a) Write out the full Born-Haber cycle for K2S then construct the ladder diagram for K2S, labeling the chemical reactions and each enthalpy step. b) Next, look up the lattice energies for K and S and calculate the lattice enthalpy for K2S c) Use the Born-Lande equation to calculate the lattice energy. Use the Madelung constant for the Fluorite structure, assume only the average of one cation and one anion to find the Born exponent, and use an inter-ionic distance of 322 pm. Show all of your work.

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11 Dec 2019

a) Write out the full Born-Haber cycle for K₂S then construct the ladder diagram for K₂S, labeling the chemical reactions and each enthalpy step.

b) Next, look up the lattice energies for K and S and calculate the lattice enthalpy for K₂S

c) Use the Born-Lande equation to calculate the lattice energy. Use the Madelung constant for the Fluorite structure, assume only the average of one cation and one anion to find the Born exponent, and use an inter-ionic distance of 322 pm. Show all of your work.

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Hello, I mainly need help with 11 through 15 but I would definitely not mind more help. Thank you in advance

CHM2046 Revicw Assignment Wed Feb 22, 2017 Due: Directions: Write the answers to each problem on the answer sheet prov ded. However, to receive credit must attached the work on separate paper. You may work together on these problems. Be sure to yo include proper u ts in your answer. How many protons, neutrons and electrons are present n each of the following Cr Provide the systematic names for the following: a. CaCO3 b, Cro c. N20 3. Provide the formula for the following: c. iron (II) oxide a. potassium sulfate b. sulfur hexafluoride The density of gold is about 19.32 g/cms. What is the density in units of lbs/ins? 1 kg 2.205 lbs. n 2.54 em. 5. Nicotine is a poisonous, addictive compound found in tobacco. Its form a is C10H14N a. Calculate the molar mass of nicotine b. How many nitrogen atoms are in 1.3 mg of nicotine 6. Ferrocene, first synthesized in 1951, was the first organic iron compound with direct Fe C bonds the combustion analysis of ferrocene, which contains only Fe, C, and H, a 0.9437 g sample produced 2.233 g of CO2 and 0.457 g of H2O. What is the empirical formula of ferrocene? 7, Balance the reactions listed on the answer sheet. Be sure to include "1" as coefficients so each specie has a coefficient 8. One of the first steps in the enrichment of uranium for use in nuclear power plants involves a displacement re between UO2 and aqueous HF to produce the green salt, UF4, and water. a. Write the balance reaction If the reaction in part b resulted in 3481 g of UF4, what is the percent yield of that reaction? 9. For the reaction of aqueous strontium chloride and lithium sulfate, a. write the balanced molecular equation, including correct states of matter b. complete ionic equation, including correct states of matter c. the net ionic, including correct states of matter 10. Automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d 4 g/mL M-62.07 g/mol) and water (d 1.00 g/mL, M 8.02 g/mol). Ethylene glyco the solute and water is the solvent. Assume that the volumes are additive, calculate concentration in the following units a. molarity b. weight/vo me percent c. volume/volume percent Given the following data, calculate the lattice energy of K2O. Show work via Born-Haber cycle or Hess's law Enthalpy of formation of K2O 363.2 kJ/mol Enthalpy of sublimation for K 89.24 kJ/mol ionization energy for K 4.18.8 kJimol Bond dissociation energy of O2 498 kJ/mol electron affinity of O 142 kJ/mol 2'd electron affinity of O 744 J/mol

Practice problems for exam 2 ______________

Useful Information:

h=6.626Ã10-34JÂ·s.; c=3.0Ã108 m/sec; E=hï® ; E= hc , ï¬ = h/mv; 1J = 1 kg-m2/s2 ï¬

mass of electron = 9.11 Ã 10-28 g, ïE= q + w ; 1 cal = 4.184 Joules Please Show all Work

1. Which of the following substances have standard heats of formation that are equal to zero by definition (circle your answers): H2(g), H(g), O3(g), H2O(s), H2O(l), Hg(l), Hg(s), Hg(g).

2. Limestone stalactites are formed in the reaction: Ca2+(aq) + HCO3-(aq) ï CaCO3(s) + CO2(g) +

H2O(l)
If one mole of CaCO3 is produced at 298 K under one atmosphere of pressure, the reaction performs 590 calories of expansion work, pushing back the atmosphere as CO2 is formed. At the same time, 9310 calories of heat are absorbed from the environment. What is ïE in Kcal/mole for CaCO3.

3. What is the minimum wavelength of light in AÌ (1 AÌ = 10-8 cm) needed to provide enough energy per quantum to rupture the chemical bond in hydrogen iodide (HI). The bond dissociation energy of HI is 71.4 Kcal/mole.

4. Sketch the shape and orientation of the following types of orbitals: s, px, dxy, dz2, dx2-y2

5. Give the values of (n) , (l) and (ml) for each orbital in the 4p subshell.

6. Write the complete electron configuration for the following: Ti 2+_____________________________________ Cr_______________________________________

N______________________________________

7. Calculate the standard enthalpy of formation ( ï Ho) for diamond from graphite [i.e. C (graphite) ï C (diamond)] given that:

C (graphite) + O2 ï CO2 (g) ( ï Ho = -393.5 KJ/mole) C (diamond)] + O2 ï CO2 (g) ( ï Ho = -395.4 KJ/mole)

If 1.0g of graphite is converted to diamond, what is the energy change? Is this an endothermic or exothermic reaction?

8. An 160 pound astronaut on his way to Mars is buzzing along at 10,000 miles per hour. (a) Express his weight in grams (one pound = 454 grams) so that you can calculate the astronautâs wavelength (1mile/hour = 44.7 cm/sec)

(b) Suppose the astronaut detects outside his spacecraft a proton (m=1.7 x 10-24 g) from a âsolar windâ moving at exactly the spacecraft velocity. What is the proton wavelength is in AÌ (1 AÌ = 10-8 cm.

9. What is the maximum number of electrons that can occupy each of the following subshells? a) 3d_________________ b) 1s____________________ c) 2p ____________________

10. Identify the element represented by the following electronic configuration.

a) [Ne] 3s2____________________

b) What is the electron configuration for the first excited state of this atom.______________

11. Determine the number of valence electrons for each element.
(a) Br___________ (b) Na _________ (c) Sn __________

12. 175 g of Fe at 15.0oC is mixed with 225 g of H2O at 95.0oC. What is the final temperature of the mixture? The specific heats of iron= 0.448 J/g oC and water = 4.184 J/g oC). (keep in mind the following: heat gained + heat lost = 0 and q=mass x heat capacity x ïT)

13. (5 pts) Calculate values of ÎHrxn for the following reactions: CS2(g) + 3O2(g) ï® CO2(g) + 2SO2(g)

The heat of formation for the following substances is given in kJ/mol:

CS2 CO2 SO2 117.4 -393.51 -296.83

14. (6 pts) Use the electron configuration of Li and Be and determine which element has the greatest second ionization energy. Defend your answer.

15. Mark beside each of the following processes either âexoâ or âendoâ according to whether you think the process will release heat or absorb heat.

a. Ca(g) ï Ca(g)+2 + 2e-
b. I(g)+1e-ï I(g)-1
c. Ca(g)+2 + S(g)-2 ï CaS(s) d. I2(g)ï 2I(g)

( ) ( ) ( ) ( )

16. (6 pts) In each of the following pairs, which of the two species is larger?
a) O-2 or Na+ b) Ti+4 or Ti+2 c) B or C d) N or N-3

17. Write down the Lewis dot structure for the following (a) N_______________ (b) Ne________________

18. THE BORN HABER CYCLE: I may have a problem on the Born Haber cycle. Please check my lecture notes to see how to set up the process and then calculate the lattice energy from the various thermodynamic quantities such as in the NaCl example below;

ï H ï¯ f NaCl = -411KJ

Na(s) ï® Na(g) ï H =108KJ
1â2 Cl2 ï® Cl(g) ï H = 122KJ Ionization Energy of Na ï H = 496 KJ Electron affinity of Cl ï H = -349KJ

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