Inorganic Nomenclature

Metals: Form positive ions. Non-metals: Form negative ions. (H is the exception). Anion: negatively charged ion (Cl -, O 2 -, NO 3 - ). Cation positively charged ion (K +, Al 3+, NH 4 + ). Monatomic: only one atom (Ne, Na+, I-). Diatomic: two atoms (O 2, NaCl, I 2, LiBr). Triatomic: three atoms (K 2 S, O 3, H 2 O). Polyatomic: many atoms. (Poly means more than one). (CH 4, C 2 H 6 O, NaCl)

a) Naming Monatomic ions * monatomic metal ions: Place the word ion after the name of the metal. eg. Potassium metal (K) forms the potassium ion (K+). (monatomic metal ions will have a charge) * monatomic metal ions with more than one possible combining #: * place the roman numeral charge value in brackets between the metal name and the word ion. * eg. Fe 3+ = Iron (III) ion, * Fe 2+ = Iron (II) ion, * Cu 3+ = Copper (III) ion.

* Change the ending of the non- metal to “ide”. (means negative charge.) Element name SymbolIon nameIon symbol FluorineFFluorideF-F- ChlorineClChlorideCl - BromineBrBromideBr - IodineIIodideI-I- OxygenOOxideO 2- SulphurSSulphideS 2- SeleniumSeSelenideSe 2- NitrogenNNitrideN 3- PhosphorusPPhosphideP 3-

* Polyatomic ions are compounds that carry a charge. Carbonate = CO 3 2- Nitrate = NO 3 - Phosphate = PO 4 3- Hydroxide = OH - Sulphate = SO 4 2- Permanganate = MnO 4 - Chromate = CrO 4 2- Acetate = CH 3 COO - Dichromate = Cr 2 O 7 2- Ammonium = NH 4 +

Polyatomic Ion NamesSymbol AmmoniumNH 4 1+ NitrateNO 3 1- NitriteNO 2 1- SulfateSO 4 2- SulfiteSO 3 2- BisulfateHSO 4 1- CarbonateCO 3 2- BicarbonateHCO 3 1- HydroxideOH 1- PhosphatePO 4 3- ChlorateClO 3 1- ChloriteClO 2 1- PermanganateMnO 4 1- ChromateCrO 4 2- DichromateCr 2 O 7 2-

An Ionic Compound is a compound made of ions. The 3 Formula Rules: 1.Put down the symbols of the ions. Add brackets around any complex ion. Write the positive (metallic) ion first. e.g. Ca Clor Ca(OH) 2. Put combining numbers above each symbol. e.g. Ca 2+ Cl 1- orCa 2+ (OH) cross out the positive and negative signs criss-cross the combining numbers and use them as subscripts. eg. Ca +2 + Cl -1  Ca 1 Cl 2 = CaCl 2 orCa(OH) 2

* If the subscript is “one”, you don’t need to write it. (Na 1 Cl 1 = NaCl) * You must reduce subscripts if possible. Is there a number that will divide evenly into both subscripts? (i.e. Mg 2 O 2 = MgO) * Subscripts inside brackets of complex ions must NOT be changed * eg. Ca 2+ + NO 3 1-  Ca(NO 3 ) 2 * If the subscript outside brackets is one, don’t write the brackets * eg. Na(OH) 1  NaOH

Lead (IV) Oxide: Pb +4 O -2  Pb 2 O 4 = PbO 2 Lead (II) Oxide: Pb +2 O -2  Pb 2 O 2 = PbO

1.magnesium and oxygen__ Mg 2 O 2  MgO 2. potassium and sulphate___________ K 2 SO 4 3. hydrogen and fluorine___________ HF 4. calcium and hydrogen____________ CaH 2

A. Binary Compounds / Only two elements /a metal and a non-metal To name: a) Name the metal first without changing its name b) Name the non-metal second and change its ending to ide E.g. BeBr 2 = Beryllium bromide

Sodium and Bromine  ________________  __________________ Potassium and Oxygen  ______________  ______________________

Sodium and Bromine  ____________ NaBr  __Sodium Bromide___________ Potassium and Oxygen  __________ K2OK2O  __Potassium Oxide___

-Some elements can have multiple charges/comb. #s -Use Roman numerals to specify which ion it is: Eg Fe(II) = Fe 2+ Look at the periodic table Fe(III) = Fe 3+ see more than one comb cap To name: a) find combining # by reverse criss-cross b) change combining # to roman numeral, put after metal name *Only metals can form more than one possible type of ion* E.g. FeCl 2 = Fe 2+ and Cl 1- = _Iron (II) Chloride_____________________

* Iron (II) and Oxygen  _________ FeO  __Iron (II) Oxide___ * Copper (I) and Bromine  ______ CuBr  _Copper (I) Bromide

To name: Refer to your Periodic Table of Common Ions Put: 1. positive ion first. 2. negative ion second. E.g. Ba 2+ + SO 4 2- = BaSO 4 = Barium sulphate E.g. Ba 2+ + PO 4 3- = Ba 3 (PO 4 ) 2 = Barium phosphate

Potassium and Bicarbonate  _________ KHCO 3 __  Potassium Bicarbonate _ Magnesium and Nitrate  _______ Mg(NO 3 ) 2 __  __Magnesium Nitrate

* Class work: p. 71 – 72 * #4. a – o * #5. a – o

Crystals of ionic compounds often have water “stuck” to them. eg. when Copper (II) Sulphate is crystallized from a water solution, the resulting crystals have the formula: CuSO 4 · 5H 2 O 5 water molecules are attached to every CuSO 4 the waters attached are called “Hydrates” prefixes are used to tell the number of Hydrates attached

Prefix Used# of water molecules mono1 di2 tri3 tetra4 penta5 hexa6 hepta7 octa8 nona9 deca10

Hydrate name =compound name + prefix + “hydrate” eg. name of CuSO 4 · 5H 2 O = “copper (II) sulfate pentahydrate” Ca(NO 3 ) 2 · 4H 2 O= “calcium nitrate tetrahydrate” Homework: p. 73 #6. a,c,e,g,i #7. a,c,e,

* usually are covalently bonded molecules * composed of two different types of atoms * it is assumed one particle is cation-like and the other is anion- like

1. Use prefix system (mono, di, tri, …) 2. Cation-like element written 1st, anion-like element written 2nd 3. Ending of name changed to “ide” eg. CO = Carbon monoxide.

4. Place prefix, according to the number of that atom within the molecule, in front of the elements’ name So P 2 S 3 is written: “Diphosphorus trisulphide ” ****exception: if only one atom in cationic spot, then do not place the prefix mono in front of the elemental name. eg. NO 2 = Nitrogen dioxide, not mononitrogen dioxide.

* NCl 3 = Nitrogen trichloride. * P 4 O 6 = Tetraphosphorus hexaoxide. * S 2 F 2 = Disulphur difluoride. * NI 3 = Nitrogen triiodide. * ICl = Iodine monochloride.

* Homework p. 74 #8 a,c,e,g * #9 a,c,e,g,i

An acid is a compound starting with an H (hydrogen), and has a pH < 7. Most acids contain: oxygen, hydrogen a non-metal. When dissolved in water, an acid breaks apart: H+H+ “anion” + acid eg: HNO 2 + water → NO H + acid anion

ACIDANION HFHydrofluoric acid HClHydrochloric acid HBrHydrobromic acid HIHydroiodic acid HNO 2 Nitrous acidNO 2 - Nitrite ion HNO 3 Nitric acidNO 3 - Nitrate ion H 3 PO 4 Phosphoric acidPO 4 3- Phosphate ion H 2 SO 3 Sulphrous acidSO 3 2- Sulphite ion H 2 SO 4 Sulphuric acidSO 4 2- Sulphate ion HClO Hypochlorous acidClO - Hypochlorite ion HClO 2 Chlorous acidClO 2 - Chlorite ion HClO 3 Chloric acidClO 3 - Chlorate ion HClO 4 Perchloric acidClO 4 - Perchlorate ion