Midterm-2_FormB_Solutions

Midterm-2_FormB_Solutions - Chem 1C Midterm-2 FORM B First...

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Chem. 1C Midterm-2 FORM B First letter of your last name: May 21, 2008 Name: Last Name First Name Perm # INSTRUCTIONS: No hats allowed. No sharing of calculators. Cell Phones, iPods, headsets, etc. must be turned off and put away. SCANTRON FORM: Use a PENCIL 1) Write your name 2) Bubble in FORM B 3) Bubble in your PERM number (7 digits only, no extra numbers) There are 6 pages, 21 questions. Each question is worth 5 points. There is only one correct answer per question. Turn in the Scantron form ONLY. 1. Identify the most important types of interparticle forces present in the solids of CH 4 , methane: a. ionic b. dipole c. hydrogen bonding d. London dispersion (see lecture notes and exercise 16.14) 2. Closest packing describes the most efficient method of arranging uniform spheres, so that a. the density of sphere per unit cell is the highest b. the number of spheres per unit cell is the highest c. the fractional volume of spheres per unit cell is the highest d. the coordination number per sphere in the unit cell is the highest (see lecture notes)
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3. X rays with wave length h = 1.54 Ǻ were diffracted at an angle of 14.22 degrees by a solid crystal of silicon. Assuming first-order diffraction (n = 1 in the Bragg equation), what is the inter-planar spacing, d , in silicon? a. 313 pm b. 413 pm c. 213 pm d. 113 pm (see lecture notes and exercise 16.41) 4. Manganese crystallizes in a structure that has a body-centered cubic lattice. What is the coordination number for Mn in this structure, and how many atoms are there in each unit cell? a. coordination number = 8 and 2 atoms per unit cell b. coordination number = 8 and 1 atom per unit cell c. coordination number = 8 and 3 atoms per unit cell d. coordination number = 4 and 2 atoms per unit cell (see lecture notes and exercise 16.42) 5. The unit cell for a pure xenon fluoride compound is shown in the following diagram. What is the formula of the compound? a. XeF b. XeF 4 c . XeF 2 d. Xe 9 F 10 (see lecture notes and exercise 16.67) 6. Which of the following is NOT a typical characteristic of a classic metal? a. Metal bonding is more covalent than ionic b. Metal bonding has no preferred direction so that they can be easily rearranged within a metal crystal packing c. Valence electrons fill up the bonding molecular orbital band with a small energy gap to the antibonding molecular orbital band so that electron conduction can take place d. Metal displays lower electrical conductivity at higher temperatures (see lecture notes and exercise 16.51)
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7. Why is steel stronger / harder than iron?
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This note was uploaded on 08/06/2008 for the course CHEM 1C taught by Professor Hooker during the Spring '06 term at UCSB.

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Midterm-2_FormB_Solutions - Chem 1C Midterm-2 FORM B First...

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