UNIT 1 Nomenclature KEY IDEAS. anion. cation. neutral. monatomic. diatomic. triatomic. polyatomic. combining capacity. multivalent

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1 UNIT 1 Nomenclature Vocabulary anion KEY IDEAS What does it mean? cation neutral monatomic diatomic triatomic polyatomic combining capacity multivalent Nomenclature: the naming system Quick Review: Are the following compounds ionic (I) or covalent (C)? NaCl: I CO 2 : C LiBr: Al 2 O 3 : SiO 2 : FeO: H 2 O: MgO: P 5 Cl 7 : Na 3 N: CCl 4 : Cu 2 S: BeI 2 : SF 2 : CH 4 : KOH: Na 2 SO 4 : CoO: 1

2 1.1 Binary Ionic Compounds Naming 1. Write the name of the metal 2. Write the name of the non-metal, but change the ending to ide Practice: Name the following binary ionic compounds CaI 2 GeO 2 MgO GaCl 3 NaBr Ta 3 N 5 Li 2 S WSe 3 Ca 3 P 2 Ag 2 O AlAs CdI 2 ZnI 2 Sr 3 P 2 ScF 3 KBr Formula 1. Overall charge must be 0 2. Write the metal first, followed by the non-metal Write the symbol for the cation and anion. Calcium oxide Ca 2+ O 2- Criss cross the charges. Calcium oxide Ca 2+ O 2- Reduce the charges if necessary. Calcium oxide Ca 2 O 2 becomes CaO Practice: Write the molecular formula for the following ionic compounds. Potassium iodide Rubidium sulfide Magnesium nitride Beryllium chloride Yttrium telluride Cesium phosphide Lithium oxide Calcium selenide Zirconium oxide Tungsten arsenide 2

3 1.2 Multivalent Ionic Compounds A multivalent metal is a metal that have more than one possible ion charge. These metals are usually found in the transition metals family. The ion charge of multivalent metals is included when naming. They are indicated using roman numerals I II Formula Write the symbol for the cation and anion. chromium (II) oxide Cr 2+ O 2- Criss cross the charges. chromium (II) oxide Cr 2+ O 2- Reduce the charges if necessary. chromium (II) oxide Cr 2 O 2 becomes CrO Practice: Write the molecular formula for the following ionic compounds. ***Be careful of Hg!*** manganese (II) chloride tin (IV) oxide manganese (II) fluoride mercury (I) selenide chromium (III) oxide copper (II) oxide molybdenum (III) sulfide mercury (II) chloride Naming Write the name of the ionic compound Do the charges make sense? Uncriss-cross the charges Cr 2+ O 2- chromium (II) oxide there is no O -, multiply by 2 Cr O 3

4 Practice: Write the name of the following ionic compounds CuO TiN NiN SnSe MoF 3 Bi 3 As 5 HgS PbBr 4 Ni 2 S 3 AuP 4

5 1.3 Polyatomic Ionic Compounds A polyatomic ion is an ion made of more than one atom. The group of atoms acts as ONE ion. Name 1. Write the name of the metal 2. Write the name of the polyatomic ion Practice: Write the name of the following ionic compounds NaNO 3 sodium nitrate Al(HSO 3 ) 3 Li 2 SO 4 Fe(OH) 3 Ca 3 (PO 4 ) 2 Ag 2 Cr 2 O 7 NH 4 MnO 4 (NH 4 ) 3 PO 3 Formula Write the symbol for the cation and anion. calcium nitrate Ca 2+ NO 3 - Criss cross the charges. Reduce if necessary calcium nitrate Ca 2+ NO 3 - If there is more than 1 polyatomic ion, put it in parentheses CaNO 3 2 Ca(NO 3 ) 2 Practice: Write the molecular formula for the following ionic compounds. calcium sulphate calcium sulphite zinc carbonate titanium (III) nitrate magnesium permanganate ammonium chromate manganese (IV) acetate aluminum cyanide lithium dichromate cobalt (III) bicarbonate 5

6 1.4 Covalent Compounds Combining capacities are not used when making covalent compounds! For this reason, we must name the number of each type of atoms in the covalent compound name using prefixes. Steps to naming: 1. Name the first non-metal 2. Name the 2 nd non-metal and change the ending to ide 3. Add a prefix in front of each non-metal to show the number of atoms 4. If there is only one of the first non-metal, DO NOT write mono Number of Atoms Prefix Practice: Write the name of the following covalent compounds SiO 2 silicon dioxide PCl 3 P 5 Cl 7 AsI 3 CO S 4 F 3 CBr 4 TeO SF 6 N 3 O 8 H 3 O H 2 O OF 3 CO 2 Practice: Write the molecular formula for the following covalent compounds. tetracarbon nonafluoride silicon monosulphide trinitrogen diphosphide oxygen dibromide arsenic monoxide oxygen gas phosphorous pentachloride sulphur dioxide dihydrogen monoxide carbon tetraiodide diarsenic trioxide bromine gas 6

7 1.5 Hydrates What is a hydrate? a molecule with molecules attached occurs when an ionic compound is evaporated from aqueous solution Naming uses prefixes to indicate how many water molecules are attached to the ionic compound. 1. Name the compound as you normally would 2. Indicate the number of water molecules attached with prefixhydrate Number of Atoms Prefix Practice: Write the name or molecular formula for the following hydrates. CuSO 4 5H 2 O Zn(CH 3 COO) 2 2H 2 O Ca(NO 3 ) 2 4H 2 O FeBr 3 6H 2 O chromium (ll) oxalate monohydrate Li 2 Cr 2 O 7 2H 2 O Al 2 O 3 3H 2 O CoF 2 4H 2 O aluminum nitrate nonahydrate cadmium nitrate tetrahydrate Na 2 CO 3 H 2 O Na 2 S 9H 2 O Na 2 SO 4 10H 2 O nickel (ll) chloride hexahydrate Ni 3 (PO 4 ) 2 8 H 2 O MgHPO 4 7H 2 O iron (lll) phosphate octahydrate copper (ll) phosphate trihydrate 7

8 1.6 Acids What is an acid? an acid is a compound with molecular formula starting with H many dissolve in water to release H + and form aqueous solutions exceptions: H 2 S and HCN, these are normally gases, but are acidic when dissolved in water Naming 1. Look at the anion 2. Does the ion name end in -ide, -ate, or -ite? 3. Do you find the anion on the periodic table? 8

9 H x IDE Acids or Binary Acids The anion is made of ONE element Acid Formula What is the Anion Name? Acid Name HF HCl HBr HI *H 2 S *H 3 P H x ATE Acids The anion name ends in "ATE" Acid Formula What is the Anion Name? Acid Name H 2 CO 3 HClO 3 H 2 CrO 4 H 2 Cr 2 O 7 CH 3 COOH HNO 3 H 2 C 2 O 4 HClO 4 HMnO 4 *H 2 SO 4 *H 3 PO 4 H x ITE Acids The anion name ends in "ITE" Acid Formula What is the Anion Name? Acid Name HClO 2 HClO HNO 2 *H 2 SO 3 *H 3 PO 3 9

10 Self-Test: Name or write the formula for the following acids HNO 3 H 2 CO 3 H 2 SO 3 HNO 2 CH 3 COOH H 3 PO 4 HBr chromic acid hydrofluoric acid phosphoric acid hydroiodic acid hypochlorous acid permanganic acid sulphuric acid 10