1. Determine whether each statement below is True (T) or False (F). a. ____ If A,B and C are elements whose electronegativities satisfy xA > xB > xC, then then (ΔAC)1/2 = (ΔAB)1/2 + (ΔBC)1/2 if the Pauling electronegativity scale is valid. b. ____ There is no interelectronic repulsion in the H2+ molecule. c. ____ The wave function N(1sA + 1sB) is the exact electronic wave function for the ground electronic state of H2+. d. ____ The plane perpendicular to the molecular axis at the midpoint between the nuclei in H2+ is a node for the first excited state. e. ____ The molecular electron probability density is experimentally observable. f. ____ The molecular wave function is experimentally observable. g. ____ The bonding MOs of BeH2 extend over all three atoms and the hybridization of AOs are approximately sp2. h. ____ A SCF wave function is one in which each electron is assigned to a single spin-orbital, the spatial part of each spin-orbital is expressed as a non- linear combination of basis functions, and the coefficients in these combinations are found by solving the Hartree-Fock equations. i. ____The molecular-mechanics method is an empirical quantum mechanical method that treats the molecule as atoms held together by bonds and writes the molecular steric energy as the sum of contributions from bond bending and stretching, bond torsion and van der Waals and electrostatic interactions of non-bonded atoms. j. ____ The molecular-mechanics method can be applied to very large molecules and yields good results when applied to molecules similar to those for which the force field was parametrized. k. ____ The maximum electron probability density in the ground electronic state of H2+ occurs at each nucleus. l. ____ If sufficient basis functions are used, the Hartree-Fock wave function of a many-electron molecule will reach the true wave function. m. ____ In a homonuclear diatomic molecule, combining two 2p AOs always yields a π MO. n. ____ In homonuclear diatomic molecules, all u MOs are antibonding. o. ____ A decrease in viscosity with increasing rate of flow of a solution indicates the presence of long rod-like molecules that are orientated by the flow.

Explain the inductive affect in acids and bases

At a certain temperature, the equilibrium constant for the following chemical equation is 2.20. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.73 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.

Why does a change in polarizability in a molecule allow a vibrational mode to be Raman active? Why does a change in dipole moment allow a vibrational mode to be IR active? Why do they differ?

If the Kb of a weak base is 4.1 × 10-6, what is the pH of a 0.50 M solution of this base?

Aqueous hydrobromic acid HBr reacts with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O. What is the theoretical yield of water formed from the reaction of 79.3g of hydrobromic acid and 52.9g of sodium hydroxide? Be sure your answer has the correct number of significant digits in it.

what is the pH of 0.124 M pyridine (C5H5N)?

A 1.00 L flask is filled with 1.20 g of argon at 25 ∘C. A sample of ethane vapor is added to the same flask until the total pressure is 1.450 atm . What is the partial pressure of argon, PAr, in the flask?

Find the pH of a solution made by dissolving 0.195 g of phenol (C6H5OH) in enough water to make 125 mL of solution.

When an ant bites you, the reason it stings is because of an injection of formic acid. What is the pH when 50.00 mL of 0.1480 M formic acid (HCOOH) is titrated with 40.2 mL of 0.1841 M of NaOH? pKa of formic acid = 3.745

Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O .

Suppose 60. g of hydrobromic acid is mixed with 48.8 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

A 110.0 −mL sample of a solution that is 2.8×10^−3 M in AgNO3 is mixed with a 220.0 −mL sample of a solution that is 0.11 M in NaCN. A complex ion forms. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?

Titanium occurs in the magnetic mineral ilmenite (FeTiO3), which is often found mixed up with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO3(s)+3Cl2(g)+3C(s)→3CO(g)+FeCl2(s)+TiCl4(g)TiCl4(g)+2Mg(s)→2MgCl2(l)+Ti(s) Suppose that an ilmenite-sand mixture contains 22.6 % ilmenite by mass and that the first reaction is carried out with a 91.1 % yield. If the second reaction is carried out with an 86.1 % yield, what mass of titanium can be obtained from 1.30 kg of the ilmenite-sand mixture?

a) Copper solutions are typically blue to blue green in color. What color of light would they be expected to absorb in the greatest amount?

b) Based on your answer to the previous question (hopefully you have the correct answer), what wavelength range would you expect to see the maximum absorption of light (in the visible range)?

c) Given the information that the tartrate ion is the conjugate base of a weak acid, how do you expect the solubility of copper (II) tartrate to be affected by pH?

d) It was an intention to have a common ion experiment with the lab, but it did not work when we tested the experiment. What would the solubility of copper (II) tartrate be in a solution that contains 0.19 M sodium tartrate? (Use the literature for copper (II) tartrate K_sp = 4.0 x 10^-4) Please enter answer in standard notation.

e) Your value for K_sp will not be the same as the literature. It may not even be close. It is likely to be larger than the literature value. What is one logical reason your value may be larger?

Calculate the mass of NaCN that must be added to 250.0 mL of water in order to obtain a solution having a pH of 11.25? [Ka of HCN = 4.9 × 10–10] Also, calculate the % ionization of the of the solution.