Chemical Nomenclature (a.k.a. naming compounds)

 Considered by many to be the “ Father of Modern Chemistry ”  ‘To each and every compound there can correspond one and only one correct name; to each and every name there can correspond one and only one compound.”  Major contributions included  Established the Law of Conservation of Mass  Developed a method of producing better gunpowder  Observed that oxygen and hydrogen combined to produce water (dew)  Invented a system of chemical nomenclature (still used in part today!)  Wrote the 1 st modern chemical textbook

 Made with positive cation and a negative anion.  Type I Ionic compound, the metal has only 1 charge. (+1, +2, or +3)  Metals lose electrons, become cations, positive ions.  Charge on the cation is equal to the number of electrons “lost”.  Non-metals gain electrons, become anions, negative ions.  Charge on the ion is equal to the number of electrons gained.  Each ion will lose or gain electrons so that it will have the nearest Noble gas configuration.

 1. Find charge of positive ion. Use periodic table to find the oxidation state. Oxidation state is equal to the number of electrons “lost”.  2. Each column generally contains ions with the same charge. Column 1, Alkali Metals all lose 1 electron and have a 1+charge. Column 2, Alkaline Earth Metals all lose 2 electrons and have a 2+ charge. Binary compounds have 2 elements

 Write the formula for the positive ion with the charge written in the exponent location on the symbol. If the charge is 1 then the + sign is used without a number. Ex: Na +, Mg 2+  Name the ion by using the element name followed by the word ion. Ex: Na + Sodium ion Mg 2+ Magnesium ion

 Write the formula for the negative ion with the charge written in the exponent location on the symbol. If the charge is 1, then – sign is used without a number. Ex: F -, O -2  Name the ion by using the root of the element name and change the ending to “ide”. Ex: F - is fluoride, O -2 is oxide.

 Determine charges on ions.  Write cation first and anion second  Combine ions so that charge on compound is 0.  Criss-cross charges for subscripts so that compound has 0 charge.  The oxygen atom in the formula does not receive a subscript since it is 1.  If charges are same, then both subscripts are 1. (1 is not written)  Sodium ion = Na +  Oxide ion = O 2- Na + O 2- Na 2 O Na + F - NaF Making a compound from a cation and anion

 Name the cation first. It is the name of the element.  Name anion second. Use the root of the element name, drop ending and add “ide”  Ex. Na 2 O, sodium oxide  Ex. NaF, sodium fluoride  Formation of ionic cmpds Naming the binary ionic compounds. 1&spos=1&var=animations

 Some transition metals have more than 1 charge for the ion.  To determine the charge from the formula, remember that the charge on compound =0. Figure out the charge by choosing the charge that makes the compound neutral.  Ex: FeO, Since O has to be a 2- charge according to the table, Fe must be a 2+charge to make the compound = 0. Type II, metals have more than one charge possible.

 Systematic Name- Charge of the metal is written as a Roman Numeral between the cation and anion.  Ex: FeO is Iron II Oxide, since the charge on Fe= 2+  Common name uses Latin name plus endings. The lesser of the charges ends in “ous” and the greater of the charges ends in “ic”  Ex: Fe 2+ ion in FeO, Ferrous oxide  Fe 3+ ion in Fe 2 O 3, Ferric oxide Two Naming Systems for Type II Ionic Compounds

 WRITE FORMULA AND NAME COMPOUND BETWEEN THESE IONS.  Chromium III and Oxide  Cr 2 O 3, chromium III oxide  Chromium II and Sulfide  CrS, chromium II sulfide  Cobalt II and Chloride  CoCl 2, cobalt II chloride  Cobalt III and Fluoride  CoF 3, cobalt III fluoride

 2. LITHIUM IODIDE  3. ALUMINUM FLUORIDE  4. IRON II CHLORIDE  5. MAGNESIUM OXIDE  11. LEAD II SULFIDE  13. BARIUM FLUORIDE  15. SILVER IODIDE  18. SODIUM NITRIDE

 Polyatomic ions contain two or more elements that are covalently bonded and act as a single ion. The charge of the ion is distributed over the entire polyatomic ion. Ex: SO 4 2-  Write the formulas for compounds with polyatomic ions so that the compound has a 0 charge. If there is more than 1 polyatomic ion, then it is written in () with a subscript outside the () to indicate the number of ions. Ex: Ca(NO 3 ) 2 Ca has a 2+ charge and NO 3 has a 1- charge 1, 2, 3 Nice Carl Sandburg People Nitrates and Nitrites 1-, Carbonates,Sulfates and Sulfites 2-, Phosphates 3- charges

 1. Write the name of the first ion, usually a metal. Only 1 positive polyatomic ion, NH 4 +, ammonium ion.  2. Write the name of the polyatomic ion. Use the tables to determine the name.  Ex: Ni 2+ and PO 4 3-  Nickel II ion and Phosphate ion  Ni 3 (PO 4 ) 2 Criss-cross charges for the subscripts.  Name is Nickel II Phosphate  Write formula and name with both systematic and common name. Cu 1+ ion and CrO 4 2- Writing the name of the polyatomic ionic compound

 Compare atom size to ion size.

 7 diatomic elements are molecular compounds.  Gases and only exist in nature as diatomic, 2 atoms bonded covalently.  H 2, N 2, O 2, F 2, Cl 2 Br 2, and I 2  Names are same as periodic table element name. Sometimes the word gas follows the element name. Ex: Oxygen gas  BrINClHOF your elements

Molecular formulas show the number and type of atoms in the molecule. Binary Molecular compounds have 2 elements. Writing molecular formula names: Write the name of the first element adding the Greek prefix for the number of atoms. Mono is not used for the first element. Write the name of the second element changing the ending to “ide” using the Greek prefix for the number of atoms. Ex: N 2 O 5, Dinitrogen Pentoxide

1)Mono- 2) Di- 3) Tri 4) Tetra- 5)Penta- ) Prefixes are used when the compound does not have a metal present (or when H is the first element in the formula) 2) Prefixes must be used for every element present in the compound 3) mono- is not used for the first element in a compound name (e.g. carbon dioxide) 6. Hexa 7) Hepta 8) Octa 9) Nona 10) Deca

1. Mono6. Hexa 2. Di7. Hepta 3. Tri8. Octa 4. Tetra9. Nona 5. Penta10. Deca  1) Prefixes are used when the compound does not have a metal present (or when H is the first element in the formula)  2) Prefixes must be used for every element present in the compound  3) mono- is not used for the first element in a compound name (e.g. carbon dioxide)

Write the nameWrite the formula SiO 2 Carbon Tetrachloride CO 2 Dinitrogen pentoxide SO 3 Nitrogen trifluoride PBr 3 Dihydrogen monosulfide PCl 5 Dichlorine monoxide Cl 2 O 7 Sulfur hexafluoride N 2 I 2 Phosphorous tribromide

 NameFormula Silicon dioxideCCl 4 Carbon dioxideN 2 O 5 Sulfur trioxideNF 3 Phosphorus TribromideH 2 S Phosphorus PentachlorideCl 2 O Dichlorine heptoxideSF 6 Dinitrogen DiodidePBr 3

Acids  From the Latin term for “ sour ” {Acids are sour to the taste}  Acids are substances that donate protons (H + ) (usually when dissolved in water)  Chemical formula usually begins with H Example: hydrochloric acid, HCl Bases  Taste bitter  Usually metal containing hydroxides  Chemical formula usually contains an OH,  except for NH 3 Example: potassium hydroxide, KOH

Let’s separate acids into 2 types:  Acids that contain oxygen  Acids that do not contain oxygen Binary acids have a H and a non-metal. Naming binary acids- begin with hydro prefix Follow by name of non-metal with ending of “ic” Ex: HF, hydrofluoric acid HCl, hydrochloric acid Ex: HCN, hydrocyanic acid

Naming acids containing oxygen:  For acids containing “ -ate ” anions: 1. Use root of the anion (for sulfate, SO 4 2-, use sulfur) 2. Add “ -ic ” suffix then end with “ acid ” Example:H 2 SO 4 is sulfuric acid  For acids with “ -ite ” anions: 1. Use root of the anion (for sulfite, SO 3 2-, use sulfur) 2. Add “ -ous ” suffix then end with “ acid ” Example:H 2 SO 3 is sulfurous acid

IF YOU “ ATE ” “ IC ” YOU WILL GET AN “ ITE ” “ OUS ”

Oxyanions with more than 2 forms are named using prefixes. ClO - HypochloriteClO 2 - Chlorite ClO 3 - ClorateClO 4 - Perchlorate Lowest # Oxygens = Hypo…ite Second lowest # Oxygens = …ite Third lowest # Oxygens = …ate Most # oxygens = per…ate

ClO - HypochloriteClO 2 - Chlorite HClO =Hypochlorous acid HClO2 Chlorous acid ClO 3 - ClorateClO 4 - Perchlorate HClO 3 = Choric acidHClO 4 = Perchloric acid

 Hydrates are compounds with water molecules attached.  Formulas for hydrates show the compound then a dot,a number then water  Ex: CuSO 4  5 H 2 O  Translate numbers after a dot into Greek prefixes to name. (Same as molecular names)  Ex: Copper II Sulfate Pentahydrate

 Write the formulas for these acids: 1. Hydrobromic Acid 2. Perfluoric acid 3. Nitric acid 4. Sufurous acid 5. Chromic acid  Write the names for these acids  6.HNO 2  7. HC 2 H 3 O 2  8. H 2 CO 3  9. HIO 3  10. HI

1.HBr 2. HFO 4 3. HNO 3 4. H 2 SO 3 5. H 2 CrO 4 6. Nitrous Acid 7. Acetic Acid 8. Carbonic acid 9. Iodic Acid 10. Hydroiodic Acid

PRACTICE ANSWERS  Potassium carbonate trihydrate  Lead II phosphate heptahydrate  Magnesium Bromate monohydrate  Tin IV sulfate pentahydrate  Calcium dichromate hexahydrate  NiSO 4  8H 2 O  Cu 2 C 2 O 4  2H 2 O  BaCrO 4  4H 2 O  HClO 4  HBr  H 3 PO 4  HBrO  HC 2 H 3 O 2  Chromic acid  Carbonic acid  Nitric acid

PRACTICE PRACTICE PRACTICE  K 2 CO 3  3H 2 O  Pb 3 (PO 4 ) 2  7H 2 O  Mg(BrO 3 ) 2  H 2 O  Sn(SO 4 ) 2  5H 2 O  CaCr 2 O 7  6H 2 O  Nickel II Sulfate octahydrate  Copper I oxalate dihydrate  Barium chromate tetrahydrate  Hydrobromic acid  Perfluoric acid  Nitric acid  Sulfurous acid  Chromic acid  HNO 2  HC2H3O2  H 2 CO 3  HIO3  HI