matter can be classified to mixtures and pure...

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


Matter can be classified to mixtures and pure substances. Compounds falls under the category of pure substances


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.


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


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.


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.


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.



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]


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]


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 +


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


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


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

matter can be classified to mixtures and pure...

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