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Transcript of Chapter 6 Chemical Names and Formulas. Section 6.1 Introduction to Chemical Bonding OBJECTIVES:...
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Chapter 6Chapter 6Chemical Names and Chemical Names and
FormulasFormulas
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Section 6.1Section 6.1Introduction to Chemical Introduction to Chemical
BondingBondingOBJECTIVES:OBJECTIVES:
Distinguish between ionic and molecular Distinguish between ionic and molecular compounds.compounds.
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Section 6.1Section 6.1Introduction to Chemical Introduction to Chemical
BondingBondingOBJECTIVES:OBJECTIVES:
Define cation and anion, and relate Define cation and anion, and relate them to metal and nonmetal.them to metal and nonmetal.
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Molecules and Molecular Molecules and Molecular CompoundsCompounds
About 100 different elementsAbout 100 different elementsMillions of compounds from themMillions of compounds from themNaming is essential in chemistryNaming is essential in chemistryNoble gases, such as He and NeNoble gases, such as He and NeIsolated atoms- monatomic, they Isolated atoms- monatomic, they
consist of single atomsconsist of single atoms
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Molecules and Molecular Molecules and Molecular CompoundsCompounds
Molecule- smallest electrically neutral Molecule- smallest electrically neutral unit, still has properties of the unit, still has properties of the substancesubstance
Made from only nonmetalsMade from only nonmetalsCan be from one element- OCan be from one element- O22
Can make a compound- COCan make a compound- CO22
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Molecules and Molecular Molecules and Molecular CompoundsCompounds
Properties of molecular compoundsProperties of molecular compoundsLow melting and boiling pointsLow melting and boiling pointsUsually gas or liquidUsually gas or liquidComposed of two or more Composed of two or more
nonmetalsnonmetalsOO22, O, O33, H, H22OO
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Systematic NamingSystematic Naming
There are too many compounds to There are too many compounds to remember the names of them all.remember the names of them all.
Compound is made of two or more Compound is made of two or more elements.elements.
Put together atoms.Put together atoms.Name should tell us how many and Name should tell us how many and
what type of atoms.what type of atoms.
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Atoms and ionsAtoms and ions
AtomsAtoms are electrically neutral. are electrically neutral.Same number of protons and electrons.Same number of protons and electrons. IonsIons are atoms, or groups of atoms, with a are atoms, or groups of atoms, with a
charge (positive or negative)charge (positive or negative)Different numbers of protons and Different numbers of protons and
electrons.electrons.Only electrons can move.Only electrons can move.Gain or lose electrons.Gain or lose electrons.
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AnionAnion
A negative ion.A negative ion.Has Has gainedgained electrons. electrons.Nonmetals can gainNonmetals can gain electrons. electrons.Charge is written as a superscript on the Charge is written as a superscript on the
right.right.
F-Has gained one electron (-ide is new ending= fluoride)
O2- Gained two electrons (oxide)
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Cations Positive ions. Formed by losing electrons. More protons than electrons. Metals can lose electrons
K+ Has lost one electron (no name change for positive ions)
Ca2+ Has lost two electrons
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Ionic CompoundsIonic Compounds
Ionic compoundsIonic compounds- from joining - from joining metal metal cations and nonmetal anionscations and nonmetal anions- they - they are are electrically neutralelectrically neutral
Usually solid crystalsUsually solid crystalsMelt at high temperaturesMelt at high temperatures
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Two Types of CompoundsTwo Types of Compounds
Molecular compoundsMolecular compoundsMade of molecules.Made of molecules.Made by joining Made by joining nonmetalnonmetal atoms atoms
together into molecules.together into molecules.
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Two Types of CompoundsTwo Types of Compounds
Ionic CompoundsIonic CompoundsMade of cations and anions.Made of cations and anions.Metals and nonmetalsMetals and nonmetals..The electrons lost by the cation are The electrons lost by the cation are
gained by the anion.gained by the anion.The cation and anions surround each The cation and anions surround each
other.other.Smallest piece is a Smallest piece is a FORMULA UNIT.FORMULA UNIT.
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Two Types of CompoundsTwo Types of Compounds
Smallest piece
Melting Point
State
Types of elements
Formula Unit Molecule
Metal and Nonmetal
Nonmetals
solidSolid, liquid or gas
High >300ºC Low <300ºC
Ionic Molecular
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Section 6.2Section 6.2Representing Chemical Representing Chemical
CompoundsCompoundsOBJECTIVES:OBJECTIVES:
Distinguish among chemical formulas, Distinguish among chemical formulas, molecular formulas, and formula units.molecular formulas, and formula units.
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Section 6.2Section 6.2Representing Chemical Representing Chemical
CompoundsCompoundsOBJECTIVES:OBJECTIVES:
Use experimental data to show that a Use experimental data to show that a compound obeys the law of definite compound obeys the law of definite proportions.proportions.
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Chemical FormulasChemical Formulas
Shows the Shows the kindkind and and numbernumber of atoms of atoms in the smallest piece of a substance.in the smallest piece of a substance.
Molecular formulaMolecular formula- number and kinds - number and kinds of atoms in a molecule.of atoms in a molecule.
COCO22
CC66HH1212OO66
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Chemical FormulasChemical Formulas
More than one atom? –use a More than one atom? –use a subscript (Hsubscript (H22O)O)
There are 7 There are 7 diatomicdiatomic elements elementsHydrogen (HHydrogen (H22), Nitrogen (N), Nitrogen (N22), ),
Oxygen (OOxygen (O22), Fluorine (F), Fluorine (F22), Chlorine ), Chlorine
(Cl(Cl22), Bromine (Br), Bromine (Br22), and Iodine (I), and Iodine (I22))Remember: “Br I N Cl H O F”Remember: “Br I N Cl H O F”
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Ionic CompoundsIonic Compounds
This formula represents not a This formula represents not a molecule, but a molecule, but a formula unitformula unit
The smallest whole number ratio of The smallest whole number ratio of atoms in an ionic compound.atoms in an ionic compound.
Ions surround each other so you can’t Ions surround each other so you can’t say which is hooked to which. (p. say which is hooked to which. (p. 140)140)
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Some Laws:Some Laws:
1. 1. Law of Definite ProportionsLaw of Definite Proportions- in a - in a sample of a chemical compound, the sample of a chemical compound, the masses of the elements are always in masses of the elements are always in the same proportions.the same proportions.
HH22O (water) and HO (water) and H22OO22 (hydrogen (hydrogen
peroxide)peroxide)
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Some Laws:Some Laws:
2. 2. Law of Multiple ProportionsLaw of Multiple Proportions- - Dalton stated that whenever two Dalton stated that whenever two elements form more than one elements form more than one compound, the different masses of compound, the different masses of one element that combine with the one element that combine with the same mass of the other element same mass of the other element are in the ratio of small whole are in the ratio of small whole numbers.numbers.
Figure 6.11, p. 141Figure 6.11, p. 141
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Section 6.3Section 6.3Ionic ChargesIonic Charges
OBJECTIVES:OBJECTIVES:Use the periodic table to determine the Use the periodic table to determine the
charge on an ion.charge on an ion.
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Section 6.3Section 6.3Ionic ChargesIonic Charges
OBJECTIVES:OBJECTIVES:Define a polyatomic ion, and give the Define a polyatomic ion, and give the
names and formulas of the most names and formulas of the most common polyatomic ions.common polyatomic ions.
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Charges on ionsCharges on ions
For most of the Group A elements, For most of the Group A elements, the Periodic Table can tell what the Periodic Table can tell what kind of ion they will form from their kind of ion they will form from their location; location; monatomicmonatomic ions ions
Elements in the same group have Elements in the same group have similar properties.similar properties.
Including the charge when they are Including the charge when they are ions.ions.
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2+
1+
3+ 3- 2- 1-
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What about the others?What about the others?
Groups 4A and 0 do not usually form Groups 4A and 0 do not usually form ions (in fact, Group 0 rarely forms ions (in fact, Group 0 rarely forms compounds!)compounds!)
Many transition metals have Many transition metals have more more than one than one common ionic chargecommon ionic charge
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Naming ionsNaming ions
Two methods if more than one Two methods if more than one charge is possible:charge is possible:1. Stock system – uses roman 1. Stock system – uses roman
numerals in parenthesis to numerals in parenthesis to indicate the numerical valueindicate the numerical value
2. Classical method – uses root 2. Classical method – uses root word with suffixes (-ous, -ic)word with suffixes (-ous, -ic)Does not give true valueDoes not give true value
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Naming ionsNaming ions
We will use the Stock system.We will use the Stock system.Cation- if the charge is always the Cation- if the charge is always the
same (Group A) just write the name of same (Group A) just write the name of the metal.the metal.
Transition metals can have more than Transition metals can have more than one type of charge.one type of charge.
Indicate the charge with roman Indicate the charge with roman numerals in parenthesis (Table 6.3, numerals in parenthesis (Table 6.3, p.144)p.144)
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Name theseName these
NaNa++ CaCa2+2+ AlAl3+3+ FeFe3+3+ FeFe2+2+ PbPb2+2+ LiLi++
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Write Formulas for theseWrite Formulas for these
Potassium ionPotassium ionMagnesium ion Magnesium ion Copper (II) ionCopper (II) ionChromium (VI) ionChromium (VI) ionBarium ionBarium ionMercury (II) ionMercury (II) ion
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluorineine
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluorinin
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluorii
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluor
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluorii
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – ideChange the element ending to – ideFF-- Fluor Fluoridid
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Naming AnionsNaming Anions
Anions are always the same chargeAnions are always the same chargeChange the element ending to – Change the element ending to – ideideFF-- Fluor Fluorideide
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Name theseName these
ClCl-- NN3-3- BrBr-- OO2-2-
GaGa3+3+
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Write theseWrite these
Sulfide ionSulfide ioniodide ioniodide ionphosphide ionphosphide ionStrontium ionStrontium ion
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Exceptions:Exceptions:Some of the transition metals have Some of the transition metals have
only one ionic charge:only one ionic charge:Do not use roman numerals for Do not use roman numerals for
these:these:SilverSilver is always 1+ ( is always 1+ (AgAg++))CadmiumCadmium and and ZincZinc are always are always
2+ (2+ (CdCd2+2+ and and ZnZn2+2+))Note Fig. 6.13, p. 145Note Fig. 6.13, p. 145
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Polyatomic ionsPolyatomic ionsGroups of atoms that stay together and Groups of atoms that stay together and
have a charge.have a charge.Learn these - Table 6.4, p.147Learn these - Table 6.4, p.147
Acetate Acetate CC22HH33OO22--
Nitrate Nitrate NONO33--
Nitrite Nitrite NONO22--
Hydroxide Hydroxide OHOH-- and Cyanide and Cyanide CNCN-- Permanganate Permanganate MnOMnO44
--
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Polyatomic ionsPolyatomic ionsSulfate Sulfate SOSO44
2-2-
Sulfite Sulfite SOSO332-2-
Carbonate Carbonate COCO332-2-
Chromate Chromate CrOCrO442-2-
Dichromate Dichromate CrCr22OO772-2-
Phosphate Phosphate POPO443-3-
Phosphite Phosphite POPO333-3-
Ammonium Ammonium NHNH44++
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Section 6.4Section 6.4Ionic CompoundsIonic Compounds
OBJECTIVES:OBJECTIVES:Apply the rules for naming and writing Apply the rules for naming and writing
formulas for binary ionic compounds.formulas for binary ionic compounds.
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Section 6.4Section 6.4Ionic CompoundsIonic Compounds
OBJECTIVES:OBJECTIVES:Apply the rules for naming and writing Apply the rules for naming and writing
formulas for ternary ionic compounds.formulas for ternary ionic compounds.
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Naming Binary Ionic CompoundsNaming Binary Ionic CompoundsBinaryBinary Compounds - 2 elements. Compounds - 2 elements. Ionic - a cation and an anion.Ionic - a cation and an anion.To write the names, just name the two To write the names, just name the two
ions.ions.Easy with Representative elements Easy with Representative elements
(which are Group A elements)(which are Group A elements)NaCl = NaCl = NaNa++ ClCl-- = sodium chloride = sodium chloride
MgBrMgBr22 = = MgMg2+2+ BrBr-- = magnesium bromide= magnesium bromide
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Naming Binary Ionic CompoundsNaming Binary Ionic Compounds
The problem comes with the The problem comes with the transition metals.transition metals.
Need to figure out their charges.Need to figure out their charges.The compound must be neutral.The compound must be neutral.same number of + and – charges.same number of + and – charges.Use the anion to determine the Use the anion to determine the
charge on the positive ion.charge on the positive ion.
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Naming Binary Ionic CompoundsNaming Binary Ionic Compounds
Write the name of CuOWrite the name of CuONeed the charge of CuNeed the charge of CuO is 2-O is 2-copper must be 2+copper must be 2+Copper (II) oxideCopper (II) oxideName CoClName CoCl33 Cl is 1- and there are three of them = 3-Cl is 1- and there are three of them = 3-Co must be 3+ Cobalt (III) chlorideCo must be 3+ Cobalt (III) chloride
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Naming Binary Ionic CompoundsNaming Binary Ionic Compounds
Write the name of CuWrite the name of Cu22S.S.
Since S is 2-, the CuSince S is 2-, the Cu22 must be 2+, so must be 2+, so
each one is 1+.each one is 1+.copper (I) sulfidecopper (I) sulfideFeFe22OO33 Each O is 2- 3 x -2 = -6Each O is 2- 3 x -2 = -62 Fe must = 6+, so each is 3+.2 Fe must = 6+, so each is 3+. iron (III) oxideiron (III) oxide
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Naming Binary Ionic CompoundsNaming Binary Ionic Compounds
Write the names of the followingWrite the names of the following KClKCl NaNa33NN
CrNCrN
ScSc33PP22
PbOPbO
PbOPbO22
NaNa22SeSe
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Ternary Ionic Compounds Ternary Ionic Compounds
These will have polyatomic ionsThese will have polyatomic ionsAt least three elementsAt least three elementsname the ionsname the ionsNaNONaNO33
CaSOCaSO44
CuSOCuSO33
(NH(NH44))22OO
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Ternary Ionic CompoundsTernary Ionic Compounds
LiCNLiCNFe(OH)Fe(OH)33
(NH(NH44))22COCO33
NiPONiPO44
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Writing FormulasWriting Formulas
The charges have to add up to The charges have to add up to zero.zero.
Get charges on pieces.Get charges on pieces.Cations from name on table.Cations from name on table.Anions from table or polyatomic.Anions from table or polyatomic.Balance the charges by adding Balance the charges by adding
subscripts.subscripts.Put polyatomics in parenthesis.Put polyatomics in parenthesis.
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Writing FormulasWriting Formulas
Write the formula for calcium chloride.Write the formula for calcium chloride.Calcium is Calcium is CaCa2+2+ Chloride is Chloride is ClCl-- CaCa2+2+ Cl Cl-- would have a 1+ charge. would have a 1+ charge.Need another Need another ClCl-- CaCa2+2+ Cl Cl22
1-1- (use criss-cross method) (use criss-cross method)
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Write the formulas for theseWrite the formulas for these
Lithium sulfideLithium sulfide tin (II) oxidetin (II) oxide tin (IV) oxidetin (IV) oxideMagnesium fluorideMagnesium fluorideCopper (II) sulfateCopper (II) sulfate Iron (III) phosphideIron (III) phosphidegallium nitrategallium nitrate Iron (III) sulfideIron (III) sulfide
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Write the formulas for theseWrite the formulas for these
Ammonium chlorideAmmonium chlorideammonium sulfideammonium sulfidebarium nitratebarium nitrate
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Things to look forThings to look for
If cations have ( ), the number in If cations have ( ), the number in parenthesis is their charge.parenthesis is their charge.
If anions end in If anions end in -ide-ide they are probably they are probably off the periodic table (Monoatomic)off the periodic table (Monoatomic)
If anion ends in If anion ends in -ate-ate or or -ite-ite it is it is polyatomicpolyatomic
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Section 6.5Section 6.5Molecular Compounds and Molecular Compounds and
AcidsAcidsOBJECTIVES:OBJECTIVES:
Apply the rules for naming and writing Apply the rules for naming and writing formulas for binary molecular formulas for binary molecular compounds.compounds.
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Section 6.5Section 6.5Molecular Compounds and Molecular Compounds and
AcidsAcidsOBJECTIVES:OBJECTIVES:
Name and write formulas for common Name and write formulas for common acids.acids.
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Molecular compoundsMolecular compounds
made of just made of just nonmetalsnonmetalssmallest piece is a smallest piece is a moleculemoleculecan’t be held together because of can’t be held together because of
opposite charges.opposite charges.can’t use charges to figure out how can’t use charges to figure out how
many of each atommany of each atom
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Molecular are easier!Molecular are easier!
Ionic compounds use charges to Ionic compounds use charges to determine how many of each.determine how many of each.Have to figure out charges.Have to figure out charges.Have to figure out numbers.Have to figure out numbers.
Molecular compounds Molecular compounds name tellsname tells youyou the number of atoms.the number of atoms.
Uses Uses prefixesprefixes to tell you the number to tell you the number
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Prefixes (Table 6.5, p.159)Prefixes (Table 6.5, p.159)
1 = mono-1 = mono-2 = di-2 = di-3 = tri-3 = tri-4 = tetra-4 = tetra-5 = penta-5 = penta-6 = hexa-6 = hexa-7 = hepta-7 = hepta-8 = octa- 8 = octa-
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PrefixesPrefixes
9 = nona-9 = nona-10 = deca-10 = deca-To write the name, write two words:To write the name, write two words:
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PrefixesPrefixes
9 = nona-9 = nona-10 = deca-10 = deca-To write the name, write two words:To write the name, write two words:
Prefix name Prefix name -ide
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PrefixesPrefixes
9 = nona-9 = nona-10 = deca-10 = deca-To write the name, write two words:To write the name, write two words:
One exception is we don’t write mono- if One exception is we don’t write mono- if there is only one of the first element.there is only one of the first element.
Prefix name Prefix name -ide
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PrefixesPrefixes
9 = nona-9 = nona- 10 = deca-10 = deca- To write the name, write two words:To write the name, write two words: One exception is we don’t write mono- if One exception is we don’t write mono- if
there is only one of the first element.there is only one of the first element. No double vowels when writing names No double vowels when writing names
(oa oo)(oa oo)
Prefix name Prefix name -ide
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Name TheseName These
NN22OO
NONO22
ClCl22OO77
CBrCBr44
COCO22
BaClBaCl22
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Write formulas for theseWrite formulas for these
diphosphorus pentoxidediphosphorus pentoxidetetraiodine nonoxidetetraiodine nonoxidesulfur hexafluoridesulfur hexafluoridenitrogen trioxidenitrogen trioxidecarbon tetrahydridecarbon tetrahydridephosphorus trifluoridephosphorus trifluoridealuminum chloridealuminum chloride
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AcidsAcids
Writing names and FormulasWriting names and Formulas
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AcidsAcids
Compounds that give off hydrogen Compounds that give off hydrogen ions when dissolved in water.ions when dissolved in water.
Must have H in them.Must have H in them.will always be some H next to an will always be some H next to an
anion.anion.The The anionanion determines the name. determines the name.
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Naming acidsNaming acids
If the anion attached to hydrogen If the anion attached to hydrogen ends in ends in -ide-ide, put the prefix , put the prefix hydro- hydro- and and change -change -ideide to to -ic acid-ic acid
HCl - hydrogen ion and chlorHCl - hydrogen ion and chlorideide ion ionhydrohydrochlorchloric acidic acidHH22S hydrogen ion and sulfS hydrogen ion and sulfideide ion ionhydrohydrosulfursulfuric acidic acid
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Naming AcidsNaming Acids
If the anion has oxygen in it, then it If the anion has oxygen in it, then it ends in -ate of -iteends in -ate of -ite
change the suffix change the suffix -ate -ate to to -ic acid -ic acid (use no (use no prefix)prefix)
HNOHNO33 Hydrogen and nitr Hydrogen and nitrateate ions ionsNitrNitric acidic acidchange the suffix change the suffix -ite -ite to to -ous acid-ous acidHNOHNO22 Hydrogen and nitr Hydrogen and nitriteite ions ionsNitrNitrous acidous acid
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Name theseName these
HFHFHH33PP
HH22SOSO44
HH22SOSO33 HCNHCNHH22CrOCrO44
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Writing Acid FormulasWriting Acid Formulas
Hydrogen will always be firstHydrogen will always be firstname will tell you the anionname will tell you the anionmake the charges cancel out.make the charges cancel out.Starts with hydro?- no oxygen, -ideStarts with hydro?- no oxygen, -ideno hydro?, no hydro?, -ate -ate comes from comes from -ic-ic, , -ite -ite
comes from comes from -ous-ous
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Write formulas for theseWrite formulas for these
hydroiodic acidhydroiodic acidacetic acidacetic acidcarbonic acidcarbonic acidphosphorous acidphosphorous acidhydrobromic acidhydrobromic acid
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Section 6.6Section 6.6Summary of Naming and Summary of Naming and
Formula WritingFormula WritingOBJECTIVES:OBJECTIVES:
Use the flowchart in Figure 6.21 to write Use the flowchart in Figure 6.21 to write the name of a compound when given its the name of a compound when given its chemical formula.chemical formula.
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Section 6.6Section 6.6Summary of Naming and Summary of Naming and
Formula WritingFormula WritingOBJECTIVES:OBJECTIVES:
Use the flowchart in Figure 6.23 to write Use the flowchart in Figure 6.23 to write a chemical formula when given the a chemical formula when given the name of a compound.name of a compound.
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Helpful to remember...Helpful to remember...
1. In an ionic compound, the net ionic 1. In an ionic compound, the net ionic charge is charge is zero zero (criss-cross method)(criss-cross method)
2. An 2. An -ide-ide ending generally indicates a ending generally indicates a binary compoundbinary compound
3. An 3. An -ite-ite or or -ate-ate ending means there ending means there is a polyatomic ion that has oxygenis a polyatomic ion that has oxygen
4. 4. PrefixesPrefixes generally mean molecular; generally mean molecular; they show the number of each atomthey show the number of each atom
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Helpful to remember...Helpful to remember...
5. A 5. A Roman numeralRoman numeral after the name of after the name of a cation shows the a cation shows the ionic chargeionic charge of of the cationthe cation
Use the Use the handout sheetshandout sheets provided provided by your teacher!by your teacher!
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Summary of Naming and Summary of Naming and Formula WritingFormula Writing
For naming, follow the flowchart- Fig. For naming, follow the flowchart- Fig. 6.21, page 1616.21, page 161
For writing formulas, follow the For writing formulas, follow the flowchart from Fig. 6.23, p. 162flowchart from Fig. 6.23, p. 162