p o s t l a b biochem d l s l
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BIOCHEMISTRY POST-LAB DISCUSSIONS
EXPERIMENT 1:DIFFERENCES BETWEEN ORGANIC AND INORGANIC COMPOUNDS AND TESTS FOR ELEMENTS FOUND IN ORGANIC COMPOUNDS
1. Organic compounds are the result of activities of living beings while inorganic compounds are created either due to natural processes unrelated to any life form or the result of human experimentation in the laboratory.2. Inorganic compounds can make salt, while organic cannot.3. Organic compounds contain carbon, while inorganic do not.4. Organic compounds have carbon-hydrogen bonds, while inorganic do not.
5. Inorganic compounds contain metal atoms, whereas organic compounds do not.6. Organic compounds are biological and inorganic are mineral in nature.7. Organic compounds are part of a class of chemical compounds the molecules of which contain carbon and hydrogen, while inorganic compounds mostly comprise of metal containing compounds even if they happen to exist in living organisms.
SUGAR (CH22O11) vs. SALT (NaCl) organic compounds have lower melting and boiling points than inorganic compounds Sugar: 146oC, Salt: 801oCCHLOROFORM (CHCl3) vs. SALT Solution (NaCl) organic slow; inorganic quickAgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
DETECTION OF ELEMENTS:HYDROGEN & OXYGENC2H5OH + 3O2 2CO2 + 3H2OCARBONCa(OH)2 + CO2 = CaCO3 + H2ONITROGENUrea ------> NH3 + CO2
If you add sodium hydroxide solution to an unknown organic compound, and it gives off ammonia on heating then it is an amide.You can recognize the ammonia by smell and because it turns red litmus paper blue.
SULFURWhen proteins containing sulfur are decomposed by sodium hydroxide, sodium sulfide is formed; the latter is converted into lead sulfide by lead saltsThe presence of sulfur-containing amino acids such as cysteine can be determined by converting the sulfur to an inorganic sulfide through cleavage by base. When the resulting solution is combined with lead acetate, a black precipitate of lead sulfide results.
Comparison between Organic and Inorganic compounds
Properties Inorganic compounds Organic compounds
A. Elements Involved All elements C,H,O,N.& S
B. Physical Properties
1. physical state
2. combustibility
3.melting point
4.boiling point
5.Solubility in water
6.solubility in organic solvents
7.conductivility in the fused state
Solid
Non-combustible
Very high
Non-volatile/very high
Soluble
Insoluble
conductivity
Solid, liquid, gas
Usually combustible
Very low
Relatively low
Insoluble
Soluble
nonconductor
C. Structure of the solid
1.crystalline type
2.units of structure
Bonding between units
Ionic crystals
+ and – ions
Electrostatic/ionic
Molecular crystals
Molecules
Van der waals forces/covalent
EXPERIMENT 2:STRUCTURES OF HYDROCARBONS
BONDING PATTERN OF
CARBON
ARRANGEMENT OF BONDS AROUND CARBON
BOND ANGLES
4 SINGLE TETRAHEDRAL 109.5O
2 SINGLE1 DOUBLE
TRIGONAL PLANAR
120O
2 DOUBLE LINEAR 180O
1 SINGLE1 TRIPLE
LINEAR 180O
HydrocarbonsHydrocarbons
C C
C C
C C
C
C
C
C
C
C
H
H
H
H
H
H
C C C C C
H
H
H
H
H H
H
H
H
H
H
H
Alkanes Alkenes
Alkynes Aromatics
C C C C C
H
H
H
H
H
H
H
H
H
H
C C C C CH
H
H
H
H
H
H
H
Drawing structures
of Hydrocarbons
The First ten Straight-chain AlkanesHydrocarbon/molecular formula
Condensed structural formula No. of carbon atoms
Methane-CH4 CH4 1
Ethane –C2H6 CH3-CH3 2
Propane C3H8 CH3 – CH2 – CH3 3
Butane C4H10 CH3-(CH2)2-CH3 4
Pentane C5H12 CH3-(CH2)3-CH3 5
Hexane C6H14 CH3-(CH2)4-CH3 6
Heptane C7H16 CH3-(CH2)5-CH3 7
Octane C8H18 CH3-(CH2)6-CH3 8
Nonane C9H20
Decane C10H22
CH3-(CH2)7-CH3
CH3-(CH2)8-CH3
910
14
• Molecular formula describes the numbers of different kinds of atoms in a molecule,
• Structural formula represents a two-dimensional model of how the atoms are bonded to each other. Each dash represents a bonding pair of electrons.
16
structural and condensed formulasThis is a full structural or displayed formula. All the bonds are shown including all the hydrogen atoms
shows the exact way in which the atoms are connected to each other.
This is a form of a condensed structural formula
shortcut method in presenting molecular formula
Drawing structures: it’s all good
CH3
CH
CH
CH3
CH3
CH3
CH3
CHCH
CH3
2-butene
This is called the “condensed structure”
C C C C
H
H
H
H H H
H
H
CH3 CH CH CH3
On a test, choose a method that shows all Hs
CH3CH=CHCH3
Using brackets can also shorten some formulas: CH3(CH2)4CH3 vs. CH3CH2CH2CH2CH2CH3
Background: formulas for HCs
• Alkanes= CnH2n+2, enes= CnH2n, ynes= CnH2n-2
• Remember enes, then think of what would happen if bond was single or triple instead.
Q - how many hydrogens in each of these:6 carbon alkaneAlkene: C22H
14448 (2x5 - 2 = 10 - 2)CH3 CH3
Numbering carbonsQ- draw penteneA- Where’s the bond?
We number C atoms
• Always give double bond the lowest number
• Q - Name these
C C C CCH3
H
H
H
H H H
HCH31
C2
C3
C4
C5
H
H
H
H H H
HCH35
C4
C3
C2
C1
H
H
H
H H H
H
Ethene
3-nonyne
2-buteneCH3
CH
CH
CH3
CH3 CH3
C2H4
1-pentene
2-butene
propene
1-butyne
CH3 CH CH2
CH3 CH CH CH3
CH3 CH CH C
CH3 CH3
CH3
2,4-dimethyl-2-pentene
CH C CH2 CH3
Draw the structures of the following:2,2-dimethyloctane
1,3-dimethylcyclopentane
1,1-diethylcyclohexane
6-ethyl-5-isopropyl-7-methyl-1-octene
Hydrocarbons: IUPAC names
Naming Hydrocarbons (nomenclature)
Basic names of hydrocarbons• Hydrocarbon names are based on: • 1) class • 2) # of C, • 3) side chain type and • 4) position • 5) name will end in -ane, -ene, or -yne• 6) the number of carbons is given by a “Prefix”
1 meth- 2 eth- 3 prop- 4 but- 5 pent- 6 hex- 7 hept- 8 oct- 9 non- 10 dec-
• Actually, all end in a, but a is dropped when next to a vowel. E.g. a 6 C alkene is hexene
Q - What names would be given to these:7C, 9C alkane2C, 4C alkyne1C, 3C alkene
heptane, nonaneethyne, butynedoes not exist, propene
CH3 CH3
CH3
CH3Naming hydrocarbons and side chain• Names are made up of:
side chains, root
• Root is the longest possible HC chain• Must contain multiple bonds if present• Add -yl to get name of side chain• Common side chains include:
CH3- methyl CH3CH2- ethyl
CH3CH2CH2- propyl (CH3)2CH- isopropyl
• 2,3-dimethylpentane
CH3 C H3
C H3
C H3
CH3CH
CH3
* “iso” (branched) is not an IUPAC
convention• Br- (bromo), Cl- (chloro), F- (fluoro), I- (iodo)
ene
Rules in Naming HydrocarbonsB. Alkenes
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
Rule 1: choose the correct ending
ene
Rule 2: longest carbon chain
Rules in naming hydrocarbons
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
1-hexene ene
Rule 3: attach prefix (according to # of C)
Rules in Naming Hydrocarbons
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
Rule 4: Assign numbers to each carbon
1-hexene
Rules in Naming Hydrocarbons
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
Rule 4: Assign numbers to each carbon
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
1-hexene 1-hexene
Rules in Naming Hydrocarbons
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
Rule 5: Determine name for side chains
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
1-hexene 1-hexene
Rules in Naming Hydrocarbons
ethyl
methyl
methyl
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
1-hexene2-ethyl-4-methyl-4-methyl-1-hexene
Rules in Naming Hydrocarbons
ethyl
methyl
methylRule 6: attach name of branches
Rule 7: list alphabetically
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
1-hexene2-ethyl-4-methyl-4-methyl-1-hexene
Rules in Naming Hydrocarbons
ethyl
methyl
methyl
Rule 8,9: group similar branches
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
1-hexene2-ethyl-4-methyl-4-methyl-1-hexene
Rules in Naming Hydrocarbons
ethyl
methyl
methyl
Rule 8,9: group similar branches
CH3 CH2 C
CH2
CH2 C
CH2
CH3
CH3
CH3
CH3 CH2 C2
CH21
CH23
C4
CH25
CH3
CH3
CH36
2-ethyl-4,4-dimethyl-1-hexene
Rules in Naming Hydrocarbons
ethyl
methyl
methyl
Naming Multiple bonds: C. Alkenes; Alkynes
• Give 1st bond (1st point of difference) lowest #• include di, tri, tetra, penta, etc. before ene/yne• Comma between #s, hyphen between #-letter• You need to know ene and yne
2,3-heptadieneCH3CH3
CH3
CH2CCCCCCCH3
2,4,6-nonatriyne
C C C C
H
H
H
H
H
H
CH3CH2CH2CH=C=CH2
CH2CCH
CHCH2
2-butyne
1,2-hexadiene1,2,4-pentatriene
C
C
C
CC H
HHH
H
H
HH H
H
D.Naming Cyclic structures• Cyclic structures are circular• Have “cyclo” in name• Benzene is not a cyclic structure
• cyclopentaneQ- Draw these (note: carbons in a double bond
should be consecutive- 1 and 2, 5 and 6, etc.): cyclobutene 1,3-cyclopentadiene cyclopropane
CH2
CH
CH2
CHCC
C CCH
H H
H
H H
CH2
CH2
CH2
CH3 CH3
CH3
CH3
Practice exercise:Name the following hydrocarbons
CH3 CH2
CH CH3
CH2CH2
CH3
CH3 CH
CH
CH3
CH
CH3
CH2 CH2 CH3
CH2 CH3
CH3CH2CH CH CH CH2CH CH3
CH3
CH2CH3
CH3 CH3
3-methylhexane4-ethyl-2,3-dimethylheptane
5-ethyl-2,4,6-trimethyloctane
3-ethyl-2-methylpentane
3-ethyl-1,5,5-trimethylcyclohexene
CH3
CHCH
CH2CH3
CH3
CH2CH3
CH3 CH3
CH3CH3
Name the structures below
More practice
4-bromo-7-methyl-2-nonene
5-fluoro-7,7-dimethyl-2,4-octadiene
BrBr Br
Cl
CH3 C CH2C CH CH CH CH3
CH3
CH3
F
2,5-dibromo-6-chloro-1,3-cycloheptadiene
b) same
c) 5-ethyl-4-methyl-2-heptyne
a) 3,3-dimethyl-1-pentene
CH2 CH C CH2 CH3
CH3
CH3
CH3 C CH CH2
CH3
CH2 CH3
CH CH CH2
CH2 CH3
CC
CH3CH3
CH3
For more lessons, visit www.chalkbored.com
Aromatic compounds: Benzene
• -originally referred to certain compounds that had a pleasant odor and similar chemical and physical properties.
• It has the formula of C6H6
• Have several double bonds to fulfill the bonding requirements for carbon, thus making it unsaturated.
• Is a colorless liquid with a distinct gasoline like odor• it is insoluble in water but soluble in alcohol and ether• It is toxic when taken internally, contact with the skin is
harmful and continued inhalation of benzene vapors deceases red and white blood cell counts.
• benzene is now considered mildly carcinogenic, and care must be taken with its use,
44
You need to recognize the benzene structure in structural formulas
This is the general layout with a perfect hexagon. In this particular diagram you do not see the double bonds.
45
Two Lewis structures for the benzene ring.
46
Shorthand notation for benzene rings.
Benzene formula
CC
CC
C
C
H
H
H
H
H
H
CHCH
CHCH
CH
CH
There are 2 naming methods1) Numbering carbons2) ortho, meta, para (stomp)
Aromatic nomenclature
CH3
Ortho
Para
ST Meta
CH3
CH3
CH3
CH3
CH3CH3
1,2-dimethylbenzeneorthodimethylbenzene
1,3-dimethylbenzenemetadimethylbenzene
1,4-dimethylbenzeneparadimethylbenzene
Benzene is very stable (does not generally undergo addition)
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Some common mono-substituted benzene molecules
Toluene, sometimes you see this on marker pens ”contains no toluene”
Has the condensed structural formula C6H5CH3
EXPERIMENT 3:PROPERTIES OF HYDROCARBONS
ODORAlkane: Gasoline odor; Alkene: sweet odor; Alkyne: sweet odorIGNITION TESTAromatic hydrocarbons burn with a yellow, sooty flame due to their high carbon content. Aliphatic hydrocarbons burn with flames that are yellow, but less sooty.SOLUBILITYAlcohol: miscible; Alkane, ene, & yne: immiscible
SOLUBILITY OF HYDROCARBONS IN EACH OTHER: “Like dissolves Like”REACTIVITY OF BROMINE WITH HYDROCARBONS:Bromine is slightly soluble in water, but it is highly soluble in organic solvents such as carbon disulfide, aliphatic alcohols, and acetic acid.
Pentene is an unsaturated hydrocarbon (One that does not have many possible side branches) It reacts readily with halogens to form new substances.In this case, bromine reacts with pentene in an addition reaction, this changes pentene into 1,1-dibromopentane.Thus, removing bromine from the solution, hence the distinct orange color is removed.
BROMINE SUBSTITUTION REACTION WITH ALKANESAlkanes react slowly or not at all with Bromine at room temperature in the dark, but in the presence of sunlight, substitution is fairly rapid.
POTASSIUM PERMANGANATE TEST FOR UNSATURATED HYDROCARBONShexane + KMnO4 ===> no reaction toluene + KMnO4 ===> benzoic acid When alkenes like 1-pentene are oxidised with cold, alkaline KMnO4, dihydroxy compounds (diols or glycols) are formed. The KMnO4 gets decolorized.
KMnO4 reacts with unsaturated hydrocarbons but not with saturated hydrocarbons and aromatic hydrocarbons.PURPLE dilutes to LIGHT PURPLE = saturatedPURPLE to BROWN = unsaturatedPREPARATION OF ETHYNE AND TEST FOR FLAMMABILITYCaC2+2H2O=C2H2+Ca(OH)2
ACETYLENE: FLAMMABLE
EXPERIMENT 4:PREPARATION AND
PROPERTIES OF ESTERS AND SOAPS
PREPARATION OF SOME ESTERCH3COOH + CH3CH2OH → CH3COOCH2CH3 + H2O ACETIC ACID + ETHANOL ETHYL ACETATE + WATER
C6H4(OH)(COOH ) + CH3OH C6H4(OH)(COOCH3) + H2OSALICYLIC ACID + METHANOL METHYL SALICYLATE + WATER
CH3COOH + CH3(CH2)3CH2OH CH3COOCH2(CH2)3CH3 + H2OACETIC ACID + PENTANOL PENTYL ACETATE + WATER
C6H5COOH + CH3CH2OH C6H5COOCH2CH + H2O BENZOIC ACID + ETHANOL ETHYL BENZOATE + WATER
Saponification and Soap• Hydrolysis with a strong base• Triglycerides split into glycerol
and the salts of fatty acids • The salts of fatty acids are
“soaps”• KOH gives softer soaps
Properties of TriglyceridesHydrogenation
• Unsaturated compounds react with H2
• Ni or Pt catalyst• C=C bonds C–C bonds
Hydrolysis• Split by water and acid or enzyme catalyst• Produce glycerol and 3 fatty acids
Saponification
3+ Na+ -O C (CH2)14CH3
O
CH
CH2 OH
OH
CH2 OH
CH
CH2
CH2 O
O
O
C (CH2)16CH3
O
C
O
(CH2)16CH3
(CH2)16CH3C
O
+ 3 NaOH
salts of fatty acids (soaps)
Hydrogenation
CH
CH2
CH2 O
O
O
C
O
(CH2)5CH CH(CH2)7CH3
C
O
(CH2)5CH CH(CH2)7CH3
C
O
+
(CH2)5CH CH(CH2)7CH3
H23Ni
Product of Hydrogenation
Hydrogenation converts double bonds in oils to single bonds. The solid products are used to make margarine and other hydrogenated items.
CH
CH2
CH2 O
O
O
C (CH2)14CH3
O
C (CH2)14CH3
O
C (CH2)14CH3
O
HydrolysisTriglycerides split into glycerol and three fatty acids (H+ or enzyme catalyst)
CH
CH2
CH2 O
O
O
C (CH2)14CH3
O
C (CH2)14CH3
O
C (CH2)14CH3
O H2O+3
3+ HO C (CH2)14CH3
O
CH
CH2 OH
OH
CH2 OH
H+
SALTING OUT SOAPThe soap is separated from the saltwater and glycerin obtained from the saponification.FORMATION OF FATTY ACIDSCH3(CH2)16CO2
-Na+ + HCl → CH3(CH2)16CO2H + Na+ + Cl-
FORMATION OF SOAP SCUM2 CH3(CH2)16CO2
-Na+ + Mg2+ → [CH3(CH2)16CO2
-]2Mg2+ + 2 Na+
EXPERIMENT 5:PROPERTIES OF
ALCOHOLS, ALDEHYDES, AND
KETONES
• Common examples of alcohols with one, two, and three hydroxyl groups per molecule. The IUPAC name is given above each structural formula, and the common name is given below.
4C alcohols
1-butanol 2-butanol
CH2CH2CH3 CH2
OH
CHCH2CH3 CH3
OH
CHCH3 CH2
OH
CH3
1-isobutanol,
2-methyl-1-propanol
2-isobutanol,
2-methyl-2-propanol
CCH3 CH3
CH3
OH
• The carbonyl group (A) is present in both aldehydes and ketones, as shown in (B). (C) The simplest example of each, with the IUPAC name above and the common name below each formula.
4C aldehydes
butanal
isobutanal,
2-methylpropanal
CH
O
CH2CH2CH3
CH
O
CHCH3
CH3
4C ketones
2-butanone, (butanone)
C
O
CH2CH3 CH3
The end….thank you…