Nomenclature i.e. Naming chemical compounds. Binary compounds Compounds consisting of a metal and a nonmetal Compounds consisting of two nonmetals.

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