CHEM 1133 Ch. 20.1 – Flashcards
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Unlock answersSpontaneous change |
A chemical or physical change that occurs by itself under specified conditions without a continuous input of energy from outside the system |
Non-spontaneous change |
A physical or chemical change that occurs only if the surrounding supplies the system with a continuous input of energy. |
The second law of thermodynamics |
All real processes occur spontaneously in the direction that increases the entropy of the universe. |
The third law of thermodynamics |
A perfect crystal has zero entropy at a temperature of absolute zero. |
Prediction of relative S° values of a system |
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Solubility |
The maximum amount of solute that can dissolve in a given volume of solvent @ a given temperature. |
Molar solubility |
Number of moles of solid dissolved per liter liter of solution |
The common ion effect |
The solubility of a salt is less in the presence of a common ion already present in the solution as is predicted in Le Cheatliers principle. |
How to find pH at which a medal hydroxide ionic solution precipitates: |
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How to find the molarity of an ionic medal in a medal hydroxide ionic solution given the solutions pH: |
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How to find the percent ionic medal left in a solution after its concentration has been changed (for example due to precipitation by addition of pH etc.): |
Percent concentration left in solution: [(Current concentration)/(initial concentration)](100) |
Formation constant: |
The equilibrium constant for the one step formation of a complex ion from a metal ion and its ligands. |
Coordinate covalent bond: |
A bond between two atoms in which one atom contributes both electrons. |
Saturated |
When the maximum amount of solute has been dissolved the solution is saturated. |
Supersaturated |
An unstable solution with more solute dissolved compared to normal levels of saturation. |
Insoluble |
A substance that won't dissolve in a solution.; |
Solubility product constant (Ksp) |
The equilibrium constant for a solid dissolving into ions. ; Ksp = products/reactants ; Since reactants are solids and solids are not included in equilibrium calculations there is no denominator and on products are multiplied and raised by their coefficient. |
Situation where Ksp's of salts cannot be compared to determine which is more soluble |
In cases where the stoichiometry is not 1/1. |
Crystal field theory |
A theory developed to explain the character in color and magnetism of complex ions by explaining the effect the d orbital influence on the ligands. |
Crystal field splitting energy (?) |
The magnitude of splitting of the d orbital affected by the binding of ligands to a metal ion. |
Strong field ligands vs. weak field ligands |
Stronger field ligands cause a larger split of the d orbital when creating a complex ion with the metal ion. |
High spin vs. low spin complexes |
High spin complexes: created by weak crystal fields, such complex ions contain the least amount of unpaired electrons.
Low spin complexes: created by strong crystal fields, such complex ions contain the maximum amount of unpaired electrons. |
Chemical kinetics |
The study of reaction rates, the changes in concentrations of reactants (or products) as a function of time. |
Four factors that affect the rate of a given reaction |
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Reaction rate |
The changes in concentrations of reactants or products per unit time. |
Instantaneous rate |
The rate at a particular instant in a reaction. |
Initial rate |
The instantaneous rate of a reaction at the moment the reactants mix. |
The rate law (rate equation) |
The rate law expresses the rate as a function of reactant concentrations, product concentrations , and temperature. The components of the rate equation include the rate constant and the reaction order. The rate law is deduced by calculating the initial rate of a reaction, using initial rates from several experiments to find the reaction orders, using the values obtained from the initial rate and and reaction order to find the rate constant. |
The rate constant |
A constant specific for a given reaction and is not changed by the stage in the reaction. |
Reaction orders |
Define how the rate is affected by reactant concentration. The reaction orders are not derived from a reactions stoichometry (coefficients) but from rate data. Reaction orders cannot be negative or fractions; they are zero or positive integers. |
Three ways to determine the initial concentration rate |
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Transition metals with electron configuration exceptions: |
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How to predict the effect of solubility by the introduction of acid |
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How to caluclate the solubility of a precipitate when given Ksp |
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How to solve for solubility given a precipitates Ksp and an initial concentration of one of the solutes (the common ion effect) |
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Find Ksp given solubility values |
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Complex ion |
A central metal ion covalently bonded to two or more anions or molecules. |
Ligands |
The anions or neutral molecules bonded to an ionic metal in a complex. |
Integrals of the 1st 2nd and 3rd order |
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Solubility rules |
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Classifying acids and bases (strong vs. weak) |
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First integrated law |
ln([A]0/[A])t = kt |
Fraction of reactant decomposed in a RxN with concentration change over time |
([A]0-[A]t)/[A]0
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Half life |
The time required for a reactant's concentration to reach half its initial value. |
The time it takes to reach one half life |
t=ln(2)/k |
Half life of a first order reaction |
t(1/2)=ln(2)/k |
Half life of a second order reaction |
t(1/2)=1/(k[A]0) |
Half life of a zeroth order reaction |
t(1/2)=[A]0/(2k) |
Activation energy |
The minimum energy molecules must have to react. |
Arrhenius equation |
k=Ae^-(Ea/RT) ; Ea/RT: gives the number of molecules at a given temperature that will have enough energy to react.; ; A: the "pre-exponential factor"and accounts for the fact that some molecules won't form products upon interaction (for example incorrect orientation upon collision). The pre-exponential symbol expresses the number of molecules that receive an adequate amount of activation energy but do not proceed the hump to and evolve into products. |
Collision theory |
The collision theory claims that reactant particles, atoms, molecules, and ions, must collide in order to react. |
Radioactivity - Ch. 23.1 |
Decay, of an unstable nucleus, by emitting radiation. |
Nucleons (23.1) |
Elementary particles, the protons and neutrons, that make up the nucleus. |
(23.1) Nuclide |
A nuclear with a specific number of two types of nucleons. When an element has two isotopes, each isotope is a unique number of neutrons but the same number of protons. |
Isotopes |
Atoms with a characteristic number of protons but a different number f neutrons. |
Chemical changes vs. nuclear reactions |
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(18.2) Number of of sigfigs |
The number of sig figs in a concentration equals the number of sigfigs to the right of a pH/pOH decimal. |
(18.1) Arrhenius acid - base definition |
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(18.1) Neutralization |
When H ions and OH ions combine to form H2O. |
(18.2) Comparison of hydronium in different solutions |
a pH of one is 10 times stronger than a pH of 2 and 100 times stronger than a pH of 3. |
(18.2) The relations among pH, pOH, and pKw |
Kw = [H30+][OH-] = 1e-14
pKw = pH+pOH = 14
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(18.2) Acid base definition of Arrhenius vs. Bronstead lowry vs. lewis |
Arrhenius acid base definition: an acid is any molecule that contains a hydrogen ion and dissociates ions into H+ in aqueous solutions. A base is any compound containing a OH- complex that dissociates into OH- ions when in aqueous solution.
Bronstead lowry definition: An arrhenius and Bronstead lowry acid are the same. A Bronstead Lowry base accepts H+ in aqueous solutions and other situations.
Lewis acid base definition: An acid is any compound that donates accepts a lone pair of electrons. A base is any compound that donates a pair of lone electrons. |
(18.3) Conjugate acid base pairs |
HS- and H2S
NH3 and NH4 |