Term
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Definition
| Random electron motion produces an unbalanced charge distribution producing a temporary dipole |
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Term
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Definition
Fluorine
chlorine
bromine
iodine |
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Term
| dispersion forces occur for |
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Definition
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Term
| the relative strength of dispersion forces depend on |
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Definition
| the polarizability of the particle |
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Term
| polarizability depends on |
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Definition
| the number of electrons and the shape of the particles |
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Term
| the total number of energy levels produced equals the |
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Definition
| total number of orbitals used |
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Term
| the hydrogen bond is a special case of |
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Definition
| dipole dipole interaction |
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Term
| DNA is an example of ____ bonding |
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Definition
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Term
| a solution is a ______ mixture |
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Definition
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Term
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Definition
| maximum amount of solute that will dissolve in a fixed quantity of solvent |
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Term
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Definition
| soluble in each other in all portions |
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Term
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Definition
| not soluble in any portions |
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| mol of solute / L of solution |
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Term
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Definition
| mol of solute / mass (kg) of solvent |
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Term
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Definition
| mass of solute / mass of solution |
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Term
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Definition
| volume of solute / volume of solution |
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Term
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Definition
| mol of solute / (mol of solute + mol of solvent) |
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Term
| substances with similar types of intermolecular forces ____ in each other |
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Definition
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Term
| solute particles separate from each other |
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Definition
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Term
| solvent particles separate from each other |
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Definition
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Term
| solute and solvent particles mix |
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Definition
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Term
| solvation of ions by water is always |
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Definition
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Term
| the idea of energy was first developed by |
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Definition
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Term
| solubility of gases usually decrease with |
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Definition
|
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Term
|
Definition
| solubility of gases in a liquid is proportional to the pressure of the gas over the liquid |
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Term
Boiling point elevation
DTb = |
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Definition
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Term
Freezing point depression
DTf = |
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Definition
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Term
| Osmotic Pressure Equation |
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Definition
pie = M R T
where M is the molarity,
R is the ideal gas law constant and
T is the Kelvin temperature |
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Term
| symbol of osmotic pressure is |
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Definition
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Term
| The van’t Hoft factor, i, tells us |
|
Definition
hat the “effective”
number of ions are in the solution. |
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Term
|
Definition
measured value for electrolyte solution/
expected value for nonelectrolyte solution |
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Term
| Four factors can be controlled during the reaction |
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Definition
1. Concentration - molecules must collide to react;
2. Physical state - molecules must mix to collide;
3. Temperature - molecules must collide with enough energy to react;
4. The use of a catalyst. |
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Term
|
Definition
| changes in the concentrations of reactants or products per unit time |
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Term
| reactant concentrations ______ while product concentrations _____ |
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Definition
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Term
|
Definition
k [A]^m [B]^n
k = rate constant
m = order of reaction in A
n = order of reaction in B
m+n = overall order of reaction |
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Term
|
Definition
| Chemical Reactions occur during collisions |
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Term
| The Collision must be effective: |
|
Definition
1. Have enough energy to produce the reaction
2. Have the correct orientation to produce the reaction |
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Term
| Transition state theory (TST) explains |
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Definition
the reaction rates of elementary chemical reactions.
The theory assumes a special type of chemical equilibrium (quasi-equilibrium) between reactants and
activated transition state complexes |
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Term
| A complex reaction can proceed by a series of _____ ______ |
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Definition
|
|
Term
| The rate of reaction is often determined by one slow step |
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Definition
| (rate-determining or rate- limiting step). |
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Term
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Definition
| They are in the same phase as the reactants (usually liquid) |
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Term
| Homogeneous Catalysts are Often |
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Definition
| acids, bases, transition metal complexes |
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Term
|
Definition
| Catalyst is in a different phase from the reactants (usually solid) |
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Term
| ____ are considered Heterogeneous Catalysts |
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Definition
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Term
|
Definition
|
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Term
| potential energy in the form of intermolecular forces tends to |
|
Definition
| draw the molecules together |
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Term
| kinetic energy associated with the random motion of molecules tends to |
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Definition
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Term
| intramolecular forces exists |
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Definition
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Term
| intermolecular forces exist |
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Definition
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Term
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Definition
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Term
| liquid compressibility is |
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
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Term
|
Definition
| condensing, freezing and depositing |
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Term
|
Definition
| melting, vaporizing and subliming |
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Term
| heating cooling curve shows |
|
Definition
| the change in temperature of a sample when heat is absorbed or released at a constant rate |
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Term
|
Definition
|
|
Term
| within a phase, heat flow |
|
Definition
| is accompanied by a change in temperature |
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Term
| during a phase change heat flow |
|
Definition
| occurs at a constant temperature |
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Term
|
Definition
|
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Term
|
Definition
|
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Term
|
Definition
| the rate of condensation equals the rate of vaporization, form this point forwards the pressure is constant |
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Term
| temperature has a major effect on water vapor because |
|
Definition
| it changes the fraction of molecules moving fast enough to escape the liquid and, by the same token, the fraction moving slow enough to be recaptured |
|
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Term
| the _____ the temperature, the ____ the vapor pressure |
|
Definition
|
|
Term
| the ______ the intermolecular forces, the _____ the vapor pressure |
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Definition
|
|
Term
|
Definition
| the temperature at which the vapor pressure equals the external pressure |
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Term
| the boiling point depends on the |
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Definition
|
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Term
|
Definition
| the temperature at which the melting rate equals the freezing rate |
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Term
|
Definition
|
|
Term
| bonding forces are relatively strong because |
|
Definition
| larger charges are closer together |
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|
Term
| intermolecular forces are relatively weak because |
|
Definition
| smaller charges are farther apart |
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Term
| what force takes place when an ion dissolves in water |
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Definition
|
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Term
|
Definition
| when an ion and a nearby polar molecule attract |
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Term
|
Definition
| the positive pole of one molecule attracts the negative pole of another |
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Term
|
Definition
| when an H molecule bonds with an O, N or F molecule |
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Term
|
Definition
|
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Term
|
Definition
| how easily the electron cloud of an atom can be distorted |
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Term
| smaller particles are _____ polarizable than larger ones |
|
Definition
|
|
Term
|
Definition
| down a group because atomic size increases |
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|
Term
| (larger/smaller) electron clouds are easier to distort |
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Definition
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Term
|
Definition
|
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Term
|
Definition
| intermolecular force responsible for the condensed states of nonpolar substances |
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Term
| dispersion forces are present in |
|
Definition
| all atoms, ions and molecules because they are caused by the motion of electrons in an atom |
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Term
| an interior molecule is attracted by others |
|
Definition
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|
Term
| a surface molecule is attracted by |
|
Definition
| other below and to the sides, so it experiences a net attraction downward |
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Term
|
Definition
| dipole-dipole and dispersion |
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Term
|
Definition
|
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Term
|
Definition
|
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Term
|
Definition
|
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Term
|
Definition
|
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Term
|
Definition
| the resistance of fluid to flow |
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Term
|
Definition
|
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Term
|
Definition
| a measure of the energy required to increase a liquid's surface area |
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Term
|
Definition
| the rising of a liquid through a narrow space |
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Term
|
Definition
|
|
Term
| the great solvent power of water results from its |
|
Definition
| polarity and h bonding ability |
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Term
|
Definition
| well defined shapes because of their particles occur in an orderly arrangement |
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Term
|
Definition
| poorly defined shapes because their particles lack an orderly arrangement |
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|
Term
| examples of amorphous solids |
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Definition
|
|
Term
| the centers of 8 identical particles define the corners of a cube |
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Definition
|
|
Term
| the simple cubic unit cell has a coordination number of |
|
Definition
|
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Term
|
Definition
| number of nearest neighbors of a particle |
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Term
| identical particles lie at each corner and at the center of the cube |
|
Definition
| body centered cubic unit cell |
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Term
| the body centered cubic unit cell has a coordination number of |
|
Definition
|
|
Term
| identical particles lie at each corner and in the center of each face but not in the center of each cube |
|
Definition
| face centered cubic unit cell |
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Term
| the face centered cubic unit cell has a coordination number of |
|
Definition
|
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Term
|
Definition
| percentage of the total volume occupied by the spheres themselves |
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|
Term
| hexagonal unit cell has ______ _____ packing |
|
Definition
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|
Term
| face centered unit cells has ______ _____ packing |
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Definition
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|
Term
|
Definition
| individual atoms held together only by dispersion forces |
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Term
| only substances that form atomic solids |
|
Definition
|
|
Term
| inter-particle forces in atomic solids |
|
Definition
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|
Term
| inter-particle forces in molecular solids |
|
Definition
| disoersion, dipole dipole and h bonding |
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Term
| inter-particle forces in ionic solids |
|
Definition
|
|
Term
| inter-particle forces in metallic solids |
|
Definition
|
|
Term
| inter-particle forces in network covalent solids |
|
Definition
|
|
Term
| examples of network covalent solids |
|
Definition
|
|
Term
| electron sea model proposes |
|
Definition
| that all metal atoms in a sample pool their valence electrons to form an electron sea that is delocalized throughout the piece |
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Term
| the regularity and mobility of the valence electrons in the electron sea model of metallic bonding account for three major physical properties: |
|
Definition
| phase change, mechanical properties and conductivity |
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Term
| the valence and conduction bands of a conductor have _______ energy gap so |
|
Definition
| no; electrons flow when a tiny electrical potential difference is applied |
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Term
| the valence and conduction bands of a semiconductor have _______ energy gap so |
|
Definition
| small; thermally excited electrons can cross the gap, allowing a small current to flow |
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Term
| the valence and conduction bands of a insulator have _______ energy gap so |
|
Definition
| large; no current is observed even when the substance is heated |
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Term
|
Definition
| two or more substances mixed together physically, not combined chemically |
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Term
| mixture has two defining characteristics: |
|
Definition
1) its composition can be variable
2) it retains some properties of its components |
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Term
| a ____ dissolves in a ____ to form a solution |
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Definition
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|
Term
| ion induced dipole forces arise when |
|
Definition
| an ion's charge distorts the electron cloud of a nearby nonpolar molecule |
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Term
| dipole induced forces arise when |
|
Definition
| a polar molecule distorts the electron cloud of a nearby nonpolar molecule |
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Term
| intermolecular forces listed in decreasing strength |
|
Definition
ion-dipole
H bond
dipole-dipole
ion-induced dipole
dipole-induced dipole
dispersion |
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Term
| solubility in water is high for |
|
Definition
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|
Term
| solubility in water is low for |
|
Definition
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|
Term
| solubility in hexane is low for |
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Definition
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|
Term
| solubility in hexane is high for |
|
Definition
|
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Term
|
Definition
| all gases are miscible with each other |
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Term
|
Definition
| when a gas dissolves in a solid, it occupies the spaces between the closely packed particles |
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Term
|
Definition
| solids diffuse so little that their mixtures are usually heterogeneous |
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Term
|
Definition
| mixtures of substances that have a metallic character and are solid solid solutions |
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Term
|
Definition
| the process of surrounding a solute particle with solvent particles |
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Term
|
Definition
|
|
Term
|
Definition
| ratio of a ion's charge to its volume |
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|
Term
| heats of hydrations exhibit trends based on |
|
Definition
|
|
Term
|
Definition
| freedom of motion of particles |
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|
Term
| a _____ usually has higher entropy than the ______ solute or solvent |
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Definition
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|
Term
| most solids are more soluble at |
|
Definition
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|
Term
| the solubility of any gas in water decreases with |
|
Definition
|
|
Term
| ____ has little effect on liquids and solids because |
|
Definition
| pressure; the are almost incompressible |
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Term
|
Definition
| the solubility of a gas is directly proportional to the partial pressure of the gas above the solution |
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|
Term
| symbol for Henry's Law constant |
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Definition
|
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Term
|
Definition
| (volume of solute / volume of solution ) x100 |
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Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| colligative properties of solutions |
|
Definition
| vapor pressure lowering, boiling point elevation, freezing point depression and osmotic pressure |
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Term
|
Definition
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|
Term
|
Definition
| doesnt conduct electricity |
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Term
|
Definition
soluble salts, strong acids, strong bases
dissociate completely into ions |
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Term
|
Definition
weak acids and bases
dissociate very little into ions |
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Term
|
Definition
| vapor pressure of solvent above a solution equals the mole fraction of solvent times the vapor pressure of the pure solvent |
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Term
|
Definition
| ones that allows solvent but not solute to pass through |
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Term
|
Definition
| net flow of solvent into the more concentrated solution |
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Term
| the net flow of water into a solution increases its ______ and decreases its _______ |
|
Definition
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Term
|
Definition
| pressure that must be applied to prevent net movement of water from solvent to solution |
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Term
|
Definition
| study of how fast change occurs |
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Term
|
Definition
| change in the concentrations of reactants (or products) as a function of time |
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|
Term
| reaction rate is proportional to |
|
Definition
| concentration of reactants |
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|
Term
| the greater the surface area |
|
Definition
| the faster the reaction occurs |
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|
Term
| concentration affects rate by |
|
Definition
| influencing the frequency of collisions between molecules |
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|
Term
| physical state affects rate by |
|
Definition
| determining how well reactants mix |
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|
Term
| temperature affects rate by |
|
Definition
| influencing the frequency and the energy of the collisions |
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Term
|
Definition
| change in position / change in time |
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Term
|
Definition
|
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Term
|
Definition
| the slope of the line joining tow points on the curve |
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Term
|
Definition
| rate at a particular instant during the reaction |
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Term
|
Definition
| instantaneous rate at the moment the reactants are mixed (at t=0) |
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Term
| the rate law expresses the rate as |
|
Definition
| a function of concentrations and temperature |
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Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| three lab methods for determining the initial rate |
|
Definition
change in color
change in pressure
change in conductivity |
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Term
| the reaction is first order overall if |
|
Definition
| the rate is directly proportional to [A] |
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Term
| the reaction is second order overall if |
|
Definition
| the rate is directly proportional to the square of [A] |
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Term
| the reaction is the zero order overall if |
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Definition
| the rate is not dependent on [A] at all, the rate doesn't change when [A] changes |
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Term
|
Definition
| times is takes a given reactant concentration to reach half of its initial value |
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|
Term
| the half life of a second order reaction is |
|
Definition
| inversely proportional to the initial reactant concentration |
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|
Term
| the half life of a zero order reaction is |
|
Definition
| directly proportional to the initial reactant concentration |
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Term
|
Definition
| particles (atoms, molecules or ions) must collide to react |
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Term
|
Definition
| energy threshold that the colliding molecules must exceed in order to react |
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Term
| if particles move faster they collide _____ |
|
Definition
|
|
Term
|
Definition
| sequence of single reaction steps that sum to the overall equation |
|
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Term
| rate determining step limits |
|
Definition
| how fast the overall reaction proceeds |
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Term
|
Definition
| substance formed and used up during the reaction |
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|
