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Chemistry 308FINAL EXAM REVIEW

-?

gi rtant Notes:ImpOrKan

You will be provided with:1(1;3Qe

Periodic Table

Prefixes (covalent naming)Organic PrefixesFlow Chart for IMF's

Ion Table

Electronegativity TableOrganic Suffixes

Mole Road

Solubility ChartGas Laws Formulae

Unit 1 - CHEMICAL REACTIONSWhat you need to know:Review Concepts

Determine whether a compound is tonic or covalentDetermine numbers of protons, electrons, and neutrons in a compoundName tonic compoundsName covalent compoundsBalancing Chemical Equations

Percent CompositionDetermine the percent composition of any atom in a given moleculeDetermine the percent composition of water in a hydrate

IsotopesWhat are they?Calculate the average mass of an element given the percent abundanceof its isotopes

Moles

What is a mole? Why do we use them in chemistry?What is Molar Mass? Where do you find them?Convert between moles and numbers of moleculesConvert between moles and grams

Empirical and Molecular FormulasSimilarities and differences between empirical and molecular formuiasDetermining EF based on percentagesDetermining MF using EF and Molar Mass

StoichiometryUsing an equation and a known amount of one substance to determinethe amount of another substance

1

Some example questions:1.,oo 65 ,,1 a,1) Fort eatomrepresentedby zn30 etermrne.

a. Numberofprotons - f'=30b. Numberofelectrons - '6-=.3ryc. Numberofneutrons - (,,q -3@ = 3r- n

d. Atomicmass(inamu)- ,S,,,,

2)

)

%i-i : ) ( ?,6( y! 1%. 3)rFlnda. :}%?eap(e0rcHe)n,( cosm,p. o7.l :ilo. nA IjOT eba.chsa:8om inXh,ee{oll:Jowl,Iinfg : . (, (1. . cO) J /'rl ? ti f ,. b0 7,llnL.? ,T,???J,,n c!,a,!.t,.'-,.a((vll,:cs):,?T. x? (II(IC,)],/1. o../:(7. .:,'l?.l?.oo.l1'lJ:,n"x:0(01?',??":J,"' tna/.7'/.lG5/Yl l t 'l,, a lj/h

'/?<Ca=g. J/n>Iag?/,=5a?q,i)q'/- E' ( / 'i ?"O S ' h g i @ L1 l/ i' ??7'l.rc3tn , o ,2 ( il,uc'izh 'T lg.1,(2,=:..2(:i'l,'Juc53jn'.l'l.io.)ix)Xicc'i='l31'X! ?'C'j?4) pnd the percent composition O! water in the hydrate CoCl2 o 6 H20.

t(lr.ail xmat = 'K.q-g7.'l 3al , '? g7n

-/-F= S':2.S'?'/.

7= t-i,@ -=

5) What is an isotope? How do isotopes explain the non-perfect m,asses of thee'lementson'theperiodictable'). rtv: c-i :mc? f';>rm*a c-' t?!xt ta,, !"We,-

clc?JereJe.ltwe'v?it 'RJcy't cmtaivr -e7pot n'um6e;ya (7'F ,p."oto*i,5 9cciH,? ,t'e'7Ja-( Vlll?beri' vr'yD;'OTO*l*i' bLlr Cl{'ytt'. 7' Jqe marsc-r eF e(lLln -e?lewv-br €4 , f4aieyy'vw!e?rs vf ncpy'n-eqsa.

- r(,y@':i'5kecL ec?rQ!'e (-?F ckll 'ysU'*c;?eJ,inclut.li'vsjc %l4@;',"((l@,%'y?€3'u?ht(o'iy6 (l i(4 vicc.

6) Chlorine consists of two major isotopes, one with 18 neutrons, 75.77% ofchlorine atoms, and one with 20 neutrons, 24.23% of chlorine atoms. Calculate ,?he ayeraae a(om!c mass of'a chlorine a?0m. 35 (' { (,?'l- 7 q ? ' 7 7 s/. ' a3 1 (' l (y f?theaverageatomicmassofachlorineatom. 35 C ( ,-l l.r,-1-H, @ 31(l (,

3 s-' c-,?a K .1a;'- 71 '/a 1 :3'lob?ui )(a al 'l o "'lec -ta, i ec o{.

26, S-l gr-avviu f f. g6r ? ctmv :

'3q,33'}=

36', V ('yhtlA

Name Formula lonic or Covalent?

'br'rari 'iTiffi[Thik BBr3 (:

lron (11) Phosphide Fe,.. P, 1

Disilicon Hexabromide-'4r-atiJ I Q- D 'o( (/

t kn,wii itm(iia ctx*mitx'fe Cr(CO3)3 ' l

-ltaac{ (i-il X (';: l!iJ ' - PbS l

Copper (I) Phosphate C*POq i

7) What is a mole? whyisitusefulinchemistry? A mcle.. iJo G-O.lXIO"rF, %-( <s 'bssc(xk 'r cslc"Jste., oy>t"unaPy {/l ( uew<gatt7-any f!ai n <-

8) How much does one mole of Boron atoms weigh? How do you know?

ct F e leomevi?U'.

=J:..:..,:.-.,,,:2 2 1:, ,l,, . ,,;=, e,,fl (:;,r: i-.,i,, ttLlJa!9) What is Avagadro's number?ft;vxd ;vt i mc;ic eF7 ty ,.s-ddttvtce, ( <hi?f- rsa 'ttta nuwber t>F @y)??r- jh 'eX(,e'tlsy il j)?(?'%J''=?rtyv'i<kar.4 C;Ccel?eck % Sciev'i'tid4sz+r,?ir{61ye4"(l@ ,10) Calculate the number of moles in 2.06 x 1024 atoms of sodium.2,cCxioa2'ci+o-ws : 3A-xmc(

r.02Xta". ...3aa+?.4( i" l

11 ) Calculate the number of molecules of AIN3 in O.46 moles.

0.!tvqetet X j?,;f%l?ql,zc,,3e.x = 23)(1@?3mci-ecai6i%l'k.

12) How many moles of Barium are present in a sample having a mass of 22.3g? 22&3 7 A i?col = e-lbal 'cli

13a7. s

13) A chemical reaction requires 3.7 moles of Boron. What mass, in grams, ofBoron must be used in the reaction?

3,"7 n X .$ = '40. Jn

14) A chemical reaction results in 57.2 g of CO2. How many molecules of gaswere produced?

S7,1! : l- 3(JQ, Vkcl l 3(70Mcl )( (j.01X,}d" ;4tV]ecA't((:?p7

q4,c(3/yHciyH c l

7. g 1 X ] O Z 3?hto re ca(ey

3

15) Calculate the mass of O.025 moles of ammonia, NH3.

0.62?n K 11.0,'3'lclJ'l

,.-c,q3)

16) Calculate the number of molecules in 12.5 g of Nitrogen (N2).

,,s L1 ? .K 6.(3????ly,?(oi'm?lttuies = 2.09 A ra '3*tlecJesQ)71(j AJ }),, j/)A(7(

17) What is empirical formula? What is molecular formula? How are theydifferent? Are there any cases where they are the same?

,,e!,';- i j' +lle lav4esT u'i'vtcAe 'ry?t0@.( r tdaal'o oF "-rJ' !'l 01 a co'4xOtwrido- , IL,,?,a.a,',?F J'r' r': ra,:c--f'u3{-'W-LA;vk?p-er vf 'CtW3' CF ectclx S(J?e /'O Oi? C?Cru)ncl

ctrva(evi'rky 6cnaecl dI-f'?S ,.H, (' , i r U(s'{d phly 'w' r c.trvalevi'; (yb (- = vi (-?ui!ipn C(rVdllee:VpL*-l?Wa'mr , F . uU'ken cvva(e'nt c?@ctty:nck 6acvex a vu,n recjkucs'bi-b

18) Determine the empirical formula of a compound with the. following (o> flo@ ,6 (5 (,,a .,+t%, .ri.compos,ition b.y ma?+S: 48.0 1% C,, 4.0,% H. anod 4h8.]O o/o, o-, l ....?t4g,(B;1. X ,e,-'i, ,,Q

' S' a o o/' ? X i 'a a' X ]-(ffC' s saqle. ! iffoJg X .j,.?, 4,,.. l(]'-t"j, j6. (,rO

tw/? 1,oe&:)l = 3,ticn 0Io'c"l'. i:2,GriJ = 3.'?7nalf'= qauuz?19) a) Determine the empirical formula of a compound with tHe following. C 0 m p O S al t jo n, b J T a? S S a-? ,ie o. i- O oA. C - 12 - P oA? H? a n d.. 2a8 /- 0 ' oA N - f ?n C. '?? a , s'a? n H : S'aIJ q s.. -

a?,(ffi:1'===I='::"-.u C- < i g v qioeo? -i

'N t onN -t-!CH

'l,r(,) ])€b

CqHia.N1kQ Xl

i,7 '% crm'hnv'ek?')

3(r @, '7/?)16'Cq/v(

formula? M', c',- pf,b) If this compound ha?s a,,molar: "::,&amo ' a' (,,":':.o. '.,3',o-o 'r?: ' ::=hai: ' L '3=.".. '=:"ioJ%

mciecgicrr" 9r'mu(a €s Cts; H3(', Af G' tOO.l(ri6..l?

/1

=s-nC-

?'C -? i-j ?M = ( - 3/1 (,I ng

Cl'l.O/,J /-3 lr'3

<.y aY3

C'l'fi

SC

20) Balance each of the following equations and determine whether they aresynthesis, decomposition, single replacement, double replacement, orcombustion reactions.

a) l CuSO4+ :2 NaOH-) I Cu(OH)2+ l Na,?SO4

b) / Os04+ 2 PtCl4) L Pt02+ l OsClB

c) l CF4+ '1 Br2) / CBr4+ 2 F2

d) L Hg212+ ' 02) lHg20+ 2 12

e) l Y(NO3)2+ ! GaPO4) ' YPO4+ l Ga(NO3)2

f) ' C7H16+ " O>+ I CO2+ 11 H20

g) -3 c+ff Hz-) l C3H8

21 ) Write the correctly balanced chemical equation for each of the following.

('4i-(l. ?-( C(>,-) (?a,QoJ. ?-f tf,Ga) calcium hydroxide + carbon dioxide -4 caicium carbonate + water

l..(m + ca, -+ [t-i(?o3b) potassium hydroxide + carbon dioxide -> potassium hydrogen carbonate

-: H,5 + aPbci3 -> (i-tcl -+ih2S3c) hydrogen-sulfide + lead @) chloride -) hydrogen chloride + lead@

sulfide ->?

'S'

(?22) Given th4dlreaction'/Fe + SB -> <iFeS

a) What mass of iron is required to react with 1 .8 g of Sulfur?

O o.ec7ti yl r, X p??2??'e?@.1,'go, 0 . 00 -70 mal

== (},0S G vht=t F';L i' sF32.Ub =?hX gj

(3J;S c-ouvi K rr.€s-1 = 3.iJ

23) Potassium reacts with chlorine gas to produce potassium chloride.a) Write a balanced chemical equation for the reaction.

0 1 K + ctL -;ikCib) How many grams of KCI can be produced from 5.9 g of K and excess Cl2?

C.??' r? '1 . = 0. vs-set l( @ c-ir +'i t< X ?lVl xct = c.is-n Iccl'l? i

43.so2 In .,' 2 s l((?- a,lrn kcl )( Pl-?;'-J . il

/l)

/

c) How many grams of KCI could be produced from 16.00 g * Cl2 and excess K?',.,

(,, I"-oo'? . 0.?i5'7r, c(.i @ 0.'i2s'lrt Cl,x -litl(C%2 C=,r.q0 /,)

l(c 1, o. '{S'i3

(---- ------{a-" o C?-)(e '/ S73n X. $ = 3 3 , Q r sri

tJ4

/1

Unit 2 - GAS LAWSWhat you need to know:

Describe the basic principles of Kinetic Molecular TheoryDescribe the idea and conditions of STPConvert between units of pressure (mm Hg, atm, kPa)Conveit between units of temperature (K and C)What is a manometer? What does it measure?Solve problems involving missing measurements on manometersBoyle's Law: Describe the relationship between pressure and volume anduse it to solve problems (PIV1 = P2V2)Charles' Law: Describe the relationship between temperature and volumeand use it to solve problems V1 a'j

T, T,Gay-Lussac's Law: Describe the relationship between temperature andpressure and use it to solve problems Pi = P2

Use the combined gas law to solve problems PIV1 = ?4T, T2

Some example questions:1 ) Determine the missing value for each of the following:

X kPa105.9 kPa X mm Hg

%

X atm

Ans. (A) =

gaii'fi':';;;>"'irl"ii'pi =.Voa- q (4 m % uj= /Sl if ('cx ='f),2e

k('cr

p()p:J:' =s '9%'h'w'.,"' A Igt)6y '= (':j'?aa::'a"'

x = (ls-y -tty zo)i< (,o,X= tto,i<Pa

95 mm

Pqtts > 9a:r3ctS'>

!qasa = Pq ?f?m a+-Jir(y,sa =25-),'tida 760,?xnxffy':'?lf?=9ial3zrkP.

tt:y q s-mway idKi { W 'l iuwilj = (ahii tf'l

?% Q

Pa?%m -gq$,,,,";}, laKmmll)

844 mm Hg

7

2) Assuming only the parameters given change, what happens to:a. Temperature, if the volume of a gas increases?

'ttw'p-e?'hyr-c inctec5se?.S'b. Volume, if the pressure of a gas decreases?

ylvre- :nc(ecqe.xc. Pressure, if the temperature of the gas decreases?

(ir-esswe, aect-eccses

3) Convert the following temperatures to Kelvin.a.?'23'o'C'-h'2'Th"3' ?""v?b.?-42o-C"l'3';'3" c. l20oC X....lK ?* 21321tK aat k ioC

3qJic

4) Convert the following pressures to the unit indicated.a. 1 .75 atm to mm Hg

X .'T(co wimlj = I'3:)ci WIVIA?-si. ?S- s?ms{afx

S

c. 156kPatoatm ,t!,-(,

b. 720 mm Hg to kPa

7 ;,10 ;,qm% 3 )( . l0,].F :S.?I ,K,llJo. = 7/f, (i(i g '?q @r % k ('(4?'?'?<h o a? M 14.) ?/kPuKi

kf==

-i.S-Llethm

5) What is STP? What does it stand for, what is it used for, and what are the

valuesasso.ciatedwithit?'. S4anc'lord %emygttcta%r@,. ancl @te!!txte..cvnciia+i'evu' Tyi,yts-e' usca m '5vs ?tat-cvy ca(cix(a-afiaowy,

l 0'C

6) If1 A,.2>.5 L of nitrogen at 748 mm Hg

A. A -'at 748 'rrim Hg are compressed to 725 mm Hg at

constant temperature. What is the new volume? 7)j'-

Pi 'a '= po> v, i-1, < V,X 11@.S-L = iqs-'rvtvyshl K ll-s7q;5a ntmH,"7).5-mrs7X- vhh

l/, -zg.:>L

ViAr'

04Lv"

-?V, 1,7) lflO.O liters of oxygen at STP are heated to 51',;? oC, what will be the new

volume of gas if the pressure is also increased to 1520.0 mm of mercury?v, - ff .- v', v, P.

l i,I ' g?7&(jmmH.>ai'}-€JL -= 75-20,Ovviyl4cXVx- I ),i Ja731c (.rixac at)i33r

i,'tatl/,?Dl ->P,

8) The pressure of a gas is reduced from 1200.O rn'm Hg to 850.0 mm Hg asthe volume of its container is increased by moving a"piston -from 85.0?mL'J,

ptem.,aso.o mL. What would the final temperature be if the original'J> (temperature was 90.O oC? {1 (,:r , 0 'V

-T al I - 'lol-T,'aT- .-/,

q a g s-,. a r4(?i 2 do .ci )%ml-l (1??: g(" lv '-c -tr ,;l 13?,) ((

V, 74,4L

?11.5)MW L

-tQ!!a . C/ 3 2 k-' = 'lct '7gci'rml?8 'S?) = Q wsm 14 q X 35-6 ,C

ffl

Tit

lcSfl7j

10(iO[T, Cr

9) If 15.O liters of neon at 25.O oC is allowed to expand to 45.O liters, whatmust the new temperature be to maintain constant pressure?

./'

T, 7,-/S-.OL

.S oc tx 13 )}(

Ll§-,Ol,-

T,'l,-? (-fs-,t{,. ... .,ffqt4{(

, -l0,(i5133<4l?-[

%, P.l,pi,(510)A 40.O L tank of ammonia has a pressure of 12.7 kPa. Calculate the

volume of the ammonia if its pressure is changed to 8.4 kPa while itsP.temperature remains, constant.

Pl Cj" ?A Ca/:x?12,1[f(,?){ ?J!>.C:'L

0 % ?

S .1 k (q !:?Sk rq

E = 'l K (' (( X 'A

gr :' 0(;@?

q

Unit 3 - SOLUTIONS

What you need to know:Saturated, Unsaturated & Supersaturated solutions: what they mean,similarities, differences, how to make themHeterogeneous and homogeneous solutions - define and determineSolute, Solvent, Solution - define and determineRead a solubility curve and use it to answer questionsWhat is Molarity?Use the molarity formula (c = n/V or Molarity = mol/L) to calculate theconcentration of a solutionPercent volume by volume and Percent mass by mass calculationsGive detailed instructions on how to make a solutionGive detailed instructions (and show calculations) on how to dilute asolution

use a solubility chart to determine whether a given compound will dissolvein water or not

use the notations (aq) or (s) in a chemical equation to show whether acompound will dissolve or notWrite Dissolving Ionic Equations, Overall Ionic Equations, and Net lonicEquations for a chemical reactionUse Stoiehiometry (the ratio between compounds in a balanced equation)to determine how much of a product can be formedIdentify a limiting factor and use it to determine how much of a product canbe formedCalculate the concentrations of remaining ions tri solutions after a reactionis complete

/i

Some example questions:1) Describe the differences between unsaturated,

supersaturated solutions.7;l':';';2::(c4::'({:s'oalv-e, in f'!e? soive.nT%0

u n ! a'k recte cl - mvr'e 5,'?IM(?.!lf."Mo'cX"LHA-?LkK j oaF S'v(ut e r :>' rlj S'f'dlvc?t{ m -elexrtzt-e?ck ?ks,p6.4*l,H

S' ccrrahJ - '2'lA:keon a,/t- yc.?f?ur<tt? !plwh'c'2 cxf wss ! (ic rasshsrxre J 4r= ; ra+t=l:'I?ccele-c(-'a;b( 'rlvt tX,CeSE S'OllAk (;'eVVVksrB ilY(iteC.ter

saturated, and

r-(

2) What is solubility? How do we indicate in a chemical equation whether ornot a substance is soluble?

yF ts J'ttbr-(xn(7 % Cl;tSrc(vec a,(7act?t7(;e)vb[e .J"Ub!A.tnc.e., 25 refrer(A'Fei a-' a(7Uec!'l4-!;o -

C, H,(,, (S) ?-+ C< t-Itio( (cl)

5a{vevy'J.m (X77,t

,4

J?t>iecp(ar( ' ?() ?????Un

](Jn'i'(. Ct"WlfOLl&'ld ?Nae.l 7)??Nf(3i?7 ) + C I (b-y )mq- ;lJa

i4-=C-V

(!UHy );ffl'F' C'7 'a /a. I?ai.qll...2)l/?or'3) How many grams of ammonium sulfate a"re required to make 5L of a O.5

M solution? @,( ?nxcl )( S-L = a,r?v)L

2, i wycyl K ]')l.l4'l '?,yla'l (tl

) Bo.')Mn?4) What is the concentration of a solution of a solution with a volume of 2.5 L

and that contains 6.54 g of calcium phosphate?

=)-,b-l

n:c=u5) Explain how you would make the following solutions. Include directions as

to how to do !t. Ui NO :3a) 250 mL of 2 M Iithium nitrate

2 fiil X 2';?'77 zt L- * Sl>C' Yh*icii K d7)

-.} 43 eo M3

. 0..00 8q 'IV{

b) 2.5 L of O.75 M NaCl

0,7r 4 y,2,<-L = /, g'l': hy4L

i x, 4 . llOJc;{ . i C)= 3'l'i7r YK5 lS'??;[1J

b ' ?" ? " a "-j eL) ii':io'!iu'ie '2'5'l""'Li:%,'v vi?'sy':':oc"?H?0,?' ?:f?a(ho)::aa'ioB???':i:l?iavo"iNlili'o'i":':o,'fi'l'!':'F"']??'c:a;?'-'is the concentration of the solution?

C', 5yA" a ?:2 s-a asa'L,??o = C 2? a )- c>? '? C-C,= c).cGzs-M or- c.o5R

7) If I had s mL of 12 M sulfuric acid and l added 105 mL of water to thesolution, what would be the final concentration of the acid?

/2 -/'1- X-'r -hx L - '4 ' Q r o (.a 'o S' + s??-) s LC, : 0,J;5-M cyr C,S M

8) Wh3ch of the following solutions would generate an insol?u51e precipitateell combined with a solution of calcium chromate7-

%

* S4mmoniumhydroxidy @ Potassiumiodide * 'Q.odiBmcarbonate?.>

it

Use the solubility curve to answer the questions below. Be sure to include units!

150

,An 'X 9)a. What is the solubility of KNO3 at130 =-J

' as %ll,,C)'480H wR&.gazo(!)a.

???"d'A

?A

c. What is the solubility of KCl03 at

soocz q l q]

d. What is the solubility of Ce2(SO4)3 at

(,, (.1sooc";>

60

30

NaCl'Th- l

J

20

10r

-7-i-.ce,, (SQ4)3//

00 10 20 30 40 50 60 70 80 90 100

Temperature (oC) /

10) At 40oC, you dissolved 10 g of Ce2(SO4)3 in 100 g of water. Is this solution saturated or

Sa%rcSeJ ' ('.oirt{y J1 2) a'issalvvs)unsaturated?

X

b.Howdoyouknow? bec?re, 'f?!e. ?g @(owOiBvxt- f?krsr ca?sre?tv'sy ctvdirhibot<':]clisroki,rt o,-t Liooc i.S 7 q, S'0 3cai -J

i'F ytr e y %o )x+e-k'- '?(1)11 ) a) Which compound is most soluble at 40 oC?

b") W' hich is (he l'eas( soluble at 80 oc? C e ';l (70?a?(1)'?

e,>gci ,< xvcL= L}@ mmclL

? y'tcac /YIL = 7(I! /)l)1L

12) 200 mL of O.2 M sodium sulfate solution is combined with 700 mL of O.10M of silver nitrate.

a. What is the limiting factor in this reaction?b. calculate the mass of precipitate.c. Write DIE's, the OIE, and the NIE (ICE table)d. Calculate the concentration of all ions in solution

=' :;a;'=:-i -:.N.q"-) a I,c=hav ) 4=,Fi,-h .5j,+,l,, ,137(,aJ(3 ygcl

(5':r<= yr,+ t so,' t2/!t-q q Ja3 ? x,2 SO,,J + x',t + so, -

NA..C - 'l ] 5??+ "O=i 2' ??' ? 4 3 x S (" ti ;X 70%Yl 'IOma o

Q -70M'( - 3':r4 t 3SWt}l

?3'- O 5?g qa.'Sa'?'X?. 3 ? ' = € G as X' .za ??? i o . q 2 ,/1 IUQQ;Haa

@r- l!2)r', +-T(??A53?= C'q

'[?,}(1! ?), S-mn-- = 0.oo'b€fl crr U,tiO(,y4

FC! +2CO S%(.

[J'ia+ ?. y6mhcA -? c.ognMar- c..olxl')' Q(,r vu L

Tezyi = Ozol€hgr- (].q IVITrro l7s0 va(.

}3

Unit 4 - PHYSICAL PROPERTIES

What you need to know:How to draw Lewis structures for compoundsWhat does polarity mean?What does electronegativity mean?Determine whether or not a bond is polar and indicate using arrows or snotation

Determine whether or not a compound is polar based on its bond polarityand shapeDetermine which types of Intermolecular Forces are present in asubstance (Dispersion, Dipole-dipole, Hydrogen Bonding, Ion-lon) giventhe IMF Flow chart6etermine which -compound will have thei" higher melting/boiling point,volatility, and vapor pressure based on IMF'sDetermine whether a reaction is endothermic or exothermic

Analyze a heating or cooling curve to determine melting and boiling pointsAnalyze a p!iase diagram (include critical point, triple point, normal meltingand boiling points)Analyze a vapor pressure diagram and relate to IMF's

?qiWi

Some example questions:1 ) Draw Le*is structures for the following compounds:

a) CCI4 b) H2S c) CO2 *I ,Jl

@ ':? () -. O:cl:-k

-cl-C-C?-t

?i). l < i

= C(:€. /

/l

(*

2) Identify the main type of intermolecular force in each compound.b) Carbondisulfide CS,,?'?., a) NayQP??='=T 'g ?C' l 'i???ei d !ii

5; , (2 -=? S, § (..li?':perK'C<Jgs-t 11 11 - .1-l" ?"b

r.} @w

&?@

%

g=Oc) Ammonia (NH3)JlJ (< }(Lr?,,

r ??s

%h

a

di'.x 7(r.ri= .?Fvce-'/u-H 1-H?J?5enoti'h';r3 .i-(l

i4 <==-==-l"-) ,c,H...-4-4-e) CH2F2!L

:F,,(

ld(L-H

11

/ .S'..-HH

.} *

<qrrvx Httletr

2>?

Fg

/'

pvr 6ttar-d) Oxygen

H -

]n(;aYr (JcilOlr

(cli'7ofi 14 Jqrces({4J(ie.r'?'(O'h(

% (-li

f(Asr

3) Rank the following compounds by increasing melting point.a) C2H6, C2H50H, C2H5F

LbF- in-

Cll??16 < CIHS-F < C?Hs-oHb) H2S, H20, Hz L'fsF

ck;'palt 1

L?B'r I tJ)F-

H, <. H,s < i-f,O

Bci. < 'BAr < BI':= ,s 3

lawe,es?'?) m(t3,?( pblata3a&l'4) Explain how dipole-dipole forces cause molecules to be attracted to each

ttYta!?e. cLU%ibi.x'r(oaa iYl {Crlgr'-gec;s cwe Bml A 'A- mci-acW(e,":ra-pc-;-i?L:w (Aind' &

?5) Rank the following compounds fromn d S f r 0 m 19 W e S { f O h j g h e S f b 0 jlj n g p O ' n f : X a ' f' % ( c h a 'c i

methanol, dimethyl ether (CH30CH3).calcium carbonate, methane,{CM fO'/l Cl-t, C)SOH c{tOole? ? - ckt'(ie'lq

" F i?* !ina iao !iCl-4,4 'C Ci{30Cl-L) < C'i-{tO < Cc?C0-,

6) State whether the following proqe,sses are endothermic or exothermic:proqesss<?R@'%-6a. Snowmelting (2yltA,@.jh(:rMC(.

b. A box exploding 'fi M(; '+!'ervt%-ca Cook'nganegg e'4a(2i'i!(i-m;c

Use tl'ie graph at nght to ansiver t}ie folloii-iixg qiiestions:

L 'il'batisthevaporpressuy'eofCHCN:at50?C?7C'KPa

D. 'll'bat is the boiling point of H20 iiheii theexternal pl'essul'e is -qo kpar

t wl?7o oC

M -l3. I'%'batisthenoi'nialboilingpoii'itofCC'l4?.

lSac204. 'A't'fficli s?it+st.ai'ice lxas lhc weakest I?krP?.

c s-( Cl.3s. l'xiJiat does each S? c?u-ve represi

l0'l3kPa

ir

lf C 4a.IIl l IE3..!b l Jrw [I r,4l

ff

7ffi

}

rrl JLffil

?1-J-

Ilr'-Thly

7T

yJl T

77

,-

/

77

7

...-'./'

7r

Name Period Da te

Changes of State

PART A - INTERMOLECULAR FORCES

1 . Fill in the diagram (with high or Iow) to show how intermolecular forces influence the volatility,vapor pressure, and boiling point of a substance.

r l

?ciik

s

%Vlici'i IMF xxrc. .?.

'(

-l;:-lj;I'l?)'!l-l"VT-S -W-:!h? 7x?:Ji') :i:'!'!:'i 'y ?':'s'-??'.'.'. . .'. 'l '.'.'0 it ig.s

!fll'p(')r pI-essL{re ts 'x)iipnr?;css-ure is Ig.(iQ? .

strt+l)ii..f

t'+iiiliiig lioiiii is (5 hniliiig lic+inl is ){ i

s

PART B - VApoR PRESSURE GRAPHS Use the graph below to answerthe following questions. r

2. What is the vapor pressure of CHCl3 at 50oC?7ok.('t+

1

;F6

iooi

Wl

--?-*-. -M-

3. What is the boiling point of H20 when theexternal pressure is 30 kPa?

4. What is the normai boiling point of CCl4?

s. Which substance has the weakest IMF?

ei

R

}

mi

20

N 'f??tyr?17'?lVn[)

rr l?J7'9

bmpataiuth (oq

PART C - HEATING CURVES. Use the heating curve below to answer the following questions.

25 6. What is the melting point of the substance? 5'c-

7. What is the boiling pqint of the substance? !r?c-

8. Which letter represents heating of the solid? Cl

9. Which letter represents heating of the vapor? ?

10. Which Ietter represents melting of the solid? b

11.Whichletterrepresentsboilingoftheliquid? ???d?.?

H{

-l ioi-ixPa

7,) @c,-1': of04Cat,

9

40i

e,

S)-!U 15:5

a$

Eo s

d

c

s

a

4

Changes in State - Ch. 12

EfihTg'l -+%

PART D - PHASE DlAGuMS. Use the phase diagram for water below to ariswer the following questions.

l!, W;12. What is the s!ate of water at 2 atm and 50o(iqa

t

13. What phase change will occur if the temperature isIowepd frorp 80'-'C to -5oC at 1 atm?rered

frete?3(rrq]

14. You have ice' at-lOoC and 1 atm. What could you

D

)S7.lS

(ri:ycril

p?(%S!irr

112)#

Eifl Normal

§', i.00

freezingpoint

iSolid

(ri(i(al p0smc

do in order cause the ice to sublime?l(fMer Of?l35:cLf§, fflo?gUJ (:, z00€->Odlhf'A

?('(Q teuitr -Haieui &ecj)0.0050 :,?

A

l " 'l'ripleB ?(hint

0.00 0 01

Vapot

100.00 373.9'l

Temperature ('C)OI{I(al

a-'r(!IpClah-rC.

CHEM

c

iiqiiid

Nomtal

baHlngp".iln!

C! (1.l/'Irsl IJ

!%l.rt4

Heating CurveHomework

Name

Date Per

25

lO l

l6'

! 15:}-!m&m-

a)aE(k)k

X,,(, a, S <2 cS % t* s 'i n.Sa.'b?e

//=/

%arnel*v3 cc4e *e,

id

Energy?

ANSWER THE FOLLOWING USING THE ABOVE HEATING CURVE

1 . What is the melting temperature of the above substance? 5- cC2. What is the freezing temperature of the above substance? ???3. What is the boiling temperature of the above substance? ??j51(-4. The part of the graph labeled "e" represents temperatures at which gas is being

heated. Describe what is happening for each of the other lettered sections of thegraph:

a. S'c!idi c!.fCirmC'4qb. Mel+i'vl-i a6vdC. Liox<da bk=r'mt'nqd. 6Thci ?an -t- J

J T

s. In which section of the graph are atoms moving the least? ? (.6. In which section of the graph is this substance all Iiquid? C7. On your graph, draw an arrow to and Iabel each of the following: "melting

begins", "melting complete", and "boiling begins".

1l

For each of questions (7) - (12), reler to the phase diagram for mysterious compound X.

Phase diagram for ?erious compound X

-100 0?'f00 20€l 300 400 50€l 600 700 8€)€I/

Temperature (degrees Celsius)

Ue critical temperature of compound X?(7) What is tly

7€VC 21'C(8) If you were to have-a bottle containing compound X in your closet, what phase would it

most Iikely be in?

0asa(9) At what temperature and pressure will all three phases coe,xist?

S?s oc r ) r;x?

' 0(10) If l have a bottle of compound X at a pressuye of 45 atm and temperature of 100 C, what

. .. a a 0will happen if l raise the temperature to 400 C?

fl::-:;?':=:=';a:t k A a" ' (=', 'S")

, -' . 0(11 ) Why can t compound X be boiled at a temperature of 200 C?

6ec?se i+ csvs c-vily pas3 fr? Saiic)-" 5a53a:s '+c g,qli-cL.O(?'-

f'J6% uv(4c-vf s'eric-us Jli'FFt'cvl4'(12) lflwantedto,couldldrinkcompoundX?

a+J at =4re=it rt:lc h ycu?v- h-a?('f'A!1

/S/0 '.'.

!

o

/ i)r

liquic'/r

sol id ir

i/

z//

1 >//li14 >

// gas

//

:lll

Unit s - ORGANIC CHEMISTRY

What you need to know:Identify whether a substance is organic or not by formulaNaming alkanes, including branchesNaming alkenes and alkynes, including branchesGeneral form of an alkane, alkene, and alkyneIdentify an alcohol and name itUnderstand one method of creating an alcohol from an alkeneIdentify a carboxylic acid and name itIdentify an ester and name itUnderstand one method of creating an alcohol from a carboxylic acid andan alcohol

Some example questions:1) Identify the following as either alkane, alkene, alkyne, alcohol, carboxylic

acid, or ester.a. CH3CH2COOH b. CH4 c. CH3CH20H

(2.?)(, A oL

d. Cshio

E

e. C7H12

Y

f. CH,CH,COOCH2CH,,CH,

ES

2) Name the following.

a.

'-ft-i.,c-Q-l,i - CH,, -(,)H - CH, -CH:.-(:H

l

4-e'H%?(kep+ttnDC?!:! == C, H :=

b.

C.

, CH,

l- .

H 3 C - C H - c H - .9,111

C H - C

H-C-C-O-C-C -t-lI

H HH

'ek( l c t'! q?ncrqfe?

H,('3'-i

/'/

d. CH-CH,CH,CH, H

(" : €?

H CH=(?H2(-aHl

(J:an s?!;e-h'?)e- CH3 - CH2 - (-H - CH2 - CH,

oH al )(-H7" CH';= ?C'H3

g)ol>C-CH-CH.>-CH-CH.

t I }

X

H3C?' 9?(l?CH'?'.?9'.H??'(JFall?' .C.H?'CH2""?CH',3ll I

CH, CH3CH3

C?;2, 3 ,- q, r ( - +e?6+we+kyio?c+anQl-1, o,

%

H (;-(:H. s, -OHa%' t?

? H3

(,H2

I

H,3C-CH2-C-CH

I

CH2

I

CH3

-,:,ZJ,,;"J.44,'?Yx)s;:-')

f.

i.

qH3 qH3

C

.}C - C H 3

l

CH3

3) Draw the following.a. 2 - butanol

0i-4/

H- ci'i cH- cJ{3 i3

Ql{, - C/-/ -

b. pentanoic acid

@

il( H - c?i-i - CH- cjf L,

b. 3-ethyl-2,2-dimethyl heptane

',' ") C, < gi3

Q-ISc, cis-4-methyl-2-hexene

C (-t,

. 1.?)c ? a4 Cl{z,.iz3

CH= (.i-l

d. ethyl butanoate ,.l/

H?, C - CH - o -c '-cH-c% - c i4,5 L L L 3

lie,<,I-5!nethyl-2,1:?x?ynee. 4,,

C-14- c,l-I.33

i-le -CEC --IC3

I i.c?i-( - CH

2+

4) Under what conditions are the prefixes cis- and trans- required in naming.J;it.- b?nd,. t'h

Under what conditions are the prefixes cis- and trans- requiredan,organ5cor7pound'- k cut al)'-2a6 U.i.!u ct clrt?o

arc kvc'7'? ?(elclle-fF 'ffi:a ((ryf"(r5(p(>l ?(1?I'l"e'r?e?. "/'I'le-re?,P-

A.rri&le D'kl! 't?0 0cr:'ih'tibq f?lte. ctttO(.th a+r:=svs? f'kat (lcrnte,z P 'F (' f?. (L'lcl ' Q F k (" k C 'o C-' (!i (" )al l-

5) Draw and name all three isomers of pentane (C5H12)cg

i-t,C Ci4,- ?/'/ C-i4.3 i-5( - e - Ci-(31-z(2

I.

(,-i4-€

'Hty 16 a.f-a;i4-6) Draw and name at Ieast three isomers of hexene (C6H12). Include at least

'/.-?C c:r3 orkatr3-oQ- 5%e;naone branched isomer.

4/%//l'?

/-J?e?' 6,+'7. C7sacr+ran5---3 ht%tyie,], :2 , 3 -cA-t ?'f% / - z -& uateh e.

/?,.j, . 2-%efkyJ=l -pe)'l+ehe,-

li(? - ciiA- ci-1?- C!- CH3(t Yl h>,vc ej

/))

7) 2-pentene and water react at a really high temperature with an acidcatalyst.

a. Whatisacatalyst? A ckemicqr ?]actf? '3;pee&' L(l Hicccc*e c(7 CA clacimi'cJ raeryc?%1-(pv, ixi'Hir-cif 'oeino qtrecl uy) ,

b. Draw and name the products of the reaction.l-1. (li H+'-

Ac=$A . .+ Hei-( ?4 (-!C - ;cl4,-cil.H-ci4,r(-1, - .-Ct4, oH

'x

{-('Cl-1J .,,.,,. (, ,,,:.,,4=,.,,=-)aFraris 1 (yeh+'ene,'- 'F cvsFer- " l

8) What is the general form of an alkane? Alkene? Alkyne? C' c c e Pl ' ('€lne- CalAl,(z -ewc CnH2. ?-yne. CriH2y(-2.

9) Draw anQ name two organic compounds that would react to produce ethylhe-xanoate. What is the"other product of the reaction?

,.Hl,,,01 + k€?yxnorc? c?(,ad -e

71

S L i 2 2. L2. JHO

10) Draw and name the products of the reaction between 1-propanol andethanoic acid.

O

i/

ell, - c-i-( - cy - o - A ca, + r-i,r.r(>rqygy/ tH-==qv=Jc -+ bo ts fie r-