Term
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Definition
| Solid and liquid states are known as the __ states |
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Definition
| Solid and liquid states are __ similar to each other than they are to the gas state |
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Definition
| In the __ state, constituent particles – atoms or molecules – are separated by large distances and do not interact with each other very much |
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Definition
| In the _ states, constituent particles are close together and exert moderate to strong attractive forces on one another |
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Definition
| __ – attractive forces that exist between all molecules and atoms |
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Definition
| Intermolecular forces are responsible for the very existence of __ states |
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Definition
| The state sample of matter – solid, liquid, or gas – depends on __ of intermolecular forces between constituent particles, relative to the amount of thermal energy in the sample |
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Definition
| The molecules and atoms composing matter are in constant random motion that increases with increasing temperature. The energy associated with this motion is called __ |
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Definition
| When thermal energy is high relative to intermolecular forces, matter tends to be __ |
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Definition
| When thermal energy is low relative to intermolecular forces, matter tends to be _ |
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Term
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Definition
| Densities of the solid and liquid states are much __ than the densities of the gas state |
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Term
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Definition
| Solid and liquid states are _ similar in density and molar volume to one another than they are to the gas state |
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Definition
| For water, the solid is slightly __dense than the liquid. This is atypical behavior |
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Definition
| Most solids are slightly __ than their corresponding liquids because the molecules move closer together upon freezing |
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Term
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Definition
| Major difference between liquids and solids is the freedom of __ of the constituent molecules or atoms |
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Term
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Definition
| Even though the atoms or molecules in a liquid are in close contact, __ energy partially overcomes the attractions between them, allowing them to move around one another |
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Definition
| The atoms or molecules in a __ are virtually locked in their positions, only vibrating back and forth about a fixed point |
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Definition
| Liquids assume the shape of their containers because the atoms or molecules that compose liquids are __ to flow (or move around one another) |
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Definition
| __ are not easily compressed because the molecules or atoms that compose them are already in close contact – they cannot be pushed much closer together |
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Definition
| The molecules in a __ have a great deal of space between them and are easily compressed |
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Definition
| __ have a definite shape because the molecules or atoms that compose solids are fixed in place – each molecule or atom merely vibrates about a fixed point |
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Definition
| Solids have a definite volume and generally __ be compressed because the molecules or atoms composing them are already in close contact |
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Definition
| Solids may be __, in which case the atoms or molecules that compose them are arranged in a well-ordered 3-D array |
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Definition
| Solids may be __, in which case the atoms or molecules that compose them have no long-range order |
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Term
| temperature, pressure, or both |
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Definition
| We can transform one state of matter to another by changing the __ |
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Term
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Definition
| Increases in pressure favor the __ state, so increasing the pressure of a gas sample results in a transition to the liquid state |
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Term
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Definition
| When something changes states its chemical composition __ change |
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Term
| state – solid, liquid, or gas – |
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Definition
| The strength of the intermolecular forces between the molecules or atoms that compose a substance determine its __ at a given temperature |
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Term
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Definition
| At room temperature, moderate to strong intermolecular forces tend to result in __ (high melting and boiling points) and weak intermolecular forces tend to result in __ (low melting and boiling points) |
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Term
| charges, partial charges, and temporary charges |
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Definition
| Intermolecular forces originate from the interactions between __ on molecules (or atoms and ions), much as bonding forces originate from interactions between charged particles in atoms |
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Term
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Definition
| According to __, the potential energy (E) of two oppositely charged particles (with charges q¬¬1 and q2) decreases (becomes more negative) with increasing magnitude of charge and with decreasing separation (r) |
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Term
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Definition
| Protons and electrons are attracted to each other because their potential energy __ as they get closer together |
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Definition
| Molecules with partial or temporary charges are attracted to each other because their __ decreases as they get closer together |
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Definition
| Intermolecular forces, even the strongest ones, are generally much weaker than __ forces |
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Term
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Definition
| Bonding forces are the result of __ (the charges on protons and electrons) interacting at very close distances |
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Term
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Definition
| Intermolecular forces are the result of __ interacting at greater distances |
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Term
| dispersion forces, dipole-dipole forces, hydrogen bonding, and ion-dipole forces |
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Definition
| what are the different types of intermolecular forces |
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Term
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Definition
| __ forces can potentially occur in all substances |
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Definition
| __ forces occurs only in mixtures |
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Term
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Definition
| The one intermolecular force present in all molecules and atoms is the dispersion force (also called the __) |
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Term
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Definition
| Dispersion forces are the result of fluctuations in the __ within molecules or atoms |
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Term
| instantaneous dipole or a temporary dipole |
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Definition
| The electrons in an atom or molecule may, at any one instant, be unevenly distributed. Having the electrons be unevenly distributed around the nucleus will give the different sides of an atom or molecule slightly negative or positive charges. This fleeting change separation is called an __ |
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Term
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Definition
| An instantaneous dipole on one atom induces an instantaneous dipole on its __ atoms because the positive end of the instantaneous dipole attracts electrons in the neighboring atoms |
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Definition
| The neighboring atoms then attract one another – the positive end of one instantaneous dipole attracting the negative end of another. This attraction is the __ |
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Term
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Definition
| The magnitude of the dispersion force depends on how easily the electrons in the atom or molecule can more or __ in response to an instantaneous dipole, which in turn depends on the size (or volume) of the electron cloud |
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Term
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Definition
| A larger electron cloud results in a __ because the electrons are held less tightly by the nucleus and therefore polarize more easily |
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Term
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Definition
| The dispersion force __ with increasing molar mass because molecules or atoms of higher molar mass generally have more electrons dispersed over a greater volume |
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Definition
| As the molar masses and electron cloud volume increases, the greater the dispersion force which results in __ boiling points |
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Term
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Definition
| molar mass alone does not determine the magnitude of the dispersion force. __ can also determine magnitude of the dispersion force |
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Term
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Definition
| The dipole-dipole force exists in all molecules that are __ |
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Term
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Definition
| Polar molecules have permanent dipoles that interact with the permanent dipoles of neighboring molecules. The positive end of one permanent dipole attracts the negative end of another; this attraction is the __ force |
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Term
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Definition
| Polar molecules, therefore have __ melting and boiling points than nonpolar molecules of similar molar mass |
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Term
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Definition
| All molecules (including polar ones) have dispersion forces, but polar molecules have, in addition, dipole-dipole forces. Polar molecules have a raised melting and boiling points relative to __ molecules because of the additional attractive force (dipole-dipole forces) |
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Term
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Definition
| Boiling points __ with increasing dipole moment |
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Definition
| The polarity of molecules composing liquids is also important in determining the __ of liquids |
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Term
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Definition
| _ – the ability to mix without separating into two states |
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Definition
| Polar liquids __ miscible with other polar liquids but __ miscible with nonpolar liquids |
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Definition
| Polar molecules containing hydrogen atoms bonded directly to small electronegative atoms – most importantly fluorine, oxygen, or nitrogen – exhibit an intermolecular force called __ |
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Term
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Definition
| The large electronegativity difference between hydrogen and any of these electronegative elements causes the hydrogen atom to have a fairly large partial positive charge (g+) within the bond, while the __ atom has a fairly large partial negative charge (g-) |
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Term
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Definition
| Since these atoms are quite small, the H atom on one molecule can approach the F, O, or N atom on an adjacent molecule very closely. This results in a strong attraction between the H atom on one molecule and the F, O, or N on its neighbor, an attraction called __ |
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Term
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Definition
| Chemical bonds occur between individual atoms __ a molecule, whereas hydrogen bonds are intermolecular forces that occur __ molecules |
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Definition
| Hydrogen bonds are __ than dipole-dipole forces and dispersion forces |
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Term
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Definition
| Substances composed of molecules that form hydrogen bonds have __ melting and boiling points than substances composed of molecules that do not form hydrogen bonds |
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Term
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Definition
| Ion-dipole force occurs when an __ compound is mixed with a polar compound; it is especially important in aqueous solutions of ionic compounds |
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Definition
| __ forces are the strongest of the types of intermolecular forces |
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Term
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Definition
| __ – the tendency of liquids to minimize their surface area |
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Definition
| The molecule at the surface has relatively fewer neighbors with which to interact and is therefore inherently __ stable – has higher potential energy – than those in the interior |
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Term
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Definition
| Attractive interactions with other molecules __ potential energy |
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Term
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Definition
| In order to increase the surface area of the liquid, molecules from the interior have to be moved to the surface, and, since molecules at the surface have a higher potential energy than those in the interior, this movement __ energy |
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Term
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Definition
| liquids tend to __ their surface area |
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Term
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Definition
| The __ of a liquid is the energy required to increase the surface area by a unit amount |
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Term
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Definition
| Surface tension __ as intermolecular forces decrease |
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Term
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Definition
| the resistance of a liquid to flow |
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Term
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Definition
| Viscosity is measure in a unit called the __, defined as 1 g/cm x s |
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Term
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Definition
| Viscosity is greater in substances with _ intermolecular forces because if molecules are more strongly attracted to each other, they do not flow around each other as freely |
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Definition
| Viscosity also depends on _, increasing in longer molecules that can interact over a greater area and possibly become entangled |
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Term
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Definition
| Notice the increase in viscosity with increasing __ (and therefore increasing magnitude of dispersion forces) and with increasing __ (and therefore increasing potential for molecular entanglement) |
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Term
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Definition
| Viscosity also depends on __because thermal energy partially overcomes the intermolecular forces, allowing molecules to flow past each other more easily |
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Term
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Definition
| Nearly all liquids become __ viscous as temperature increases |
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Term
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Definition
| the attraction between molecules in a liquid, called __ forces, and the attraction between these molecules and the surface of the tube, called __ forces |
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Term
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Definition
| The adhesive forces cause the liquid to __ over the surface of the tube, while the cohesive forces cause the liquid to __ |
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Term
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Definition
| If the adhesive forces are greater than the cohesive forces, the attraction to the surface draws the liquid up the tube and the cohesive forces pull along those molecules not in direct contact with the tube walls |
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Term
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Definition
| If the adhesive forces are __ than the cohesive forces, the liquid does not rise up the tube at all (and in fact will drop to a level below the level of the surrounding liquid) |
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Term
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Definition
| __ = curved shape of a liquid surface within a tube |
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Term
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Definition
| __ – the process by which thermal energy can overcome intermolecular forces and produce a state change from liquid to gas |
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Term
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Definition
| The higher the temperature, the greater the average __ of the collection of molecules |
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Term
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Definition
| At any one time, some molecules would have more __ energy than the average and some would have less |
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Term
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Definition
| transition from liquid to gas to called __ |
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Term
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Definition
| transition from gas to liquid is called |
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Term
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Definition
| if we increase the temperature of the water within the beaker, the shift in the energy distribution to higher energies will make it to where more molecules now have enough energy to break free and evaporate, so __ occurs more quickly |
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Term
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Definition
| if we spill the water on the table/floor, the same amount of water is now spread over a wider area, resulting in more molecules at the surface of the liquid. Since molecules at the surface have the greatest tendency to evaporate – because they are held less tightly – vaporization also occurs __ quickly |
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Term
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Definition
| substances with weaker intermolecular forces allow more molecules to evaporate at a given __, again increasing the rate of vaporization |
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Term
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Definition
| liquids that vaporize easily = __ |
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Term
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Definition
| liquids that do not vaporize easily = __ |
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Term
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Definition
| The rate of vaporization __ with increasing temperature |
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Term
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Definition
| The rate of vaporization __ with increasing surface area |
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Term
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Definition
| The rate of vaporization increases with __ strength of intermolecular forces |
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Term
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Definition
| Vaporization is an _ process; it takes energy to vaporize the molecules in a liquid |
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Term
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Definition
| condensation is __ – heat is released when a gas condenses to a liquid |
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Term
| heat of vaporization (ΔHvap) |
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Definition
| The amount of heat required to vaporize one mole of a liquid to a gas is its __ |
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Term
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Definition
| The heat of vaporization is always __ because the process is endothermic – energy must be absorbed to vaporize a substance |
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Term
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Definition
| The heat of vaporization is __ temperature dependent |
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Term
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Definition
| When a substance condenses from a gas to a liquid, the __ of heat is involved, but the heat is emitted rather than absorbed |
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Term
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Definition
| The sign of ΔH when a gas condenses from a gas to a liquid is negative because the process is __ |
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Term
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Definition
| __: rate of evaporation = rate of condensation |
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Term
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Definition
| As the rate of concentration (or partial pressure) of gaseous water molecules increases, the rate of __ also increases |
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Term
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Definition
| As long as water remains at a __ temperature, the rate of evaporation remains constant |
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Term
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Definition
| The pressure of a gas in dynamic equilibrium with its liquid is called its __ |
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Term
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Definition
| The vapor pressure of a particular liquid depends on the intermolecular forces present in the liquid and the __ |
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Term
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Definition
| Weaker intermolecular forces result in __ substances with high vapor pressures because the intermolecular forces are easily overcome by thermal energy |
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Term
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Definition
| Strong intermolecular forces result in nonvolatile substances with __ vapor pressures |
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Term
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Definition
| A liquid in dynamic equilibrium with its vapor is a balanced system that tends to __ to equilibrium if disturbed |
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Term
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Definition
| If the pressure above a liquid-vapor system in equilibrium is decreased, some of the liquid evaporates, restoring the equilibrium pressure. If the pressure is increased, some of the vapor condenses, bringing the pressure back down to the equilibrium pressure |
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Term
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Definition
| When a system in dynamic equilibrium has an increase in volume, the vapor pressure __. More gas vaporizes so that pressure is restored, and dynamic equilibrium is restored |
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Term
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Definition
| When a system in dynamic equilibrium has a decrease in volume, the vapor pressure __. More gas condenses so that pressure is restored, and dynamic equilibrium is restored |
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