Post on 02-Jan-2016
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Molecules and Compounds: Nomenclature
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Compounds vs. ElementsCompound 1: Table Salt
Properties: Soluble crystals, stable, edibleElements (Components)• Sodium – shiny, reactive, poisonous• Chlorine – pale yellow gas, reactive,
poisonous
Compound 2: Table sugarProperties: sweet, soluble crystalElements (Components) :• Carbon – pencil or diamonds• Hydrogen – flammable gas• Oxygen – a gas in air Sugar:
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Law of Constant CompositionPure substances have constant composition
all samples of a pure substance contain the same elements in the same percentages (ratios): Water (H: 11%, O: 89%), Table salt (Na: 39%, Cl: 61%), Sugar
mixtures have variable composition: Air, Seawater, Concrete, Rocky road ice cream, Coke
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Why do Compounds ShowConstant Composition
• the smallest piece of a compound is called a molecule: Water molecule, Sugar molecule
• every molecule of a compound has the same number and type of atoms.
Water molecule: 2 Hydrogen atom + 1 Oxygen atom;
Sugar molecule: 12 Carbon atom + 22 Hydrogen atom + 11 Oxygen atom
every sample of the compound will have the same ratio of the elements
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Chemical FormulaChemical formula: describe the compound by
describing the number and type of each atom in the simplest unit of the compoundmolecules or ions (Table salt: Cl+, Na-)
• Element represented by its letter symbol: H instead of hydrogen; Na instead of Sodium
• #Atoms of each element: the right of the element as a subscript, H2O (unless if there is only one atom, the 1 subscript is not written)
• Polyatomic groups (multiple atoms in group, example: CO3) are placed in parentheses if more than one
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From Composition to Chemical Formula
water = H2O two atoms of
hydrogen and 1 atom of oxygen
table sugar = C12H22O11 12 atoms
of C, 22 atoms of H and 11 atoms O
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Classifying Pure Substances
Element• Atomic: consists of single atoms
(Metals, Noble gases)• Molecular: consists of multi-atom
molecules (O2, N2, Cl2, etc)
Compound• Molecular: consists of molecules
made of only nonmetals (CO2, H2O)• Ionic: consists of cations (Na+) and
anions (Cl-)
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Elements and Compounds
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Classify each of the following:Element atomic/molecular
Compound molecular/ionic
• aluminum, Al
• aluminum chloride, AlCl3
• chlorine, Cl2
• acetone, C3H6O
• carbon monoxide, CO
• cobalt, Co
• aluminum, Al = atomic element
• aluminum chloride, AlCl3 = ionic compound
• chlorine, Cl2 = molecular element
• acetone, C3H6O = molecular compound
• carbon monoxide, CO = molecular compound
• cobalt, Co = atomic element
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Molecular ElementsCertain elements occur as 2 atom molecules• Rule of 7’s
there are 7 common diatomic elements find the element with atomic number 7, Nmake a figure 7 by going over to Group 7A, then downdon’t forget to include H2
H2
Cl2
Br2
I2
7VIIA
N2 O2 F2
Molecular Elements
IBrCl
N O FH
= Metal
= Metalloid
= Nonmetal
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Molecular Compounds
• two or more nonmetals• smallest unit is a
molecule
• Common examples: H2O
• CO2 (as in soda and dry ice)
• NH3 (as in Windex),
• Table sugar C11H22O11
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Ionic Compounds
Ions: Metals (Cation Mx+) and Nonmetals (Anion Ny-)
• No individual molecules!!• have a 3-dimensional array
of cations and anions made of formula units: NaCl, MgO
• Na+ Cl- Na+ Cl- Na+ Cl- • Cl- Na+ Cl- Na+ Cl- Na+
• Na+ Cl- Na+ Cl- Na+ Cl-
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Binary Molecular Compounds:Two Nonmetals (such as CO2)
1. Name first element in formula first use the full name of the element
2. Name the second element in the formula with an -ide as if it were an anion, however, remember these
compounds do not contain ions!
3. Use a prefix in front of each name to indicate the number of atoms
a) Never use the prefix mono- on the first element
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Subscript - Prefixes
• 1 = mono-; not used on first
nonmetal
• 2 = di-
• 3 = tri-
• 4 = tetra-
• 5 = penta-• 6 = hexa-• 7 = hepta-• 8 = octa-• drop last “a” if
name begins with vowel
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Exceptions when Naming Molecular Compounds
of course, water
Other common exceptions:• NH3: ammonia (as in Windex)• H2S: hydrogen sulfide• HCl: hydrogen chloride (same for HX, where X =
halogen)• CH4: methane (as in natural gas)
• H2O2: hydrogen peroxide
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Example – Naming Binary Molecular
BF3
1. Is it one of the common exceptions?H2O, NH3, CH4, C12H22O11 = No!
2. Identify Major ClassB = is a nonmetal because it is on the right side of the PT
F = is a nonmetal because it is on the right side of the PT
Molecular
3. Identify the Subclass2 elements Binary Molecular
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Example – Naming Binary Molecular BF3
4. Name the first element boron5. Name the second element with an –ide
fluorine fluoride6. Add a prefix to each name to indicate the subscript
monoboron, trifluoride7. Write the first element with prefix, then the second
element with prefix Drop prefix mono from first element
boron trifluoride
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Practice:
Naming Molecular Compounds
• CO
• ClO3
• SO2
• P2O5
• N2O4
• IF7
• SF6
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• CO carbon monoxide
• ClO3 chlorine trioxide
• SO2 sulfur dioxide
• P2O5 diphosphorus pentoxide
• N2O4 dinitrogen tetroxide
• IF7 iodine heptoxide
• SF6 sulfur hexafluoride
Key to Naming Molecular Compounds
• CO
• ClO3
• SO2
• P2O5
• N2O4
• IF7
• SF6
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Ionic Compounds
• Made of Cation (+) and Anion (-)• Name: Cation Anion
example: NaCl Sodium ChlorideCation:
Type I metalType II metal Polyatomic ion: ammonium NH4
+
Anion:Nonmetal: Chloride Cl-, Oxide O2-
Polyatomic ion: SO42- , OH- , NO3
-
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Metal Cations: Type IType I (Groups IA, IIA, AZA)
only have one possible chargeGroups IA, IIA, Ag+, Zn2+, Al3+
Charge by position on the Periodic TableIA = +1, IIA = +2, Ag+ (IB), Zn2+(IIB) Al3+(IIIA)
How do you know a metal cation is Type II?
its not Type I !!!
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Metal Cations: Type IIType II: Metal ions that are
other than Type I
Common Examples: Fe2+/3+, Cu+/2+, Cr3+/6+, Mn2+/4+, Mn2+/4+, Pb2+/4+, Sn2+/4+, etc ) have more than one possible
chargedetermine charge by charge on
anion
How do you know a metal cation is Type II?
its not Type I !!!
Metal Cations: Type I vs. Type II
AgZn
Al
= Type II Metal
= Type I Metal
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Monatomic Nonmetal Anion (An-)
• How much is the charge? the position on the Periodic Table
• Name of the anion: change ending on the element name to –ide
4A = -4 5A = -3 6A = -2 7A = -1
C4- = carbide N3- = nitride O2- = oxide F- = fluoride
Si4- = silicide P3- = phosphide S2- = sulfide Cl- = chloride
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Net charge of Ionic Compound = 0
• Net charge = Positive charge from cation(s) + Negative charge from Anion(s) = 0
• Example: Compound Al2(SO4)3, the Net
charge = 2 x (+3) + 3 x (-2) = +6 - 6 = 0
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Name of Ionic Compounds
• Name: Cation Anion: Sodium ChlorideCation:
Type I metal = metal name : Na+ => Sodium, Mg2+ => Magnesium
Type II metal = metal name(charge): Fe3+ Iron(III), Cu2+ Copper(II)
Polyatomic ion = name of polyatomic ion, NH4+ => Ammonium
Anion:Nonmetal = stem of nonmetal name + ide, Chloride, OxidePolyatomic ion = name of polyatomic ion, SO4
2- => Sulfate, OH- => Hydroxide, NO3
- => Nitrate
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Type I Binary Ionic CompoundsBinary: only two kinds of ions in one UNIT
Example: MgO, CaCl2
• Metal listed first in formula & name
1. Metal Cation Nonmetal Anion2. Cation name <= Metal name: Magnesium,
Calcium3. Nonmetal anion <= Nonmetal name ends with
–ide: Oxide, Chloride
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Example – Naming Binary Ionic, Type I Metal CsF
1. Is it one of the common exceptions?
H2O, NH3, CH4, C12H22O11 No!
2. Identify Major ClassCs = is a metal because it is on the left side of the PT
F = is a nonmetal because it is on the right side of the PT
Ionic
3. Identify the Subclass2 elements, Binary Ionic
4. Is the metal Type I or Type IICs is in Group IA, Type I
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Example – Naming Binary Ionic, Type I Metal
CsF5. Identify cation and anion
Cs = Cs+ because it is Group 1F = F- because it is Group 7
6. Name the cationCs+ = cesium
7. Name the anionF- = fluoride
8. Full name: Cation name first, Anion name lastcesium fluoride
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Type II Binary Ionic Compounds
Metal listed first in formula & name
1. Metal cation Nonmetal anion2. metal cation Metal(Roman Numeral): to indicate
its charge. Iron(II), Copper(I) determine charge from anion charge Common Type II cations in Table 5.5
3. Nonmetal anion Nonmetal name ended with –ide: Chloride, Oxide
Example: Iron(II) chloride, Copper(I) oxide
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How to find the charge on Type II metal ions?
• Example: Name Compound Fe2(SO4)3
Since the sum of all charges equals zero, the charge on iron ions are unknown and sulfate each has –2 charge, then we have
2 x Fe + 3 x (-2) = 0
Fe = +3, each iron ion has a charge of +3
Name: iron(III) sulfate
Key: knowing the charge on ANIONs!
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Example – Naming Binary Ionic, Type II Metal
CuCl1. Is it one of the common exceptions?
H2O, NH3, CH4, C12H22O11 = No!2. Identify Major Class
Cu = is a metal because it is on the left side of the PTCl = is a nonmetal because it is on the right side of the PT
Ionic
3. Identify the Subclass2 elements, Binary Ionic
4. Is the metal Type I or Type IICu is not in Group IA, IIA, or (Al, Ga, In) Type II
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Example – Naming Binary Ionic, Type II Metal CuCl
5. Identify cation and anionCl = Cl- because it is Group 7
Cu = Cu+ to balance the charge
6. Name the cationCu+ = copper(I)
7. Name the anionCl- = chloride
8. Write the cation name first, then the anion namecopper(I) chloride
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Practice: Naming Ionic compounds
• HgF2
• CuI2
• CaCl2
• Fe2O3
• SnCl4
• Mg3N2
• Ag2S
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Naming Ionic compounds Hints: find type II ion charge from anion
• HgF2 : Two F- = -2
• CuI2 : Two I- = -2
• CaCl2 : both fixed charges
• Fe2O3 : Three O2- = -6
• SnBr4 : Four Br- = -4
• Mg3N2 : both fixed charges
• Ag2S : both fixed charges
• HgF2 : Two F- = -2 Hg = +2
• CuI2 : Two I- = -2 Cu = +2
• CaCl2 : both fixed charges
• Fe2O3 : Three O2- = -6 Fe = +3
• SnBr4 : Four Br- = -4 Sn = +4
• Mg3N2 : both fixed charges
• Ag2S : both fixed charges
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Answer key: names of ionic compounds
• HgF2 = Mercury(II) fluoride
• CuI2 = copper(II) iodide
• CaCl2 = calcium chloride
• Fe2O3 = Iron(III) oxide
• SnBr4 = tin(IV) bromide
• Mg3N2 = magnesium nitride
• Ag2S = silver sulfide
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Polyatomic Ions
Mg(NO3)2
compound calledmagnesium nitrate
symbol of the polyatomic ion called nitrate
symbol of the polyatomic ion called sulfate
CaSO4
compound calledcalcium sulfate
implied “1” subscripton magnesium
implied “1” subscripton calcium
parentheses to group two NO3’s no parentheses for one SO4
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Polyatomic Ions:Nitrate NO3
-, Sulfate SO42-
Mg(NO3)2
compound calledmagnesium nitrate
CaSO4
compound calledcalcium sulfate
subscript indicatingtwo NO3 groups
no subscript indicatingone SO4 group
implied “1” subscripton nitrogen, total 2 N
implied “1” subscripton sulfur, total 1 S
stated “3” subscripton oxygen, total 6 O
stated “4” subscripton oxygen, total 4 O
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Polyatomic Anions: -ATE ions
CO32-
carbonate
NO3-
nitrate
SiO32-
silicate
PO43-
phosphate
SO42-
sulfate
ClO3-
chlorate
AsO43-
arsenate
SeO42-
selenate
BrO3-
bromate
IO3-
iodate
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Periodic Pattern of Polyatomic Ions-ate groups
BO33- NO3
-
SiO32-
PO43-
SO42-
ClO3-
AsO43-
SeO42-
BrO3-
TeO42-
IO3-
CO32-
IIIA IVA VA VIA VIIA
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Patterns for Polyatomic Ions
1. elements in the same Group form similar polyatomic ions
same number of O’s and same charge
ClO3- = chlorate (-1 charge)
BrO3- = bromate (-1 charge)
2. if the polyatomic ion starts with H, the name adds hydrogen- prefix before name and add 1 to the charge
CO32- = carbonate HCO3
-1 = hydrogen carbonate
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Patterns for Polyatomic Ions-ate ion
chlorate = ClO3-
• -ate ion + 1 O same charge, per- prefixperchlorate = ClO4
-
• -ate ion – 1 O same charge, -ite suffixchlorite = ClO2
-
• -ate ion – 2 O same charge, hypo- prefix, -ite suffixhypochlorite = ClO-
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Polyatomic Anions: -ite, hypo- -ite, (-ate), per- -ate
ClO-
hypochlorite
NO2-
nitrite
PO33-
phosphite
SO32-
sulfite
ClO2-
chlorite
NO3-
nitrate
PO43-
phosphate
SO42-
sulfate
ClO3-
chlorate
ClO4-
perchlorate
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-ATE/-ITE ions in Our Lives
ClO-
(bleach)
NO2-
(preserve meat)
PO33-
(plant medicine)
SO32-
(wine, oxygen buster)
ClO2-
(bleach, disinfect)
NO3-
(fertilizer, explosives)
PO43-
(bone/teeth, fertilizer, soda)
SO42-
(plaster, car battery, sea salt)
ClO3-
(older pyrotechnics)
ClO4-
(pyrotechnics, solid fuel rocket)
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Polyatomic Ions to RememberNameName FormulaFormula
acetate C2H3O2–
carbonate CO32–
hydrogen carbonate(aka Bicarbonate)
HCO3–
hydroxide OH–
nitrate NO3–
nitrite NO2–
permanganate MnO4–
chromate CrO42–
dichromate Cr2O72–
ammonium NH4+
NameName FormulaFormula
hypochlorite ClO–
chlorite ClO2–
chlorate ClO3–
perchlorate ClO4–
sulfate SO42–
Hydrogen sulfate(aka Bisulfate)
HSO4–
sulfite SO32–
Hydrogen sulfite(aka Bisulfite)
HSO3–
cyanide CN–
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Other Polyatomic Ions in Our Lives
C2H3O2– In vinegar as acetic acid
CO32– Soda drink
HCO3– Baking soda, baking power, acid spill
neutralizer
OH– In liquid plumber/Drano as NaOH
MnO4– Disinfectant, “aging” for movie making
CrO42– Chrome plating (faucet, etc.)
CN– Highly Poisonous; Plant seeds; blue pigment
NH4+ Fertilizer; metabolic waste from animals
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Other Polyatomic Ions in Our Lives
ClO-
(bleach)
NO2-
(preserve meat)
PO33-
(plant medicine)
SO32-
(wine, oxygen buster)
ClO2-
(bleach, disinfect)
NO3-
(fertilizer, explosives)
PO43-
(bone/teeth, fertilizer, soda)
SO42-
(plaster, car battery, sea salt)
ClO3-
(older pyrotechnics)
ClO4-
(pyrotechnics, solid fuel rocket)
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Compounds Containing Polyatomic Ions
• Type I metal + Polyatomic ion: NaNO3
• Type II metal(charge) + Polyatomic ion : CuSO4
• Polyatomic cation + Nonmetal ion (-ide): NH4Cl
• Polyatomic cation + Polyatomic ion: (NH4)2SO4
Important!:Important!: If, and only if, more than ONE polyatomic ions are present in a formula, use parenthesis and subscript to indicate the number of polyatomic ions
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Example – Naming Ionic with Polyatomic Ion
Na2SO41. Is it one of the common exceptions?
H2O, NH3, CH4, C12H22O11 = No!
2. Identify Major ClassNa = is a metal because it is on the left side of the PT
SO4 = is a polyatomic ion
Ionic
3. Identify the Subclasscompound has 3 elements Ionic with Polyatomic Ion
4. Is the metal Type I or Type IINa is in Group IA, Type I
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5. Identify the ionsNa = Na+ because in Group 1
SO4 = SO42- a polyatomic ion
6. Name the cationNa+ = sodium (Type I)
7. Name the anionSO4
2- = sulfate
8. Write the name of the cation followed by the name of the anion
sodium sulfate
Example – Naming Ionic with Polyatomic Ion
Na2SO4
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Example – Naming Ionic with Polyatomic Ion Fe(NO3)3
1. Is it one of the common exceptions?
H2O, NH3, CH4, C12H22O11 = No!
2. Identify Major ClassFe = is a metal because it is on the left side of the PT
NO3 = is a polyatomic ion because it is in ( )
Ionic
3. Identify the Subclassthere are 3 elements Ionic with Polyatomic Ion
4. Is the metal Type I or Type IIFe is not in Group IA, IIA, or (Al, Ga, In) Type II
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Example – Naming Ionic with Polyatomic Ion Fe(NO3)3
5. Identify the ionsNO3 = NO3
- a polyatomic ion
Fe = Fe+3 to balance the charge of the 3 NO3-1
6. Name the cationFe+3 = iron(III) (Type II)
7. Name the anionNO3
- = nitrate
8. Write the name of the cation followed by the name of the anion
iron(III) nitrate
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Practice: Naming Ionic compounds
• Hg2SO4
• CuClO3
• Zn(NO3)2
• FeCO3
• Sn(SO3)2
• CoPO4
• Al(ClO4)3
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Hints: Naming Ionic compounds
• Hg2SO4 : charge of sulfate = -1
• CuClO3 : charge of chlorate = -1
• Zn(NO3)2 charge of nitrate = -1
• FeCO3 : charge of carbonate = -2
• Sn(SO3)2: charge of sulfite = -1
• CoPO4 : charge of phosphate = -3
• Al(ClO4)3 : charge of perchlorate = -1
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Keys: Naming Ionic compounds
• Hg2SO4 : mercury(I) sulfate
• CuClO3 : copper(I) chlorate
• Zn(NO3)2 zinc nitrate
• FeCO3 : iron(II) carbonate
• Sn(SO3)2: tin(IV) sulfite
• CoPO4 : cobalt(III) phophate
• Al(ClO4)3 : aluminum perchlorate
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Acids• Contain H+ cation and
anion• Hydrogen (H) as first
element in formula
• Binary acids (HnX) have H+ cation and nonmetal anion
• Oxyacids (HnXOm) have H+ cation and polyatomic anion
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Naming AcidsAll names have acid at end• Binary Acids (HnX) = hydro prefix + stem of the
name of the nonmetal + ic suffixExample: HCl (Hydrochloric acid)
• Oxyacids (HnXOm : H2CO3 , H2SO4) if polyatomic ion ends in –ate = name of polyatomic ion
with –ic suffix :
H2SO4 (Sulfuric acid); H2CO3 (Carbonic acid);
HNO3 (Nitric acid); H3PO4 (Phosphoric acid)
if polyatomic ion ends in –ite = name of polyatomic ion with –ous suffix
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Naming Binary Acids – HF
1. First of all, it is binary acid HX
2. Identify the anionF F-, fluoride because Group 7A
2. Name the anion with an –ic suffixF- = fluoride fluoric
3. Add a hydro- prefix to the anion namehydrofluoric
4. Add the word acid to the endhydrofluoric acid
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Naming Oxyacids: H2SO4
1. Identify the anionSO4 = SO4
2- = sulfate
2. If the anion has –ate suffix, change it to –ic. If the anion has –ite suffix, change it to -ous
SO42- = sulfate sulfuric
3. Write the name of the anion followed by the word acidsulfuric acid
(kind of an exception, to make it sound nicer!)
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Practice: Naming Acidsfirst: what is the anion?
• HNO3
• HClO3
• HBr
• H2CO3
• H2SO3
• H3PO4
• HClO4
Practice: Naming Acids
• HNO3 nitrate
• HClO3 chlorate
• HBr bromide
• H2CO3 carbonate
• H2SO3 sulfite
• H3PO4 phosphate
• HClO4 perchlorate
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Practice: Naming Acids
• HNO3 nitrate nitric acid
• HClO3 chlorate chloric acid
• HBr bromide hydrobromic acid
• H2CO3 carbonate carbonic acid
• H2SO3 sulfite sulfurous acid
• H3PO4 phosphate phosphoric acid
• HClO4 perchlorate perchloric acid
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Formula-to-Name Flow Chart
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Review: Naming Compounds
• CuSO3
• AgClO
• N2O5
• H2S
• FeI2
• Sn(NO3)4
• Ba3(PO4)2
• (NH4)2S
1. Common exceptions? H2O, NH3, CH4, C12H22O11
2. Identify as Molecular or Ionic?
3. Identify • Binary molecular
• Type I or II metal ion
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Review: Naming Compounds
• CuSO3 copper(II) sulfite• AgClO silver hypochlorite• N2O5 dinitrogen pentoxide• H2S hydrosulfuric acid• FeI2 iron(II) iodide• Sn(NO3)4 tin(IV) nitrate• Ba3(PO4)2 barium phosphate • (NH4)2S ammonium sulfide
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Write Chemical Formula using the charge of known ions
• Example: Compound between Ca2+ and PO4
3- , the number of ions of each needs to
be 3 and 2, so that the combined charge
= 3 x (+2) + 2 x (-3) = 0
Therefore the formula for the compound is Ca3(PO4)2
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Write Chemical Formula using the charge of known ions
“Criss-Cross-Simplify”:• The charge of an ion turns into the subscript (the
number) of the counterpart ion
Pb4+ O2- Pb2O4
• Since the subscripts in an ionic compound represents the RATIO among the ions, the subscripts need to be simplified when there is common denominator
Pb2O4 PbO2
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Practice: Writing formulas (I)
• copper(II) chloride• aluminum oxide• magnesium phosphide• iron(II) bromide• lead(II) sulfide• zinc iodide • sodium nitride
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Hints for Writing formulas (I): Charges on Cations and Anions
• copper(II) chloride: Cu2+ and Cl-
• aluminum oxide: Al3+ and O2-
• magnesium phosphide : Mg2+ and P3-
• iron(II) bromide : Fe2+ and Br-
• lead(II) sulfide : Pb2+ and S2-
• zinc iodide : Zn2+ and I-
• sodium nitride : Na+ and N3-
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Key for Writing formulas (I): use criss-cross-reduce
• copper(II) chloride CuCl2
• aluminum oxide Al2O3
• magnesium phosphide Mg3P2
• iron(II) bromide FeBr2
• lead(II) sulfide FeS• zinc iodide ZnI2
• sodium nitride Na3N
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Practice: Write Chemical Formulae
• Chromium(II) Chloride • Cesium phosphate• Lead(II) oxide• Zinc nitrate• Iron(III) sulfite• Strontium nitride• Ammonium carbonate
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Key: Write Chemical Formulae
• Chromium(II) Chloride • Cesium phosphate• Lead(II) oxide• Zinc nitrate• Iron(III) sulfite• Strontium nitride• Ammonium carbonate
CrCl2
Cs3PO4
PbO
Zn(NO3)2
Fe3(SO3)2
Sr3N2
(NH4)2CO3
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Practice: Writing formulas (I)
• copper(I) sulfate• aluminum chlorate• magnesium phosphate• iron(II) carbonate• lead(II) acetate• zinc sulfite • sodium nitrite• Nitrogen gas
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Hints for Writing formulas (I): Charges on Anions
• copper(I) sulfate: -2 for sulfate • aluminum chlorate: -1 for chlorate• magnesium phosphate: -3 for phosphate• iron(II) carbonate : -2 for carbonate• lead(II) acetate: -1 for acetate• zinc sulfite : -2 for sulfite• sodium nitrite: -1 for nitrite • Nitrogen gas: atomic or molecular element?
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Key: Writing formulas (I)
• copper(I) sulfate: Cu2SO4
• aluminum chlorate: Al(ClO3)3
• magnesium phosphate: Mg3(PO4)2
• iron(II) carbonate : FeCO3
• lead(II) acetate: Pb(C2H3O2)2
• zinc sulfite : ZnSO3
• sodium nitrite: NaNO2
• Nitrogen gas: N2
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More on Writing formulae
• copper(II) sulfate• aluminum perchlorate• hydroiodic acid• iron(III) bromide• Diphosphorus pentoxide• lead(IV) nitride• zinc carbonate • helium gas
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Key: Writing formulae
• copper(II) sulfate CuSO4
• aluminum perchlorate Al(ClO4)3
• hydroiodic acid HI• iron(III) bromide FeBr3
• Diphosphorus pentoxide P2O5
• lead(IV) nitride Pb3N4
• zinc carbonate ZnCO3
• ammonium nitrite NH4NO2
• helium gas He