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CH110/120 Assignment #5 Version A General Instructions Specific Assignment Instructions:    Your student number has nine digits: 123456789

Chemistry

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CH110/120 Assignment #5 Version A General Instructions

Specific Assignment Instructions: 

 

1. Your student number has nine digits: 123456789. Replace the numbers that are bolded and highlighted in yellow with the corresponding value from your student number. For example, if your student number is 009820864, then:

 

0.123 mol/L = 0.009 mol/L (this means that 1, 2 and 3 refer to the 1^st, 2^nd, and 3^rd digits in your student number)

0.456 mol/L = 0.820 mol/L (this means that 4, 5 and 6 refer to the 4^th, 5^th, and 6^th digits in your student number)

7.89 x 10² mL = 8.64 x 10² mL (this means that 7, 8 and 9 refer to the 7^th, 8^th, and 9^th digits in your student 

                  number)

If you do not understand this instruction, email your instructor with your student number and the version of your assignment, and your course instructor with clarify these requirements.

 

2. For Q1, you are expected to identify at least four problem solving strategies used in arriving at your answer. You can find problem solving strategies on slides 6-8 from “Directions_for_Groupwork_and _Problem_Solving”, under Course Information on MyLS. You are not required to do this for Q 

 

3. For Q1 you are required to identify a relevant course learning outcome. These can be found at the end of your syllabus. Please do not make up your own learning outcomes. You are not required to do this for Q2.

 

4. At the end of your assignment, you must rewrite and sign the Academic Integrity Pledge.

 

             

Q1) LCl₃(s) is the ionic compound formed from chlorine and a metal with the form L(s) at 1.00 bar and 298 K. 

1. Draw the Lewis structure for LCl₃. Assume that all the valence electrons from L are required.
2. Use the following information to determine the third ionization energy for L.

?H_sub for L(s) = (78 +100) kJ mol^-1

First ionization energy for L(g) = 456 kJ mol^-1

Second ionization energy for L(g) = (456 + 200) kJ mol^-1 Bond dissociation energy for Cl₂(g) = 244 kJ mol^-1

Electron affinity for Cl(g) = -349 kJ mol^-1 (Note that this is a negative value.)

789	+ 3000) kJ mol-1  (Note that this is a negative value.)

Lattice energy for LCl₃(s) = - (

?_fH for LCl₃(s) = 693 kJ mol^-1

As part of your problem solving you must show the full equations with phases for all steps in the Born-Haber process, and in your problem solving strategy, you must label each step with the words in bold found on slide 14 from “Introduction to Ionic and Covalent Bonding Part 1”. Note that you may need to use some of these labels more than once, and that these labels are your roadmap, which is only one problem solving strategy. You will need to include three more.

Your student number
Problem solving strategy	Problem solving
State one course learning outcome achieved from this activity.

Q1=3.5 points                                                                                    Insert extra pages if required.

             

Q2=3 points                                                                Student number:

 

Q2) SCl₄(s) is synthesized from the reaction of SCl₂(l) with Cl₂(g).

 

1. Draw two Lewis structures for SCl₄ and include formal charges on atoms with non-zero values. One must be the best Lewis structure based on formal charge, and the other structure must obey the octet rule.
2. Write the balanced equation for the synthesis of SCl₄ from SCl₂(l) with Cl₂(g). Based on the best Lewis structure determined in (a), determine ?rH using Table 9.1 and Example 9.5 in your textbook. (This is not ?_fH, so all stoichiometric coefficients must be whole numbers.)