Exam1.Yellow.S05

Exam1.Yellow.S05 - Exam 1 Yellow Version I Consider the...

Info iconThis preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

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

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

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

View Full DocumentRight Arrow Icon
Background image of page 4
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Exam 1 Yellow Version April 20, 2005 I. Consider the following alcohols and their normal boiling points. CH3CH2CH20H CH3CH2CH2CH20H CH3CH2CH2CH2CH20H Boiling Point (°C) 97.4 l I7 137 a) (3 pts) What types of intermolecular forces are present in alcohols? H- loamdfng mural LD l: b) (3 pts) What is the dominant intermolecular force present? H—bondl‘hg c) (4 pts) Why does the boiling point increase as the molar mass of the alcohol increases? LDF {increases as molar W55 .‘hcrcaSe> 2. (12 pts) Indicate the dominant intermolecular force for each of the following substances. a) HOCN H-f bonding b) 0C12 wpola du‘patz c) CHzClz Wade Magda d) xer LDF e) No 4.8m '(l/HEDLL 0CH3CH2CH3 L DF 3. (6 pts) For each of the following molecules, write the Lewis structure, predict the molecular geometry, and if the molecule is polar, indicate the direction of the net dipole. W molecular eometr polarigl . ' I' - Z a 7 ll 2" ‘ Z' 3) S032 .1 _‘ n ‘ ‘~ I \‘ :0-5-0. _/ [/ I H " ' . .O~ 0 O 96 valence e 3 :Cly‘ .Q ‘lv’\o 3 - 6 ~- , I 31' :3 bar/Wis irr‘tgomal Paar a Pbrawfioi . . “0" n b) N037 :01. X‘— \l mph‘Pola‘r '1lewde‘5 .. “ u .. /N \ I, 2H W6 “N ‘Q‘ {0‘\r sap—flit]: ‘llWMU ‘h’lg0lflfld a Flammr 4. (6 pts) Indicate the type of crystalline solid formed for each of the following substances. a)NH4N03 iamic b)H20 molecular c) Hg meta/MIC Exam 1 Yellow Version April 20, 2005 5. (8 pts) Circle the formula that best fits each of the following descriptions: a) Number of n-bonds in HOCN l i! 2 3 4 H'O'CEN b) Are all atoms in HOCN in the same plane? no I no /0\6\ \\\ N c) Highest vapor pressure HOCHZCHZOH CH3CH2CH20H H d) Highest boiling point HF HBr F2 ‘ NH4Cl H— loawWo/‘fl OUpoll LD r. ‘. amt 6. (4 pts) On average are the intermolecular forces greater in H200) or H20(g)? Circle the answer. ! H200) H20(g) 7. (6 pts) Rank the following from lowest to highest boiling point. NH3 CH3OH CH3F CH4 p “MO” C‘qu < CF13 F < NHS < CV3 P E/P' a 8. (8 pts) Draw the Lewis structure and molecular geometry for each of the following molecules. Lewis Structure Molecular Geometry H H ‘. ,, I N I O H-C-—0'-'C’H H\ / \ [,Jl CHgOCHg : H I “C /C_<i H H H H v H H C 1’ \ O I H g H . I H C CHgCOOH H'c/C gogH \C/ \O/H ‘ ll I.’ ', ‘x H H 4 Exam 1 Yellow Version April 20, 2005 9. Consider the skeletal structure for the following molecule. Draw the structure showing all carbon and hydrogen t . a oms 9 1 B H / C’U l’l \ (Ii—OH H\../C\ /H C G \ H y a / H OCH3 H/ \c/ \0~CH3 / \ H H a) (4 pts) Write the molecular formula? I C 8 ’V I2 03 b) (2 pts) How many n-bonds are there in this compound? :2 c) (2 pts) How many cs-bonds are there in this compound? 2 3 d) (8 pts) Indicate the hybridization on the labeled oxygen and carbon atoms in the structure shown. 0 Hybridization on n 5 3 3 $.0H Oxygen(1): ——P— , 3 4 2 Carbon (2): AL 2 1 Carbon (3): _5L OCH3 2 Carbon (4): _SP_ e) (12 pts) Indicate the approximate bond angles for the structure shown. Approximate Bond Angle O 10 or 10 of <‘067 e |C|—OH a —7_’ 7 ’ 101 ,0 a C ”\ «,QTCHs d 44L 6 I Q 0 f l 20 t) (2 pts) Are all the atoms in the same plane? Circle the answer. Yes No I Exam 1 10. Yellow Version April 20, 2005 (10 pts) A 0.72 g sample of liquid water was placed into an evacuated 2.00 L flask. The flask was then sealed and heated to 37°C. What percentage, by mass, of the water remained as liquid? The vapor pressure of water at 37°C is 0.063 atm. vapor ’— PV: n R T h_ Pv (0.06‘361/llm) (aooL) ' 7Z7 2 ' a -_ (0. 083106 Lfir)(3wlc) V1 : appulq; mole’s HZOM) a} 370C Haw/{01 +‘ . IW‘ - , I“.._'__,..swl 0 722 9( [39 2 0.0 H W: HZOMJ r‘eWIWWl/lg {nrhwl Vll’l20(j) Z HHZO('1) —' VlHl0(9) 0.0% mol — 0,0047; MAC'l :0,055 Wal “lam ...
View Full Document

This note was uploaded on 10/26/2008 for the course CHEM 1C taught by Professor Hooker during the Spring '06 term at UCSB.

Page1 / 4

Exam1.Yellow.S05 - Exam 1 Yellow Version I Consider the...

This preview shows document pages 1 - 4. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online