The state of matter that changes significantly with pressure and temperature
gas
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•Gases have relatively ____ densities.
low
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Gases form a solution in any _______
proportions
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arises from the force exerted by atmospheric gases on the earth’s surface; decreases with altitude
atmospheric pressure
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devices used to measure the pressure of a gas in an experiment.
Manometer
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a gas that exhibits linear relationships among these variables (pressure, temp, moles, and volume)
ideal gas
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do ideal gases exist?
no
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At constant temperature, the volume occupied by a fixed amount of gas is ***inversely*** proportional to the external pressure.
Boyle’s law
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Boyle’s law
*V* 1/P
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At constant pressure, the volume occupied by a fixed amount of gas is ***directly*** proportional to its absolute (Kelvin) temperature
Charles law
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charles law
*V* *T*
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at fixed temperature and pressure, equal volumes of ***any*** ideal gas contain equal numbers of particles (or moles).
avagadros law
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STP
1 atm and 0 degrees Celsius,
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standard molar volume
22\.4 L
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is the volume of 1 mol of an ideal gas at STP.
standard molar volume
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The pressure exerted by each gas in a mixture
partial pressure
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the total pressure in a mixture is the sum of the partial pressures of the component gases.
Dalton’s Law of partial pressures
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At a given *T*, all gases in a sample have the same….
average kinetic energy
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Kinetic energy depends on both the
mass and the speed of a particle
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At the same *T*, a heavier gas particle moves more _____ than a lighter one.
slowly
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the process by which a gas escapes through a small hole in its container into an evacuated space.
effusion
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the rate of effusion of a gas is inversely proportional to the square root of its molar mass.
Graham’s law of effusion
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Real gases deviate most from ideal behavior at ***__*** *temperature* and __ *pressure*
low; high
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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
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Each physical state of matter is a ***____***, a physically distinct, homogeneous part of a system.
phase
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The properties of each phase are determined by the balance between the ***____***and ***___*** energy of the particles
potential, kinetic
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The ***____*** energy, in the form of ____ ***____***, tends to draw particles together
potential; attractive forces
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The ***potential*** energy, in the form of ***attractive forces***, tends to draw particles together
average speed
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found ***within*** a molecule
intramolecular forces (or bonding forces)
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found ***between*** __all__ molecules with partial charge, or between ions and molecules
intermolecular forces (or nonbonding forces)
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The ***physical*** behavior of each phase of matter is different because ….
the ***strength*** of these forces differ from state to state.
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gas has ____ attractions
no
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liquid has ____ attractions
stronger
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solid has ___________ attractions
predominant
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compressibility of a gas is…
high
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compressibility of a liquid is…
very low
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compressibility of a solid is….
almost none
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what is the relationship between temperature and kinetic energy of particles?
direct relationship
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what is the relationship between temp and attractive forces in a particle?
inverse relationship
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solid to liquid
melting/fusion
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liquid to gas
vaporizing
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gas to liquid
condensing
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liquid to solid
freezing
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solid to gas
sublimation
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gas to solid
deposition
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the heat released/gained as the substance changes from liquid to gas
heat of vaporization
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the heat released/gained as the substance changes from liquid to solid
heat of fusion
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*Within a phase*, heat flow is accompanied by a
change in temp
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***During a phase change***, heat flow occurs at…
constant temp
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Shows the change in temperature of a sample when heat is absorbed or released.
heating-cooling curve
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where molecules are leaving and entering the liquid at the *same rate in a closed flask*
dynamic equilibrium
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vapor pressure and temperature have a ____ relationship
direct
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This equation relates vapor pressure to temperature.
clausius-clapeyron equation
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•the temperature at which the vapor pressure equals the external pressure.
boiling point
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•is observed at standard atmospheric pressure or 760 torr.
normal boiling point
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As the external pressure on a liquid ***increases***, the boiling point….
increases
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the densities of the liquid and gas phases become equal
critical point
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all three phases are in equilibrium
triple point
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Intermolecular forces are relatively ***___*** compared to bonding forces
weak
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Like charges repel each other; unlike charges attract
coulomb’s law
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one-half the closest distance between the nuclei of two ***nonbonded*** atoms
van der Waals radius
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the distance between two ***nonbonded*** atoms in ***adjacent*** molecules
van der Waals distance
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The Van Der waals radius is ***always ___*** than the covalent radius
large
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the average distance between the nuclei of two bonded atoms
bond length
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one-half the distance between the nuclei of two covalently bonded atoms of the same element in a molecule
covalent radius
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periodic table trends for covalent and van der Waals radii
increase down and to the left
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the basis of attraction in a metallic bond is….
cations-delocalized electrons
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ion charge- dipole charge
ion-dipole
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polar bond to H- dipole charge
h bond
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dipole charges
dipole dipole
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ion charge- polarizable electron cloud
ion induced dipole
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dipole charge- polarizable electron cloud
dipole induced dipole
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polarizable electron cloud
dispersion (London)
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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
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the ease with which its electron cloud is distorted.
polarizability
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***Smaller*** particles are ***____ polarizable***
less
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trend for polarizability on periodic table
increase down a group and decreases left to right
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arises when an ***instantaneous dipole*** in one particle ***induces*** a dipole in another, resulting in an attraction between them
dispersion/London forces
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***stronger*** for ***more polarizable*** particles.
dispersion forces
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intramolecular forces are _________ than intermolecular forces
stronger
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the energy required to increase the surface area of a liquid
surface tension
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The ***stronger*** the forces between the particles the ***___*** the surface tension
higher
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surface tension decreases with ….
increasing temp
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the rising of a liquid through a narrow space against the pull of gravity
capillarity (capillary action)
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the resistance of a fluid to flow; Results from intermolecular attractions that impede the movement of molecules around and past each other
viscosity
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viscosity and intermolecular attractions have a ______ relationship
direct
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viscosity and temp have __ relationship
inverse
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water is the perfect solvent bc
•High specific heat capacity
•High heat of vaporization
•High surface tension
•High capillarity
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have well defined shapes due to the orderly arrangement of their particles
***Crystalline*** solids
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lack orderly arrangement and have poorly defined shapes.
***Amorphous*** solids
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composed of particles packed in an orderly three-dimensional array called the ***crystal lattice***
crystal
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smallest portion of a crystal lattice that yields the crystal if it is repeated in all directions
unit cell
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the number of nearest neighbors of a particle in a crystal.
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Flashcard (26)