Naming Chemical Compounds

1. Naming Chemical Compounds

2. Binary Ionic Compounds • Binary = 2 types of elements • Ionic = made of ions • Compound = atoms bonded together

3. Ionic Compounds • Positive ions are attracted to Negative ions • FORMULA UNIT • Cation always comes first, then anion

4. Elemental anions • When an element becomes an anion, it starts to end in –ide • Fluoride • Chloride • Bromide • Oxide • Sulfide • Nitride • Phosphide

5. Type I • The cation has a predictable charge • Alkali Metals +1 • Alkaline Earth Metals +2 • Group 3A +3 • Silver Ag+ • Zinc Zn2+

6. Type II • The cation has a variable charge • All Transition metals except for Ag and Zn (for our purposes) • The name will have a roman numeral to denote the CHARGE on the cation Fe2+ Fe3+ Cu+ Cu2+ Iron(II) Iron(III) Copper(I) Copper(II) Ferrous Ferric Cuprous Cupric

7. Naming ionic compouds (Type I and II) • First name cation • Just the name of element if Type I • Name of element and roman numeral with charge on cation if Type II • Then name anion • Elemental anions end in “–ide” • When determining the formula, remember “swap ‘n’ drop”

8. Na3N MgCl2 Al2O3 CuCl CuCl2 PbBr4 Sodium nitride Magnesium chloride Aluminum oxide Copper(I) chloride Copper(II) chloride Lead(IV) bromide Name the following:

9. Aluminum chloride Magnesium Oxide Sodium nitride Calcium chloride Copper(I) sulfide Lead (II) bromide Iron(III) oxide AlCl3 MgO Na3N CaCl2 Cu2S PbBr2 Fe2O3 Determine the formula of the following

10. Polyatomic Ions • Many anions are not just ions of elements. • Polyatomic Ions = many atomed particle with an overall charge • Mostly nonmetals bonded to Oxygens

11. Polyatomic Ion Naming • Main polyatomic ion • Ends in “–ate” • Example: Chlorate ClO3- • One fewer oxygens • Ends in “-ite” • Example: Chlorite ClO2- • Even fewer oxygens • Hypo = under • Example: Hypochlorite ClO- • More oxygens than main ion • Hyper = over, shortened to “per” • Example: Perchlorate ClO4-

12. Common Polyatomic Ions

13. Common Polyatomic Ions • Hydrogen can attach to the polyatomic ions as H+ • This adds an H and reduces the overall charge by 1

14. AlPO4 Cu(NO3)2 Na2SO4 NaHCO3 Mg3(PO4)2 Aluminum phosphate Copper(II) nitrate Sodium sulfate Sodium bicarbonate Magnesium Phosphate Name these compounds with PAIs

15. Molecular Compounds • Molecular compounds are not bonded by positive and negative ions • They SHARE electrons • Made of two non-metals • Cannot predict or explain charges (no charges, because not LOSING or GAINING electrons – SHARING)

16. Naming Molecular Compounds (Type III) • Because there is no way to neutralize the compounds (like for ions) we must determine how many there are another way: • Use PREFIXES

17. How to tell if it’s Type III • Check the FIRST element – is it a non-metal? • If YES, it’s a Type III • Name the first element as the element • Name the second element ending in “-ide”

18. 1 2 3 4 5 6 7 8 9 10 Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca Prefixes

19. Using prefixes • If there is only one of the first element, you may omit the “mono” • You may not omit any other prefixes • The more electronegative element goes last (upper right hand corner) • F, O, N, Cl,

20. PCl3 CO2 NO N2O4 N2F5 OF2 Phosphorus trichloride Carbon dioxide Nitrogen monoxide Dinitrogen tetroxide Dinitrogen pentafluoride Oxygen difluoride Name the following

21. Naming Practice! For each of the following compounds, determine whether it is type I, II, or III. • FeCl3 • NaCl • Cu(OH)2 • N2O • BaSO4 • PO5 • (NH4)CO3 • SnBr2

22. Naming Practice! For each of the following compounds, determine the CHARGE on the cation (+1, +2, +3, or +4) • FeCl3 • Cu(OH)2 • Cr2S3 • NiS • Pb(NO3)2 • SnCl4 • 3 • 2 • 3 • 2 • 2 • 4

23. Acids • All acids have the H+ ion in them as the cation. • All acids have “acid” in their name • Consider Hydrochloric Acid • HCl

24. Naming Acids • If the anion DOES NOT CONTAIN OXYGEN: • Prefix hydro- • Root name of anion element • Suffix –ic • Examples • HF • H2S Hydrofluoric Acid Hydrosulfuric Acid Hydrooxygenic acid

25. Naming Acids • If the anion CONTAINS OXYGEN (ie: is a polyatomic ion) • Root name of the PAI • If anion ends in -ate, • acid ends in –ic • If anion ends in –ite, • acid ends in –ous

26. H2SO4 H2SO3 HNO3 HNO2 HC2H3O2 Phosphoric Acid Carbonic Acid Sulfuric Acid Sulfurous Acid Nitric Acid Nitrous Acid Acetic Acid H3PO4 H2CO3 Naming Acids Examples

27. Organic Molecules • Carbon based • Naming is based on number of carbons • Functional groups • Sets of molecules attached to the carbons • Naming is also based on what functional groups are where

28. Alkanes • The simplest organic molecules are Alkanes. • Carbons are all single bonded to each other • When not bonded to another carbon, bonded to a Hydrogen • All alkanes end in -ane

30. Prefixes • Note that the prefixes pertain to all types of carbon based molecules with any types of functional groups or chains • Meth • Eth • Prop • But • Pent • Hex • Hept • Oct

31. Alkenes and Alkynes • A functional group can be a set of atoms, or the way they are bonded. • Alkenes • Carbons have double bonds between them • Alkynes • Carbons have triple bonds between them

32. Alkenes and Alkynes • To Name • All alkenes end with –ene. • All alkynes end with –yne • Number the carbons in the longest chain. • Carbon 1 is at the end of the chain closest to the first functional group • Put the number that the bond is on, then the chain length • (some name by putting the number BEFORE the functional group ending)

33. Isomer = molecule with SAME formula but DIFFERENT structure

34. Alcohols • Have an –OH group attached • Name the carbon chain (prefix and bond) • End in –ol • Indicate which carbon the –OH is on • 2-propanol • 1-Butanol • 3-Octenol

35. What are the formulas for these alcohols?

36. Alcohols Some alcohols have common names like glycerol

37. Branched Hydrocarbons • The longest continuous chain of carbon atoms gives the root name/prefix. • Substituent is named by the number of carbons. • Specify location of substituent by numbering carbon atoms in longest chain. • Substituent often referred to as R or R’ (for second substituent)

38. Substituent often referred to as R or R’ (for second substituent) • If more than one alkyl group, use prefix di, tri, etc. to alkyl name • Substituents listed in alphabetical order (disregarding prefix)

39. Branched Hydrocarbon SubstituentAlkyl groups

40. What is the name of the compound? • Hints • Number Carbon chain from on side closest to first alkyl group • Single carbon branch called methyl, triple carbon group called propyl • More than one branch, use prefixes di-, tri-, etc. 4 ethyl,5 methyl heptane 2,4 dimethyl hexane

41. Tricky ones!!! Each END of a line is a Carbon atom. No H’s are indicated, but they are assumed See if you can name these.

42. Halohydrocarbons • Functional group is a halogen (X = F, Cl, Br, I) • General Formula • R – X • Naming • Select longest chain containing halogen • Number so that C with halogen gets lowest number

43. Ethers • Functional group • - O – • General Formula • R – O – R’ • Naming • Name the R group as an alkyl • Name the R’ group as an alkyl • End in ether

44. || || O O Aldehydes • Functional group • - C – H • General Formula • R – C – H • Naming • Name the R group • Change the ending to -al