Starter S-73 Give the scientific name for three chemical compounds.

Chemical Names and Formulas Chapter 9 Chemical Names and Formulas

Chapter 9 9.1 Naming Ions

9.1 Naming Ions Monatomic Ions – only one atom Review Cations (metals) form positive charges

9.1 Naming Ions Monatomic Ions – only one atom Review Group 1: +1

9.1 Naming Ions Monatomic Ions – only one atom Review Group 2: +2

9.1 Naming Ions 8.1 Molecular Compounds Some metals have more than one charge (oxidation number) They are named using the name and the charge Symbol Name Classical Name Cu+ Copper (I) Cuprous Cu2+ Copper (II) Cupric Fe2+ Iron (II) Ferrous Fe3+ Iron (III) Ferric Pb2+ Lead (II) Plumbous Pb4+ Lead (IV) Plumbic

9.1 Naming Ions Monatomic Ions – only one atom Review Anions – negative ions (names end in –ide)

9.1 Naming Ions Monatomic Ions – only one atom Review Group 17: -1

9.1 Naming Ions Monatomic Ions – only one atom Review Group 16: -2

9.1 Naming Ions Monatomic Ions – only one atom Review Group 15: -3

9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Ammonium

9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Hydrogen Sulfate

9.1 Naming Ions Polyatomic Ions – a charged group of atoms bonded covalently Examples – Carbonate

9.1 Naming Ions See page 257 for a list of polyatomic ions. There will be a quiz.

9.2 Naming & Writing Formulas: Ionic Chapter 9 9.2 Naming & Writing Formulas: Ionic

9.2 Naming & Writing Formulas: Ionic Binary Compounds – composed of two elements and can be ionic or covalently bonded For Ionic names Write the name of the cation first Write the name of the anion Change the ending of the anion to -ide Sodium Bromide Sodium Bromine NaBr Sodium Br

9.2 Naming & Writing Formulas: Ionic If the compound has a metal with more than one charge, we must calculate the charge Write out the formula and the charge of the anion Calculate the total negative charge This is the total charge on the cation, so divide the charge by the number of atoms PbCl4 PbCl4-1

9.2 Naming & Writing Formulas: Ionic Name the cation Name the anion Change the ending to -ide Lead (IV) Chloride Lead (IV) Chlorine Lead (IV) Cl4 PbCl4

9.2 Naming & Writing Formulas: Ionic Example 1: Example 2: Example 3: Example 4: Sodium Sulfide Sodium Sulfur Sodium S Na2S Copper (II) Oxide Copper (II) Oxygen Copper (II) O CuO Zinc I2 Zinc Iodine ZnI2 Zinc Iodide Iron (III) Sulfide Iron (III) Sulfur Fe2S3 Iron (III) S3

9.2 Naming & Writing Formulas: Ionic To write the formula from the name Write the ions Cross the values of the charges Confirm it is the smallest ratio NiF3 Nickel (III) Fluoride Ni+3 F-

9.2 Naming & Writing Formulas: Ionic Example 1: Example 2: Example 3: Example 4: CaBr2 Calcium Bromide Ca+2 Br- PbO2 Pb2O4 Pb+4 O-2 Lead (IV) Oxide MgS Mg2S2 Mg+2 S-2 Magnesium Sulfide V2O5 Vanadium (V) Oxide V+5 O-2

Starter S-74 Name the following ions Pb+2 C2H3O2- Mg+2 Cl-

9.2 Naming & Writing Formulas: Ionic Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for Write the formula and charge for Ammonium Write the formula and charge for Carbonate NH4+1 CO3-2 Ammonium Carbonate NH4+1 Carbonate

9.2 Naming & Writing Formulas: Ionic Polyatomic Ions – Use the same rules as other ionic compounds The endings do not change So to write the formula for Criss Cross If the polyatomic ion has a subscript, parenthesis are placed around the polyatomic ion (NH4)2CO3 NH42CO3 NH4+1 Carbonate Ammonium Carbonate NH4+1 CO3-2

9.2 Naming & Writing Formulas: Ionic Example 1 Example 2 Example 3 Example 4 Na3PO4 Sodium Phosphate Na+ PO4-3 Fe(H2PO4)3 Fe+3 H2PO4- Iron (III) Dihydrogen Phosphate NH4+ O-2 (NH4)2O Ammonium Oxide Cu(ClO4)2 Copper (II) Perchlorate Cu+2 ClO4-

9.2 Naming & Writing Formulas: Ionic So to write the name for Name the first ion (check charges if it needs a roman numeral) Name the second ion Silver Sulfate Silver SO4 Ag2SO4 Lead (IV) Nitrate Pb(NO3)4 Lead (IV) (NO3)4

9.2 Naming & Writing Formulas: Ionic Example 1 Example 2 Example 3 Example 4 Ammonium Dichromate (NH4)2Cr2O7 Nickel (III) Oxalate Ni2(C2O4)3 CaSiO3 Calcium Silicate Cobalt (II) Hydrogen Phosphate CoHPO4

Starter S-76 Write the names for the following Pt(NO2)2 Platinum (II) Nitrite B. Mg(ClO)2 Magnesium Hypochlorite Write the formula for the following Cesium Carbonate Cs2CO3 Copper (I) Suflite Cu2SO3

9.3 Naming & Writing Molecular Compounds Chapter 9 9.3 Naming & Writing Molecular Compounds

9.3 Naming & Writing Molecular Compounds Prefix Number Mono 1 Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10 Molecular Compounds (two non-metals) Prefixes are used to name the subscript in the molecular formula So to name Never use mono on the first element Prefix and element Silicon Dioxide SiO2 Silicon O2

9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Nitrogen Trichloride NCl3 Dinitrogen Tetrahydride N2H4 Cl2O7 Dichlorine Heptaoxide TetraPhosphorus Trisulfide P4S3

9.3 Naming & Writing Molecular Compounds Prefix Number Mono 1 Di 2 Tri 3 Tetra 4 Penta 5 Hexa 6 Hepta 7 Octa 8 Nona 9 Deca 10 Writing formulas invloves just writing the symbols and the prefixes Write the first element with the proper subscript Second element and subscript CBr4 Carbon Tetrabromide C Tetrabromide

9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 P2O3 Diphosphorus Trioxide IF7 Iodine Heptafluoride Nitrogen Monoxide NO Tetraphosphorus Hexaoxide P4O6

Starter S-77 Write the names for the following N2O5 Dinitrogen Pentaoxide B. CCl4 Carbon Tetrachloride Write the formula for the following Xenon Hexafluoride XeF6 Carbon Dioxide CO2

Starter S-78 Write the names for the following CO3-2 Carbonate B. H2PO4- Dihydrogen Phosphate Write the formula for the following Hypochlorite ClO- Dichromate Cr2O7-2

Chapter 9 9.4 Naming & Writing Acids

9.4 Naming & Writing Formulas for Acids Acid – a compound that has one or more hydrogen atoms and produces hydrogen ions (H+) in solution The basic formula is Three rules for naming When the anion (X) does not have Oxygen in it a. The name begins with hydro b. The anion’s name ends in –ic c. And the word acid is added to the end HnX Hydrochloric Acid Hydrochloric HCl Hydro Cl

9.4 Naming & Writing Formulas for Acids 2. When the anion (X) does have Oxygen and the polyatomic ion ends in -ite a. Use the name of the anion, but change the ending to –ous b. Add the word acid Sulfurous Acid H2SO3 Sulfurous

9.4 Naming & Writing Formulas for Acids 3. When the anion (X) does have Oxygen and the polyatomic ion ends in -ate a. Use the name of the anion, but change the ending to –ic b. Add the word acid Sulfuric Acid H2SO4 Sulfuric Oxygen? NO YES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid

9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 Chloric Acid HClO3 Hydrocyanic Acid HCN HNO3 Nitric Acid Chlorous Acid HClO2

9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion Hydro means no Oxygen – so Fluoric means Fluoride H+ Hydrofluoric Acid H+ F- Hydrofluoric Acid HF Oxygen? NO YES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid

9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion ous means the ion ended in ite, so phosphite H+ Phosphorous Acid H+ PO3-3 Phosphorous Acid H3PO3 Oxygen? NO YES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid

9.4 Naming & Writing Formulas for Acids To write the formulas, we go backwards through our list Acids always have an H+ ion ic means the ion ended in ate, so phosphate H+ Phosphoric Acid Phosphoric Acid Oxygen? NO YES --ous acid Ending of Polyatomic Ion? -ite -ate Hydro—ic acid --ic acid

9.3 Naming & Writing Molecular Compounds Example 1 Example 2 Example 3 Example 4 HI Hydroiodic Acid HC2H3O2 Acetic Acid Hypochlorous Acid HClO H2CO3 Carbonic Acid

Starter S-79 Name the following SO3 Ag2SiO3 H2SO3 Write the formula for Nitrogen Triiodide Lead (II) Acetate Phosphorous Acid

9.5 The Laws Governing Formulas and Names Chapter 9 9.5 The Laws Governing Formulas and Names

9.5 The Laws Governing Formulas and Names The Law of Definite Proportions – in any chemical compound, the masses of the elements are always in the same proportion The ratio of this molecule is always Or (Same Ratio) 1.00:0.34 Carbon:Hydrogen 2.98:1.00

9.5 The Laws Governing Formulas and Names The Law of Multiple Proportions – Whenever the same two elements form multiple compounds, the different masses of one element that combine with the same mass of the other element are in the ratio of small whole numbers Huh? For example one compound A second compound might be The ratio of the two masses would be 5g A 10g A 2g B 2g B

Starter S-80 Write Copper (II) Acetate Acetic Acid Aluminum Dihydrogen Phosphate Name HF H2C2O4 Zn(OH)2

Starter S-81 Write Copper (I) Dichromate Hydrosulfuric Acid Sodium Permaganate Name HCN Fe(OH)3 Sn(SO3)2

Starter S-82 Write Vanadium (V) Hydroxide Hypochlorous Acid Magnesium Oxylate Name H2C2O4 ZnSO4 SO2

Starter S-83 Test Day!!

Starter S-84 Add the following using sig figs for the answer 14.03 + 1.8 0.087221 + 1.30 Multiply the following numers using sig figs 3.070 x 2.8 0.00280 x 3

Starter S-85 Name the following compounds (NH4)2CrO4 AgCN Pt(ClO3)4 PtSO3 HBr

No, the Test isn’t that hard Really Starter S-87 No, the Test isn’t that hard Really