Inorganic Chemistry

QUESTION 3: In question 2 you worked with octahedral complex anions of [VCl₂(O₂CCO₂)₂]³ in this question you are asked to consider trigonal prismatic [VCl₂(0₂CCO2)2]³ complex anions. a) Draw 2 distinguishable isomers of the [VCl₂(O₂CCO2)2]³ complex with trigonal prismatic geometry and determine their point groups. You must use dashes and wedges correctly. Indicate all atoms including the ligand atoms. i. Isomer 3 (trigonal prismatic): 3-dimensional structure: Point group:

What is the mass of 4.00 mol of boron trichloride, BC13(g)?

1) Draw the Bohr diagram for ONE METAL ATOM and ONE NON METAL ATOM (between atomic numbers 1-20).

3) What is the molai* mass of lead (II) nitrate? What is the mass of 4.2 moles? How many formula units are in this sample?

Consider the Frost diagram of some actinoids (An) in aqueous solution shown below: Answer the following questions and fully explain your reasoning in each case. Why does Bk show only 2 oxidation states while Am, Pu, U show 4 different oxidation states? Why is the oxidation state +4 particularly stable for the element Th?[6] The oxocations AnO2* and AnO2²* (An = U, Pu, Am) have been isolated and studied. However, the oxocations LnO2+ and LnO2²+(Ln = Nd, Sm, Eu) areunknown. How can these observations be explained? Would you expect the following molecules to be observed? Explain your answer. CIF7 ArF4 Fully explain the origin of the difference in overall stability constants, measured in aqueous solution, for the two copper complexes in the table below.

1) Classify each equation Single Replacement, Formation, Combustion, Double Replacement, Decomposition. Predict the products of the reaction and balance each equation. Make sure to include states of matter for each product a) Classify: b) Classify: c) Classify: \text { _a } \mathbf{C a}(\mathbf{O H}) 2(a q)+\ldots \mathbf{N H} 4 \mathrm{CI}(a q) d) Classify: \mathrm{C} 5 \mathrm{H} 12(\mathrm{~g})+\mathrm{O}_{2} 2(\mathrm{~g})^{\wedge} e) Classify: A solution of chloric acid is mixed with a solution of copper (II) sulfate \mathrm{H}_{2} \mathrm{SO}_{3} \mathrm{Fe} 2(\mathrm{C} 03) 3 \text { CuCl } \mathrm{H}_{2} \mathrm{~S}

8. The dipole moment of HF is 1.92 D. Given that the bond length is 91.7 pm, calculate the separated charge q, assuming the point charge model.

I need an electron to be traveling at 0.970c. What potential difference should I use to accelerate it, assuming it starts from rest? Recall U=qV.

Complete the table with the positive ion , negative ion, and the formula for the compounds. Use the subscript(X2) and superscript (X2) buttons as needed.

QUESTION 1: You have prepared for the first time ever the XeCl3FO₂ molecule. Naturally the molecule can only be prepared at very low temperatures and tends to undergo instantaneous decomposition into its elements at elevated temperatures. a) You are storing 2 grams of XeCl3FO₂ in a sealed flask at 111 Kelvin. You decompose XeCI-FO₂ into its elements by raising the temperature in sealed flask to 20°C. (i) Write down the decomposition reaction. (ii) Calculate the minimum volume of this flask (in units of liters) in order to keep the pressure at 20°C below 3 bar.