{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

105a_Practice_Final_key_3

105a_Practice_Final_key_3 - Chemistry 105 A Final Exam Dr...

Info icon This preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
1 Chemistry 105 A PLEASE PRINT YOUR NAME IN BLOCK LETTERS Final Exam Name: __________________________________________ 05/09/08 Last 4 Digits of USC ID:_____ _____ _____ _____ Dr. Jessica Parr Lab TA’s Name: _________________________________ Lab: W 1 / W 4 / Th 9 / Th 1 / Th 4 Please circle lab section above . Question Maximum points Score Grader Question Maximum points Score Grader 1 10 11 10 2 10 12 20 3 12 13 14 4 12 14 10 5 8 15 8 6 8 16 8 7 5 17 10 8 5 18 10 9 10 19 12 10 10 20 8 (Sub-T) (110) (Sub-T) (90) TOTAL 200 Please Sign Below: I certify that I have observed all the rules of Academic Integrity while taking this examination. Signature: __________________________________________________________________ Instructions: 1. You must show work to receive credit. 2. If necessary, please continue your solutions on the back of the preceding page (facing you). 3. YOU MUST use black or blue ink. (No pencil, no whiteout.) 4. There are 20 problems on 17 pages. Please count them before you begin. A periodic table is on the last page. 5. Good luck!! =) Final exam viewing on Mon May 12 and Tues May 13 Sign up for 15-minute viewing appointment on class website. First Letter of last Name
Image of page 1

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
2 1. (10 pt) Consider the following phase diagram for sulfur, which has two solid phases. a. How many triple points are there in the phase diagram? ______________________ b. Circle the phase that is the most dense: monoclinic or liquid c. What phase will the sulfur be at 1500 atm and 100 o C? ______________________ d. What is the normal boiling point of sulfur? _______________________________ e. What is the normal melting point of monoclinic sulfur? _____________________
Image of page 2
3 2. (10 pt) In the ground state of xenon: a. How many electrons occupy orbitals with n = 4? ________________ b. How many electrons occupy d-orbitals? ________________ c. How many electrons occupy p y orbitals? ________________ d. How many electrons have m s = -1/2? ________________ e. How many unpaired electrons are there? ________________ 3. (12 pt) Fill in the table below assuming each column represents a neutral atom: Symbol ( X A Z ) Protons 25 82 Neutrons 30 64 Electrons 48 56 Mass Number 137 207 4. (12 pt) Give the ground state electron configurations for the following atoms or ions. Cu : __________________________________________________________________________ At : __________________________________________________________________________ Rh 3+ : ________________________________________________________________________
Image of page 3

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
4 5. (8 pt) The two naturally occurring isotopes of rubidium are rubidium-85, with an atomic mass of 84.91179 amu, and rubidium-87, with an atomic mass of 86.90919 amu. What are the percent natural abundances of these isotopes?
Image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.