Chapter 2: Antacids

Antacids This chapter will introduce the chemistry needed to understand how antacids workSection 2.1: Types of MatterSection 2.2: Naming ChemicalsSection 2.3: Writing FormulasSection 2.4: Acids & BasesSection 2.5: Chemical ReactionsSection 2.6: Balancing Chemical EquationsSection 2.7: Speeding up Chemical Reactions

IntroAntacids

Why do we need antacids?Your body needs hydrochloric acid to digest foodToo much causes heartburn, ulcers and can damage your esophagus

Antacids versus Acid InhibitorsAcid InhibitorsAntacidsNeutralizes the acid currently in your systemControls the amount of acid your body producesThere are two types of medicines you can useWork quickly but your body will make more acid againLong-term solution, but needs to build up in your system to be most effectiveAlka-Seltzer , Rolaids , Tums , Malox , Mylanta Tagamat , Zantac , Pepcid AC Is it fair when a commercial compares the fast action of an antacid to an acid inhibitor that takes up to 7 days to build up?

Section 2.1Types of Matter

Matter is.Anything that has mass and takes up space (volume)Anything made from atomsExamples: elements, molecules, cells, people, air, water, paperNon Examples: dreams, energy (light, heat), emotions

Pure Substances versus MixturesMixturesPure Substances

Contain only 1 type of particleElements or Compounds

Contain 2 or more pure substancesHomogeneous or HeterogeneousMatter is classified as either a pure substance or a mixture

Pure SubstancesCompoundElements2 or more elements chemically bonded together to form molecules. Each is the same fixed ratio of elements.H2O, NaCl, CO2

ElementsPure substanceEvery atom is the sameElements can be found on the periodic table!ElementSingle AtomCannot be separated by chemical or physical processes

Elementshttp://www.youtube.com/watch?v=7FesjAdIWBk

CompoundsPure substanceEvery molecule is the sameCompoundSingle Molecule Made of more than one type of atom bonded togetherCan only be separated by chemical reactions

MixturesNot a pure substancePhysical combination of more than 1 type of pure substanceMixtureMore than 1 different type of matterCan be separated physically byDistillationFiltrationChromatography

MixturesHeterogeneousHomogeneous (aka solution)It looks the same throughout; substances evenly dispersedEx. salt water, alloys, clean airDifferent substances can be seen (chunks, bubbles, floaties, layers)Ex. salad dressing, fog, chocolate chip cookies, soilMixtures can be classified as homogeneous or heterogeneous

Mixture possibilitiesMixtures can be any combination of solids, liquids and gases:Solid-solid: Medicine tabletSolid-gas: Pop Rocks candySolid-liquid: Ice waterLiquid-liquid: lemon waterGas-Liquid: Carbonated waterGas-Gas: Air

Homogeneous MixturesBrass: copper in zinc Air: oxygen gas in nitrogen gasKool-Aid: sugar in waterMilk: fat, proteins, sugar in water

Heterogeneous MixturesOil in waterItalian Salad DressingChicken Noodle SoupFruit Salad

Classification of Matter

True Solutions, Colloids & SuspensionsColloidTrue SolutionSMALL particles dont settle out and are too small to scatter lightEx: salt water, air, brassINTERMEDIATE particles dont settle out but are large enough to scatter light:Ex: fog, foam, jello, paintSuspensionLARGE particles that settle out over timeEx: oral medicines, italian dressing, paintDissolved Particle Size IncreasesHomogeneous Heterogeneous Heterogeneous

True Solutions

Suspensionsvinegar and oil salad dressing

Particles Scattering LightIf the dissolved particles are large enough to scatter light, we say it exhibits the Tyndall EffectSolutionLight passes through unchangedColloids exhibit the Tyndall EffectLight is scattered by larger solute particles

Connect these concepts with AntacidsWhat type of matter do you think antacids are?Pure substance (Element or compound)Mixture (homogeneous or heterogeneous)

Connect these concepts with AntacidsAntacids are mixtures.They contain active & inactive ingredientsWhat purposes could the inactive ingredients serve?

Connect these concepts with AntacidsInactive ingredients mightAdd volume to make the pill able to be handledAdd color and flavorAllow the tablet to be compressed and formed

Lets Practice: Not in NotesTin can (Sn)Example:Determine if each is element, compound, homogeneous or heterogeneous mixturesCopper pipe (Cu)ConcreteCarbon tetrachloride(CCl4)Sports drink

Lets PracticeElementTin Example:Determine if each is element, compound, homogeneous or heterogeneous mixturesElementCopper pipeHeterogeneous mixConcreteCompoundCarbon tetrachlorideHomogenous mixSports drink

You Try! In NotesAluminum foil (Al)Example:Determine if each is element, compound, homogeneous or heterogeneous mixturesWater (H2O)sodasoilCarbon dioxide(CO2)Tap water

You Try!ElementAluminum foil (Al)Example:Determine if each is element, compound, homogeneous or heterogeneous mixturesCompoundWater (H2O)Homogeneous mixFlat sodaHeterogeneous mixsoilcompoundCarbon dioxide(CO2)Tap waterHomogeneous mix

The Science of Macaroni Saladhttp://www.freetech4teachers.com/2013/08/the-science-of-macaroni-salad.html#.UkySCODvSDo

Section 2.2Naming ChemicalsWe need to be able to name the chemicals in the antacids!

The Language of ChemistryChemistry has a language all of its ownEach element symbol starts with a capital letterEnglishChemistryElement SymbolsLettersChemical FormulasWordsChemical EquationsSentences

ELEMENTS: made of atomsAn atom consists of subatomic particlesThere are 3 subatomic particles: protons, electrons and neutrons

Neutral atoms have the same number of protons and eletrons

IONSAn atom or group of atoms with a charge.The number of protons does not equal the number of electrons.

WHY? Atoms can gain or lose electrons to acquire stability like a noble gas element.

The Periodic Table of Elements Metals form cations NonMetals form anions

HHeLiBeBCNOFNeNaMgAlSiPSClArKCaScTiVCrMnFeCoNiCuZnGaGeAsSeBrKrRbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXeCsBaLuHfTaWReOsIrPtAuHgTlPbBiPoAtRnFrRaLrRfDbSgBhHsMtUunUuuUubUut

MetalsMetalloidsNon-metals

Monatomic Ions (formed from a single atom) CationsPositive chargeMetal atoms that lose electronsGroup A (Representative metals/Type I ) The group # for metals in columns 1A, 2A, & 3A is equal to the charge of the cation

Naming them: Take the element name and add the word ion

Monatomic Ions of Group A /Type I MetalsGroup BGroup AGroup A

Group B (Transition/Type II Metals): have more than one chargeYou should be familiar with the following transition metals with more than one charge.Fe+2 Fe+3 Sn+2 Sn+4 Pb+2 Pb+4 Co+2 Co+3 Cr+2 Cr+3 Mn+2 Mn+3 Cu+1 Cu+2

Naming them: Take the element name and place in parentheses the charge number as a roman numeral and add the word ion

Monatomic Ions of Transition/Type II Metals+

Monatomic Ions (formed from a single atom) Cu+2, F-1AnionsNegative charge Nonmetals that gain electronsGroup A (Representative nonmetals) Subtract the group # in columns 4A, 5A, 6A, and 7A from 8 to get the charge.

Naming them: Drop the ending of the elementand add ide and then ion

You Try!Try These: Write the formula for each ion and name it.Calcium Chromium Chlorine Sulfur

You Try!Try These: Write the formula for each ion and name it.CalciumCa+2 calcium ion

ChromiumCr+2 chromium(II) ionCr+3 chromium (III) ion ChlorineCl-1 chloride ion SulfurS-2 sulfide ion

Self CheckTry These: Write the formula for each ion and name it.Aluminum Zinc Iron Phosphorus

Al+3 Aluminum IonZn+2 Zinc ionFe+2 Iron (II) ion orFe+3 Iron (III) ionP-3 Phosphide ion

Binary Ionic CompoundsBinary Ionic Compound- compound containing 2 elementsone metal and one non-metal+Cation-AnionMetal NonmetalThe atoms are held together by Ionic Bonds- bond formed by attraction between + ions and ions

Metals & Non-MetalsIonic Bonds are between metals & non-metals

HHeLiBeBCNOFNeNaMgAlSiPSClArKCaScTiVCrMnFeCoNiCuZnGaGeAsSeBrKrRbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXeCsBaLuHfTaWReOsIrPtAuHgTlPbBiPoAtRnFrRaLrRfDbSgBhHsMtUunUuuUubUut

MetalsMetalloidsNon-metals

Look for:2 elements (binary)A type I metal & a non-metal (ionic)To name these compounds:Write the name of the type 1 metal (the cation)Write the name of the non-metal (the anion) with the suffix -ideHow to Identify & Name a Binary Ionic CompoundThe subscripts in the formula do not matter when naming this type

Example #1NaCl

NaClCationAnionSodiumChlorine becomes ChlorideSodium Chloride

Example #2CaBr2

CationAnionCalciumBromine becomes BromideCaBr2Calcium Bromide

Example #3K2O

K2OCationAnionPotassiumOxygen becomes OxidePotassium Oxide

Self CheckExample:Write the name for the following compoundsLi2OSr3P2MgSBaI2

AnswersLithium oxideStrontium phosphideMagnesium sulfideBarium iodideExample:Write the name for the following compoundsLi2OSr3P2MgSBaI2

Ternary Ionic Compounds+CationTernary Ionic Compound- a compound containing at least one polyatomic ion+PolyatomicCation-AnionPolyatomic Ion- an ion that has more than one atom that together have a single charge

Common Polyatomic IonsYou dont need to memorize them. Look at your reference sheet.

COMMON POLYATOMIC IONSAcetate, CH3COO-1 or C2H3O2-1Ammonium NH4+1Bromate, BrO3-1Bromite, BrO2-1Carbonate, CO3-2Carbonite, CO2-2Chlorate, ClO3-1Chlorite, ClO2-1Chromate, CrO4-2Cyanide, CN-1Dichromate, Cr2O7-2Dihydrogen phosphate, H2PO4-1Hydrogen carbonate or bicarbonate, HCO3-1Hydrogen phosphate or biphosphate, HPO4-2Hydrogen sulfate or bisulfate, HSO4-1Hydroxide, OH-1Hypochlorite, ClO-1Iodate, IO3-1Iodite, IO2-1Nitrate, NO3-1Nitrite, NO2-1Oxalate, C2O4-2Perchlorate, ClO4-1Permanganate, MnO4-1Peroxide, O2-2Phosphate, PO4-3Phosphite, PO3-3Silicate, SiO3-1Sulfate, SO4-2Sulfite, SO3-2

The only cation (front-half) polyatomic ion is NH4+All other polyatomic ions are anions (back-half)The subscripts within the polyatomic ion are important (it must match exactly with the one on your ion list)If there are parentheses, the polyatomic ion is inside (ignore the number outside)Identifying Polyatomic Ions: Hints

Practice Identifying Polyatomic IonsExample:Underline& name the polyatomic ion in each compoundNaNO3NH4ClCa(OH)2(NH4)3PO4K2CO3

Practice Identifying Polyatomic IonsExample:Identify and name the polyatomic ion in each compoundNaNO3NH4ClCa(OH)2(NH4)3PO4K2CO3NitrateAmmoniumHydroxideAmmonium & phosphateCarbonate

Look for:More than 2 capital letters next to one another (not starting with H)Contain at least 1 metal & 1 non-metalTo name these compounds:Write the name of the cation (either the metal element name or Ammonium for NH4+)If the anion is a polyatomic ion, write the given polyatomic ions name If the anion is a single non-metal element, write its name with the suffix -ideHow to Identify & Name Ternary Ionic Compounds

Ca(NO3)2Example # 4

Ca(NO3)2CationPolyatomicAnionCalciumNitrateCalcium Nitrate

Example #5Na3PO4

CationPolyatomicAnionSodiumphosphateNa3PO4Sodium phosphate

Example # 6K2CO3

K2CO3 CationPolyatomicAnionpotassiumcarbonatePotassium carbonate

Self CheckExample:Write the name for the following compoundsCa(C2H3O2)2Li2SO3Ba(OH)2(NH4)2S

AnswersCalcium acetateLithium sulfiteBarium hydroxideAmmonium SulfideExample:Write the name for the following compoundsCa(C2H3O2)2Li2SO3Ba(OH)2(NH4)2S

Worksheet 1 (1-10 Answers)1. Sodium sulfide

2. Aluminum oxide

3. Sodium chloride

4. Rubidium iodide

5. Zinc bromide6. Silver chloride7. Boron nitride8. Barium fluoride9. Strontium nitride10. Magnesium chloride

Worksheet 2 (1-10 Answers)1. copper(I) fluoride

2. copper (II) fluoride

3. chromium (III) oxide

4. lead (II) iodide5. lead (IV) chloride6.chromium (VI) oxide7. gold(I) bromide8. nickel(II) oxide9. vanadium(III) iodide10. tin(IV) oxide

Worksheet 3 (1-10 Answers)1. vanadium(V) chlorate

2. rhenium(VI) sulfate

3. osmium(III) iodate

4. iridium(IV) phosphate5. palladium(IV) sulfiteGold(I) nitrate7. iron(III) phosphite8. nickel(II) bromate9. lead(IV) sulfide10. Manganese (VII) dichromate

Worksheet 4 (1-10 Answers)1. ammonium chloride

2. hydrogen chlorite

3. calcium bromate

4. beryllium sulfate

5. ammonium nitride6. ammonium nitrate7. strontium phosphate8. zinc chlorate9. silver iodate10. potassium dichromate

Transition Metals RevisistedTransition Metal- group B or Type II metal that has the possibility of having more than one cation charge; IMPORTANT: Although group B metals, SILVER (+1), CADMIUM (+2), and ZINC (+2) only have 1 chargeAlthough the elements of TIN and LEAD are group A elements, they do have more than one chargeSn(+2 and +4) and Pb(+2 and +4)

Common multivalent metals and their charges

Cobalt Co+2 Co+3Copper Cu+1 Cu+2Iron Fe+2 Fe+3Manganese Mn+2 Mn+3Mercury Hg2+2 Hg+2

Look for:One of the transition metals, excluding Ag, Cd, and ZnTo name these compounds:Write the name of the Type II metal element (cation)Write the name of the anion (element name with -ide or polyatomic ion name)Determine the charge of the transition metal1. Total negative charge = total positive charge for all neutral compounds2. Divide total positive charge by the number of metal atoms3. Write the charge in roman numerals in parentheses after the Type II metals nameHow to Identify & Name Ionic Compounds with Transition Metals

Example # 7CuCl

CuClCationAnionCopperChlorine becomes ChlorideCopper Chloride

CuClCationAnionCopperChlorine becomes ChlorideCopper ChlorideChloride has a 1 charge-1 charge * 1 ion = -1A 1 charge needs a +1 chargeTherefore, copper must be +1, (I)(I)

Example # 8Fe2(CO3)3

Fe2(CO3)3CationPolyatomic AnionIronCarbonateIron carbonate

Fe2(CO3)3CationPolyatomic AnionIronCarbonateIron carbonateCarbonate has a 2 charge-2 charge * 3 ions = -6A 6 charge needs a +6 charge and there are 2 iron ionsTherefore, iron must be +3 (III)(III)

Example # 9ZnBr2

ZnBr2Cationmonatomic AnionZincbromideZinc bromide

ZnBr2CationPolyatomic AnionZincbromideZinc bromidebromide has a 1 charge-1 charge * 2 ions = -2A 2 charge needs a +2 charge and there is 1 zinc ionTherefore, zinc must be +2 (notneeded) it only has one charge

Self CheckExample:Write the name for the following compoundsPbCl2PbCl4MnOMn2O3

AnswersLead (II) chlorideLead (IV) chlorideManganese (II) oxideManganese (III) oxideExample:Write the name for the following compoundsPbCl2PbCl4MnOMn2O3

Binary Covalent (Molecular) CompoundsNonmetalNonmetalBinary Molecular Compounds are made from two non-metals that are covalently bonded Covalent bond a bond formed from atoms that share electrons

These compounds have:2 elements (binary)Both non-metals (covalent)To name these compounds:Write the name of the first element with the prefix indicating the number of atoms (except dont use mono- if only 1 atom)Write the name of the second element with the prefix indicating the number of atoms (including mono-) and the suffix ideIdentifying & Naming Binary Molecular

Covalent Prefixes

PREFIXES USED IN MOLECULAR COMPOUNDSmonodi-tri-tetra-penta-hexa-hepta-octa-nona-deca-

Example #10P2O5

P2O5PhosphorusOxygen2 = di-5 = penta- oxideDiphosphorus pentaoxide

Example #11SiF4

SiliconFluorineDont use mono- on first element4 = tetra- fluorideSiF4Silicon tetrafluoride

Self CheckExample:Write the name for the following compoundsSO2N2Cl4P4O10CO

Answerssulfur dioxideDinitrogen tetrachlorideTetraphosphorus decaoxideCarbon monoxideExample:Write the name for the following compoundsSO2N2Cl4P4O10CO

Mixed Practice: Determine the type of compound, Ionic (m/nm) or Covalent (nm/nm) & then follow rulesExample:Write the name for the following compoundsNa2OK3PO4Cu(OH)2N2SMgCl2

AnswersSodium oxidePotassium phosphateCopper (II) hydroxideDinitrogen monosulfideMagnesium chlorideExample:Write the name for the following compoundsNa2OK3PO4Cu(OH)2N2SMgCl2

Section 2.3Writing Chemical FormulasWe need to be able to read the formulas for chemicals in the antacids!

Your Reference sheet has a list of:Common polyatomic ionsUse your periodic table is used to determine the charges of common elements when they form ionsYou must memorize the 10 prefixes for covalent compoundsReminders from Section 2.2

Binary Ionic Compoundscontaining two elementsone metal and one non-metalformed by attraction between + and - ions

+Cation-Anion

These compounds:End in -ide (except hydroxide and cyanide)Do NOT contain covalent prefixesTo write these formulas:Write the symbol & charge of the first element (the metal, cation)Write the symbol & charge of the second element (the non-metal, anion)Add more of the cations and/or anions to have a neutral compoundUse subscripts to show how many of each type of ion is there.

How to Write Formulas for Binary Ionic Compounds

Example #1Sodium chloride

Sodium chlorideCationAnionNa+1Cl-1NaCl

Example #1Sodium chlorideCationAnionNa+1Cl-1NaClNa+1Cl-1+1 + -1 = 0The compound is neutralno subscripts are needed.

Example #2Calcium bromide

Example #2Calcium bromideCationAnionCa+2Br-1

Example #2Calcium bromideCationAnionCa+2Br-1CaBr2Ca+2 Br-1+2 + -1 = +1Ca+2 Br-1 Br-1The subscript 2 is used to show that 2 anions are needed.+2 + -1 + -1 = 0

The Criss - Cross Method:Write the symbol & charge of the first element (the metal, cation)Write the symbol & charge of the second element (the non-metal, anion)Cross ONLY the charge numbers down diagonally to make subscripts IF they are not equal to each otherSimplify subscripts if you can Ca +2 Br-1 Ca1Br2 CaBr2 1 2A Simple Method to Writing Binary Ionic Formulas

Self CheckExample:Write the following chemical formulasCesium chloridePotassium oxideCalcium sulfideLithium nitride

AnswersCsClK2OCaSLi3NExample:Write the following chemical formulasCesium chloridePotassium oxideCalcium sulfideLithium nitride

Ternary Ionic Compounds+Cationcompound containing at least one polyatomic ionEither in the front, the back or in both places

These compounds:Do not end with -ide (except hydroxide & cyanide)Do not use covalent prefixesTo write these formulas:Write the symbol & charge of the cation & anionAdd additional cations or anions to have a neutral compoundUse subscripts to show the number of ionsWhen using subscripts with a polyatomic ion, you must put the polyatomic ion in a parenthesis with the subscript on the outsideHow to Identify & Name Ternary Ionic Compounds

Example #3Sodium carbonate

Sodium carbonateCationPolyatomicAnionNa+1CO3-2

Sodium carbonateCationPolyatomicAnionNa+1CO3-2Na2CO3Na1+ CO32-+1 + -2 = -1Na+ Na+ CO32-The subscript 2 is used to show that 2 cations are needed.+1 + 1 + -2 = 0

Example #4Magnesium nitrate

Magnesium nitrateCationPolyatomicAnionMg+2NO3-1

Magnesium nitrateCationPolyatomicAnionMg+2NO3-1Mg(NO3)2Use parenthesis when adding subscripts to polyatomic ionsMg+2NO31-+2 + -1 = 1Mg+2 NO3- NO3-The subscript 2 is used to show that 2 anions are needed.+2 + -1 + -1 = 0

Self CheckExample:Write the following chemical formulasSodium nitrateCalcium chloratePotassium sulfiteCalcium hydroxide

AnswersNaNO3Ca(ClO3)2K2SO3Ca(OH)2Example:Write the following chemical formulasSodium nitrateCalcium chloratePotassium sulfiteCalcium hydroxide

Transition Metalsmetal that has more than one possibility for cationic charge

These compounds:Will have roman numeralsTo write these formulas:Same as binary ionic or polyatomic ionic.The roman numerals tell the charge of the metal (cation)How to Identify & Name Ionic Compounds with Transition Metals

Example #5Iron (III) oxide

Iron (III) oxideCationAnionFe+3O-2

Iron (III) oxideCationAnionFe+3O-2Fe2O3Fe+3 O2-+3 + -2 = -1Fe+3 Fe+3 O2- O2-The subscript 2 and 3 are used to show the numbers of atoms needed.+3 + 3 + -2 + -2 + -2 = 0

Example #6Copper (II) nitrate

Copper (II) nitrateCationPolyatomicAnionCu+2NO3-1

Copper (II) nitrateCationPolyatomicAnionCu+2NO3-1Cu(NO3)2Cu+2 NO31-+2 + -1 = 1Cu+2 NO3- NO3-Use parenthesis when adding subscripts to a polyatomic ion+2 + -1 + -1 = 0

Self CheckExample:Write the following chemical formulasIron (II) nitrateCopper (I) chlorideLead (IV) hydroxideTin (II) oxide

AnswersFe(NO3)2CuClPb(OH)4SnOExample:Write the following chemical formulasIron (II) nitrateCopper (I) chlorideLead (IV) hydroxideTin (II) oxide

Binary Covalent Compoundscompound made from two non-metalsbetween atoms that share electrons

NonmetalNonmetal

These compounds:Use covalent prefixesTo write these formulas:Write the symbols of the first and second elementUse the covalent prefixes (assume the first element is 1 if theres no prefix) as the subscripts to show number of atoms.How to Identify & Name Binary Covalent CompoundsAtoms do not form charges when bonding covalentlyyou DO NOT need to worry about charges with this type! NOR CRISS CROSS METHOD!

Example #7Dinitrogen Tetraoxide

Dinitrogen TetraoxideNODi- = 2Tetra- = 4N2O4

Example #8Silicon dioxide

Silicon dioxideSiOMono- is not written for the first elementDi- = 2SiO2

CAUTION!!!bi-di-Stands for 2 in covalent compoundsMeans theres a hydrogen in the polyatomic aniondi and bi do not mean the same thing!Carbon dioxide = CO2Sodium biphosphate = Na2HPO4

Self CheckExample:Write the following chemical formulasCarbon monoxideSulfur tetraiodideTrichlorine pentasulfide

AnswersCOSI4Cl3S5Example:Write the following chemical formulasCarbon monoxideSulfur tetraiodideTrichlorine pentasulfide

Self Check: Mixed PracticeExample:Write the following chemical formulasMagnesium hydroxideCopper (II) nitrateIron (III) oxideNitrogen dioxideSodium bicarbonate

AnswersMg(OH)2Cu(NO3)2Fe2O3NO2NaHCO3Example:Write the following chemical formulasMagnesium hydroxideCopper (II) nitrateIron (III) oxideNitrogen dioxideSodium bicarbonate

Section 2.4We need to know how acids behave when talking about ant-acids!

What is an Acid? Arrhenius DefinitionA substance that produces hydrogen ions (H+1) when dissolved in water.

H+1 immediately reacts with water to make the hydronium ion, H3O+1

How do Acids produce Hydronium?wateracidHydrogen cation with some anion

How do Acids produce Hydronium?+1

How do Acids produce Hydronium?+1Hydronium ionAnion

How to Identify an AcidLook for a hydrogen ion, H+ as the first element in an aqueous covalent compound.

H2SO4 HCl H2CO3 HNO3 HC2H3O2

These compounds have to :Start with H (more than 1 H is OK, too).Do not contain oxygenTo name these compounds:Use hydro____ic acidFill in the blank with the root of the anions nameNaming Binary Acids: Non-Oxygen Acids

Example #1HBr(aq)

HBr(aq)Hydrogen cationBromineIts an acidNo oxygenUse hydro___icHydrobromic acid

These compounds have:Start with H (more than 1 H is OK, too).Must contain oxygenTo name these compounds:Use ___ic acids for -ate anionsUse ___ous acids for -ite anionsNaming Oxyacids: contain oxygenDo not use hydro with thesethe word acid is how you know it begins with hydrogen, not hydro-

Example #2HNO2(aq)

Hydrogen cationnitrite ionIts an acid-ite ionUse ___ous acidHNO2(aq)Nitrous acid

Example #3HC2H3O2(aq)

Hydrogen cationacetate ionIts an acid-ate ionUse ___icHC2H3O2(aq)acetic acid

Self CheckExample:Write the name for the following acidsHFH2SH3PO4

AnswersHydrofluoric acidHydrosulfuric acidPhosphoric acidExample:Write the name for the following acidsHFH2SH3PO4

To write these formulas:Write the cation, H+1Write the anion symbol and chargeBalance the charges by adding the appropriate subscript to the hydrogen cation OR Criss Cross MethodWriting the chemical formula for Hydro- acids

Example #4 Hydrobromic acid

Hydrobromic acidHydrogen cationDoes not contain oxygenH+1Br-1

Hydrobromic acidHydrogen cationDoes not contain oxygenH+1Br-1HBrH+1Br-1+1 + -1 = 0The compound is neutral.Subscripts are not needed

To write these formulas:Write the cation H+1If it is an -ic acid, determine the polyatomic ion ending in -ate If it is an -ous acid, determine the polyatomic ion ending in -ite Add subscript to the hydrogen cation to balance charges OR use Criss Cross MethodWriting chemical formulas for Oxyacids

Example #5Carbonic acid

Carbonic acidHydrogen cationFrom the ___ate anionH+1CO3-2

Carbonic acidHydrogen cationFrom the ___ate anionH+1CO3-2H2CO3H+ CO32-+1 + -2 = -1H+ H+ CO32-+1 + 1 + -2 = 0

Example #6Chlorous acid

chlorous acidHydrogen cationFrom the ___ite anionH+1ClO2-1

Chlorous acidHydrogen cationFrom the ___ite anionH+1ClO2-1HClO2

H+ClO2-1+1 + -1 = 0

Self CheckExample:Write the formula for the following acidsPhosphorous acidHydroiodic acid

Phosphorous acidHydroiodic acidAnswersH3PO3HIExample:Write the formula for the following acids

You Really Only Need to Know These Acids! Memorize them!Hydrochloric acid HClSulfuric acid H2SO4Carbonic acid H2CO3Nitric acid HNO3Acetic acid HC2H3O2

What is a Base? Arrhenius DefinitionA substance that produces hydroxide ions, OH-1 in water H2ONaOH(s) Na+1(aq) + OH-1(aq)

Hydroxide IonONaHNa+1

How to Identify a BaseLook for an ionic compound that has a metal paired with the hydroxide ion, OH-OR Look for the ammonia molecule

NaOH Ca(OH)2 NH3**Do not assume all compounds ending in OH are bases: CH3OH is not a base but an alcohol

Follow the rules for ionic compounds. The most common exception to this is ammonia, NH3NH3 (ammonia) is a base even though it doesnt contain -OH as the anionNaming & Writing Formulas for Metal Hydroxides

Example #7NaOH

NaOHSodiumHydroxideSodium Hydroxide

Self CheckExample:Write the formula or name for eachCa(OH)2KOHCopper (II) hydroxideLithium hydroxide

AnswersCalcium hydroxidePotassium hydroxide Cu(OH)2 LiOHExample:Write the formula or name for eachCa(OH)2KOHCopper (II) hydroxideLithium hydroxide

What is an Acid according to Bronsted-Lowry?Is a substance that is a proton or hydrogen donorExample: HCl + H2O H3O+1 + Cl-1 acid base

What is a base according to Bronsted-Lowry?Is a substance that is a proton acceptor

Example: NH3 + H2O OH- + NH4+ base acid conjugate conjugate base acid

Conjugate Acid-Base Pairs Conjugate Acid- substance formed when a base gains a [H+] ion. Conjugate Base- substance formed when an acid loses a [H+] ion.Label the acid & base on the left side of the reaction & the conjugate acid & conjugate base on the right side.a) HNO3 + H2O H3O+ + NO3 ______ ______ ______ ______

b) NH3 + H2O NH4+ + OH _____ ______ ______ ______acidbaseC.A.C.B. baseacidC.A.C.B.

Characteristics of Acids & BasesBasesAcidsProduce H3O+1 (hydronium ion) in waterProduce OH-1 (hydroxide ion) in waterTastes sourTastes BitterReact with active metals to form hydrogen gasFeels slipperyBoth forms ions when dissolved: conducts electricity: They are called ELECTROLYTESNeutralizes a base to form salt and waterNeutralizes an acid to form salt and water

Strength versus Concentration

strong acid ALL acid molecules separate (dissociate) into [H+] ions in water; only ions presentExamples: HCl, HNO3, H2SO4

weak acid Most acid molecules stay together, only a FEW separate into [H+] ions when in water; few ions present, mostly moleculesExamples: HC2H3O2 (vinegar) , H2CO3

Strong Acid Weak Acid

Strong versus Weak AcidsStrong acidMost of the acid molecules have donated the H+1 to waterHow many hydronium ion anion pairs can you find?How many intact acid molecules can you find?31

Strong versus Weak AcidsWeak acidOnly a few of the acid molecules have donated the H+1 to waterHow many hydronium ion anion pairs can you find?How many intact acid molecules can you find?13

Strong Acids vs. Weak Acids

Concentrated versus DilutesolutesolventDILUTE(low concentration)Very little solute (whats being dissolved) particles in solutionCONCENTRATED (higher concentration)Lots of solute (whats being dissolved) particles in solution

Combinations of Concentration & StrengthDiluteConcentratedA lot of acid/base added & all dissociatesNot much acid/base added, but all of whats there dissociatesA lot of acid/base added, but little dissociatesNot much acid/base added and very little dissociatesStrongWeak

Bases follow the same pattern as acidsA common misconception is acids are dangerous but bases are not!Vinegar is an acid we eatsome of them are safe!Sodium hydroxide is a very caustic basenot all of them are less harmful than acids!The stronger and acid or base is & the more concentrated it is), the more dangerous it is for you!Bases Strength & Concentration

The pH scale to measure the acidity of a sampleThe Power of the Hydrogen: pH

Indicators change color based on pHLiquid indicators phenolphthalein or bromothymol blueBromothymol Blue: Acid: turns Yellow Base: turns bluePhenolphthalein: Acid: stays clear Base: turns pink

pH meters or pH probesElectronically determine pH and give a read-outWays to measure pHAcidBase

Indicators change color based on pHPaper with a liquid indicator on it (pH paper or Litmus paper)pH paper turns a color which matches to a pH number

LITMUS PAPER (Mnemomic: See board!)Blue Litmus stays blue in a base but turns pink in an acidRed Litmus stays red in an acid but turns blue in a base

Ways to measure pH

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