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71 Cards in this Set
- Front
- Back
Liquids are_____________ because its molecular motion is_____________ but the molecularspacing is ____________ |
Incompressible; free relative to one another;close together |
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Data that have random error but otherwise fall in a narrow range are |
precise but not accurate |
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The polymer backbone and the monomer are the constituent parts of an alkane |
false |
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The polymer backbone and the monomer are the constituent parts of a polymer |
true |
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____________________ explained the law of conservation of mass, as well as other laws and observations, by proposing that all matter was composed of small, indestructible particles called atoms |
Dalton |
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what is a lattice |
In an ionic bond, ions are assemble into an extended array called a lattice that are heldtogether by the attraction between oppositely charged ions |
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what is an alkane |
a hydrocarbon connected with only single bonds |
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what is an isomer |
A molecule with the same chemical formula butdifferent structure |
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The molar fraction of a gas is " " to its partial pressure: directly/inverse proportional |
directly |
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no more than 2 electrons can occupy any orbital |
Pauli exclusion principle |
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electrons occupying orbitals must start with the lowest energy level andproceed to the higher |
Aufbau principle |
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if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs |
Hund's rule |
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Van der Waals equation |
has a correction factor for the volume, b, and a correction factor that accounts for the attractions between particles in the gas, a |
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Calorimetry technique measures the heat evolved or absorbed by the system by measuring the_______________ change in the surroundings |
temperature |
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1. When a chemical bond breaks, energy is released/absorbed/either/neither |
absorbed |
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specific heat |
c physical property of a substance that describes the amount of heat required to raise the temperature of one gram of substance by one °C q=mc(change in)T |
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(molar) heat capacity |
Cp physical property of a substance that describes the amount of heat required to raise the temperature of one mole of substance by one °C. q = nCp(change in)T |
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Dispersion forces are also called |
London forces |
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a small separation of charge (positive or negative) that happens because of a fluctuation in the position of the electrons of an atom or molecule |
instantaneous dipole
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What are the two specific intermolecular forces for liquids |
Surface tension and Viscosity |
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exists in all polar molecules as they have permanent dipoles that interact withpermanent dipoles of other molecules |
dipole-dipole force |
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occurs in mixtures where ionic compounds and polar compounds are present |
Ion-dipole force |
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occurs in polar molecules with hydrogen atoms bonded to fluorine, oxygen, or nitrogen |
Hydrogen bonding |
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the amount of energy required to remove an electron |
ionization energy |
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the amount of energy required to add an electron |
electron affinity |
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what determines strength of an ion's lattice energy |
smaller ions = greater lattice energy bigger charge = greater lattice energy |
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What are the units of k for a zero orderreaction |
(mol)(L^-1)(s^-1) |
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What are the units of k for a first order reaction |
s^-1 |
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What are the units of k for a second order reaction |
(L)(mol^-1)(s^-1) |
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uses a combination of adiabatic (no heat is exchanged) and isothermal processes(temperature is constant) |
the Carnot cycle |
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In the following equilibrium reaction in a closed system, indicate how theequilibrium is shifted by the addition of HF(g) to the system: HF(g) + H2O(l) > H3O+(aq)+ F-(aq) |
equilibrium will shift toward the products |
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an energy threshold that reactants must overcome to become products |
Activation energy |
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Determine the formula of the conjugate base for this acid HSO4(-), andthe conjugate acid for this base HPO429(2-) |
SO4(2-) and H2PO4(-), respectively |
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The rate of reaction decreases as the temperature of the reaction is decreases: t/f |
true |
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randomness/disorder of a system |
entropy |
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Bronsted-Lowry acid |
proton doner |
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Bronsted-Lowry base |
proton receiver |
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conjugate base |
The conjugate base of an acid is the base formed when the acid donated a proton |
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conjugate acid |
The conjugate acid of a base is the acid formed when the base accepted a proton |
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Spontaneous processes take place without continuous intervention, according tothermodynamics: T/F |
true |
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Sig figs in multiplication & division |
result should have same number of SIG FIGS as the number with the least number of sig figs |
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sig figs in addition and subtraction |
result should have the same number of DECIMAL PLACES as the number with the least number of decimal places |
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What is Charles' law and how is T and V related |
V1/T1 = V2/T2 |
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What is Boyle's law and how are P and V related |
P1xT1 = P2xT2 |
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What is Avagodro's law and how are n and V related |
V1/n1 = V2/n2 |
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what is the value of R, the universal gas constant |
R = .08206 (L*atm)/(mol*K) |
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What is the law of partial pressures |
Total pressure is equivalent to the sum of the partial pressures of each proponent gas |
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what is the law of partial pressures expressed in terms of the mole fraction |
the mole fraction(Xi) for a gas is the moles of the gas(ni) divided by the total moles of the different gases present(n): (Xi= ni/n) the partial pressure of each gas is related to its molar: (Pi = P*Xi) |
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Van der Waals equation |
(P + an^2/V^2)(V - nb) = nRT a corrects for attractive forces b corrects for volume occupied by gas molcs. |
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what is the speed of light and Planck's constant |
c = 2.99 x 10^8 m/s h = 6.626 x 10^-34 |
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what is the energy equation |
E = hc/(wavelength) |
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Binding energy |
energy holding an electron to a metal |
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threshold frequency |
minimum frequency of light needed to emit an electron |
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what is electronegativity |
the attraction of an atom for the shared electrons in a covalent bond |
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Exceptions to the Octet rule |
odd number of electrons small elements expanded octet |
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zero order integrated rate law |
[A]t = [A]o - kt |
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first order integrated rate law |
[A]t = [A]oe^(-kt) |
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second order integrated rate law |
1/[A]t - 1/[A]o = -kt |
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the degradation of metals by chemical reactions with the environment |
corrosion |
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uniform corrosion |
even corrosion over a large portion of a surface |
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galvanic corrosion |
occurs when two different metals contact each other in the presence of an appropriate electrolyte |
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crevice corrosion |
occurs when two pieces of metal touch each other leaving a small gap or crevice between metals |
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What is oxidation |
loss of electrons from some chemical species |
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What is reduction |
the gain of electrons from some chemical species |
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Reducing agent |
species undergoing oxidation |
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Oxidizing agent |
species undergoing reduction |
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an electrochemical cell in which a spontaneous chemical reaction can be used to generate an electric current |
GALVANIC CELL
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electrode |
electrically conducting sites at which either oxidation or reduction occurs
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anode |
electrode where oxidation occurs |
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cathode |
electrode where reduction occurs |
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what is proper cell notation |
anode | anode electrolyte || cathode electrolyte | cathode |