Ch 11-12 Quiz

Units for pressure

atm, torr, mmHg, kPa, psi

Atmospheric energy

Pressure of the atmosphere

Average kinetic energy

Total kinetic energy of all the molecules of a sample, divided by number of molecules, only depends on temperature

Avogadro’s Law

Equal volumes of gas at same temperature and pressure contain an equal number of gas particles

Boyle’s Law

P1V1=P2V2

Charles’ Law

V1/T1 = V2/T2

Combined gas law definition

For a given sample of gas, volume directly proportional to absolute temperature and inversely proportional to pressure

Combined gas law equation

(P1V1)/T1 = (P2V2)/T2

Dalton’s Law partial pressures

Total pressure of a gas mixture equal to sum of the partial pressures of its components

Diffusion

Spreading out of gas particles by random motion and collisions to occupy an entire volume

Effusion

The movement of gas particles through a tiny opening without collisions

Force

Push or pull

Gas

State of matter, sample of matter that has its volume and shape determined by the volume and shape of its container

Gay-Lussac’s Law of combining volumes

At equal temperatures and pressures, volumes of separate gases involved in a chemical reaction are directly proportional to their coefficients in balanced chemical equation

Graham’s Law of Effusion

R1/R2 = Sqrt(M2/M1)

Ideal gas

Hypothetical gas whose behavior is predicted by the gas laws and explained by kinetic molecular theory

Ideal gas constant formats

0.08206 L*atm/mol*K, 8.3145 J/K*mol

Ideal gas law

PV=nRT, R= 0.08206

Kinetic molecular theory

Explains gas laws in terms of motions and characteristics of the molecules of gas

Mole fraction

Number of moles in component in mixture divided by total number moles in mixture

Partial pressure

Pressure of one gas in mixture of gases

Root mean square speed

Measure of the average speed of a gas particle

Vrms=

sqrt (3RT)/M

Standard temperature and pressure (STP)

0*C, 100 kPa

Torr

Equal to 1 mmHg, 1/760 atom

Pounds/sq in (psi)

14.7 equal to 1 atm

Pascals

Newton/m², 101,325 equal to 1 atm

Kilopascals (kPa)

101.325 equal to 1 atm

Van der Waals equation

Modification of ideal gas law to account for finite volumes of particles and intermolecular forces between particles

KE avg per mole

3/2 RT

KE avg per particle

(3/2RT)/NA

5 postulates kinetic molecular theory

Gas particles in constant random motion, volume individual particles negligible, particles assumed to not attract or repel each other, molecular collisions perfectly elastic, average kinetic energy of the collection of particles proportional to temperature gas

Adhesion

Attraction to different particles

Amorphous solid

Solid whose structure consists of irregular arrangements of the constituent particles

Capillary action

Ability to flow against gravity up narrow tube

Clausius-Clapeyron equation

Relationship among vapor pressure, temperature, and Enthalpy of vaporization

Cohesion

Attraction to like particles

Condensation

Transition from gas to liquid phase

Coordination number

The number of nearest neighbors for each atom in crystalline structure

Covalent network solid

Solid whose constituent particles are atoms that interact via covalent bonds (macromolecular solid)

Critical point

Pressure and temperature above which substance no longer exists as either liquid or gas

Critical pressure

Pressure above which substance no longer exists as either liquid or gas

Critical temperature

The temperature above which substance no longer exists as either liquid or gas

Crystalline solid

Solid whose structure consists of regular repeating arrangements of constituent particles

Deposition

Transition from gas to solid

Dipole dipole attraction

Temporary attraction between polar molecules

Dispersion forces

Temporary weak attraction between instantaneous dipole and induced dipole (aka London forces)

Distillation

Process of vaporizing liquid and collecting its vapors

Ductile

Able to be drawn into thin wire

Electron-sea model

Mole in which valence electrons of atoms in metallic solid form sea of mobile electrons surrounding metal cations

Enthalpy of fusion

Energy required for melting of 1 mole of solid

Enthalpy of sublimation

Energy required for sublimation of 1 mole of solid

Enthalpy of vaporization

Energy required for vaporization of 1 mole of a liquid

Equilibrium

Dynamic situation in which two opposing processes occur at the same rate, resulting in no net change

Freezing

Transition from liquid to solid phase

Fusion

Transition from solid to liquid phase

Heating curve

Graph showing how temperature and phase changes as energy added to pure substance

Hydrogen bond

Strong dipole-dipole attraction formed between partially positive hydrogen atoms and highly electronegative atom with lone pair electrons

Atoms for hydrogen bonds

Fluorine, oxygen, nitrogen

Hydrogen bond acceptor

Molecule containing highly electronegative atom with lone pair of electrons

Hydrogen bond donor

Molecule containing H-N, H-O, or H-F bond

Induced dipole

Temporary uneven distribution of electrons caused by proximity of spontaneous dipole

Instantaneous dipole

Temporarily uneven distribution of electrons caused by spontaneous shift in electron density

Intermolecular force

Attractive force that forms between particles in liquid and solid phases

Ion dipole attraction

Temporary attraction between ions and polar molecule

Ionic solid

Solid whose constituent particles are ions that interact via ionic bonds

Malleable

Able to bend or change shape without breaking when force is applied

Metallic solid

Solid whose constituent particles are metal atoms that are loosely held by valence electrons

Molecular solid

Solid whose constituent particles are molecules that interact via intermolecular forces

Nonvolatile

Does not easily vaporize

Normal boiling point

Heat that liquid boils at 1 atm

Packing

How layers of atoms arranged in crystalline solid

Phase diagram

Graph showing phase of substance under all possible pressure and temperature combos

Sublimation

Direct transition from solid phase to gas phase

Supercritical fluid

Fourth phase of matter, all three phases in equilibrium

Surface tension

Surface film of liquid caused by attraction of particles to minimize surface area

Triple point

Pressure and temperature at which all three phases of substance are in equilibrium

Unit cell

Simplest repeating unit of crystal structure

Van der waals forces

General term for intermolecular force, synonym for dispersion forces

Vapor

Gas in contact with its liquid phase

Vaporization

Transition from liquid to gas phase

Viscosity

Resistance to flow of liquid

Volatile

Substance that can easily vaporize

KJ to change state

q=n(H)

J to change state

q=m(H)

Clausius-Clapeyron equation

ln P(vaporization) = (-H(vaporization)/R)(1/T)+lnB