Stable Ion Charges Metals Form Cagons. Nonmetals Form Anions

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Ions Ions • Anions: Atoms can gain one or more • electrons to form negaGve ions called anions. Metal elements tend to lose electrons and Chemical Nomenclature form caGons (posiGve ions).

• Nonmetal elements tend to gain electrons and Naming Compounds – – Cl + e à Cl form anions (negaGve ions). I. Ionic Compounds General Rule: Name the cation first, anion second.

*If cation can have variable charges, remember to specify charge in (Roman numerals)

after the name of cation. *!-r{!..+ *{fl A. Binary Ionic Compounds: METAL + NONMETAL 1. Cation (Metal)

a) Monatomic metal cations with fixed charge (mostly main group metals) have same

suol suol 'sa1nra1o141'sruolv € pu Z Z UIIICIVHf, name as the element. 99 • Anions are named by using the root of the parent + 2+ Eg. Na = sodium ion Ca = calcium ion- atom followed by the suﬃx -ide: Cl chloride ion; Br- bromide ion; Ob) Monatomic metal cations with variable charges 2- oxide ion; S2- sulﬁde ion (mostly transition metals) have name of element followed by a Roman numeral in parentheses to indicate charge.Ex Probs: wriGng symbols Eg. Cu+ = copper (I) Cu2+ = copper (II)

2. Anion (Nonmetal) Monatomic anions have name of element followed by –ide.

F– = fluoride O2– = oxide

sleleru sleleru Cl– = chloride S2– = sulfide uoqrsuEJl Br– = bromide N3– = nitride I – = iodide H– = hydride

Examples of Binary Ionic Compounds KCl potassium chloride CuBr copper (I) bromide MgBr2 magnesium bromide PbO2 lead (IV) oxide

*Memorize the following Common Ion Charges!Stable Ion Charges Ionic Compounds • Most commonly, ionic compunds form when

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11 B. Polyatomic Ionic Compounds: Contain polyatomic ion as the cation, anion, or both.

*Memorize the following names and charges of polyatomic ions! 1. Polyatomic cations: Names end in -ium. + + NH4 = ammonium H3O = hydronium

2. Polyatomic anions: Many contain oxygen. – 2– OH = hydroxide CO3 = carbonate – 3– NO3 = nitrate PO4 = phosphate 2– – SO4 = sulfate CN = cyanide

Examples of Polyatomic Ionic Compounds NH4Cl ammonium chloride Na2CO3 sodium carbonate Mn(OH)2 manganese (II) hydroxide (NH4)2SO4 ammonium sulfate ------A List of Some Polyatomic Ions Cations + Ammonium = NH4 2+ Mercury(I) = Hg2

Anions - - 2- Acetate = C2H3O2 or CH3COO Thiosulfate = S2O3 Cyanide = CN- 3- Hydroxide = OH- Phosphate = PO4

2- - Carbonate = CO3 Perchlorate = ClO4 - - Hydrogen Carbonate (bicarbonate) = HCO3 Chlorate = ClO3 Hypochlorite = ClO- - Nitrate = NO3 - 2- Nitrite = NO2 Chromate = CrO4 2- Dichromate = Cr2O7 2- Sulfate = SO4 2- - Sulfite = SO3 Permanganate = MnO4 - Hydrogen Sulfate (bisulfate) = HSO4

II. Molecular Compounds (Binary): NONMETAL + NONMETAL General Rules: Name first element first, second element second. 1. First element: Greek prefix + parent element (Exception: Don’t use “mono-”). 2. Second element: Greek prefix + parent element + “-ide” (as if it were an anion). Greek Prefixes Examples of Binary Molecular Compounds mono one N2O5 dinitrogen pentoxide di two P4O6 tetraphosphorus hexoxide tri three BF3 boron trifluoride tetra four NO nitrogen monoxide penta five CO carbon monoxide hexa six hepta seven Chem 30A Kim octa eight

III. Acids 1. Binary acids: “hydro” + parent element + “ic acid” HCl hydrochloric acid HBr hydrobromic acid

2. Oxoacids: Names are derived from oxoanions. If oxoanion name ends with –ate, then acid name ends with –ic acid. – eg. NO3 is nitirite à HNO3 is nitric acid If oxoanion name ends with –ite, then acid name ends with –ous acid. – eg. NO2 is nitrite à HNO2 is nitrous acid.

*Memorize the following common acids! Strong Acids Weak Acids HCl hydrochloric acid HC2H3O2 or CH3COOH acetic acid HBr hydrobromic acid H2CO3 carbonic acid HI hydroiodic acid HNO3 nitric acid H2SO4 sulfuric acid HClO4 perchloric acid

Writing Formulas

I. Ionic Compounds Balance charges, since compounds must be neutral! (Principle of Electrical Neutrality) Positive Charge + Negative Charge = 0

eg., magnesium bromide = MgBr2 iron(II) sulfide = FeS

II. Molecular Compounds (Binary) Greek prefixes indicate number of atoms. eg., dinitrogen pentoxide = N2O5 boron trifluoride = BF3

Chem 30A Kim