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Nomenclature
i.e.
Naming chemical compounds
Binary compounds
• Compounds consisting of a metal and a nonmetal
• Compounds consisting of two nonmetals
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+
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
Naming Type I• MgCl2• Na2O
• Ag2O
• Al2O3
• ZnI2
• Ca3P2
• Magnesium chloride• Sodium oxide• Silver oxide• Aluminum oxide• Zinc iodide• Calcium phosphide
Type II Metals
• Most transition and heavy metals
• Have multiple oxidation numbers
• Oxidation numbers found mathematically or given
Determining Type II Oxidation Numbers
• Anion oxidation Known
• Find Cation by working from Anion and subscripts
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
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
Naming Type II cont.
• Example
• Fe2O3
– Fe = Iron– O = oxide– O2- , 6- total / 2 = Fe3+
– Name - Iron (III) oxide
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
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)
Type III Prefixes• Mono - 1• Di - 2• Tri - 3• Tetra - 4• Penta - 5
• Hexa - 6• Hepta - 7• Octa - 8• Nona - 9• Deca - 10
example
• NO3
• Nitrogen - 1- mono-• Oxygen - 3- tri-• Do Not use Mono-• Nitrogen trioxide
• N2O
• Nitrogen 2- di• Oxygen 1- mono• Dinitrogen monoxide
Type III Practice
• CO2
• CO
• SO3
• P2O5
• SF2
• SF6
• Carbon dioxide• Carbon monoxide• Sulfur trioxide• Diphosphorus
pentaoxide• Sulfur difloride• Sulfur hexafloride
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
Ternary Compound NamingType of Cation ?
Type ICation polyatomic ion
Type IICation (Roman Numeral) polyatomic ion
example
• Na2(CO3)
• Na1+ - sodium
• (CO3)2- - carbonate
• Sodium carbonate
• Fe2(SO4)3
• Fe3+ = Iron (III)
• (SO4)2- = sulfate
• Iron (III) sulfate
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
Did you ever Wonder Where Pumpkin Pies Come From?
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
example• HCl• No oxygen• Hydro-• Chlorine - -chloric• Hydrochloric acid
• H2SO4
• Contains oxygen
• SO4 - sulfate
• -ic replaces -ate• Sulfuric acid
Practice• HBr• HClO
• HNO3
• H2SO3
• HC2H3O2
• HF
• Hydrobromic acid• Hypochlorous acid• Nitric acid• Sulfurous acid• Acetic acid• Hydrofloric acid
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
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%
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
Percent to Formula
• Convert percents to grams
• Find Moles of Each Element
• Mole to Mole ratio
• Reduce to Smallest Whole Number ratio
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