed to increase the kinetic energy of the molecules to break these forces.

Heat of Vaporization

The application of heat disrupts the intermolecular forces of attraction of the liquid molecules and allows them to vaporize

Crystalline and Amorphous based on the arrangement of their particles.

Solid can be classified as?

AMORPHOUS SOLIDS

Have considerable disorder in their structure

AMORPHOUS SOLIDS

Formed rather rapidly that its constituent particles do not have time to align or organize into a more definite crystalline lattice.

CRYSTALLINE SOLIDS

Have a high regular arrangement of particles

CRYSTALLINE SOLIDS

Has a well-defined crystal lattice

Lattice

three-dimensional system of points designating the positions of the components (atoms, ions, or molecules) that make up a crystal

Unit Cell

Smallest repeating unit of a lattice

PHASE CHANGES

Are transitions between different states of matter: solid, liquid, and gas.

False, changes

Phase Changes happen when the temperature or/and pressure of a substance stay constant

Melting

Solid to liquid phase

Freezing

Liquid phase to solid phase

Evaporation

Liquid phase to the gas phase

Condensation

Gas phase to the liquid phase

Sublimation

Solid phase to the gas phase

Deposition

Gas phase to the solid phase

Phase Diagram

Shows the states of a substance (solid, liquid, gas) at different temperatures and pressures, indicating where phase changes occur.

Phase Diagram

It is a graphical representation of the physical states of a substance under different conditions of temperature and pressure.

SOLID, LIQUID, AND GAS AREAS

THREE AREAS IN PHASE DIAGRAM

Solid Area:

Lower temperatures, higher pressures.

Liquid Area:

Intermediate temperatures and pressures.

Gas Area:

Higher temperatures, lower pressures

Melting/Freezing Curve

The boundary between the solid and liquid phases.

Melting/Freezing Curve

Moving along this line shows where a substance will melt (solid to liquid) or freeze (liquid to solid) at different pressures.

Vaporization/ Condensation Curve

The boundary between the liquid and gas phases.

Vaporization/ Condensation Curve

This line shows where vaporization (liquid to gas) or condensation (gas to liquid) happens at various temperatures and pressures.

Sublimation/ Deposition Curve

The boundary between the solid and gas phases.

Sublimation/ Deposition Curve

Indicates where sublimation (solid to gas) or deposition (gas to solid) occurs directly, skipping the liquid phase.

Triple Point

The point on the phase diagram where all three phases (solid, liquid, gas) coexist in equilibrium.

Triple Point

It represents the unique temperature and pressure where this balance occurs.

Critical Point

The highest temperature and pressure at which a substance can exist as a liquid and gas in equilibrium.

supercritical fluid

Beyond the critical point, the substance becomes a?