University:
Carleton College
Course:
CHEM 122 | Introduction to Chemistry
Academic year:

2022
Views:

89

Pages:

2
Author:

larbiwxcvbn

Hour Name Date Couqlent Bonding Reuiew/Prqctice Arrerment For each molecule, draw the Lewis structure, determine the VSEPR shape, bond polarity using the electronegativity values from your notes (nonpolar covalent, polar covalent, or ionic), and molecular larity otafltv. pr' oFz 5* 5tfl bt e(?)r 7Q =t{( € tL. '1. il .. ac 1t ;F_g_rt r. ,?( .t, VSEPR shape: VSEPR shape: Bond Polarity: {,1 Bond Polarity: Molecule Polarity: Molecule Polarity: BeHz ;1 2( t). 4 FI vsEPR r tt('l) " 34 1+5(t)= i{ A_ ,.{5ri ,b.l_ l, , ?f: hi'I ,.? VSEPR shape: MOnftlaf : Bond Polarity: 4, i0 -a. Molecule Polarity: ?O BF: 3t3(r) o' r/ . f: , ? 'ioni C - = 2L{ -6't': lc^nar VSEPR shape: Bond Polarity (l Molecule Polarity Bond Polarity: Molecule Polarity: 2')a (o+,.t(Lo){, e i-r cro3 Q: ..leI -\\/ -o: ,r rl lO. IA,f VSEPR shape: soo'- :f : :F-.in 3e * l-l shape: lirtOaf Bond Polarity: c(, Molecule Polarity: rBr5 TeF+ (a onic lr_ ff/Oh fn [r. rz c ?+3Lb)+1,2\o atl rr :o- CI-QJ I I :O: J :o: VSEPR shape: VSEPR shape: Bond Polarity: Molecule Polarity: Bond Polarity: Molecule Polarity: a^'I ldr 1 iTtlH;T"J"i? frans knd (ionic) o r sharnd (c ovdtltr4) (^) tll: sTAtslLraul trb GChieVp a futt oc]/c* ;ioil 2. Describe the relationship between bond length, bond strength, and bond dissociation "n.rgy.(6pF) Tr\0 shorb.r. {-,1.,.0 bond ,*l4a strvongt and +4ru hiq}'ur \r -{J^0 tsD€ ( ton$es* 'Silgto ) shor+rj{ -4;,pLr) Discuss differences between an ionic compound and a covalent cognpound. 3. 4*;sit; ;il"^o.dj), $ti (qood d,hadlbri+lle, "aI^i+c,t"f poorconducfur c.s asol',d hiqh vn.p i bPr -cortducfor(aq) ,fr v' r*'i'-e- . skrcren (a ngnrno*als ), litrrli d. or ea!, so6l, low hi,qh ,mp.tb.p. , pur un&,octors't n0dr/allg Name the folloWlng mVlecules:' covnrrruf, o- 4. a siF4 Sitrco; U*oFtuorid0 b. rv,sa dinilro g*.Fr 4rri SOltft fu c penta Flaor''cLp d. poou*?'traP hosPh or.qs rr, lodine ' hexoxi d0 5. Write the formula for the following molecules: a. Diboron hexahydrid bat* t, " b. Nitrogen tribromide N 6f a P*03 d. Hexaboron monosilicid" BU 3 c. 6. Diphosphorus pentoxide ldentify exceptions to the octet rule for Lewis structures. H, s{riva to; l$?onn3il.HJn i3iryt, covateril bond) v aLan u e- ) lond s (.Ll ll furry 3 co\ralzr* bond.s ( b val *i e- ) 6;i p, s, cr, s", B'., I' ro0m .FD,', r'r';o(gt t{ran E Vatqn Lo-Q-:Ci"fuZ1*-ran L{ c ova\ ut+ DOnd-;> 1 " A Be & B: Be urll l-Forrn 2 c ov aleln+ How many resonance structures are possible for COa' 7. Describe how the ? J C-O bonds of CO32- compare to a double bond in terms of bond length and energy. GO bonds in CO"a- Gre. lonqu and rec6,s\re .te33 io Wtc^L +atfan d orlbb boncl- ) ffifiU ,rrii#e a- ayQ*no'l-shared c1uallq . Or,t - rylorn i s 5-(highv FN) and ono ahrn 1s SP Ctodw tN) ?,tnerq.4 C,rr eak-tr) 8. o oescri##olar bond. 9. Explain how electronegativity determines what type of bond will form between two atoms. i; OiFkrsnLos (cova\r,r+l-) or / o,=n0nplar ?N dgl*{rni,\, i( t- will b4 sha red \rans ftrr td ( ionic) O.5- l.J = po\a r covc:lcr* > {. ? ionic