Lab Module 1: Chemical Formulas & Nomenclature PDF

FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Chemical Writing Lab Mod...

FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Chemical Writing Lab Module 1 Far Eastern University IAS – Dept. of Mathematics Biochemistry Cluster 1 Outline Chemical Formulas & Nomenclature Ionic Compounds Binary Covalent Compounds Chemical Equation Writing 2 1 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Chemical Formulas & Nomenclature 3 Ionic Compounds Ionic compounds are compounds made up of ions that are formed when atoms donate and receive electrons. The transfer of electrons lead to positive and negative charges (ions) that attract each and form an ionic bond. Cations – positively-charged atoms or molecules Anions – negatively-charged atoms or molecules Naming ionic compounds is usually based on the cation’s name followed by the anion’s name. 4 2 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Ionic Compounds Types of Ionic compounds 1. Binary ionic compounds – ionic compounds formed from just two elements and commonly ends with the suffix –ide 2. Ternary compounds – ionic compounds formed from a combination of more than two elements. They have variety of suffixes other than -ide 5 Rules in Naming Cations Cations formed from metal atoms bears the name of the metal itself. Ion Name !! Potassium ion "#! Sodium ion $#"! Calcium ion %&"! Magnesium ion 6 3 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Cations Some metal ions can have more than one charge such as those in the transition metals. We name them as the name of the metal itself and a Roman numeral enclosed in parenthesis to indicate the charge. Ion Name '( "! Iron (II) ion '( #! Iron (III) ion $)! Copper (I) ion $)"! Copper (II) ion 7 Rules in Naming Cations Usually, metals with two charges only can be named using their root Latin name / old metal name followed by the suffix –ous and –ic. The suffix –ous indicates the ion with the lowest charge, while –ic indicates highest. Ion Name Old Name Suffix '( "! Ferrous ion Latin: Ferrum -ous for +2 charge '( #! Ferric ion Latin: Ferrum -ic for +3 charge $)! Cuprous ion Latin: Cuprum -ous for +1 charge $)"! Cupric ion Latin: Cuprum -ic for +2 charge 8 4 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Cations Cations formed from nonmetal atoms have the suffix –ium There are only two of them Ion Name Derived from *! Hydronium ion Hydrogen (*) atom "*$! Ammonium ion Ammonia ("*#) 9 Rules in Naming Anions Monoatomic anions will have the suffix -ide Ion Name *% Hydride ion +"% Oxide ion $,% Chloride ion -. % Bromide ion 10 5 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Anions Polyatomic anions with oxygens are called oxyanions. They usually bear the suffix – ate for the common oxyanion, and –ite if is one oxygen less than the common. Ion Name Suffix "+#% Nitrate ion -ate since it is the common "+"% Nitrite ion -ite since it is one O less than common /+$"% Sulfate ion -ate since it is the common /+#"% Sulfite ion -ite since it is one O less than common 11 Rules in Naming Anions The following are the common oxyanions that you have to remember Ion Name Note $+#"% Carbonate ion Does not have –ite counterpart "+#% Nitrate ion 0+$#% Phosphate ion /+$"% Sulfate ion $,+#% Chlorate ion Extendable up to four versions 12 6 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Anions Some oxyanions can be extended to form four members. We add prefix per- to the oxyanion with one oxygen more than the common, and prefix hypo- to the oxyanion that is one oxygen less to that of the –ite version. Ion Name Note $,+$% Perchlorate ion One oxygen more than common $,+#% Chlorate ion Common oxyanion $,+"% Chlorite ion One oxygen less than common $,+% Hypochlorite ion One oxygen less than -ite 13 Rules in Naming Anions Anions derived by adding ! 1 to an oxyanion are named by adding as a prefix the word hydrogen/bi- or dihydrogen !"!"# + $$ → $!"!# carbonate hydrogen carbonate bicarbonate &"%!# + $$ → $&"%"# + $$ → $" &"%# phosphate hydrogen phosphate dihydrogen phosphate biphosphate 14 7 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Summary You must remember the names of the anions and cations in Chemistry. Just simply follow the rules or use the table beside and use it as your memory guide. 15 Formula of Ionic Compounds Since we now know the names of ions, we can now make ionic compounds. Ionic compounds are made by combining cations and anions in right proportion so there would be no charge in its final form. The right proportion of cations and anions can be easily obtained by crisscrossing their number of their charges. 16 8 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Formula of Ionic Compounds Suppose we are to determine the formula for an ionic compound composed of sodium ion and chloride ion. !"! #$ " !"##$# or !"#$ the 1 in -1 charge becomes the 1 in +1 charge becomes we do not write the subscript 1 the subscript of Na the subscript of Cl as it is obvious We crisscross the number of the charge to make it the subscript. The name of an ionic compound is cation’s name followed by anion’s name. The name of this compound is sodium chloride with formula "#$% 17 Formula of Ionic Compounds Suppose we are to determine the formula for an ionic compound composed of calcium ion and bromide ion. #"$! %& " #"#%&$ or #"%&$ the 1 in -1 charge becomes the 2 in +2 charge becomes we do not write the subscript 1 the subscript of Ca the subscript of Br as it is obvious The name of the compound is calcium bromide with a formula $#&'2 18 9 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Formula of Ionic Compounds Suppose we are to determine the formula for an ionic compound composed of barium ion and oxide ion. %"$! '$" %"$'$ or %"' the 2 in -2 charge becomes the 2 in +2 charge becomes Reduce the subscripts to the subscript of Ba the subscript of O lowest terms if possible The name of the compound is barium oxide with a formula &#( 19 Formula of Ionic Compounds Suppose we are to determine the formula for an ionic compound composed of ammonium ion and phosphate ion. !(%! )'%&" '(! " )*! # or '(! " )*! the 3 in -3 charge becomes the 1 in +1 charge becomes Note that the polyatomic ions must be enclosed in a parenthesis if they have a subscript the subscript of (NH4) the subscript of (PO4) greater than 1. You can remove the parenthesis if the subscript is 1. The subscript of the polyatomic ion should be outside the parenthesis. The name of the compound is ammonium phosphate with a formula "!3 4)(3 20 10 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Ionic Compounds: Exercises I.Name the following: II. Identify the formula: 1. *2+(3 1. Strontium nitride 2. &# (! 2 2. Barium sulfate 3. Calcium hydrogen carbonate 3. "!3&' 4. Nickel (II) perchlorate 4. $'2(4 5. Sodium cyanide 5. $, "(4 2 21 Formulas of Acids Acids are ionic compounds whose cation is solely hydronium ion ! 1. The number of ! 1 ions in the formula for acid should be equal to the numerical charge of the anion pair. For an acid with anion +(325, there should be 2 ! 1 and the formula is !2+(3. If it is one oxygen less, it would be called a bisulfate ion !+(35. 22 11 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Acids Acids whose anions with suffix –ide are named by changing –ide to –ic followed by the word acid. A prefix hydro- is also needed. Anion Anion Name Acid Formula Acid Name '% Fluoride ion *' Hydrofluoric acid $,% Chloride ion *$, Hydrochloric acid -. % Bromide ion *-. Hydrobromic acid $" % Cyanide ion *$" Hydrocyanic acid 23 Rules in Naming Acids Acids whose anions with suffix –ate and -ite are named by changing –ate to –ic and –ite to –ous, followed by the word acid Anion Anion Name Acid Formula Acid Name $,+$% Perchlorate ion *$,+$ Perchloric acid $,+#% Chlorate ion *$,+# Chloric acid $,+"% Chlorite ion *$,+" Chlorous acid $,+% Hypochlorite ion *$,+ Hypochlorous acid 24 12 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Formulas of Bases Bases are ionic compounds whose anion is solely hydroxide ion (! 5. The number of (! 5 ions in the formula for base should be equal to the numerical charge of the cation pair. For a base with cation &#21, there should be 2 (! 5 and the formula is &# (! 2. 25 Rules in Naming Bases We name cations first and then anion with rules like previously discussed. Just add the ending hydroxide. Cation Cation Name Base Formula Base Name Iron (II) hydroxide '( "! Iron (II) / Ferrous '( +* " Ferrous hydroxide Iron (III) hydroxide '( #! Iron (III) / Ferric '( +* # Ferric hydroxide 6,#! Aluminum 6, +* # Aluminum hydroxide "#! Sodium "#+* Sodium hydroxide 26 13 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Names of Hydrates Hydrates are ionic compounds with specific number of water molecules attached to the molecule. We indicate the number of hydrates by using Greek prefixes then the word hydrate. Hydrate Name -#$," 7 2 *"+ Barium chloride dihydrate :;$, 7 *"+ Lithium chloride monohydrate %&/+$ 7 7 *"+ Magnesium sulfate heptahydrate Copper (II) sulfate pentahydrate $)/+$ 7 5 *"+ Cupric sulfate pentahydrate 27 Names of Binary Molecules Binary molecular compounds are covalent molecules with two elements only. Example $(2 +(2 "(2 Naming is same to that of the ionic compounds. 28 14 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Formula for Binary Molecules The name of the element farther to the left of the periodic table is usually written first. If it contains oxygen, we write the oxygen always as the last. Example !2( is written this way since ! is the leftmost element in PT $%(35 is written this way, not (3$% 5, since ( should always be at the last (the naming rule for this is the rule for anions) 29 Formula for Binary Molecules If both elements are in the same group in the periodic table, write the heaviest element first. Example +(2 is written this way, not (2+, since + is heavier than ( and it should follow the previous rule about writing ( 30 15 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Rules in Naming Binary Molecules Now we know the order of element in writing binary molecules, we name the second element with an ending –ide. Also, indicate the number of the second element using Greek prefix mono-, di-, tri-... If the second element’s name begins with vowels (such as oxide), drop the a or o in the prefix. Do not use mono- prefix for the first element. 31 Rules in Naming Binary Molecules Example Molecule Name Note "'# Nitrogen trifluoride No mono- for nitrogen $,"+ Dichlorine monoxide Not monooxide. Drop the o ""+$ Dinitrogen tetroxide Not tetraoxide. Drop the a 0$/&' Tetraphosphorus decasulfide 32 16 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Chemical Equation Writing 33 Chemical Equations Terms A chemical reaction is a process in which a substance Reactants are the substances being used in a is transformed into another substance/s. chemical reaction Products are the substances being produced in a Chemical Reactions are always represented using chemical reaction chemical equations Reaction arrow indicates the direction of the reaction. It could be single-headed arrow → or reactants products an equilibrium arrow ⇌ Chemical formula represent the number and $4!> P + 5 (2 P → 3 $(2(P) + 4 !2((P) types of atoms present in a substance chemical formula Subscript indicates the number of a specific subscript atoms in a chemical formula state of matter coefficient or Coefficient or stoichiometric coefficient tells you stoichiometric coefficient the correct proportion of the substance needed in a chemical reaction reaction arrow State of matter represent whether the substance is in solid (+), liquid (-), gas (.), or dissolved in water (/0), known as aqueous 34 17 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Writing Chemical Equations from Words Writing chemical equation from sentences is easy if you recognize some keywords and you know the chemical formula based on its name. Example Calcium hydroxide reacts with hydrochloric acid to produce calcium chloride and water. Calcium hydroxide reacts with hydrochloric acid to produce calcium chloride and water. !" #$ " $!% !"!%" $" # This tells you that !" #$ ! This tells you that !"!%! Therefore, the formula and $!% areisreactants $# (! 2 + !$% → !$#$%2 + !2 ( or $# (! and $ # are products 2 + 2 !$% → $#$%2 + 2 !2( when balanced. 35 Writing Chemical Equations from Words Writing chemical equation from sentences is easy if you recognize some keywords and you know the chemical formula based on its name. Example Methane burns with oxygen to form carbon dioxide and water. !$$ #" !#" $" # This tells you that !$" This tells you that !#! and #! are reactants and $!# are products Therefore, the formula is $!3 + (2 → $(2 + !2( or $!3 + 2 (2 → $(2 + 2 !2( when balanced. 36 18 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Writing Chemical Equations from Words Tips These are some keywords used in sentences describing chemical equations. It would be handy if you are able to recognize these: Keywords for reactants Keywords for products reacts with to produce / produces combusted with to yield / yields combined with to form / forms The reaction between … decomposes to produce … 37 Exercises 1. Glucose is combusted with oxygen to produce carbon dioxide and water. 2. Methanol is combusted with oxygen to form carbon dioxide and water. 3. Lithium reacts with water to form lithium hydroxide and hydrogen gas. 4. The reaction of ammonia and carbon dioxide produces urea "!2 2$( and water 5. Methanol is formed from carbon monoxide and hydrogen gas. 38 19 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 END Thank you for listening! 39 20 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Introduction to Inorganic and Organic Chemistry Lec Module 1 Far Eastern University IAS – Dept. of Mathematics Biochemistry Cluster 1 Outline INORGANIC CHEMISTRY ORGANIC CHEMISTRY Forces of Attraction Hydrocarbons Intramolecular Forces of Attraction Types of Functional Groups Intermolecular Forces of Attraction Ethers Polarity Alcohols Acids & Bases Thiols Definitions of Acids & Bases Amines pH Scale Aldehydes Ketones Carboxylic Acids and Derivatives Polarity of Organic Substances 2 1 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Forces of Attraction INORGANIC CHEMISTRY 3 Forces of Attraction Attractive forces between molecules allows them to form condensed phases of matter. There are two primary types of attractive forces: 1. Intramolecular forces are the forces that hold atoms together within a molecule (also known as chemical bonds. 2. Intermolecular forces are forces that exist between molecules. 4 2 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intramolecular Forces of Attraction Intramolecular forces are the forces that hold atoms together within a molecule. There are three types of chemical bonds: 1. Ionic Bond 2. Covalent Bond 3. Metallic Bond 5 Intramolecular Forces of Attraction Ionic bond It is formed when there is a complete transfer of valence electron between two atoms producing cations and anions. The two charged particles are then attracted to each other by Coulombic forces. 6 3 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intramolecular Forces of Attraction Covalent bond This bond is formed between atoms that have similar electronegativities. Because both atoms have similar affinity for electrons and neither tends to donate them, they share electrons in order to achieve octet configuration and become more stable. There are two types of covalent bonds due to the electronegativity difference of participating atoms: 1. Nonpolar covalent bond 2. Polar covalent bond 7 Intramolecular Forces of Attraction Nonpolar covalent bond A nonpolar covalent bond is formed between same atoms or atoms with very similar electronegativities—the difference in electronegativity between bonded atoms is less than 0.4. 8 4 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intramolecular Forces of Attraction Polar covalent bond A polar covalent bond is formed when atoms of slightly different electronegativities share electrons. The difference in electronegativity between bonded atoms is between 0.4 and 1.8. Electron-poor Region H F Electron-rich Region 9 Intramolecular Forces of Attraction Metallic bond This type of covalent bonding specifically occurs between atoms of metals, in which the valence electrons are free to move through the lattice. This bond is formed via the attraction of the mobile electrons (sea of electrons) and the fixed positively charged metal ions. 10 5 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intramolecular Forces of Attraction Relative Strength of Intramolecular Forces of Attraction INTRAMOLECULAR FORCE BASIS OF FORMATION RELATIVE STRENGTH Metal cations to delocalized Metallic bond 1, strongest electrons Ionic bond Cations to anions 2 Partially charged cation to partially Polar covalent bond 3 charged anion Nonpolar covalent bond Nuclei to shared electrons 4, weakest 11 Intermolecular Forces of Attraction Intermolecular forces are much weaker than the intramolecular forces of attraction but are important because they determine the physical properties of molecules like their boiling point, melting point, density, and enthalpies of fusion and vaporization. There are three types of intermolecular forces of attraction: 1. Dipole – dipole interactions 2. Hydrogen bonding 3. Van der Waals forces / London dispersion forces 12 6 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intermolecular Forces of Attraction Dipole-dipole interactions These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule. 13 Intermolecular Forces of Attraction Hydrogen bonding This is a special kind of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom. 14 7 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Intermolecular Forces of Attraction London Dispersion a.k.a. Vander waals. This type of interaction arises as a result of “temporary dipoles induced” in atoms or molecules due to collisions. 15 Intermolecular Forces of Attraction Relative strength of intermolecular forces of attraction INTERMOLECULAR FORCE OCCURS BETWEEN RELATIVE STRENGTH Strongest of the dipole-dipole Hydrogen bonding H-F, H-N, or H-F attractions Dipole-dipole attraction Partially oppositely charged ions Strong London dispersion attraction Temporary or induced dipoles Weakest 16 8 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Forces of Attraction Exercises What type of intermolecular forces exist between each of the following molecules? HBr, CH4, SO2 17 Polarity INORGANIC CHEMISTRY 18 9 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Polarity of Molecules Polar covalent bond: Bonding electrons are shared unequally Nonpolar covalent bond: Bonding pair of electrons is shared equally by the bonded atoms Electronegativity: Tendency of an atom to attract shared electrons of a covalent bond Electrons of a covalent bond are attracted toward atoms of highest electronegativity Bond polarization: Result of shared electrons being attracted to the more electronegative atom of a bonded pair of atoms 19 Polarity of Molecules 20 10 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Polarity of Molecules Polar: Molecule containing polarized bonds in which the resulting charges are distributed nonsymmetrically throughout the molecule Nonpolar: Molecule containing no polarized bonds in which the resulting charges are distributed symmetrically throughout the molecule 21 Polarity of Molecules 22 11 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Acids and Bases INORGANIC CHEMISTRY 23 Definitions of Acids and Bases Characteristics of Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with carbonates and bicarbonates to produce carbon dioxide gas Characteristics of Bases Have a bitter taste. Feel slippery. Many soaps contain bases. 24 12 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Definitions of Acids and Bases There are several definitions in Chemistry describing acidic and basic molecules. The following definitions are Arrhenius Definition Bronsted-Lowry Definition Lewis Definition 25 Definitions of Acids and Bases ARRHENIUS DEFINITION Acid is a substance that increases the concentration of !! "" /!" when it dissociates. Base is a substance that increases the concentration of "!# when it dissociates. Proton refers to !" ions. Example Arrhenius Acid !$% → !" + $% # Arrhenius Base ()"! → ()" + "!# 26 13 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Definitions of Acids and Bases BRØNSTED-LOWRY DEFINITION Brønsted and Lowry classified acids as proton donors, and bases as proton acceptor. This is broader than Arrhenius’ definition since !!"" and "! # are no longer the only basis for acidity and basicity. Example !#$ + !$" ⇌ !!"" + #$ # !#$ + '!! ⇌ '!%"#$ # 27 Definitions of Acids and Bases BRØNSTED-LOWRY DEFINITION: CONJUGATE ACIDS AND BASES Conjugate acids and bases are related to each other by the gain or loss of one !" 28 14 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Definitions of Acids and Bases LEWIS DEFINITION A Lewis acid is a substance that can accept a pair of electrons. A Lewis base is a substance that can donate a pair of electrons 29 pH Scale pH – A Measure of Acidity (! = −log[! "] If ! " = ["! #] the solution is neutral ! " = 1×10#& (! = 7 If ! " > ["! #] the solution is acidic ! " > 1×10#& (! < 7 If ! " < ["! #] the solution is basic ! " < 1×10#& (! > 7 30 15 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Hydrocarbons ORGANIC CHEMISTRY 31 What is Organic Chemistry? Organic Chemistry is the chemistry of the compounds of carbon. A feature of organic compounds is that they comprise the chemistry of carbon and a few other elements, chiefly: 1 7 8 Hydrogen Nitrogen Oxygen 1.0078 14.006 15.999 Some also contain sulfur (S), halogens (Fl, Cl, Br, or I), and phosphorus (P) 32 16 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 The Carbon Atom 6 - Can share 4 valence electrons and form 4 covalent bonds Carbon - Able to bond with one another to form 12.009 long chains and rings - Forms single, double and triple bonds to other carbon atoms - Has the ability to form an immense diversity of compounds 33 Structures of Organic Compounds Ethane actual number of atoms of each element in a molecule Molecular Formula C2H6 Expanded Formula two-electron covalent bond as a line drawn (Kekule or Line Bond between atoms Structure) atoms are listed in order in the molecule's Condensed Formula CH3CH3 structure Skeletal Formula carbon skeleton in the structure. Vertices represents C. Atoms other than C or H are still shown 34 17 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Hydrocarbons Hydrocarbon: A compound composed only of carbon and hydrogen. 35 Hydrocarbons The IUPAC system – systematic naming of compounds IUPAC name includes: Parent name (longest carbon chain) Names of substituents Location of substituents 36 18  CARBON ATOMS OF ALKANE CARBON ATOMS OF ALKANE FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria meth undec 8/14/24 eth dodec 3 prop tridec 4 but tetradec 5 pent pentadec hex eicos 7 hept Hydrocarbons: Alkanes triacont oct tetracont 9 non pentacont Identity of the parent chain – the longest consecutive chain of carbons. Name the dec parent chain based on the number of Carbon numbers. hect If there is a competition between two chains of equal length, then choose the chain with the eater number of substituents. Substituents are branches connected to the parent chain: Correct Incorrect (3 substituents) (2 substituents) The term “cyclo” is used to indicate the presence of a ring in the structure of an alkane. For ample, these compounds 37 are called cycloalkanes: Cyclopropane Cyclobutane Cyclopentane Hydrocarbons: Alkanes Identify the parent chain - the longest consecutive chain of carbons. If the parent chain is cyclic, add the prefix “cyclo” 11/07/16 12:05 PM 38 19 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Hydrocarbons: Alkanes Exercise Identify and provide a name for the parent in the following compound: 39 Types of Functional Groups 40 20 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Functional Groups 41 Functional Groups “pattern recognition” 42 21 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Ethers The functional group of an ether is an oxygen atom bonded to two carbon atoms. The simplest ether is dimethyl ether and most common ether is diethyl ether. Some examples are presented below. CH3 -O-CH3 CH3 CH2 -O-CH2 CH3 Dimethyl ether Diethyl ether 43 Alcohols A compound that containing an -OH (hydroxyl group) bonded to a tetrahedral carbon. Parent chain alcohols will have ‘-ol’ as the suffix. As a substituent, the prefix is ‘hydroxy-’. 44 22 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Thiols Thiol is a compound containing an -SH (sulfhydryl group). Thiols are known for their unpleasant odor. To show that the compound is a thiol, the final -e of the parent alkane is retained and the suffix ‘-thiol’ added. Common names for simple thiols are derived by naming the alkyl group bonded to -SH and adding the word "mercaptan". 45 Amines Amines are derivatives of ammonia, and are designated as primary, secondary, or tertiary. Naturally occurring amines are called alkaloids Parent chain amines have ‘-amine’ as the suffix. As substituents, they use the prefix ‘amino-.’ 46 23 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Amines Some naturally occurring amines are vital to neurochemistry: 47 Aldehydes Aldehyde is a functional group composed of a carbonyl group (C=O) bonded to a hydrogen atom. As a parent chain, it uses the suffix ‘-al’. In methanal (formaldehyde), the simplest aldehyde, the carbonyl group is bonded to two hydrogens. In other aldehydes, it is bonded to one hydrogen and one carbon group. (See structure below) 48 24 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Ketones Ketone is a functional group composed of a carbonyl group bonded to two carbon groups (alkyl group). As a parent chain, it uses the suffix ‘-one’. In the example below (Propanone), two methyl group (CH3) are bonded to the carbonyl group (C=O) 49 Carboxylic Acids Carboxylic acids are organic molecules that have a carboxyl group (-COOH). It is a carbonyl group (-C=O), wherein the carbon is also attached to a hydroxyl group (-OH). Parent chain carboxylic acids following IUPAC nomenclature will use the suffix ‘-oic acid.’ Some acids have common names that are widely accepted. Ethanoic acid (IUPAC), Acetic acid (Common) 50 25 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Carboxylic Derivatives: Esters Esters are carbonyl group (C=O) bonded to an -OR group. R may be alkyl or aryl. O O O O C H3 C O CH 2 C H3 O O O Ethyl ethanoate Diethyl pentanedioate A five-membered (Ethyl acetate) (Diethyl glutarate) lactone 51 Carboxylic Derivatives: Amides Amides are carbonyl group bonded to a nitrogen atom. O O O O α α β NH NH β NH NH A four-membered lactam A seven-membered lactam A four-membered lactam A seven-membered lactam (a β-lactam) (a β-lactam) 52 26 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Carboxylic Derivatives: Acid Anhydrides Anhydrides (Acid Anhydrides) are two carbonyl groups bonded to the same oxygen. The anhydride may be symmetrical (from two identical acyl groups), or mixed (from two different acyl groups). To name an anhydride, drop the word "acid" from the name of the carboxylic acid from which the anhydride is derived and add the word "anhydride”. 53 Polarity of Organic Substances 54 27 FEU BIOCHEMISTRY PROPERTY. All forms of reproduction or replication are prohibited. Seek permission from Ms. Jessa Natividad and Ms. Erika Viloria 8/14/24 Polarity of Organic Substances Organic Polarity Alkanes Non polar Alkenes Non polar Alkynes Non polar Ethers Slightly polar; but mostly non polar Alcohols Polar Thiols Non polar Aldehydes Polar Ketones Polar Carboxylic Acids Polar 55 END Thank you for Listening! 56 28 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Types of Inorganic and Organic Chemical Reactions Lab Module 2 Far Eastern University IAS – Dept. of Mathematics Biochemistry Cluster 1 Outline Types of Inorganic Reactions Specific Types of Organic Reactions General Types of Chemical Reactions Hydration and Hydrogenation of Synthesis Alkenes Decomposition Dehydration and Oxidation of Single Displacement Reaction Alcohols Double Displacement Reaction Reduction and Oxidation of Aldehydes Specific Types of Chemical Reduction of Ketones Reactions Reduction of Carboxylic Acids Combustion Reaction Precipitation Reaction Acid-Base Reaction Precipitation Reaction 2 1 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions Inorganic Reactions 3 Review There are two types of changes that matter can undergo Physical Changes Matter transforms into different physical state Example: Melting of ice to liquid water Chemical Change / Chemical Reaction Matter changes its chemical identity from one compound to another Example: Burning of wood produces carbon dioxide and water molecules 4 2 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions There are four general chemical reactions based on the structure of the chemical formula, namely 1. Synthesis / Combination Reaction 2. Decomposition Reaction 3. Single Displacement Reaction 4. Double Displacement / Metathesis Reaction 5 General Types of Chemical Reactions Synthesis or Combination Reaction - occurs when the reactants combine to form a single product. The general form is !+# →% Examples & ' + (! ) → &(! ) 2 ,) ' + (! ) → 2 ,)((') 6 3 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions Decomposition Reaction - occurs when a single reactants decomposes, usually by heating or by applying electricity, to form many products. The general form is ! →#+%+⋯ Examples 2 0!( 1 → 2 0! ) + (! ) 2 2%1(" ' → 2 2%1 ' + 3 (!()) 7 General Types of Chemical Reactions Single Displacement Reaction - occurs when one element replaces another element. !# + % → !% + # Examples 2 !)4(" 56 + 78 ' → 2 !) ' + 78 4(" ! 56 ,) ' + 2 0%1 56 → 0! ) + ,)%1! 8 4 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions When do single replacement reactions occur? Single-replacement reactions only occur when the element that is doing the replacement is more reactive than the element that is being replaced. The reactivity of elements can be described by activity series. Note: The element must be more reactive than the compound! 9 General Types of Chemical Reactions Single Displacement Reaction Example ,) + 20%1 → ,)%1! + 0! This reaction will occur because the element Mg is more reactive than H. 0! + ,)%1! → no reaction This reaction is not possible because the element H2 is less reactive than Mg. 10 5 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions Single Displacement Reaction Example #A! + 2 2B → 22#A + B! This reaction will occur because the element Br2 is more reactive than I. 22#A + B! → no reaction This reaction is not possible because the element I2 is less reactive than Br. 11 General Types of Chemical Reactions Single Displacement Reaction Exercises Identify if there will be reaction or none. 1. !C + %C&(# → 2. ,) + %C&(# → 3. %5 + 0!( → 12 6 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 General Types of Chemical Reactions Double Displacement or Metathesis Reaction - occurs the elements switch pairs, forming new compounds !# + %D → !D + %# Examples 45!& + 2 0%1 → 2 45%1 + 0!& #5%1! + 45!&(# → #5&(# + 2 45%1 13 Specific Types of Chemical Reactions Inorganic Reactions 14 7 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Chemical Reactions More specific types of chemical reactions are the following 1. Combustion Reaction 2. Precipitation Reaction 3. Acid-Base Reaction 4. Oxidation-Reduction / Redox Reaction 15 Combustion Reactions Combustion reaction occurs when an organic compound (substances containing CHO) burns in air/oxygen producing water vapor and carbon dioxide. The reaction goes into completion. %$ 0% (& + (!()) → %(! ) + 0!(()) where E, G, H are the subscripts Example %"0' ) + 5 (! ) → 3 %(! ) + 4 0!(()) 16 8 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Combustion Reactions If the combustion reaction is not complete, soot (%) or toxic carbon monoxide (%() will be formed, instead of carbon dioxide %$ 0% (& + (!()) → %( ) + 0!(()) %$ 0% (& + (!()) → % ' + 0!(()) where E, G, H are the subscripts Example 2 %"0' ) + 7 (! ) → 6 %( ) + 8 0!(()) %"0' ) + 2 (! ) → 3 % ' + 4 0!(()) 17 Reactions in Aqueous Solutions Most ionic compounds are soluble in water. That means, the ionic species from a compound separates from each other. This is called the dissociation/ionization process. Examples 45%1 ' → 45( 56 + %1 ) 56 0%1 56 → 0 ( 56 + %1 )(56) 18 9 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Reactions in Aqueous Solutions When you mix different aqueous solutions of different substances, chemical reactions may or may not take place. Example Mixing salt and vinegar when making condiments do not produce any chemical reactions (i.e. bubbling) 19 Reactions in Aqueous Solutions So, when will a reaction take place in aqueous solutions? A mixture of different aqueous solution may produce chemical reactions if: a. There are ions that can combine to form insoluble substances (precipitation reaction); b. There are ions that can neutralize each other, forming neutral substances (acid- base reaction); and c. The species present can transfer electrons (redox reaction) 20 10 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Precipitation Reactions Precipitation reaction occurs when the present ions in a solution pairs to form an insoluble compound, known as the precipitate. The insoluble compound may be solid or colloidal in form. Example ,)&(# 56 + 2 45(0 56 → ,) (0 ! ' + 45!&(#(56) https://youtu.be/KDR9HJhuvgQ 21 Precipitation Reactions In order to predict whether the reaction will produce precipitates, we must remember the solubility rules. If the solution contains ions that can form an insoluble substance when paired, then the precipitation reaction will occur. 22 11 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Precipitation Reactions Given the previous example, how did we know that ,) (0 ! precipitate will be formed? The reactants are ,)&(# and 45(0. These ionic substances will dissociate accordingly. ,)&(# 56 → ,)!( 56 + &(#!) 56 45(0 56 → 45( 56 + (0 )(56) So ,)&(# 56 + 45(0 56 → ,)!( 56 + &(#!) 56 + 45( 56 + (0 ) 56 23 Precipitation Reactions ,)&(# 56 + 45(0 56 → ,)!( 56 + &(#!) 56 + 45( 56 + (0 ) 56 The next step would be to check the existing ions if at least one combination among them can form a precipitate. Looking at the solubility rules, ,)!( can be paired with (0 ) to form an insoluble substance ,) (0 ! Recall that !"!" #$ $ → !" #$ ! 24 12 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Precipitation Reactions ,)&(# 56 + 45(0 56 → ,)!( 56 + &(#!) 56 + 45( 56 + (0 ) 56 Since ,)!( and (0 ) can form a precipitate ,) (0 !, precipitation reaction will occur. 45( and &(#!) did not participate in the precipitation reaction, hence they are called spectator ions. These ions can form 45!&(# when combined. 25 Precipitation Reactions In summary ,)&(# 56 + 45(0 56 → ,)!( 56 + &(#!) 56 + 45( 56 + (0 ) 56 ,)&(# 56 + 45(0 56 → ,) (0 !(') + 45!&(#(56) 26 13 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Precipitation Reactions: Exercises Predict if a precipitate will form upon mixing the following substances. Write the molecular equation and the net ionic equations: 1. 45!&(# and #5%1! 2. %C 4(" ! and 40# !&(# 3. !1 4(" " and 45(0 27 Acid-Base Reactions Acids are substances whose cation is a proton 0 (. Bases are substances whose anion is a hydroxide ion (0 ). When acids and bases combine, 0 ( will react with (0 ) to produce water and salts. This is called the neutralization reaction. 0 ( 56 + (0 ) 56 → 0!( 1 5NOP + Q5'R → 0!( 1 + '51S' 28 14 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Acid-Base Reactions Example 0%1 56 + 45(0 56 →? First, we must dissociate 0%1 and 45(0 into their respective ions. 0%1 56 → 0 ( 56 + %1 ) 56 45(0 56 → 45( 56 + (0 )(56) 29 Acid-Base Reactions The 0 ( from acid will combine with (0 ) of the base to produce water. The remaining anion and cation can be paired to form salt. 0%1 56 → 0 ( 56 + %1 ) 56 45(0 56 → 45( 56 + (0 )(56) 0%1 56 + 45(0 56 → 0!((1) + 45%1(56) 30 15 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Oxidation-Reduction Reactions This type of reaction involves transfer of electrons between two species. In oxidation- reduction reactions or redox reaction, two reactions are happening simultaneously, Oxidation reaction – substances lose / give off electrons Reduction reaction – substances gain / accept electrons This can be easily memorized by the mnemonic OIL RIG oxidation is losing (electron) / reduction is gaining (electron) 31 Oxidation-Reduction Reactions If an element is oxidized, its oxidation number (oxidation state) will increase. If it is reduced, its oxidation number will decrease. What is an oxidation number? Oxidation number is the actual charge of an atom in a compound or an element. How do we know the oxidation number of an element? 32 16 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Oxidation Number Oxidation number is the charge of an atom (free state or in a molecule) if electrons around it were completely transferred, rather than shared. 33 Review: Oxidation Number Exercises With all the rules, identify the oxidation numbers of each element in the following substances. 1. 40" 2. %5( 3. %A!(*)! 4. ,8(#) 5. US%1+) 34 17 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Oxidation-Reduction Reactions In redox reactions, two reactions are happening simultaneously. One of which is the oxidation reaction where a species will lose electrons. The other is reduction reaction where a species will gain electrons. (OIL RIG) Remember that when an element oxidizes, its oxidation number increases, and when it is reduced, its oxidation number decreases. 35 Oxidation-Reduction Reactions The substance that lost electrons is called the reducing agent. The substance that gained electrons is called the oxidizing agent. The complete mnemonic tool to memorize all of these is LEORA GEROA losing electron, oxidation, reducing agent / gaining electron, reduction, oxidizing agent 36 18 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Oxidation-Reduction Reactions Consider 78 ' + 0 ( 56 → 78!( 56 + 0! ) unbalanced The oxidation number of 78 increased from 0 to +2, hence it is oxidized. The oxidation number of 0 decreased from +1 to 0, hence it is reduced. 37 Oxidation-Reduction Reactions: Exercise Identify the oxidation and reduction reaction; and identify the oxidizing agent and the reducing agent. 1. 78 ' + %C!( 56 → 78!( 56 + %C ' 2. !1 ' + VR "( 56 → !1 "((56) + VR(') 3. 4O !( 56 + %A ' → 4O ' + %A !((56) 38 19 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions 39 Specific Types of Organic Reactions The types of organic reactions an organic molecule can participate in is largely dependent on the functional groups present. In biochemistry, the biomolecules being studied are organic in nature, and will behave similarly to organic chemicals. Acetaldehyde (an aldehyde) undergoing oxidation to form acetic acid (a carboxylic acid) The carbonyl group of a sugar (a biomolecule) undergoing oxidation to form the carboxyl group of a sugar acid. 40 20 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Hydration of Alkenes An addition reaction wherein the double bonds of an alkene are broken and water is added to the molecule to form an alcohol. Organic Chemistry Example Biochemistry Example 41 Specific Types of Organic Reactions Hydrogenation of Alkenes An addition reaction wherein the double bonds of an alkene are broken and hydrogen atoms are added to the molecule to form an alkane (C-C bonds only). Organic Chemistry Example Biochemistry Example 42 21 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Dehydration of Alcohols An elimination reaction wherein water is removed from an alcohol to form an alkene (C=C bond). Organic Chemistry Example Biochemistry Example 43 Specific Types of Organic Reactions Oxidation of Alcohols A redox reaction wherein an alcohol is oxidized into an aldehyde, a ketone or a carboxylic acid, depending on the type of alcohol and the strength of the oxidizing agent. Organic Chemistry Example Biochemistry Example 44 22 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Reduction of Aldehydes A redox reaction wherein an aldehyde is reduced into a primary alcohol by a reducing agent. Organic Chemistry Example Biochemistry Example 45 Specific Types of Organic Reactions Oxidation of Aldehydes A redox reaction wherein an aldehyde is further oxidized into a carboxylic acid by a reducing agent. Organic Chemistry Example Biochemistry Example 46 23 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Reduction of Ketones A redox reaction wherein a ketone is converted into a secondary alcohol by a reducing agent. Organic Chemistry Example Biochemistry Example 47 Specific Types of Organic Reactions Reduction of Carboxylic Acids A redox reaction wherein a carboxylic acid is into a primary alcohol by a strong reducing agent. Organic Chemistry Example 48 24 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Exercise: Identify what specific type of reaction is shown below. 1. 2. 49 Specific Types of Organic Reactions Exercise: Identify what specific type of reaction is shown below. 3. 4. 50 25 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Specific Types of Organic Reactions Exercise: Identify what specific type of reaction is shown below. 5. 6. 51 END Thank you for Listening! 52 26 FEU Biochemistry Property. All forms of replicatin are prohibited. Seek approval from Ms. Jessa Natividad and Ms. Erika Viloria 8/13/24 Lipid Structure & Function Lab Module 3 Far Eastern University IAS – Dept. of Mathematics Biochemistry Cluster 1 Outline Introduction to Lipids Lipids According to Function & Structure Simple Lipids (Fatty Acids & Triacylglycerols) Nomenclature Physical Properties Chemical Reactions Complex Lipids (Phospholipids, Sphingolipids, Glycolipids, & Derivatives) Structure Function Derived Lipids (Eicosanoids, Steroids & Cholesterol) Lipoproteins 2