Chem 1050 White Test 1

chapters 5 and 12

The state of matter that changes significantly with pressure and temperature

gas

•Gases have relatively ____ densities.

low

Gases form a solution in any _______

proportions

arises from the force exerted by atmospheric gases on the earth’s surface; decreases with altitude

atmospheric pressure

devices used to measure the pressure of a gas in an experiment.

Manometer

a gas that exhibits linear relationships among these variables (pressure, temp, moles, and volume)

ideal gas

do ideal gases exist?

no

At constant temperature, the volume occupied by a fixed amount of gas is ***inversely*** proportional to the external pressure.

Boyle’s law

Boyle’s law

*V* 1/P

At constant pressure, the volume occupied by a fixed amount of gas is ***directly*** proportional to its absolute (Kelvin) temperature

Charles law

charles law

*V* *T*

at fixed temperature and pressure, equal volumes of ***any*** ideal gas contain equal numbers of particles (or moles).

avagadros law

STP

1 atm and 0 degrees Celsius,

standard molar volume

22\.4 L

is the volume of 1 mol of an ideal gas at STP.

standard molar volume

The pressure exerted by each gas in a mixture

partial pressure

the total pressure in a mixture is the sum of the partial pressures of the component gases.

Dalton’s Law of partial pressures

At a given *T*, all gases in a sample have the same….

average kinetic energy

Kinetic energy depends on both the

mass and the speed of a particle

At the same *T*, a heavier gas particle moves more _____ than a lighter one.

slowly

the process by which a gas escapes through a small hole in its container into an evacuated space.

effusion

the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

Graham’s law of effusion

Real gases deviate most from ideal behavior at ***__*** *temperature* and __ *pressure*

low; high

adjusts the ideal gas law to take into account for the real volume of the gas particles and the effect of interparticle attractions

van der Waals equation

Each physical state of matter is a ***____***, a physically distinct, homogeneous part of a system.

phase

The properties of each phase are determined by the balance between the ***____***and ***___*** energy of the particles

potential, kinetic

The ***____*** energy, in the form of ____ ***____***, tends to draw particles together

potential; attractive forces

The ***potential*** energy, in the form of ***attractive forces***, tends to draw particles together

average speed

found ***within*** a molecule

intramolecular forces (or bonding forces)

found ***between***  __all__ molecules with partial charge, or between ions and molecules

intermolecular forces (or nonbonding forces)

The ***physical*** behavior of each phase of matter is different because ….

the ***strength*** of these forces differ from state to state.

gas has ____ attractions

no

liquid has ____ attractions

stronger

solid has ___________ attractions

predominant

compressibility of a gas is…

high

compressibility of a liquid is…

very low

compressibility of a solid is….

almost none

what is the relationship between temperature and kinetic energy of particles?

direct relationship

what is the relationship between temp and attractive forces in a particle?

inverse relationship

solid to liquid

melting/fusion

liquid to gas

vaporizing

gas to liquid

condensing

liquid to solid

freezing

solid to gas

sublimation

gas to solid

deposition

the heat released/gained as the substance changes from liquid to gas

heat of vaporization

the heat released/gained as the substance changes from liquid to solid

heat of fusion

*Within a phase*, heat flow is accompanied by a

change in temp

***During a phase change***, heat flow occurs at…

constant temp

Shows the change in temperature of a sample when heat is absorbed or released.

heating-cooling curve

where molecules are leaving and entering the liquid at the *same rate in a closed flask*

dynamic equilibrium

vapor pressure and temperature have a ____ relationship

direct

This equation relates vapor pressure to temperature.

clausius-clapeyron equation

•the temperature at which the vapor pressure equals the external pressure.

boiling point

•is observed at standard atmospheric pressure or 760 torr.

normal boiling point

As the external pressure on a liquid ***increases***, the boiling point….

increases

the densities of the liquid and gas phases become equal

critical point

all three phases are in equilibrium

triple point

Intermolecular forces are relatively ***___*** compared to bonding forces

weak

Like charges repel each other; unlike charges attract

coulomb’s law

one-half the closest distance between the nuclei of two ***nonbonded*** atoms

van der Waals radius

the distance between two ***nonbonded*** atoms in ***adjacent*** molecules

van der Waals distance

The Van Der waals radius is ***always ___*** than the covalent radius

large

the average distance between the nuclei of two bonded atoms

bond length

one-half the distance between the nuclei of two covalently bonded atoms of the same element in a molecule

covalent radius

periodic table trends for covalent and van der Waals radii

increase down and to the left

the basis of attraction in a metallic bond is….

cations-delocalized electrons

ion charge- dipole charge

ion-dipole

polar bond to H- dipole charge

h bond

dipole charges

dipole dipole

ion charge- polarizable electron cloud

ion induced dipole

dipole charge- polarizable electron cloud

dipole induced dipole

polarizable electron cloud

dispersion (London)

is possible for molecules that have a ***hydrogen atom*** covalently bonded to a small, highly electronegative atom with ***lone electron pairs***, specifically ***N, O, or F***.

hydrogen bonding

the ease with which its electron cloud is distorted.

polarizability

***Smaller*** particles are ***____ polarizable***

less

trend for polarizability on periodic table

increase down a group and decreases left to right

arises when an ***instantaneous dipole*** in one particle ***induces*** a dipole in another, resulting in an attraction between them

dispersion/London forces

***stronger*** for ***more polarizable*** particles.

dispersion forces

intramolecular forces are _________ than intermolecular forces

stronger

the energy required to increase the surface area of a liquid

surface tension

The ***stronger*** the forces between the particles the ***___*** the surface tension

higher

surface tension decreases with ….

increasing temp

the rising of a liquid through a narrow space against the pull of gravity

capillarity (capillary action)

the resistance of a fluid to flow; Results from intermolecular attractions that impede the movement of molecules around and past each other

viscosity

viscosity and intermolecular attractions have a ______ relationship

direct

viscosity and temp have __ relationship

inverse

water is the perfect solvent bc

•High specific heat capacity

•High heat of vaporization

•High surface tension

•High capillarity

have well defined shapes due to the orderly arrangement of their particles

***Crystalline*** solids

lack orderly arrangement and have poorly defined shapes.

***Amorphous*** solids

composed of particles packed in an orderly three-dimensional array called the ***crystal lattice***

crystal

smallest portion of a crystal lattice that yields the crystal if it is repeated in all directions

unit cell

the number of nearest neighbors of a particle in a crystal.

coordination number