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Chemical Nomenclature 1. Binary Ionic Compounds - Type I 2. Binary Ionic Compounds - Type II 3. Ionic Compounds & Polyatomic (Complex) Ions 4. Covalent.

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Presentation on theme: "Chemical Nomenclature 1. Binary Ionic Compounds - Type I 2. Binary Ionic Compounds - Type II 3. Ionic Compounds & Polyatomic (Complex) Ions 4. Covalent."— Presentation transcript:

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2 Chemical Nomenclature 1. Binary Ionic Compounds - Type I 2. Binary Ionic Compounds - Type II 3. Ionic Compounds & Polyatomic (Complex) Ions 4. Covalent Compounds Type III 5. Binary Acids 6. Oxy-Acids 7. Hydrates

3 Common Names n A lot of chemicals have common names as well as the proper IUPAC name. n Chemicals that should always be named by common name and never named by the IUPAC method are: u H 2 Owater, not dihydrogen monoxide u NH 3 ammonia, not nitrogen trihydride

4 Definitions n An IONIC COMPOUND consists of a metal cation bonded to a nonmetal anion. Electrostatic attraction holds them together. n A COVALENT COMPOUND consists of nonmetal atoms sharing valence electrons. n A BINARY compound is one that is made of just two elements.

5 Type I n Write the cation n Write the anion u Change the ending to –ide u Drop- ogen, ygen, ine, ur, urus

6 Naming Compounds n 1. Cation first, then anion n 2. Monatomic cation = name of the element n Ca 2+ = calcium ion n 3. Monatomic anion = root + -ide Cl  = chloride n CaCl 2 = calcium chloride Binary Ionic Compounds:

7 n In an ionic compound, the charges of the cations and anions must always cancel out. n Subscripts are used if more than one atom is needed to cancel the charges: sodium chloride: Na + and Cl -  NaCl lithium oxide: Li + and O 2-  Li 2 O aluminum bromide: Al 3+ and Br -  AlBr 3 zinc nitride: Zn 2+ and N 3-  Zn 3 N 2 potassium iodide: K + and I -  KI silver phosphide: Ag + and P 3-  Ag 3 P

8 Examples: Type I Binary Ionic Compounds Write the formulas: potassium oxide zinc chloride silver sulfide aluminum nitride gallium oxide calcium iodide Write the names: K 3 N AgI ZnBr 2 Al 2 O 3 Ba 3 P 2 LiH

9 Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 Sc) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

10 Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

11 Type II Binary Ionic Compounds n These are ionic compounds where the metal cation can form TWO different charges. Fe 2 + iron (II) Fe 3 + iron (III) Ni 2 + nickel (II) Ni 3 + nickel (III) Co 2 + cobalt (II) Co 3 + cobalt (III) Cu + copper (I) Cu 2 + copper (II) Au + gold (I) Au 3 + gold (III) Sn 2 + tin (II) Sn 4 + tin (IV) An older system uses suffixes and Latin names, - ous for the lower charge, - ic for the higher charge: Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic

12 Charge of Elemental Ions n The common charge (oxidation state) of many representative metals.

13 Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 -3 -2 -1 0 Cd +2

14 Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

15 Examples: Type II Binary Ionic Compounds Write the formulas: iron (II) oxide copper (II) chloride tin (IV) sulfide cupric nitride nickel (III) oxide ferrous iodide cobalt (III) selenide Write the names: Fe 2 O 3 SnS NiBr 2 CuS Pb 3 P 2 CuBr FeCl 3

16 Polyatomic (Complex) Ions n All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons. n A molecule is a particle that forms when two or more atoms bond together. n A complex ion is a charged molecule. Complex ions may be cations or anions. examples: nitrate: NO 3 - sulfate: SO 4 2 - hydroxide: OH -

17 NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

18 You can make additional polyatomic ions by adding a H + to the ion! CO 3 -2 is carbonate HCO 3 – is hydrogen carbonate H 2 PO 4 – is dihydrogen phosphate HSO 4 – is hydrogen sulfate Polyatomic Ions

19 Naming Polyatomic Compounds Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al(HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate

20 Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2.Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

21 Writing formulas with Complex Ions a) Ammonium chlorideNH 4 Cl b) Silver sulfateAg 2 SO 4 c) Aluminum hydroxideAl(OH) 3 d) Calcium phosphateCa 3 (PO 4 ) 2 e) Iron (III) nitriteFe(NO 2 ) 3 f) Copper(II) permanganateCu(MnO 4 ) 2 g) Ammonium dichromate(NH 4 ) 2 Cr 2 O 7 h) Zinc acetateZn(CH 3 COO) 2

22 Things to Notice n Most complex ions are anions. Ammonium, NH 4 +, is the most common complex cation. n Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms: perchorateClO 4 - sulfateSO 4 2- chlorateClO 3 - sulfiteSO 3 2- chloriteClO 2 - nitrateNO 3 - hypochloriteClO - nitriteNO 2 -

23 n If an ion carries a charge like “-2” or “-3”, a series of related ions can be formed by adding hydrogen cations (H + ) while still leaving a net charge: examples: Sulfide:S 2- hydrogen sulfide:HS - (bisulfide) Sulfate:SO 4 2- hydrogen sulfate:HSO 4 - (bisulfate) Carbonate:CO 3 2- hydrogen carbonate:HCO 3 - (bicarbonate) Phosphate:PO 4 3- hydrogen phosphate:HPO 4 2- dihydrogen phosphate: H 2 PO 4 -

24 More Formulas with Complex Ions a) Sodium bicarbonateNaHCO 3 b) Nickel (II) hydrogen sulfideNi(HS) 2 c) Aluminum perchlorateAl(ClO 4 ) 3 d) Barium dihydrogen phosphateBa(H 2 PO 4 ) 2 e) Iron (III) sulfiteFe 2 (SO 2 ) 3 f) Cuprous bisulfateCuHSO 4 g) Zinc periodateZn(IO 4 ) 2 h) Lithium seleniteLi 2 SeO 3

25 Ionic Nomenclature review Writing Formulas n Write each ion, cation first. Don’t show charges in the final formula. n Overall charge must equal zero. u If charges cancel, just write symbols. u If not, use subscripts to balance charges. n Use parentheses to show more than one of a particular polyatomic ion. n Use Roman numerals indicate the ion’s charge when needed (stock system)

26 Ionic Nomenclature Review Sodium Sulfate Na + and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 –2 (NH 4 ) 2 CO 3

27 Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOHb) Fe 3 OHc) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

28 Mixed Practice! Name the following: 1. Na 2 O 2. CaCO 3 3. PbS 2 4. Sn 3 N 2 5. Cu 3 PO 4 6. HgF 2

29 Mixed Up… The Other Way Write the formula: 1. Copper (II) chlorate 2. Calcium nitride 3. Aluminum carbonate 4. Potassium bromide 5. Barium fluoride 6. Cesium hydroxide

30 Covalent Compounds n Covalent compounds are made of NONMETAL elements sharing valence electrons. n There are no ions involved!! n Because there are no charges to help us write the formulas of covalent compounds, prefixes are used to indicate the number of each atom present in the formula. CO 2 is named “carbon dioxide” COCl 2 is named “carbon monoxide dichloride” HN 2 O is named “hydrogen dinitrogen monoxide” SO 3 is named “sulfur trioxide” The prefix, “mono” is never used for the first element in the formula!

31 Naming Molecular Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl)

32 PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

33 Molecular (Covalent) Nomenclature for nonmetals n Prefix System (covalent compounds) 1.Less electronegative atom comes first. *binary only 2.Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3.Change the ending of the second element to -ide.

34 CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride Molecular Nomenclature: Examples

35 Arsenic monochloride dinitrogen monochloride pentoxide tetraphosphorus decoxide AsCl N 2 ClO 5 P 4 O 10 More Molecular Examples

36 Examples of Covalent Naming n Write the names: SO 2 P 4 O 10 n Write the formulas: phosphorus pentachloride dinitrogen trioxide

37 Learning Check 1.P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2.Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

38 Mixed Review Name the following compounds: 1. CaO a) calcium oxideb) calcium(I) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachlorideb) tin(II) chloride c) tin(IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

39 Solution Name the following compounds: 1. CaO 2. SnCl 4 3.N 2 O 3 a) calcium oxide c) tin(IV) chloride b) Dinitrogen trioxide

40 Mixed Practice 1. Dinitrogen monoxide 2. Potassium sulfide 3. Copper (II) nitrate 4. Dichlorine heptoxide 5. Chromium (III) sulfate 6. Iron (III) sulfite 7. Calcium oxide 8. Barium carbonate 9. Iodine monochloride

41 Mixed Practice 1. BaI 2 2. P 4 S 3 3. Ca(OH) 2 4. FeCO 3 5. Na 2 Cr 2 O 7 6. I 2 O 5 7. Cu(ClO 4 ) 2 8. CS 2 9. B 2 Cl 4

42 Binary Acids n A simple definition of an “acid” is a substance which produces H+ ions in water. n Most acids have hydrogen ions in their formulas. n A binary acid composed of a hydrogen cation bonded to one other element: HCl HBr H 2 S hydrochloric acidhydrobromic acidhydrosulfuric acid Binary acids are always named: hydro____ic acid

43 Oxy-Acids n An acid can also be made of a hydrogen ion bonded to a complex ion. Complex ions whose names end in “ate”: NO 3 - SO 4 2- CO 3 2- PO 4 3- nitric acid: HNO 3 sulfuric acid: H 2 SO 4 carbonic acid:H 2 CO 3 phosphoric acid:H 3 PO 4 Can you propose a rule for naming oxy-acids with complex ions ending in “ate”?

44 More Oxy-Acids n Complex ions ending in “ite”: NO 2 - SO 3 2- ClO - ClO 2 - nitrous acid:HNO 2 sulfurous acid:H 2 SO 3 hypochlorous acid:HClO chlorous acidHClO 2 Can you propose a rule for naming oxy-acids with complex ions ending in “ite”?

45 Acid Nomenclature Acids Acids  Compounds that form H + in water.  Formulas usually begin with ‘H’.  In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water)  Ternary acids are ALL aqueous Examples: Examples:  HCl (aq) – hydrochloric acid  HNO 3 – nitric acid  H 2 SO 4 – sulfuric acid

46 Acid Nomenclature Review No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

47 Acid Nomenclature Flowchart

48 HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 2 elements, -ide2 elements, -ide 3 elements, -ate3 elements, -ate 3 elements, -ite3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid Acid Nomenclature

49 hydrofluoric acidhydrofluoric acid sulfuric acidsulfuric acid nitrous acidnitrous acid 2 elements2 elements 3 elements, -ic3 elements, -ic 3 elements, -ous3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2 Acid Nomenclature  H + F-  H + SO 4 2-  H + NO 2 -

50 Name ‘Em! n HI (aq) n HCl n H 2 SO 3 n HNO 3 n HIO 4

51 Write the Formula! n Hydrobromic acid n Nitrous acid n Carbonic acid n Phosphoric acid n Hydrotelluric acid

52 Special Case: Hydrates

53 Hydrated Ionic Compounds n A HYDRATE is an salt that has water molecules trapped within its crystals. n Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes. monohexa dihepta triocta tetranona pentadeca CuSO 4 · 5 H 2 O copper (II) sulfate pentahydrate MgCO 3 ·10 H 2 O magnesium carbonate decahydrate

54 Examples of hydrates: n Write the formulas: copper(II) fluoride tetrahydrate CuF 2 ·4 H 2 O calcium nitrate trihydrate Ca(NO 3 ) 2 ·3 H 2 O n Write the names: MgSO 4 · 7 H 2 Omagnesium sulfate heptahydrate FeCl 2 · H 2 Oiron (II) chloride monohydrate

55 Now it’s Study Time DONE


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