Chapter 9Chapter 9Naming Compounds and Naming Compounds and

Writing FormulasWriting Formulas

Ionic Compounds; Ionic Compounds; Molecular Compounds Molecular Compounds

and Acidsand Acids

Types of CompoundsTypes of Compounds

Compound- Compound- Formed when atoms of two or more elements Formed when atoms of two or more elements

combine CHEMICALLY.combine CHEMICALLY.Law of Definite Proportions-Law of Definite Proportions-

In ANY CHEMICAL compound the elements In ANY CHEMICAL compound the elements always combine in the same proportion by always combine in the same proportion by mass. mass. This agrees with Dalton’s Atomic Theory This agrees with Dalton’s Atomic Theory that atoms combine in small whole # ratios.that atoms combine in small whole # ratios.

Molecular CompoundsMolecular Compounds

Two Types of Compounds-Two Types of Compounds-1.1. Molecular CompoundsMolecular Compounds

2.2. Ionic CompoundsIonic Compounds1. Molecular Compounds1. Molecular CompoundsFormed between 2 or more NONMETALSFormed between 2 or more NONMETALS(Covalent Bond- Share Electrons)(Covalent Bond- Share Electrons)- Liquid or gas at room temp. and have - Liquid or gas at room temp. and have

relatively low melting and boiling points.relatively low melting and boiling points.

MoleculeMolecule

Molecule-Molecule-

NEUTRAL no charge, group of atoms that NEUTRAL no charge, group of atoms that act like a unit (one thing)act like a unit (one thing)

Molecules of a compound are all identical to Molecules of a compound are all identical to each othereach other

Molecules of different compounds are Molecules of different compounds are different.different.

Ex: COEx: CO22 (1C : 2 O); CO (1C : 1O) (1C : 2 O); CO (1C : 1O)

Molecular FormulaMolecular FormulaTells the number and kinds of atoms in a molecule Tells the number and kinds of atoms in a molecule

of a compound. (COof a compound. (CO22 & CO) & CO)

Nonmetal + NonmetalNonmetal + Nonmetal

Covalent Bond: Share ElectronsCovalent Bond: Share Electrons

Diatomic molecules: 7 nonmetallic elements that Diatomic molecules: 7 nonmetallic elements that are always paired and exist a molecules NOT are always paired and exist a molecules NOT atoms.atoms.

MEMORIZE: H O N Cl Br I FMEMORIZE: H O N Cl Br I F

Hydrogen HHydrogen H22; Oxygen O; Oxygen O22; Nitrogen N; Nitrogen N22;;

Chlorine ClChlorine Cl22; Bromine Br; Bromine Br22; Iodine I; Iodine I22; Fluorine F; Fluorine F22

Ionic CompoundsIonic Compounds

- Metal + NonmetalMetal + Nonmetal

- Made up of IONSMade up of IONS

- Relatively high melting and boiling pointsRelatively high melting and boiling points

- NEUTRAL (ion charges cancel out; total + NEUTRAL (ion charges cancel out; total + charge = total – charge)charge = total – charge)

IONION

Atom or group of atoms that have an UNEQUAL Atom or group of atoms that have an UNEQUAL number of protons and electrons number of protons and electrons

(#p+ does NOT = #e-) have a + or – charge(#p+ does NOT = #e-) have a + or – charge

Cations- atom or group of atoms with + chargeCations- atom or group of atoms with + chargeMetalsMetalsLose electronsLose electronsWhen naming cations the name stays the same as the When naming cations the name stays the same as the element.element.EX: NaEX: Na++ = sodium ion; Al = sodium ion; Al+3+3 = aluminum ion = aluminum ion

Cation ChargesCation Charges

ionic charges of Group A metals (see front ionic charges of Group A metals (see front of periodic chart)of periodic chart)ionic charges of Group B metals ionic charges of Group B metals (transitional metals) – see back of periodic (transitional metals) – see back of periodic chartchartRoman Numerals – are used to indicate the Roman Numerals – are used to indicate the charge of a transitional metal.charge of a transitional metal.Examples: Copper I = Cu Examples: Copper I = Cu ++; Copper II = Cu; Copper II = Cu+2+2

Lead II = PbLead II = Pb+2+2; Lead IV = Pb; Lead IV = Pb+4+4

AnionsAnions

Atom or group of atoms with a – chargeAtom or group of atoms with a – charge

NonmetalsNonmetals

Gain electronsGain electrons

When naming anions the ending changes When naming anions the ending changes to “ide”to “ide”

Ex: chlorine becomes chloride (ClEx: chlorine becomes chloride (Cl--); ); oxygen becomes oxide(Ooxygen becomes oxide(O-2-2); nitrogen ); nitrogen becomes nitride (Nbecomes nitride (N-3-3))

Polyatomic IonsPolyatomic IonsTightly bound group of atoms that act as a unit Tightly bound group of atoms that act as a unit (one thing) and carry a charge.(one thing) and carry a charge.

Also called RadicalsAlso called Radicals

Most end in “ite” or “ate”; “ite” ending has one less Most end in “ite” or “ate”; “ite” ending has one less oxygen than “ate” ending. Examples; chlorite oxygen than “ate” ending. Examples; chlorite ClOClO22

-1-1; chlorate ClO; chlorate ClO33-3-3

Except: hydorxide (OHExcept: hydorxide (OH--); cyanide (CN); cyanide (CN--); ); ammonium (NHammonium (NH44

++).).

Hypo – means 1 less oxygen (hypodermic means Hypo – means 1 less oxygen (hypodermic means under the skin) hypochlorite ClOunder the skin) hypochlorite ClO--

Per – means 1 more oxygen perchlorate ClOPer – means 1 more oxygen perchlorate ClO44--

Formula Unit (FU)Formula Unit (FU)

Lowest whole number ration on IONS in an ionic Lowest whole number ration on IONS in an ionic compound. compound.

- Ionic Compounds are NOT MOLECULES they are - Ionic Compounds are NOT MOLECULES they are called Formula Units.called Formula Units.

Chemical FormulaChemical Formula shows the kinds and number of shows the kinds and number of atoms in the SMALLEST UNIT of a compound.atoms in the SMALLEST UNIT of a compound.

The most positive element (metallic) is written first. The most positive element (metallic) is written first. EX: HEX: H22O = 2 Hydrogen atoms + 1 Oxygen atoms O = 2 Hydrogen atoms + 1 Oxygen atoms

COCO22 = 1 Carbon atom + 2 Oxygen atoms = 1 Carbon atom + 2 Oxygen atoms

Homework QuestionsHomework Questions

What are the differences between an ionic What are the differences between an ionic compound and molecular compound? (3)compound and molecular compound? (3)

Answer: Ionic- made up of ions; metal + Answer: Ionic- made up of ions; metal + nonmetal; High BP & MP; Formula Unit nonmetal; High BP & MP; Formula Unit Molecular- made up of nonmetals; share Molecular- made up of nonmetals; share electrons covalent bonds; usually liquids electrons covalent bonds; usually liquids or gases at room temp.; Moleculesor gases at room temp.; Molecules

Homework QuestionsHomework Questions

Why aren’t ionic compounds molecules?Why aren’t ionic compounds molecules?

Ionic Compounds are Formula Units (FU’s) Ionic Compounds are Formula Units (FU’s) and molecules are made up of 2 or more and molecules are made up of 2 or more nonmetalsnonmetals

What is the smallest ratio of an ionic What is the smallest ratio of an ionic compound called?compound called?

Formula Unit (FU)Formula Unit (FU)

Name the 7 diatomic elements and Name the 7 diatomic elements and write their formulas correctly.write their formulas correctly.

Hydrogen; HHydrogen; H22

Oxygen; OOxygen; O22

Nitrogen; NNitrogen; N22

Chlorine; ClChlorine; Cl22

Bromine; BrBromine; Br22

Iodine; IIodine; I22

Fluorine; FFluorine; F22

Homework Questions cont.Homework Questions cont.Metals form + ions called ___________.Metals form + ions called ___________.

Nonmetals form - ions called _______.Nonmetals form - ions called _______.

What group of metals have more than one What group of metals have more than one possible charge?possible charge?Group B metals; transitional metalsGroup B metals; transitional metalsWhat is a polyatomic ion?What is a polyatomic ion?A group of atoms that act as a single unit A group of atoms that act as a single unit and carry a charge.and carry a charge.

Naming compounds and Writing FormulasNaming compounds and Writing FormulasBinary compound-Binary compound-

Simplest compound made up of 2 elementsSimplest compound made up of 2 elements

Examples: [ – NaCl ] Examples: [ – NaCl ]

[iron II chloride – ][iron II chloride – ]

((NAMINGNAMING) 1.) element with the positive ionic charge is written ) 1.) element with the positive ionic charge is written first. ( )first. ( )

Group A Metals – metal name is written. Example Group A Metals – metal name is written. Example Na+ = sodiumNa+ = sodium

Group B Metals ( ) – Group B Metals ( ) –

Examples : FeExamples : Fe+2+2 = Iron II = Iron II

HgHg++ = ____________ = ____________

SnSn+4+4 = ____________ = ____________** Use the back of your periodic chart (Common Metal Ions with more ** Use the back of your periodic chart (Common Metal Ions with more

than 1 ionic charge!)than 1 ionic charge!)

Sodium chloride

FeCl2

metals

Transitional Roman Numeral Indicates the charge.

Mercury I

Tin IV

2.) element with the negative ionic charge is 2.) element with the negative ionic charge is

written next. ( )written next. ( )

Change the ending of the nonmetal to ( )Change the ending of the nonmetal to ( )

Nonmetal marries the metal and changes its Nonmetal marries the metal and changes its

name to “ide” like a bride.name to “ide” like a bride.

Examples: chlorine – chlorideExamples: chlorine – chloride

Bromine - ________________Bromine - ________________

Oxygen - ________________Oxygen - ________________

nonmetal

ide

bromide

oxide

USE THE RULES ABOVE TO NAME THE BINARY IONIC USE THE RULES ABOVE TO NAME THE BINARY IONIC COMPONDS BELOW:COMPONDS BELOW:

1. 1. MgO______________MgO______________ 5.) FeCl5.) FeCl33 ____________ ____________

2. BaS ______________2. BaS ______________ 6.) SnBr6.) SnBr4 4 ____________ ____________

3. Na3. Na33N _____________N _____________ 7.) K7.) K33P ____________P ____________

4. Cu4. Cu22O _____________O _____________ 8.) PbS ____________8.) PbS ____________

Magnesium oxide Iron III chloride

Barium Sulfide Tin IV bromide

Sodium nitride Potassium phosphide

Copper I oxide Lead II sulfide

WRITING FORMULASWRITING FORMULAS 1.) write the ion for the metal first1.) write the ion for the metal first

Group A Metals –Examples: Lithium – Li +Group A Metals –Examples: Lithium – Li +

Aluminum - ___ Magnesium - ___ Rubidium - ___Aluminum - ___ Magnesium - ___ Rubidium - ___

Group B Metals –Group B Metals –

Examples: Tin II – SnExamples: Tin II – Sn+2+2

Copper I - ____ Mercury II - ____ Lead IV - ____Copper I - ____ Mercury II - ____ Lead IV - ____

Al+3 Mg+2 Rb+1

The Roman Numeral indicates the charge

Cu+1 Hg+2Pb+4

write the ion for the non-metalwrite the ion for the non-metal

Group VA, VIA, VIIA Group VA, VIA, VIIA

The number of the charge = The number of the charge =

Examples: sulfide = 8 – 6 = 2 Examples: sulfide = 8 – 6 = 2 ionion = =

phosphide = ______phosphide = ______

Iodide = _____Iodide = _____

8 – the groupA number

S-2

P-3

I-

Cross-Over-Method Cross-Over-Method Place the charge Place the charge numbernumber of the metal as the of the metal as the subscript to the nonmetal and the charge subscript to the nonmetal and the charge numbernumber of of the nonmetal as the subscript to the metal.the nonmetal as the subscript to the metal.

You must reduce the charges if you can.You must reduce the charges if you can.ExamplesExamples: :

Lithium FluorideLithium Fluoride Magnesium Fluoride Magnesium Fluoride

Potassium SulfidePotassium Sulfide Copper I ChlorideCopper I Chloride

Aluminum NitrideAluminum Nitride Chromium III Sulfide Chromium III Sulfide

Li+ F- = LiF Mg+2 F- =MgF2

K+ S-2 = K2S Cu+ Cl- = CuCl

Al+3N-3 = AlN Cr+3 S-2 = Cr2S3

USE THE RULES ABOVE TO WRITE FORMULAS USE THE RULES ABOVE TO WRITE FORMULAS FOR THE BINARY IONICFOR THE BINARY IONIC COMPOUNDS:COMPOUNDS:

Calcium Fluoride __________ Calcium Fluoride __________ Rubidium Iodide ___________Rubidium Iodide ___________

Sodium Phosphide ________Sodium Phosphide ________ Strontium chloride__________Strontium chloride__________

Mercury I Oxide ___________Mercury I Oxide ___________ Tin II Sulfide______________Tin II Sulfide______________

Iron III nitride _____________ Copper I Selenide___________Iron III nitride _____________ Copper I Selenide___________

Ca+2 F- = Rb+ I- =

Sr+2 Cl- =

Hg+ O-2 = Sn+2 S-2 =

Fe+3 N-3 = Cu+ Se-2 =

CaF2 RbI

Na3P SrCl2

Hg2O SnS

FeN Cu2Se

Na+P3

Classwork and homework worksheet 2 & 3 Binary Ionic Compounds.

Ternary CompoundsTernary CompoundsTernary CompoundsTernary Compounds are are __________________ and and contain a _____________________.contain a _____________________.

POLYATOMIC IONPOLYATOMIC ION – –

  A group of atoms that act as a single unit and A group of atoms that act as a single unit and carry a charge.carry a charge.

Polyatomic ions end in Polyatomic ions end in “ ““ “ or or “ ““ “ EXCEPTIONS: (OH)EXCEPTIONS: (OH)- -

(CN)(CN)--

*only (+) poly atomic ions (NH*only (+) poly atomic ions (NH44))+ +

(PH(PH44))++

Polyatomic Ion

Ionic

hydroxide

ite ate

cyanide

ammonium

phosphonium

(Naming) Rules are similar to Binary (Naming) Rules are similar to Binary ionic compounds.ionic compounds.

Element with positive ionic charge is Element with positive ionic charge is written first. ( )written first. ( )

  Group A Metals: name simply written Ex. Group A Metals: name simply written Ex. CaCa2+2+ - -

  Group B Metals: need a roman numeral Group B Metals: need a roman numeral Ex. PbEx. Pb2+2+ _________ _________

cation

calcuim

Lead II

2. Polyatomic ion ( ) written next.2. Polyatomic ion ( ) written next.

Write the name as it appears on the back Write the name as it appears on the back of the Periodic Chart.of the Periodic Chart.

Ex. (CEx. (C22HH33OO22))--

(Cr(Cr22OO77))2-2-

Naming Examples: LiCONaming Examples: LiCO33

Be(CN)Be(CN)22

Sn(SOSn(SO44))22

radical

acetate

dichromate

Lithium carbonate

Beryllium cyanide

Tin IV sulfate

USE THE RULES ABOVE TO NAME THE USE THE RULES ABOVE TO NAME THE TERNARY IONIC COMPOUNDS BELOW:TERNARY IONIC COMPOUNDS BELOW:

MgSOMgSO44 ___________________________ ___________________________  

NaNONaNO3_3_______________________________________________________  

CaCOCaCO33 ___________________________ ___________________________

NaOH __________________________NaOH __________________________

Ba(ClOBa(ClO22))22 ________________________ ________________________

Magnesium sulfate

Sodium nitrate

Calcium carbonate

Sodium hydroxide

Barium chlorite

Ternary Naming ContinuedTernary Naming Continued

FeFe22(C(C44HH44OO66))33 __________________ __________________

(NH(NH44))33POPO44 ________________________ ________________________

CuCu22CrOCrO44 __________________________ __________________________

Hg(NOHg(NO22)) ____________________________________________________

AlAl22(SO(SO44))33 __________________________ __________________________

Iron III tartrateAmmonium phosphate

Copper I chromate

Mercury I nitrite

aluminum sulfate

Writing Ternary Ionic FormulasWriting Ternary Ionic FormulasWrite the ion for the metal first.Write the ion for the metal first.– Group A Metals – Group A Metals –

Ex. Calcium Ex. Calcium

RubidiumRubidium

BoronBoron

Group B Metals – The Roman Numeral Group B Metals – The Roman Numeral tells you the charge number.tells you the charge number.

Ex. Iron IIIEx. Iron III Lead IVLead IV

Mercury IMercury I Tin IITin II

Group # = charge

Group 2 = Ca +2

Group 1 = Rb +1

Group 3 = B +3

Fe +3 Pb+4

Hg +1 Sn +2

Write the polyatomic ion next (Write the polyatomic ion next (USE USE PARENTHESISPARENTHESIS))

*Remember polyatomic ions end in *Remember polyatomic ions end in

“ “ “ “ or “ “or “ “

except (OH)except (OH)-- and (CN) and (CN)--

Examples: Examples:

Sulfite Sulfite

CarbonateCarbonate

PhosphatePhosphate

NitriteNitrite

ite ate

hydroxide cyanide

SO3 -2

CO3 -2

PO4 -3

NO2 -

Cross-Over-MethodCross-Over-Methodwrite the charge number of the metal as the write the charge number of the metal as the subscriptsubscript of the of the polyatomic ion. (You MUST use PARENTHESIS if the polyatomic ion. (You MUST use PARENTHESIS if the subscript is 2 or greater but subscript is 2 or greater but DO NOT use ParenthesisDO NOT use Parenthesis if the if the subscript is 1)subscript is 1)

2. write the charge number of the polyatomic ion as the 2. write the charge number of the polyatomic ion as the subscriptsubscript of the metal. *You must reduce if you can but of the metal. *You must reduce if you can but NEVERNEVER change the polyatomic ion!! change the polyatomic ion!! DO NOT TOUCH THE DO NOT TOUCH THE POLYATOMIC ION !!POLYATOMIC ION !!

DO NOT CHANGE THE FORMULA OF THE DO NOT CHANGE THE FORMULA OF THE POLYATOMIC ION !!POLYATOMIC ION !!

Examples: Magnesium nitrateExamples: Magnesium nitrate

Aluminum sulfateAluminum sulfate

Iron II sulfiteIron II sulfite

Iron III sulfiteIron III sulfite

Tin IV nitrateTin IV nitrate

DO NOT TOUCH THE POLYATOMIC ION DO NOT TOUCH THE POLYATOMIC ION

DO NOT CHANGE THE DO NOT CHANGE THE FORMULA OF THE POLYATOMIC ION !!FORMULA OF THE POLYATOMIC ION !!

Examples: Examples:

Magnesium nitrateMagnesium nitrate

Aluminum sulfateAluminum sulfate

Iron II sulfiteIron II sulfite

Iron III sulfiteIron III sulfite

Tin IV nitrateTin IV nitrate

Mg+2 NO3- = Mg(NO3)2

Al+3 SO4-2 = Al2(SO4)3

Fe+2 SO3-2 = FeSO3

Fe+3 SO3-2 = Fe2(SO3)3

Sn+4 NO3- = Sn(NO3)4

USE THE RULES ABOVE TO WRITE TERNARY USE THE RULES ABOVE TO WRITE TERNARY FORMULAS FOR THE COMPOUNDS FORMULAS FOR THE COMPOUNDS

Ammonium sulfide __________________Ammonium sulfide __________________

Silver chromate ____________________Silver chromate ____________________

Iron III tartrate _____________________Iron III tartrate _____________________

Beryllium hydroxide ________________Beryllium hydroxide ________________

aluminum oxalate _________________aluminum oxalate _________________

Copper I cyanide ___________________Copper I cyanide ___________________

Nickel carbonate ___________________Nickel carbonate ___________________

+1;-2 (NH4)2S

+1;-2 Ag2CrO4

+3;-2 Fe2(C4H4O6)3

+2;-1 Be(OH)2

+3;-2 Al2(C2O4)3

+1;-1 CuCN

+2;-2 NiCO3

Molecular CompoundsMolecular Compounds

Writing names and FormulasWriting names and Formulas

Molecular CompoundsMolecular Compounds

Made up of 2 or more NONMETALS (NO Made up of 2 or more NONMETALS (NO METALS or IONS)METALS or IONS)

Share electrons when bondingShare electrons when bonding

Sharing Electrons is called COVALENT Sharing Electrons is called COVALENT BONDINGBONDING

The smallest unit of a molecular The smallest unit of a molecular compound is called a MOLECULE.compound is called a MOLECULE.

(NAMING(NAMING) ) To write the name, write 2 wordsTo write the name, write 2 words

1.) the non-metal closest to the metals on 1.) the non-metal closest to the metals on the periodic chart is written first.the periodic chart is written first.2.) 2.) PrefixesPrefixes are used to tell how many are used to tell how many atoms of each element are in the atoms of each element are in the compound.compound. – 1 1 6 6 – 2 2 7 7 – 3 3 8 8 – 44 9 9 – 5 5 10 10

heptadi

hexamono

tri

tetra

penta

octa

nona

deca

Exception: don’t write mono- if there is Exception: don’t write mono- if there is only one of the first element.only one of the first element.3.) The second element always uses a 3.) The second element always uses a prefix and ends in “ _prefix and ends in “ _ide ide ”. ”.

4.)No double vowels when writing 4.)No double vowels when writing names (oa, oo)names (oa, oo)

Ex. CO carbon monoxide

CO2 carbon dioxide

P2O5 diphosphorus pentoxide

Name TheseName TheseNN22OO

Dinitrogen monoxideDinitrogen monoxide

NONO22

Nitrogen dioxideNitrogen dioxide

ClCl22OO77

Dichlorine heptoxideDichlorine heptoxide

CBrCBr44

Carbon tetrabromideCarbon tetrabromide

SiOSiO22

silicon dioxidesilicon dioxide

PP22OO33

Diphosphorus trioxideDiphosphorus trioxide

((FORMULA WRITINGFORMULA WRITING) ) NO CRISS CROSSINGNO CRISS CROSSING

Nitrogen trioxide _________ carbon tetrafluoride _______

Diiodine decachloride _____ phosphorous triiodide ______

Sulfur hexabromide _______ nitrogen pentafluoride ______

Diphosphorous trisulfide ____ carbon tetrabromide ______

NO3 CF4

I2Cl10 PI3

SBr6 NF5

P2S3 CBr4

Examples: Phosphorous pentachloride - PCl5 Dinitrogen trisulfide – N2S3

AcidsAcids

Writing names and FormulasWriting names and Formulas

AcidsAcids

Compounds that give off hydrogen ions Compounds that give off hydrogen ions when dissolved in water.when dissolved in water.

Must have H in them.Must have H in them.

will always be some H next to an anion.will always be some H next to an anion.

The anion determines the name.The anion determines the name.

Naming acidsNaming acids

If the anion attached to hydrogen is ends If the anion attached to hydrogen is ends in in -ide-ide, put the prefix , put the prefix hydro- hydro- and change -and change -ideide to to -ic acid-ic acid

HCl - hydrogen ion and chlorHCl - hydrogen ion and chlorideide ion ion

hydrohydrochlorchloric acidic acid

HH22S hydrogen ion and sulfS hydrogen ion and sulfideide ion ion

hydrohydrosulfursulfuric acidic acid

Naming AcidsNaming Acids

If the anion has oxygen in itIf the anion has oxygen in it

it ends in -ate or -iteit ends in -ate or -ite

change the suffix change the suffix -ate -ate to to -ic acid-ic acid

HNOHNO33 Hydrogen and nitr Hydrogen and nitrateate ions ions

NitrNitric acidic acid

change the suffix change the suffix -ite -ite to to -ous acid-ous acid

HNOHNO22 Hydrogen and nitr Hydrogen and nitriteite ions ions

NitrNitrous acidous acid

Name theseName these

HFHF

HH33PP

HH22SOSO44

HH22SOSO33

HCNHCN

HH22CrOCrO44

Hydrofluoric acid

Hydrophosphoric acid

sulfuric acid

sulfurous acid

hydrocyanic acid

chromic acid

Writing Acid Formulas/NamingWriting Acid Formulas/Naming

Hydrogen will always be firstHydrogen will always be firstname will tell you the anionname will tell you the anionmake the charges cancel outmake the charges cancel outStarts with Starts with hydrohydro- if - if no oxygenno oxygen in the acid, in the acid, -ide-ide ending becomes ending becomes –ic–icEx. HCl = hydochloric acidEx. HCl = hydochloric acidno hydro, no hydro, -ate -ate ending from polyatomic ion ending from polyatomic ion becomes becomes -ic-ic, H, H22SOSO44 = sulfuric acid = sulfuric acid

-ite -ite ending becomes ending becomes –ous–ous, H, H22SOSO33 = sulfurous = sulfurous acidacid

Write formulas for theseWrite formulas for these

hydroiodic acidhydroiodic acid

acetic acidacetic acid

carbonic acidcarbonic acid

phosphorous acidphosphorous acid

hydrobromic acidhydrobromic acid

HI

HC2H3O2

H2CO3

H3PO3

HBr