Inorganic Chemistry Answers

Expain Crystal Field Theory briefly. 

Show the splitting of the d orbitals in

a)    An isolated metal ion  b) in a spherical field  c) in an octahedral field.

1)     Explain the phenomenon of complementary colors (Hint: Newton Wheel).

Complexes

λ1

λ2

λ3

[Ni(H₂O)₆]²⁺

720

395

-

[Co(H₂O)₆]₂⁺

510

460

-

[Cr(C₂O₄)₃]^3-

565

415

266

[Co(NO₂)₆]^3-

360

-

-

    Which parameters determine the value of Δ_o? What is the difference between high spin and low spin complexes?

 Upon addition of a strong Lewis base, NH3 to BBr3 the bond angles between the ligands are pushed towards 109 degrees. The bond angles between BF3 and NH3 in the same reaction remain close to 120 degrees. Explain these observations.

Boron is able to form a multiple array of bonding modes. Draw a molecular orbital diagram that explains why 3c2e bonds are possible.

a) By making use of chemical equation from a summary diagram of the reaction chemistry, write the chemical equation for the

successive conversions of borax to:

(i) B203

(ii) Boric acid

(iii) Impure boron metal

B) Using the summary diagram of the reaction chemistry, write chemical

the equation for the sequence of the reaction by which borax is converted to

diborane and BF3

C)Predict the probable products of the following reaction and write the

balanced chemical equations

i)BF3 and excess NaF in acid aqueous solution

ii)BCI3 and excess NaCl in acidic aqueous solution

iii)BBr3 and excess NH(CH3)2 a hydrocarbon solvent

Phosphorus pentachloride (Kp=0.0870) is one of the most important phosphorus chlorides, and is use as

a chlorinating reagent. It is produced by reacting chlorine gas and Phosphorus trichloride (PCl3) at

300°C. PCl3(g)+Cl2(g)<-> PCl5(g). In an industrial set-up, the stainless steel container was charged

with 020 atm PCl3, 0.20 atm Cl2, and 0.50 atm PCl5 at this temperature. (a) Use the reaction quotient

to determine the direction the reaction must proceed to reach equilibrium. (b) Calculate the equilibrium

partial pressures of the gases. (c) What effect will increasing the volume of the system have on the mole

fraction of Cl2 in the equilibrium mixture? (d) The reaction is exothermic. What effect will increasing

the temperature of the system have on the mole fraction of Cl2 in the equilibrium mixture

Silver chloride, AgCl(s), is an “insoluble” strong electrolyte. (a) Write the equation for the dissolution

of AgCl(s) in H2O(l). (b) Write the expression for Kc for the reaction in part (a). (c) The equilibrium

constant for the dissolution of AgCl in water is 1.6x10-10 at 25°C. In addition, Ag+

(aq) can react with

Cl-(aq) according to the reaction Ag+(aq) + 2 Cl-(aq) -> AgCl2(aq) where Kc=1.8x10-5

at 25°C. Although

AgCl is “not soluble” in water, the complex AgCl2 is soluble. At 25°C, is the solubility of AgCl in a

0.100 M NaCl solution greater than the solubility of AgCl in pure water, due to the formation of soluble

AgCl2- ions? Or is the AgCl solubility in 0.100 M NaCl less than in pure water because of a Le

Châtelier–type argument? Justify your answer with calculations. (Hint: Any form in which silver is in

solution counts as “solubility.”)

Calculate the concentration of [OH-] and pH of a weak acid in a 0.500 M pyridine (C5H5N)

solution (Kb=1.7x10-9

)