Chapter 8
Chapter 10
Chapter 11
Chapter 12
Chapter 13
Chapter 14
Chapter 15
Chapter 16
Chapter 17
Chapter 21
100
The hybridization of a molecule with a tetrahedral electron geometry.
What is sp3?
100
Rank the following intermolecular forces in order of decreasing strength. London dispersion forces, Hydrogen bonds, Dipole-Dipole forces.
What is Hydrogen bonds>Dipole-Dipole forces>London dispersion forces
100
The mass of NH3 dissolved in 475 g of methanol to make a 0.250 m solution.
What is 2.02 g
100
Given the following rate law, how does the rate change if the concentration of X is doubled?
rate = [X][Y]2
What is a factor of 2?
100
Express the equilibrium constant for the following reaction
2NH3(g) <--> N2(g) + 3H2(g)
What is
Kc = [H2]3[N2] / [NH3]2 ?
100
The conjugate base of H2PO4-.
What is HPO42-?
100
Effect on equilibrium when a substance with an ion in common with the dissolved species is added to the solution; causes a decrease in the solubility of an ionic species, or a decrease in the ionization of a weak acid or base.
What is common ion effect?
100
Change in temperature and change in state.
What are the two main factors that affect entropy?
100
Balance the following redox reaction in acidic solution.
Zn2+(aq) + NH4+(aq) --> Zn(s) + NO3-(aq)
What is
3H2O + 4Zn2+ + NH4+ --> 4Zn + NO3- + 10H+
100
The change in the nucleus when a beta particle is emitted.
What is increase in the atomic number by 1. A neutron is converted to a proton.
200
The number of pi bonds in hydrogen cyanide?
What is 2?
200
The strongest type of intermolecular force present in NH2CH3.
What is hydrogen bonding?
200
The mole fraction of MgCl2 in a aqueous solution prepared by dissolving 0.400 moles of MgCl2 in 850.0 g of water.
What is 0.00841?
200
The rate constant for the first-order decomposition of N2O is 3.40 s-1. What is the half-life for this decomposition?
What is 0.204 s?
200
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?
Fe3O4(s) + CO(g)<-->3FeO(s)+CO2(g) deltaH = +35.9 kJ
What is the reaction will shift to the right?
200
Conjugate bases are _____ when the acid is weak.
What is strong?
200
Ksp expression for PbCl2.
What is
Ksp = [Pb2+][Cl-]2
200
Consider a reaction that has a positive H and positive S. At what temperatures (high or low) will this reaction be nonspontaneous?
Low
200
Which electrode is the anode in the cell below?
Pb(s) + 2H+(aq) --> Pb2+(aq) + H2(g)
Pb electrode
200
Define the term half-life.
What is the time it takes for one-half of a sample to decay?
300
The bond order in the molecule N2.
What is 3?
300
The amount of energy required to vaporize 48.7 g of dichloromethane (CH2Cl2) at its boiling point if its Hvap is 31.6 kJ/mol.
What is 18.1 kJ?
300
Cg = kPg
What is the formula for Henry's Law?
300
Which of the 3 integrated rate laws has a negative slope?
What are zero and first order?
300
Determine the value of Kc for the following reaction
2N2(g) + O2(g) <--> 2N2O
if the equilibrium concentrations are as follows:
[N2] = 3.6 M, [O2] = 4.1 M, [N2O] = 3.3 x 10-18 M
What is 2.0 x 10-37
300
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25oC.
What is 7.1 x 10-5 M?
300
Calculate Ksp of Gd2(SO4)3 if the solubility of the compound is 6.60 x 10-2 mol/L.
What is 1.35 x 10-4?
300
A _____ sign on Gibbs free energy represents a spontaneous reaction.
negative
300
The electrode in an electrochemical cell where oxidation occurs.
What is anode?
300
A sample of rock was found to contain 8.23 mg of Rb-87. Calculate the age of the rock if the half-life of the decay of Rb by beta emission is 4.7 x 1010 y.
What is 3.8 billion years?
400
The constant motion of electrons in overlapping unhybridized p orbitals.
What is the delocalization of pi bonds?
400
Define heat of vaporization.
What is the amount of energy required to vaporize one mole of a liquid (kJ/mol)
400
The maximum amount of solute has been dissolved into a solute.
What is saturated solution?
400
What are the rate law and the value of k for the following reaction?
NO2(g) + O3(g) --> NO3(g) + O2(g)
[NO2] [O3] rate (Ms-1)
0.10 0.33 1.42
0.10 0.66 2.84
0.25 0.66 7.10
What are:
rate = k[NO2][O3]
k= 43 M-1s-1
400
Consider the following reaction at equilibrium. What effect will increasing the volume have on the system?
2H2S(g) + 3O2(g) <--> H2O(g) + 2 SO2(g)
What is the reaction will shift to the left?
400
Determine the pH of a 0.461 M C6H5CO2H solution if the Ka of C6H5CO2H is 6.5 x 10-5.
What is 2.26?
400
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of Mn(OH)2. Ksp = 2 x 10-13
What is [Mn2+] =3.7 x 10-5 M and
[OH-] = 7.4 x 10-5M?
400
Estimate the free energy of the reaction below at 449 K.
CH2O + 2H2 --> CH4 + H2O
H = -94.9 kJ; S = -224.2 J/K
What is 5.8 kJ?
400
Identify the half-reaction below as either oxidation or reduction.
Cr --> Cr3+ + 3 e-
oxidation
400
The isotope Sr-90 is one of the extremely hazardous species in the residues from nuclear power generation. The strontium in a 0.500 g sample diminishes to 0.393 g in 10.0 y. Calculate the half-life.
What is 28.8 y?
500
Molecules that exhibit paramagnetism.
What is have unpaired electrons in their molecular orbitals?
500
The number of atoms in a body-centered unit cell.
What is 2?
500
The pressure required to stop movement of a solvent across a semipermeable membrane.
What is osmotic pressure.
500
A substance that increases the reaction rate by lowering the activation energy of the reaction.
What is a catalyst?
500
The mathematical function describing the relative amounts of reactants and products in a reaction mixture that is not a equilibrium.
What is reaction quotient (Q)?
500
Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 x 10-4.
3.2%
500
Any species that can accept a pair of electrons and form a coordinate covalent bond.
What is a Lewis acid?
500
Define the 3 laws of thermodynamics.
1. Energy can neither be created nor destroyed, it can only be transformed.
2. The universe tends toward and increase in entropy.
3. The entropy of a pure, crystalline solid is 0 when T = 0 K.
500
Calculate the standard cell potential for the reaction below, and note whether the reaction is spontaneous or not.
Mg(s) + Ni2+(aq) --> Mg2+(aq) + Ni(s)
Mg2+(aq) + 2 e- --> Mg(s) E = -2.372 V
Ni2+(aq) + 2 e- --> Ni(s) E = -0.257 V
What is +2.115 V; spontaneous
500
alpha decay, beta decay, gamma emission
What are the three major types of radioactive decay?