MODULE BMODULE B

Basic ChemistryBasic Chemistry

Lesson #3 – Part 2Lesson #3 – Part 2

Nomenclature & Nomenclature &

Oxidation-Reduction Oxidation-Reduction ReactionsReactions

ObjectivesObjectives

At the end of this module, the student willAt the end of this module, the student will

– Define terms associated with the naming of Define terms associated with the naming of organic compounds and oxidation-reduction organic compounds and oxidation-reduction reactions. reactions.

– Describe the steps for naming inorganic Describe the steps for naming inorganic compounds, (ionic compounds, covalent compounds, (ionic compounds, covalent compounds, and compounds with polyatomic ions).compounds, and compounds with polyatomic ions).

– Define the components of a chemical reaction.Define the components of a chemical reaction.– Give an example of an oxidation-reduction reaction Give an example of an oxidation-reduction reaction

in Respiratory Therapy.in Respiratory Therapy.– Explain how the different chemical reactions take Explain how the different chemical reactions take

place.place.

Web SitesWeb Sites

http://www.geocities.com/Athens/Thehttp://www.geocities.com/Athens/Thebes/5118/ic/names1.htmbes/5118/ic/names1.htm

http://en.wikipedia.org/wiki/Systemathttp://en.wikipedia.org/wiki/Systematic_nameic_name

NomenclatureNomenclature

Definition: A system of words used to Definition: A system of words used to name things in a particular discipline.name things in a particular discipline.

The name of a compound has to The name of a compound has to include enough information to tell include enough information to tell chemists the composition and chemists the composition and structure of the compound.structure of the compound.

There are over 18 million compounds.There are over 18 million compounds.

NomenclatureNomenclature

IonsIons Simple ionsSimple ions Polyatomic ionsPolyatomic ions

Inorganic CompoundsInorganic Compounds

Ionic compoundsIonic compounds Molecular compoundsMolecular compounds

Simple IonsSimple Ions Metal Cations with only one formMetal Cations with only one form

(representative)(representative)– Identify the metalIdentify the metal– Add “ion”Add “ion”

KK++ = Potassium ion = Potassium ion

Metal Cations with more than one formMetal Cations with more than one form (transition)(transition)– Identify the metalIdentify the metal– Give the charge on the ion a roman Give the charge on the ion a roman

numeral in parenthesesnumeral in parentheses– Add “ion”Add “ion”

CrCr+2+2 = Chromium (II) ion = Chromium (II) ion

+

Simple ionsSimple ions

Anions Anions (representative)(representative)

– Replace the ending of the element with Replace the ending of the element with “ide”“ide”

– Add “ion”Add “ion” Cl- = Chloride ionCl- = Chloride ion

-

PracticePractice

Na+Na+

Al Al 3+ (representative)3+ (representative)

Cr Cr 3+ (transition)3+ (transition)

Br-Br-

Polyatomic IonsPolyatomic Ions

Ions with more than one atomIons with more than one atom– COCO33 -2-2

Most contain oxygenMost contain oxygen– HCOHCO33

--

Most are anionsMost are anions– OHOH--

Memorize names & formulasMemorize names & formulas– No easy way.No easy way.

Names of polyatomic ionsNames of polyatomic ions NONO22

-- nitrnitriite ionte ion NONO33

-- nitrnitraate ionte ion

NHNH44++ ammonium ionammonium ion

POPO44--33 phosphate ionphosphate ion

HPOHPO44 -2-2 hydrogenhydrogen phosphate ion phosphate ion

HH22PO PO -4-4 didihydrogen phosphate ionhydrogen phosphate ion

COCO33--22 carbonate ioncarbonate ion

HCOHCO33-- bibicarbonate ion (hydrogen carbonate)carbonate ion (hydrogen carbonate)

Names of polyatomic ionsNames of polyatomic ions SOSO33

-2-2 sulfsulfiite ionte ion SOSO44

--22 sulfsulfaate ionte ion HSOHSO44

-- bibisulfate ion (hydrogen sulfate)sulfate ion (hydrogen sulfate)

OHOH-- hydroxide ionhydroxide ion CHCH33COCO22

-- acetate ionacetate ion CrCr22OO77 -2-2 dichromate iondichromate ion CN-CN- cyanide ioncyanide ion OClOCl-- hypochlorite ionhypochlorite ion MnOMnO44

-- permanganate ionpermanganate ion

Polyatomic Ions in Polyatomic Ions in compoundscompounds

One element or ion + a polyatomic ionOne element or ion + a polyatomic ion

Steps:Steps:– Use the name of the ionUse the name of the ion– Add the Add the name of the polyatomic ionname of the polyatomic ion

Example: MgSOExample: MgSO44 (magnesium sulfate) (magnesium sulfate)– Magnesium + Magnesium + sulfatesulfate

Note: SO4 is not sulfur tetroxide

Naming compoundsNaming compounds RuleRule: The more positive portion of the : The more positive portion of the

compound is named first.compound is named first.– MetalMetal– Positive polyatomic ionPositive polyatomic ion– HydrogenHydrogen– Least negative non-metal (farthest left)Least negative non-metal (farthest left)

RuleRule: The more negative portion is named : The more negative portion is named and written last.and written last.

PracticePractice

NaNONaNO33

NaHCONaHCO33

CaCa((NONO33))22

MgMg((OHOH))22

NaOHNaOH

Ionic compoundsIonic compounds OneOne metal + metal + oneone non-metal bonding non-metal bonding

Steps:Steps:– Name the positive (cation) ionName the positive (cation) ion– Name the Name the stemstem of the negative (anion) ion of the negative (anion) ion– Add ideAdd ide

Example: NaCl = Na+ and Cl-Example: NaCl = Na+ and Cl-

– Sodium + Sodium + ChlorChlor + ide + ide (Sodium chloride)(Sodium chloride)

StemsStems

ox ox oxygenoxygen chlorchlor chlorinechlorine brombrom brominebromine iodiod iodineiodine nitrnitr nitrogennitrogen

PracticePractice CaBrCaBr

KClKCl

HClHCl

CaOCaO

Molecular compoundsMolecular compounds OneOne non-metal and non-metal and oneone non-metal non-metal

StepsSteps::– Use the Use the prefixprefix of the first element of the first element– Add element nameAdd element name– Use the prefix of the second element Use the prefix of the second element – Use the stem of the second elementUse the stem of the second element– Add ideAdd ide

Example: PExample: P22OO33 Diphosphate trioxide Diphosphate trioxide– didi + phosphate + + phosphate + tritri + ox + ide + ox + ide

PrefixesPrefixes Mono Mono oneone DiDi twotwo TriTri threethree TetraTetra fourfour PentaPenta fivefive HexaHexasixsix HeptaHepta sevenseven OctaOcta eighteight

Covalent compoundsCovalent compounds Rules:Rules:

– MonoMono means one and is only used before the means one and is only used before the second element. If no prefix appears before second element. If no prefix appears before the first element, assume one.the first element, assume one.

– If two vowels appear together, drop the vowel If two vowels appear together, drop the vowel from the prefixfrom the prefix

Example: CO (carbon monoxide)Example: CO (carbon monoxide)– ___?__ carbon + mon___?__ carbon + monoo + ox + ide + ox + ide

PracticePractice

NN22OO

COCO22

HH22OO

Chemical ReactionsChemical Reactions

ObjectivesObjectives

At the end of this module, the student At the end of this module, the student willwill

– Define the components of a chemical Define the components of a chemical reaction.reaction.

– Give an example of an oxidation-Give an example of an oxidation-reduction reaction in Respiratory reduction reaction in Respiratory Therapy.Therapy.

– Explain how the different chemical Explain how the different chemical reactions take place.reactions take place.

Chemical reactionsChemical reactions

Example of a reaction:Example of a reaction:

COCO22 + H + H22O HO H22COCO33 HCO HCO33- - + H+ H++

C.A.C.A.

One small reaction in a long chain of reactions.

Reactions taking place

at cells

Reactions taking place

at lungs

More about chemical More about chemical reactionsreactions

– Chemical reactionChemical reaction – Two substances – Two substances colliding with enough energy to colliding with enough energy to overcome the repulsion of electrons. overcome the repulsion of electrons. (electron movement)(electron movement)

– Chemical equationChemical equation – Shorthand – Shorthand method of describing a chemical change method of describing a chemical change using symbols, arrows and formulasusing symbols, arrows and formulas

Definitions:

More about chemical More about chemical reactionsreactions

– Activation energyActivation energy – Something that can – Something that can increase molecular collisions and change the increase molecular collisions and change the rate of the chemical reaction.rate of the chemical reaction. HeatHeat Increased concentrations of substancesIncreased concentrations of substances PressurePressure CatalystCatalyst

– CatalystCatalyst – Substance that speeds a reaction – Substance that speeds a reaction without being chemically changed in the without being chemically changed in the process (carbonic anhydrase)process (carbonic anhydrase)

Definitions:

More about chemical More about chemical reactionsreactions

– BalanceBalance – Atoms on one side of an – Atoms on one side of an arrow must equal the atoms on the arrow must equal the atoms on the other side of the arrow.other side of the arrow.

– Law of ConservationLaw of Conservation – Matter cannot – Matter cannot be created or destroyed – only changed.be created or destroyed – only changed.

Definitions:

More about chemical More about chemical reactionsreactions

DefinitionsDefinitions::– ReactantsReactants – substances entering into a – substances entering into a

reaction.reaction.– ProductsProducts – Substances formed by the – Substances formed by the

reaction.reaction.– ConditionsConditions – circumstances that may – circumstances that may

need to be present for the reaction to take need to be present for the reaction to take placeplace H2CO3 HCO3

- + H+

H2CO3 HCO3- + H+

Speed of chemical reactionsSpeed of chemical reactions

Speed of reactionsSpeed of reactions::Slow

DecayRust

ModerateCement setting

FastExplosion of dynamiteCoals burning

Types of chemical reactionsTypes of chemical reactions

Types of reactionsTypes of reactions::

A. Synthesis (Combination)A. Synthesis (Combination) A + B A + B AB AB

B. Decomposition (Breakdown)B. Decomposition (Breakdown) AB AB A + B A + B

C. Exchange (Replace)C. Exchange (Replace) AB + CD AD + CBAB + CD AD + CB

SynthesisSynthesis Reaction Reaction

Combination of 2 or more substances Combination of 2 or more substances (reactants) to form different, more complex (reactants) to form different, more complex substances (products).substances (products).

Substances formed are usually compounds Substances formed are usually compounds or or polyatomic ions.or or polyatomic ions.

Bonds are Bonds are formedformed in these reactions. in these reactions.

Energy is Energy is requiredrequired for this reaction to for this reaction to occur.occur.

Synthesis exampleSynthesis example

Reactions involving oxygen are often Reactions involving oxygen are often called combustion reactions.called combustion reactions.

C + OC + O22 COCO22

“ “heat”heat”

Synthesis reactionSynthesis reaction Oxidation-Reduction ReactionOxidation-Reduction Reaction

– BatteriesBatteries– Oxygen analyzersOxygen analyzers– Blood gas electrodesBlood gas electrodes

Oxidation-Reduction Oxidation-Reduction reactionreaction

Oxidation – Loss of electrons during a Oxidation – Loss of electrons during a chemical reaction.chemical reaction.

Reduction – Gain of electrons during a Reduction – Gain of electrons during a chemical reaction.chemical reaction.

Memory-Aid Acronym: OIL RIGMemory-Aid Acronym: OIL RIG OIL – Oxidation Is LossOIL – Oxidation Is Loss RIG – Reduction Is GainRIG – Reduction Is Gain

Agents in an Oxidation-Agents in an Oxidation-Reduction ReactionReduction Reaction

Oxidizing agentOxidizing agent – – AcceptsAccepts the the electrons (anion) and is being reduced.electrons (anion) and is being reduced.

Reducing agentReducing agent – – ReleasesReleases the the electrons (cation) and is being oxidizedelectrons (cation) and is being oxidized

http://library.kcc.hawaii.edu/external/chhttp://library.kcc.hawaii.edu/external/chemistry/emistry/

Simple electrolyte cellSimple electrolyte cell Components of these systems:Components of these systems:

– CathodeCathode (-) attracts cations (+), oxidation (-) attracts cations (+), oxidation takes place and electrons are releasedtakes place and electrons are released

– AnodeAnode (+) attracts anions (-), reduction (+) attracts anions (-), reduction takes place where electrons are acceptedtakes place where electrons are accepted Opposites attractOpposites attract

Causes flow of electrons and electrical Causes flow of electrons and electrical currentcurrent

DecompositionDecomposition ReactionReaction

One complex substance (a compound) One complex substance (a compound) undergoes a reaction to form two or undergoes a reaction to form two or more new (simpler) substances more new (simpler) substances (elements or compounds). (elements or compounds).

During this reaction, chemical bonds During this reaction, chemical bonds are are brokenbroken..

This often This often releasesreleases heat energy. heat energy.

Decomposition ExampleDecomposition Example

Baking soda reaction:

2NaHCO3 Na2CO3 + CO2 + H2O

(solid) (solid) (gas) (liquid)

Decomposition ExampleDecomposition Example

Breakdown of complex nutrients in a Breakdown of complex nutrients in a cell to release energy for other cell to release energy for other cellular functions.cellular functions.

CarbohydratesCarbohydrates ProteinsProteins FatsFats

– Products of these reactions are Products of these reactions are essentially “waste products”.essentially “waste products”.

EnergyEnergy

It is common for the It is common for the energy releasedenergy released during a decomposition reaction to during a decomposition reaction to be used be used to driveto drive a synthesis reaction. a synthesis reaction.

Decomposition = release of energy

Synthesis = use of energy

ExchangeExchange ReactionReaction

Breakdown of substances Breakdown of substances (reactants) to form different (reactants) to form different substances (products).substances (products).

Bonds are both Bonds are both decomposeddecomposed and and synthesizedsynthesized in these reactions. in these reactions.

Energy is Energy is requiredrequired and and releasedreleased in in this reaction.this reaction.

ExampleExample

Exchange reaction:Exchange reaction:

H . Lactic + NaHCOH . Lactic + NaHCO33 Na . Lactate + Na . Lactate + HH22COCO33

Single-replacement Single-replacement ExchangeExchange

An element and a compound react An element and a compound react where the first element replaces an where the first element replaces an element in the compound.element in the compound.

Zn + CuSOZn + CuSO44 ZnSOZnSO44 + Cu + Cu

Double-replacement Double-replacement ExchangeExchange

Two compounds exchange ions.Two compounds exchange ions.

AgNOAgNO33 + HCl + HCl HNOHNO33 + AgCl + AgCl

NeutralizationNeutralization

An acid reacts with a base , generally An acid reacts with a base , generally producing a salt, water (or weak acid) producing a salt, water (or weak acid) and heat.and heat.

HCl + NaOHHCl + NaOH NaCl + HNaCl + H22OO

(strong(strong

acid) (base) (salt) (water)acid) (base) (salt) (water)

Clinical ExampleClinical Example When glucose is converted to carbon When glucose is converted to carbon

dioxide and water by using oxygen in the dioxide and water by using oxygen in the following relationship:following relationship:

If a person eats a candy bar containing 14.2 If a person eats a candy bar containing 14.2 g of glucose, how many grams of water will g of glucose, how many grams of water will be produced?be produced?– 14.2 grams of C14.2 grams of C66HH1212OO6 = 6 = ? grams of H? grams of H22OO

OHCOOOHC 2226126 666