A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52

Compare and contrast the different types of chemical bonds and define the terms chemical bond, covalent bond (including polar and nonpolar), ionic bond, and hydrogen bond.

Balance each reaction, determine if they are ion-exchange, redox, or acid-base, and determine the direction of the reaction and if they are reverisble or irreversible and explain why.

NH₄ NO(s) – N(g) + H₂(g)

N₂ (g) + O₂ (g) – NO (g)

N₂ (g) + H₂ (g) – NH₃ (g)

H₂O (g) - O₂ (g) + H₂ (g)

CaCO₃ (s) – CaO (s) + CO₂ (g)

Cl₂ (g) + H₂O (l) – HCl (aq) + HClO (aq)

NH₄ (s) – NH₃ (g) + HCl (g)

Fe (s) + H₂SO₄ (aq) – FeSO₄ (aq) + H₂ (g)

CO₂ (g) + H₂O (l) – H₂CO₃ (aq)

Mg (s) + H₂O (l) – Mg(OH)₂ (aq) + H₂ (g)

CH₃-COOH (aq) + H₂O (l) - CH₃-COO^- (aq) + H₃O⁺(aq)

Write the formula of the coordination compound pentacarbonyliron(0)

Write a systematic name for Li₂[CoF₆].

Write a systematic name for [RuCl₂(bipy)₂].

Write a systematic name for [Co(NH₃)₃Cl₃].

9.) As mentioned below, you are required to design your own procedure for determining the heat of dissolution of your chosen salt with a coffee cup calorimeter. Answer the following questions and consider them in designing this procedure:

     a.) When you find your initial temperature T_i, should you take one measurement from the thermometer as soon as you place it in the water in the calorimeter? Why or why not? If not, what should you do instead?

     b.) Do you expect the temperature of the water in the calorimeter to rise, fall, or stay the same after you add your salt? If the temperature will change, will it continue to change indefinitely or not?

     c.) How will you know your dissolved salt solution has reached it's maximum or minimum temperature, i.e. what will you observe in your data to indicate this has happened?

     d.) Should you repeat your experiment? Why or why not? If so, what could you change from trial to trial? Give two possible suggestions, and determine which one you should change (as well as which one you should not!) in any subsequent trials you decide to perform.

*Information previously calculated is below*

1. Calculate the amount of heat (q) produced by the combustion of 4.05 g CH₄ (ΔH_comb = -890.4 kJ).

225.38 kj

2. Consider that the 4.05 g methane is burned and all of the heat from this combustion is absorbed by 1.0 kg of 20 °C water (use 4.18 g^-1 ºC^-1 for the specific heat of the water). What would be the final temperature of the water?

73.8°C

Estimate the pH of the resulting solution prepared by mixing 1.0 mole of solid disodium phosphate and 1.25 mole of hydrochloric acid. The pKas of phosphoric acid are 2.1,7.2,12.4. The answer is 2.1<pH<7.2. Please explain.

0.5 mole of a monatomic ideal gas is loaded into a cylinder and contained by a frictionless piston. The piston is set so that there is an initial volume of 2L. The gas in the cylinder is at a temperature of 298K. The gas is allowed to expand adiabatically against 1 atm of pressure. Calculate V/n initial, q per mole, w per mole, delta U per mole, delta S per mole and delta H per mole. What is the final temperature of the gas in Kelvin and Celcius?

1. What is natural radioactivity? Speak to the different types of radiation that an unstable nucleus may emit, and the different types of radiation involved.
2. Why is it important to be able to write a balanced nuclear equation for radioactive decay? Go into some of the specifics of what is involved in writing an equation.
3. What is a “half-life” and why is it important to know the half-life of a radioisotope? List a few applications of how scientists make use of having this knowledge. Why would it be so important to know the half-lives of radioisotopes when it comes to medical applications?
4. Briefly describe how we can make use our knowledge of radioactivity in medicine. Speak about the characteristics of the radioisotopes used in these types of applications. What might they have in common? What process(es) do we use to detect these radioisotopes?

1A. Determine the pH of a KOH solution made by mixing 0.251 g KOH (s) with enough water to make 1.00 × 102 mL of solution. Assume 100% purity for the KOH (s).

1B. Predict the direction in which the equilibrium will lie for the following reaction:     H3PO4(aq) + HSO4−(aq) H2PO4−(aq) + H2SO4(aq).    Ka1(H3PO4) = 7.5 × 10−3;

Ka(H2SO4) = very large    

2. For H3PO4, Ka1 = 7.3 × 10−3, Ka2 = 6.2 × 10−6, and Ka3 = 4.8 × 10−13. An aqueous solution of Na3PO4 therefore would be?

2B. Calculate the pH of a solution of 0.10 M HA- (aq). The acid H2A has Ka1 = 6.5 × 10−2 and Ka2 = 6.1 × 10–5.  

HClO(aq) = Cl2 (aq) E^o = + 1.611V

MnO4^-1(aq) = MnO2(s) E^o = + 1.679V

In a particular cell, E_cell is measured to be +0.038v when the pH in both half-cells is 4.00 and [Cl2] = 0.20 M, [HClO] = 0.10 M. What is [MnO4^-1] in the solution?

A student is given two unknown samples continuing two different compounds with the same molecular formula, C3H7NO, he annaylzes them by IR and 1H NMR

Compound A:

IR: 3366, 3189, 2976, 1662 cm-1

1H NMR: 1.15 ppm, 3H, t

2.24 ppm, 2H, q

6.21 ppm, 2H, broad

Compound B:

IR: 3294, 3099, 2946, 1655 cm-1

1H NMR: 1.98 ppm, 3H, s

2.79 ppm, 3H, s

6.40 ppm, 1H, broad

Identify the structure of each compound and justify your answer.

Use Molecular Orbital Theory to describe bonding in the following. Also find the bond order and decide if stable or not. Is species dia or paramagnetic?

i. C₂⁺   ii. Be₂⁺   iii. Ne₂

Discuss the nature of the three main types of atomic line broadening and include the relative magnitude of broadening for each. Also, discuss what can be done, if anything, to reduce the magnitude of each type in specific experiments.