Nomenclature i.e. Naming chemical compounds. Binary compounds Compounds consisting of a metal and a...
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Nomenclature
i.e.
Naming chemical compounds
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Binary compounds
• Compounds consisting of a metal and a nonmetal
• Compounds consisting of two nonmetals
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Type I Metals
• Group 1, 2, 3, & 4– Group 1, 1+ oxidation number– Group 2 , 2+ oxidation number– Group 3, 3+ oxidation number– Group 4, 4+ oxidation number
• Ge 4+,Al3+, Ga3+, In3+,Zn2+,Cd2+, Ag1+,Ta5+,Tc7+
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Binary compounds Metal & Nonmetal
• Identify the cation– Type I metal
• Single oxidation number
– Type II metal• Various oxidation numbers
• Write the cation’s name first, unchanged• Identify the anion
– nonmetal
• The anion is named by keeping the root and adding the ending -ide
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Naming Type I• MgCl2• Na2O
• Ag2O
• Al2O3
• ZnI2
• Ca3P2
• Magnesium chloride• Sodium oxide• Silver oxide• Aluminum oxide• Zinc iodide• Calcium phosphide
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Type II Metals
• Most transition and heavy metals
• Have multiple oxidation numbers
• Oxidation numbers found mathematically or given
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Determining Type II Oxidation Numbers
• Anion oxidation Known
• Find Cation by working from Anion and subscripts
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Example
• Fe2O3
• O2-
• 3 oxygen 6- total• 2 Fe • 62 = 3• so Fe3+ oxidation
state
• MnO3
• 3 (2-) = 6-• 61 = 6 +
• So Mn6+ oxidation state
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Naming Type II• Identify the cation• Identify the anion• Determine the total charge of the anion• Calculate the oxidation number of the
cation• Cation ( roman numeral) anion-ide
– Roman numeral is the oxidation number of the cation
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Naming Type II cont.
• Example
• Fe2O3
– Fe = Iron– O = oxide– O2- , 6- total / 2 = Fe3+
– Name - Iron (III) oxide
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Type II Practice• Cu2O• NiN• CoCl2• Mn2S5
• CrP2
• Cr2Se3
• VI5
• Copper (I) oxide• Nickel (III) nitride• Cobalt (II) chloride• Manganese (V)
sulphide• Chromium (VI)
phosphide• Chromium (III) selenide• Vanadium (V) iodide
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Rules for Type III• Identify the first element• Identify the second element• Determine the prefix for the first and second
element based on the number of each in the compound (DO NOT Use the prefix mono- for the first element)
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Type III Prefixes• Mono - 1• Di - 2• Tri - 3• Tetra - 4• Penta - 5
• Hexa - 6• Hepta - 7• Octa - 8• Nona - 9• Deca - 10
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example
• NO3
• Nitrogen - 1- mono-• Oxygen - 3- tri-• Do Not use Mono-• Nitrogen trioxide
• N2O
• Nitrogen 2- di• Oxygen 1- mono• Dinitrogen monoxide
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Type III Practice
• CO2
• CO
• SO3
• P2O5
• SF2
• SF6
• Carbon dioxide• Carbon monoxide• Sulfur trioxide• Diphosphorus
pentaoxide• Sulfur difloride• Sulfur hexafloride
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Binary Compound Flow Chart
Type of Cation?
Type I
Cation Anion-ide
Type III
Prefix cation
Prefix anion-ide
Type IICation (roman numeral) anion - ide
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Ternary Compound NamingType of Cation ?
Type ICation polyatomic ion
Type IICation (Roman Numeral) polyatomic ion
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example
• Na2(CO3)
• Na1+ - sodium
• (CO3)2- - carbonate
• Sodium carbonate
• Fe2(SO4)3
• Fe3+ = Iron (III)
• (SO4)2- = sulfate
• Iron (III) sulfate
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PRACTICE
• CsClO4
• KMnO4
• Co(ClO4)2
• Zn(ClO3)2
• Cu(NO3)2
• (NH4)(ClO2)
• Cesium perchlorate• Potassium
permanganate• Cobalt (II)
perchlorate• Zinc chlorate• Copper (II) nitrate• Ammonium chlorite
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Did you ever Wonder Where Pumpkin Pies Come From?
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Naming AcidsDoes the anion contain oxygen?
NoHydro + root-icHydro(anionroot-ic) acid
Yes
Anion ends in -ateReplace with -icAnion-ic acid
Anion ends in -iteReplace with -ousAnion-ous acid
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example• HCl• No oxygen• Hydro-• Chlorine - -chloric• Hydrochloric acid
• H2SO4
• Contains oxygen
• SO4 - sulfate
• -ic replaces -ate• Sulfuric acid
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Practice• HBr• HClO
• HNO3
• H2SO3
• HC2H3O2
• HF
• Hydrobromic acid• Hypochlorous acid• Nitric acid• Sulfurous acid• Acetic acid• Hydrofloric acid
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PERCENT COMPOSITION
• Calculate the Molar mass of the Compound
• Divide the total mass of each element of the compound by the Molar mass of the compound
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Example of formula to percent
• BaCl2• MW = 207 g/mol• % Ba = 137/207
– 66.2%
• % Cl = 70 /207– 33.8%
Fe3(PO4)2
MW = 358 g/mol% Fe = 168/358
46.9%% P = 62/358
17.3%% O = 128/358
35.8%
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Practice
• CaCl2• FeO
• P2O5
• H2SO4
• NaHCO3
• 36.4% Ca, 63.6% Cl• 77.7%Fe, 22.2% O• 43.7% P, 56.3% O• 2.0%H,
32.7%S,65.3%O• 27.3%Na,1.2%H,
14.3%C, 57.1%O
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Percent to Formula
• Convert percents to grams
• Find Moles of Each Element
• Mole to Mole ratio
• Reduce to Smallest Whole Number ratio
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Example• 18.7% Zr, 28.6% Cl, 52.7% O• 18.7% = 18.7 g 18.7/91 =0.205 mol Zr• 28.6% = 28.6 g 28.6/35 = 0.817 mol Cl• 52.7% = 52.7g 52.7/16 = 3.29 mol O• Ratio 0.205 : 0.817 : 3.29• Divide by Smallest value• 1 : 4:16 • Zr(ClO4)4
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