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January 10 1 Chemical Nomenclature
Please go to the Chemical Digital Library at: http://chempaths.chemeddl.org/services/chempaths/?q=book/2739/making-chemical-nomenclature-matter
January 10 2 Chemical Nomenclature
Matter can be classified to mixtures and pure substances. Compounds falls under the category of pure substances
January 10 3 Chemical Nomenclature
Compounds can be broken up in a manner in which electrons from atoms interact with each other.
If the electrons are mutually shared, these compounds are called Covalent Compounds.
If the electrons are transferred, these
compounds are called ionic compounds.
MoleculesCovalent
IonicCompounds
Polar-Covalent
PurePureSubstancesSubstances
Compounds
•Sharing electrons•non-metals
•transfer electrons•metal + nonmetal
•unequal sharing electrons•metals or non-metals
If the electrons are unequally shared, then these are called polar covalent compounds.
January 10 4 Chemical Nomenclature
Octet Rule: Atoms will transfer or share electrons in order to have the same number of electrons as its closest noble gas.
Covalent compounds are formed by atoms sharing as many electrons needed to obey the Octet Rule
January 10 7 Chemical Nomenclature
Chemical formula - Principle of electrical neutrality is applied in order to predict formulas of ionic compound.
KF F F - K + K
Example 1: Potassium and Fluorine
Potassium and fluorine combine in a 1:1 ratio because potassium (K) is positive one (+1) and fluorine (F) is negative one (-1). Only in a 1:1 combination will the charges cancel each other.
January 10 8 Chemical Nomenclature
When elements combine to form compounds, the principle of electrical neutrality allows prediction of formulas of the ionic compound.
Basic idea:
Sum of the charges must add to zero. That is the sum of the cation charge and the sum of the anion charge must
cancel each other so that the compound form is neutral.
January 10 9 Chemical Nomenclature
Barium and nitrogen combine in a 3 : 2 ratio because barium (B) is positive three (+2) and nitrogen (N) is negative three (-3). Only in a 3:2 combination will the charges cancel each other.
Example 1: Barium and nitrogen
Ba 3 N 2 N 3- Ba 2+
N N 3- Ba 2+ Ba
1. Write the symbols for the cation and the anion. 2.. Use a superscript for the charge (+/-) of each ion. 3. Criss-cross step:
• Criss-cross the superscript of the cation to the subscript position of the anion (disregard the positive sign).
• Criss-cross the superscript of the anion to the subscript position of the cation (disregard the negative sign).
4. Remove the superscript from both cation and anion. 5. If possible, divide the subscripts by their greatest common factor to
reduce to simplest whole ratio.
January 10 10 Chemical Nomenclature
January 10 13 Chemical Nomenclature
Oxy-anions Oxy-acids Add H+
Add H+
Add H+
Add H+
Remember the -ate ion and start nomenclature from there.
Per- -ate
-ate
-ite
hypo- -ite
+[O]
-[O]
-[O]
per- -ic acid
-”ic” acid
“-ous” acid
hypo- -ous acid
-[O]
-[O]
-[O]
January 10 14 Chemical Nomenclature
Oxy-anions Oxy-acids
Per -ate Per -ic acid
-ate
-ite
Hypo -ite
-ic acid
-ous acid
hypo -ous acid
Add H+
Add H+
Add H+
Add H+
Minus [O]
minus [O]
Add [O]
January 10 19 Chemical Nomenclature
Type I or Type II
Is the metal Group I, II or Al, Zn, Cd, Ag, and
Type III
Type I
metal-nonmetal
metal(Ox.#)-nonmetal
Type II
(Prefix)nonmetal1 (Prefix)nonmetal2
NH4 +
January 10 20 Chemical Nomenclature
Type Anion elemental Anion polyatomic
I (Metal – nonMetal)
Cation; Rep Metal Cation - Anion
Cation - Anion(ide)
Al2O3; Aluminum oxide Ag2S; Silver sulfide
Cation - Anion
Cd(NO3)2: cadmium nitrate (NH3)2SO4: ammonium sulfate
II (Metal - nonMetal)
(Transition) metal Cation (O St #) - Anion
Cation ; 3rd row and lower
Old method (Fe+3 vs Fe+2) higher ox.st. -ic lower ox. st. -ous
Cation (oxidation st.) Anion(ide)
FeCl3; Iron(III) chloride PbS2; Lead(IV) sulfide
Cation(ic) - Anion(ide) FeBr3 ; Ferrric bromide Iron(III) bromide Cation(ous) – Anion(ide) Fe3N2 ; Ferrrous nitride Iron(II) nitride
Cation (oxidation st.) Anion
Sn(C2H3O2)2; Tin(II) acetate Au3PO3; Gold(I) phosphite
Cation(ic) – Polyatomic anion Fe(NO3)3 ; Ferrtic nitrate Iron(III) nitrate Cation(ous) – Polyatomic anion Fe(NO2)2 ; Ferrrous nitrite Iron(II) nitrite
III Molecular compounds -
Compounds contains nonmetal
(Prefix) nonmetal1 - (Prefix ) nonmetal2
January 10 21 Chemical Nomenclature
aluminum sulfate Palladium (II) chromate tungsten(IV) hypochlorite ammonium bisulfate Tetraphosphorus octaoxide cobalt(III) phosphide calcium phosphate cesium acetate xenon dioxide silver permanganate platinum (IV) periodate magnesium phosphite chlorine monobromide Mercury(I) telluride Cadmium biphosphate
1 Mg(ClO3)2 2 CuBr2
A HClO 1 KMnO4
3 N2O4 1 Na2O2
1 NH4NO2 3 XeF4
1 Na3As 2 HgCO3
A HI A H2SO4
1 NaHCO3 1 NH4ClO4
1 Zn(C2H3O2)2 1 Li2Se
2 V3N 1 CdCO3
2 PbTe2 3 H2O2
1 NaHSO3 1 (NH4)2S
A HC2H3O2 1 FrF
3 SO3 2 NiO2
January 10 22 Chemical Nomenclature
1 Mg(ClO3)2 2 CuBr2
A HClO 1 KMnO4
3 N2O4 1 Na2O2
1 NH4NO2 3 XeF4
1 Na3As 2 HgCO3
A HI A H2SO4
1 NaHCO3 1 NH4ClO4
1 Zn(C2H3O2)2 1 Li2Se
2 V3N 1 CdCO3
2 PbTe2 3 H2O2
1 NaHSO3 1 (NH4)2S
A HC2H3O2 1 FrF
3 SO3 2 NiO2
1 aluminum sulfate 2 palladium (II) chromate 2 tungsten(IV) hypochlorite 1 ammonium bisulfate 3 tetraphosphorus octaoxide 2 cobalt(III) phosphide 1 calcium phosphate 1 cesium acetate 3 xenon dioxide 1 silver permanganate 2 platinum (IV) periodate 2 manganese(IV) phosphite 3 chlorine monobromide 2 mercury(I) telluride 1 cadmium biphosphate
13 Type I, 5 type II, 4 type III 4 Acids = 26 6 Type I, 5 type II, 4 type III