Module 4.2 Flashcards
all of these moelcules have the alcoho functional group = OH —> hyydroxyl group .
All of these alchohols only contain the alcohol functional group .. When we name alcohols what do we ?
-Start with the name of alkanae , e.g methanol is based on the alkane methane.
-remove “e” and add the suffix “ol” .
-if necssary , we can use a number to show the carbon atom is bodned to the hydroxyl group . “propan-1-ol and propan2-ol”
if an alcohol contains two hydroxyl groups ,t hen we call it a diol .
Incase of ethane-1,2diol .
-e.g diols can see , we use the whole name of the parent alchol rather droppign “e” (using numbers to show positions of hydroxyl groups )
-alchols with 3 hydroxyl groups are called diols .
-Propane 1,2,3 triol
-sometmes ,a moleucle willc ontisn an alcohol funcitonal groups with another fucitonal gorup ,
-NOw , wetreat he alcohol as the parent moelcule
so the number ,s itll with suffix ol . shown with 2 - cholorpropan-1-ol
certain fuctional group has priorirty over the alcohol functional group (aldehyde , ketones nd carboxylic acids )
-In these cases , moleucle is name is based on the hiigher priotiryg orup .
lchol group suffix is HYDROXYl .
3-hydroxypropanol and 1 hydroyl propan20one
alcohols are classified into three catgeories
primary
secondary
tertairy
defidintion of a priamry alcohol with an example
In primary alcohols , the carbona otm bodned to the hydroxyl group , is bonded to one other crbon atom
-example -ethanol and propan1-o1 and methanol (een tho it dosent fit ieth defention )
definiton of secondary alcochol
the cabron atom is bodned to the hdyroyl grop bodned to two other carbona tos
exampe propn2ol .
defintion of a tetriary atom
the carbon tom is bodned to th e hdyroxylg roup .
-is bodned to three other carbona toms .
example 2methylbutan2-ol.
whetehr n lcohol is primayr ,s econdary ,t ertairy alcohol , affects how it reacts
…
alcohols have a higher boiling point than the alkane with the same number of carbon atoms .
-can explaint his by looking at the intermoleuclr forces acting in thse m olecules .
alkenes are non polar , so due to this alck of polrit . ONLY london forces ar acting between the allkane moelcules .
-londond forces are weak and do no take lot of energy to break , therefor e, alkenes hve low boing points .
IN CONtrast alcohols are polar moleucles
oxygen atoms are much more electronegative polar bond due to the alcohcol funciotnal group
-oxygen otms are much more electronative than hydorgen aoomts .
-becuas eof this ,ocygen tom in the alcohol funcitonal grou has a negative charge and hdyeogenatom have a positive chagre .
-mening ALCOHOL MOELEUCLES can form BOTH hydorgen bonds and london forces .
HYDROGEN BONDS - are reltivleys trong intermoleuclr forces and hdyrogen bond ,t hey have a higher bolign point than lakanes with the same numbe rof cbron aotm s.
Meaning of volatility
how readily a moelcule turns into a agas
-Alcohols , have a higher bolign point than alkenes meaning alcohosl re les voaltile than alkenes with the same umber of carbon aotm s.
as we increase number of carbon aotms , bettween the alcohosl and the correcpodnign lkanes reduces .
expalin this by intermoelulcr forces .
-alaknes only london forces .
-alcohol they ahe london forces and hdyrogen bonds .
in an alcohol with a short chainc abron chin as ethene major intermoelcule forces is hydorgen bodnign to the alcohol fucntional grup .
whereas , london forces play a much less improtant role , meaning thane aoms have a greater boling point that the corresondign alkene .
HOWEVER , in alachols wih long carbon chains liek dcan–ol
the contirbution of london forces increse ,s o the relativ eimrpotant c of hydorgen bondoing is …
-Meaning hte boling point of long chain alcohosl are onl slightly greather than the corresonding atom s.
hydorgen bonding explains nother porperty of atoms
alcohools are highly souldbe inw ater .
-as the laochol funcitonal group cna form hydorgen bonds with warermoeluel .
as we increase the length of the carbonc hians , atoms become less souble inw ater .
as the non-ppolr carbon chain can;t form hydorgen bonds .
-ttherefore incfrease cabronc hain ,, a greater par o the moelcules is unable to hdyrogen bodn to the water moelcule .
-sp long carbon chain alkols , solubles freduces .
-inc ontrast ,to alchosl alkanes are nonsolube becuase they are nonpolar so cannot form hdyorgen bodns with wtaeee moelcules .
when we oxidisie a primary alcohol we make an aldehyde
ehtanol is oxidised to ethanol also we amke a moleucle if water
oxidiaiton is carried out using a chemical called oxidisin agent .
common rxmpales include potssium dichroamte with dilute sulfuric aicd .AKA(acified potassium dichromate )
-KR1CR207 /H+
-usually (o) –> showing one moelcule of the oxidising agent is takingpart in the reaction
-we need one mole of oxidisign agent to oxidisie one mole of ehtanol of one mole of ethanoi acid
during a reaction , oxidising gnet reduced from dichormte 9VI) whic is orange , to chromate (111) in which is used .
PROBLEM ; aldehydes are extremely easy to oxide meaning if we want to mke an aldehyde , have to removie it form the reation as it remains of aldheyde willeoxygen .
Aldehyded havr low boiling poin , as aldehyde moleucles rom hydorgne .
-ethanal wo degrtees ehtnol 78 degreees.
-Meanng as aldehyde when oxidies can easily make it whatt .
-
by gently hraing aldehdyes and oxididign hahent produces aldehyde
aldehyde then exceptor passes into condesor
-where condensor turns it bck into liquid
we can aslo favour the pordu ction of aldehyde by amkign sure ht estarting lcohcol in excess and the oxidiign aent litms .
aldehyde easily oixidises to form a cabroxlic acis .
*-shown oidation of ethanol to ethene and then ehtnaoic acid .
you will notice ,t his requires two moelcules of oxidisng agnet .
when carrying out this reaction , make sure that all of the aldhyde produce is oxidised to cbroxylic axid .
-TO DO THIS , we can dd EXCESS oxidising agent . need 2 molecules of (o) to oxidise primary alcohosl to COOH .
-can also suee cocnentrated sulfuric acid rather than dilute sulfuric cid . Het rection udner REFULUX .
-when we heat a reaction under efllux , onl volative porducts are condensed nd return
-by heating nder refulux , we can heat the chemials until the rection compeltes and we amke a carboxylic acid .
-at the end , reaction , we will have a mixture of cheimcals
PRODUCES ; carboxylic acid and analchold WHAT IS THIS - also hae unreactiner oxidising gent .
carboxlic acid bolign point icnreases a cabroxlylic acids can dorm hdyrogen bonds
at the end of the reaction , we caan use distillaiton to separate out our abroxlic acids and form the reaction mix .
oxidation of propan2-o1
when a secondary alcohol is oxidisd ,w emake a ketone + water .
-propan2ol makes a ketone porpanone
if we are usign cidified potassiumd ichromar – oxidising agent –> solutionturns from orange –>green .
key ; ketones cannot be oxidisied any more
-ifw e look a oixdaito of rpaimrya lcohol we can see wh .
-We can during oxidiiton , we remove a hdrogen from the atom bodned to the alcohol group ,
-Once , we form the aldehyde ,t he carbon atom bonde tot he oxygens ill has under ha tom ti aitn
-meaning aldehyde can e oxidied further to form cabroxylic acids .
however , ina ketone ,t he cabrona tom bonded ot the oxygen is not bodned anymore to the hydrogena tom .
BECAUSE OF THT , cannot oxidise ketones an futher .
when we odisie a secodnayr alcohol , we hea the reactants UDNER EFULUX , shown appartus
by heting udner refulux , we can ensure that as much ekne forms as possile .
-In the end of the reaction , we will have a micture of reactants
-We have prodcuts which a ketoenand eater
we also have a unrective alcohola nd oxidisignagent .
at the end of reaction we will have a mixture of the reaction ,w e will use distilaltion to separt our kdgod vfom ghd mitur .
ketone boiling poitn is lwoer .
tertairy alcohols ; 2methylpropan2-ol
as you can see in teritrya lcohosl , the carbon tom is bonded to the alcohol group , which is no bdoned to nydhyrogen aotms . Meaning terit lkanes are not easily oicides undern ormal lboratoryc onditosn .
-if we heat a tertiary attched in the presenc eof acidified potassium dichormte –> nor eaxcito n happens an doxidisign agen trmeians ….
cylcohexanol
we can convert alcocohls into alcohols
-we do tihs by heatting it under refulux
with concenrated sulfuric acid or concentrated phosporic acis (v) acid .
what does the cocnentrated acid do ?
the cocnentrated icd acts a a catalyst or thi clyclo hexane reaction thing .
-in this reacction what else do we produce
we also porduce a water meolcule form the apretn alcochol .
-so scieniets sa hat hte alchol underwent dehyration to form the alkee .
what is dehydration of alcohols an example of
elimaination reaction
Whhat is an elimination reactio ?
In an elimnation reaction , a smll moleucle is removd from larger prent moleucle .
-in this case of dehyration of alcohols the small moleucle in water .
dehyrdation of alchols key
look a petn2ol nd descirbe the reaction
-int hi cas e,w e can make three diffrent alkanes .
-pentan2ol alchol enxt one
-if we remove this gorup , lus he hydrogen in caron 1 ,then we make thatt /
list a few names of haloalkanes
check sheet
what classifies something as a haloalkane
haloalkanes contains a halogen atom bonded bonded to an alkane .
-halogen is the prefix , followed by a parent alkane ..
what is the general formula of a haloalkane with one halogen atom
cnh2n+1x
x is used to represent a halogen
u can also get haloalakes with more than one halogen
-when we have different halogens , h alogens are listed alphabetically not by position number .
how can haloalkanes be classed ?
haloalkanes can be classed as primary secondary tertiary .
what is a primary haloalkane ?
halogen is bonded to a carbona tom which is bonded to one other carbon aotm .
what are secondary haloalkanes
halogen is bonded to a carbon atom which is bonded to two other carbon atoms .
what is a tertiary haloalkane
halogen is bonded to a carbon atom bonded to three other carbon atoms .
what is important about the carbon halogen bond ?
the bond is polar .
-polarity affects both physical properties and reactivity of the haloalkane .
halogen atoms are electronegative meaning what ?
meaning the pair of electrons in the covalent bond bond between the carbon and the halogen atom is closer to the halogen than to the carbon .
-THEREFORE , halogen atom has a slightly negative charge and carbon atom has a slight positive charge .
physical properties of haloalkanes compared with b.p of equivalent alkanes
haloalkanes have a higher boiling point than equivalent halkanes .
-this is because of equivalnet intermolulcar forces .
alkanes are nonpolar molecules so the intermolecular forces are london forces , what does this mean ?
london forces are relatively weak and require little energy to break . so alkanes have a low boiling point .
haloalkanes have london forces , as well as what ?
however , due to the polarity of the carbon halogen bond , we also find permanent dipole dipole interactions .
-permanent dipole dipole interactions are stronger than london forces and require more energy to break .
-explaining why haloalkanes have a higher boling point than equivalnet alkanes o.
what is the boiling point of haloalkanes based on ??
-based on ethane .
-as we go down group 7 , boiling point of haloalkanes increases due to london forces .
-london forces are larger when there are more electrons ,
-larger london forces require more energy to break .
-this explains why baling point increases as the size of the halogen atom increases .
are haloalkanes soluble ?
Haloalkanes are insoluble in water .
-as haloalkanes cannot form hydrogen bonds .
-however , haloalkanes are soluble in nonpolar solvents such as cyclohexanes .
haloalkanes react with chemicals called what ?
nucleophiles
what are nucleophiles ?
nucleophiles have lone pairs of electrons.
-The lone pair of electrons is attracted to an electron deficient carbon atom .
what are electron deficient carbon atoms ?
electron deficient carbon atoms have a positive charge either a full positive charge or partial positive charge .
what does a nucleophile donate ?
a nucleophile donates a lone pair of electrons from a covalent bond between nucleophiles and the carbon atom .
shown is a haloalkane chloromethane , what does it have ?
-it has an electron deficient carbon atom with a partial positive charge . Also shown a hydroxide ion .
what does a hydroxide ion have ?
-a hydroxide ion , the oxygen atom has a lone pair of electrons and a negative charge .
-the hydroxide ion is an example of a nucleophile .
stage one of haloalkane nucleophilic substitution .
the lone pair of electrons on the hydroxide ion are attracted to the electron-deficient carbon atoms on the chloromethane .
stage two haloalkane nucleophilic substitution .
nucleophile now donates its lone pair of electrons to form a covalent bond to the electron - deficient carbon atom .
-shown the hydroxide ion forming the covalent bond from the opposite side to the hydrogen atom . (why does it do this ? )
by approaching from this side , there is less repulsion between the hydroxide ion and the negative hydrogen atom .
How do you represent the movement of electrons ?
By using a curly a .
-The curly arrow , must start at the lone pair of electrons and end at the electron deficient carbon atoms .
stage three of haloalkane nucleophilic substitution .
-carbon atom can only have 4 bonds .
-so at the same time , the covalent bonds between the carbon atom and the halogen atom breaks with a pair of electrons moving onto the halogen atom .
-This is an example of heterolytic fission .
stage four of haloalkane nucleophilic substitution .
at the end of this reaction , we produce an alcohol molecule in this case of , methanal .
-we have also released a halide ion in this case , a chloride ion .
what do we call the thing that has left the haloalkane
as the halogen has left ,we call it the halide leaving group .
what do scientists call the haloalkane nucleophilic substitution ?
a hydrolysis reaction it is an example of nucleophilic substitution .
-need to learn this mechanism and the conditions for this reaction .
what are the conditions for this reaction ?
- we use an aqueous solution of hydroxide ions for example –> sodium hydroxide or potassium hydroxide dissolved in water .
check sheet to see the reaction
…
what is the problem with the haloalakne reactio , therefore what is the solution to the rection ?
problem haloalakne are insoluble in water .
-so ethanol needs to be added to rcarry out hydrolsis rather than hydrocide ions .
this is becasue ydroxide ions rect wuith silver ions to from insoluble silver hydroxdieions
-soo can’t use hydroide ions for this extinct
- what ppt does 1-iodopentane
a yellow ppt rapildy
what ppt does 1-bromoepntane form ?
foorms a cream ppt the reaction is slower 1-iodopentane
finally 1-chloropenTne forms a ppt ?
mcuh slwpeoer
forms a white ppt
so the reaction is idoo then brormo then chloro
why do the haloalaknes react int his way specifically , what can we look at ?
- we have to look at the bond enthalpies inovvled .
-remember , during hydrolysis have to break te carbon to haloogen bod .
carbon chprine bond has a realitvely high bond enthalpy , this means it takes a lot of energy to break theb ond , therefore they hdyrolysis of chloroalakne is slow .
whereas the carbondioiden bond has a reliatviely low enthalpy and does not take a lot of energy too brek bond whihc is why aiodoalaknes react rapidly .
-bromoalaknes lie somewhere in the mideel .
step of haloalakne hydrolysis
-allow the slutions to reach the same tem[erature .
-now we then add 1cm3 of the aqueous silver nitrate to each test tube and start timing .
-rmemeber ,t han in aqueosus solutions , the solven is water and water is a nucleophole .
step 7 of haloalakne hydrolyis , how does water moelcules react with haloalaknes ?
reacts with haloalaknes by nucleophilic subistituion and hydrolysis takes place .
-during hydrolysos , the halide ion will be released from the haloalaknes .
-check sheet for all the equations .
step 8 of haloalkane hydrolysisis
halide ion will then react with silver ions to form an insolube ppt of silver halide .
-the chloride ion will form a white ppt of silver hcloride
#bromine reamppt of silver bromide
iodided from ywllow ppt of silver idoide
step 9 of haloalakne hydrolyis
-in each case , time how long it takes ofr ppt to nform .
-can notice ,w e are using waterto crry out reaction .
what iis the surface of the earth constantyl bombarded with ?
ultraviolet radiaion in the form of sunlight .
what can uv radiation damage ?
What can Iv radiation damage
It can damage dna
Too much exporsure to the Iv can be harmful to humans and is linked with skin cancer
In the atmosphere , there is a region called the ozone layer , where is this ?
This is found in the stratosphere around 20-40km above the earths surface
What is in the ozone layer and what does the ozone layer do ?
Ozone layer contains a relatively high concentration of the chemical ozone .
-ozone has the symbol 03
Ozone layer absorbs a great deal of Iv radiation from the sun before it can reach the earths surface .
What is the purpose of the ozone layer ?
How does it dk this
It protects living organisms from excessive Iv esp core
-chekc sheet , in the stratosphere , Iv radiation causes the double bone in oxygen molecules to break
In the stradolhere what do we form
2 oxygen radicals
What is a radical
A species with an unpaired electron
However we don’t show the unpaired electrons in the radical even tho they are radicals !!
What is the simple version to show the reaction in the atmosphere
Chekc sheet
Now an oxygen radical reacts with what ?
What would happen if this was the only reaction occurring ?
Ozone would do toenails increase
HOWEVER , an ozone molecule can absorb UV ligjt ? Turning back to an oxygen radical and an oxygen molecule
The absorption of Iv radiation …
Is hwk the ozone layer protects us from.
Ahh should the amount of zooms in the ozone layer remain constant ?
As ozone js formed and broken down at the same rate
However , why may the amt of ozone nkt be constant ?
As certain chemicals cause ozone in the ozone layer to be broken down .
These chemicals are called chlorofluorocarbons CFCS
What are CFCS
- ,£:,@ sheet for stirufte
They are halpwlaknes
They are very stable bevause if the high jkfn ent jsppy of the carbon tk halogen honr
And are relatively non toxic
How were cfcs used in the past ?
CFCs were produced in vast quantities and were used in a range of applications - for example in frigid and freezers
What have scientists found CFCs dk
Ty eh cause the destruction of the ozone layer
As they make there way t the strap is her e
In the stratosphere Iv radiation caused the carbon chlorine bond to break what is this called ?
- scientists call this photo dissociation .
-this is homolytic fission and produces a chlorine radical which is high rev drive .
What is the next stages in cfc
Propagation 1 and 3
Proposition 1 of cfc
A chlorine radical reacts with a molecule of ozone
This produces an oxygen molecule and w highly reactive chlroine monoxide radical
What happens in propagstoon2
As we saw here oxygen radicals are constantly formed in the straosjeojte
This produces a chlorine raid dk plus an oxygen molecule
What does the the chlorine radical in propahtoon3 do
Goes back and triggers step 1 again .
In effect the chlorine radicals are acting as a catalyst for this reactive
What is an alternative reaction for this ?
Chlorine monoxide radicals reacts with an ozone molecule chekc sheet
- but then again anfjlroine radicalnisneposcues and cycle continue s
There what is the effect of one cfc molecule
It can lead to the festirififkn of many thousand of ozone meofles
Many scientific Iv organisation provided evidence that CFCs were leading to the destruction of the doodle layer leading to ?
CFCs being phased out by less harmful alternatives
How else can ozone be destroyed ?
By nitrogen oxide radicals
- these are forced by lighting and huh
- nitrogen monoxide radical relays worj ozone to produce nitrogen dis oxide radical and a oxygen molecule
What does nitrogen dioxide radical react with oxygen to
Fork form an oxygen radical which forms an nitrogen lonodife radical plus an oxygen molecule
This takes place as a file triggering the first reaction again .
What happens in mass spectrometry part one
-A beam of electrons is fired at our sample .
-yhis causes the sample to lose an eelctron , forming a positivre ion .
-scientists cll this a moelculear ion , check the shseet .
What is mass spectrometre used for ?
It is used to idengtify organic chemicals .
What happens in a mass spectrometer prt two
the positive molecular ion moves down the mass specgtrometer er geta spectrum like shwn on the she t.
what does the m/z ratio show
the m/z ratio shows us the ratio between the mass and the charge of the molecular ion .
-HOWEVER , almost every moelcular ion ahs a 1+ charge the m/z ratio effectively tells us the mass of the molecular ion .
what does star 2 show in the mass spectrometer
pentane has a mr of 72 , shown by the m olecular ion peak .
-one small epak to the righ of the moelculear ion peak .
-what do we mmotice about the most prominent peak on the mass spectrometrer
there is one prominent peak , n the fr right of thre amss spectrum .
-this ic called a moleculear ion m+ peak ,t ellling us the relative msss of the moelolecule .
what is another reason for the peak at star 2 ?
peak is also due to the presence of isotopes , carbon-13 , representing aroufn1 15 OF CARBON ATOMS SCIENITTS call this an m+2 peak
does the m+1 peak playa role in the mass spectrum ?
it does not paly a role in the analsysis of the mass spectru .
-in rpactice ,w e can carry out mass psectroemetry on an organic moelcule ,w e can get a range of different peaks .
why do we get a range of different peaks in mass spectroemtry ?
As organic molecules break up into fragments in the mass spectrometer .
EXAMPLE IS pentane ,, breaking up into two fragments .
What happens in fragmentation in a mass spectrometer ?
When fragmentation happens , a bond breaks an we forma n ion and a radial .
-only the ion can be detected by the mass spectrometier int hsi case hte butyl ion .
frgamentation in a mass spectrometer part 2
however , bear in mind ,t hat the frgemnts could jusesily form a emthl ion and butyl radical .
-so inpractice , both fragements will be seen on the mass spectrum .
fragments porduced exmple
by breking the carbon tocarbon bond in pentane .
-all of htee four fragements iwll produce a peak on the mass psectrum .
-we cna woekout the m/z ratio of each peak by adding the aromic masses int he gramenet .
key point one bout fragmenets
some fragmenets re more stable than others .
-so each fragemnts will not have the same abndance .
try out the question in free science lessosns
3:35
second key point about fragmenets
most abudnan fragemnt is assigned a relative abundnce of 100% ceienits call this the base pek example propyl ion .
-CARBON to hydrogen bnds break in a mass spectroemter so we geta range of peaks .
how do rganic compounds move ?
they are constantly vibrating
two main types are stretching n dbednign
how do stronger bonds vibate in comparios to weaker bonds ?
stronger bonds vibrate FASTER than weaker bonds .
-If the bond is between two HEAVY atoms , then the vibration will be slower thna if the bond was between two IGHTER atoms .
what does an abosrbnce specturm show ?
% trasmittance is put on the y ais .
telling us how much infrared red radiation passes through our sample .
-te pea shows infrared rdiation has been abosrbed .
x axis shows wave numer
What happens hwen a bond abosrbs radiation
the degree of stretching and bednigng icnreases .
-so if we pass infrared radiationt hrough a sample of our orgnic moelcule ,t hen the bonds will absorb specific frequencies .
What do vibrating bonds do ?
these vibraitng bonds , can absorb radiaion which ahs he same frequenecey as the bond virbation .
-for organioc compounds this leis in the infrared region of the elctormgnetic spectrul.
key point about ir one
below 150 cm-1 , we have a finger print region , the fingerpirnt region is a complex series of peaks which are speicifc to the moclueles beign hsown .
-due to its contintti oftennaysledb y …
What is wavenumebr in IR ?
wavenumbe ris the number of wavelengths per cm .
key points about ir 2
moelcule stend to have a peak t 3,000 cm-1 caused byt he bibration of c-h bonds .
-be ware , this pek may be obserbed b y hdyrogen bonds what
first characteristic pak
alcohol peak at o-h bond in oh gruop 3200-3600
seond charcateristic prak
vibration of c-o bond in oh group peak of 100cm-1 to 1300 ccm -1 ut it is int he fingerprint regiont here difficult to tell .
aldehyde and ketone is an exmaple of ?
carbonyl group
peak centers at 1700cm-1
oeak indicated aldehyde or ketone idniciating carbonyl group for example
carboxylic acids have an o0h bond s well in o h group what does this show ?
produces a very borad absooprtion peak with a rnage of 2500cm-1 tp 3000 cm -1 .
combitiaiton of the 2 gpeks prduces c00h .
-c-o single bond 1000 -13000 but finger print region so not eays to pin point .
what can vibrating covalrnt bonds absorb ?
Infrared energy
-processes tkes place in gase in astompshere .
ir int emrs of the atmospheree
sun emits infrared and uv radiation .
-but this can pass thru the atmosphere and be abodrbedbh the wht .
+dsve f erth nore re eneters the radiationas infrared n longer wvalength .
-infrared s the sme freweucy as the virbation of frequency of bonds in greenhosue gases .
how iense of a pea useuful ?
abscence of a peak is useful to way to rule out a certain compound .
-abscenc eof carbonyl 1700cm-1 steel compound ald
aldehyde / ketone carbolic acid
ir emits into the atmospehre 2
virbating bodna sborrb the ir enegry and re emit it itnot the ariboen .
cusign the tempratue of te atmospehre it incresde ner the surfce of the erth .
combustion of fossil fuels do the the atompshere
it icnreses the cocnentration of c02 into the atompehsere , leading to global warming .
-hhence hwy ther eis a global effort ror educe carbone mmsiosns .
what are the practicl uses of ir
-montiro air pollutio of co or no2 .
-breathalsnaysers to check alcohcol ir breath
Oxidation of alcohols observation colour fhen e
Orange to fhange
Apart from tertiary
Functional group of an ester
-COOR groip where r is an alkyl chain
Common way to make an ester
Reacting an alcohol with a fsr body lid scif in the oreeenc rod an acid catalyst
During reaction well chrck 202
Skim over 212 and 213
Heck lage 214 and 215
