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Nomenclature!!!

Nomenclature!!!. What’s in a name?. REMEMBER!!!. When naming compounds ALWAYS, ALWAYS have a periodic table in front of you! Ions – positively or negatively charged atom due to an decrease or increase of electrons Cations – positively charged ( metals that loose electrons) ex. Na +

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Nomenclature!!!

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  1. Nomenclature!!! What’s in a name?

  2. REMEMBER!!! • When naming compounds ALWAYS, ALWAYS have a periodic table in front of you! • Ions – positively or negatively charged atom due to an decrease or increase of electrons • Cations – positively charged ( metals that loose electrons) ex. Na+ • Anion – negatively charged (non-metal that gains electrons) ex. Cl-

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

  4. Quick Review Write the correct formula for the compounds containing the following ions: 1. Na+, S2- a) NaS b) Na2S c) NaS2 2. Al3+, Cl- a) AlCl3 b) AlCl c) Al3Cl 3. Mg2+, N3- a) MgN b) Mg2N3 c) Mg3N2

  5. Naming Binary Ionic Compounds • Binary Ionic Compound • A compound that has 2 atoms • 1 cation and 1 anion • Cation is always first • Two types • Type I • Type II

  6. Naming Binary Ionic Compounds • Type I • The metal only forms 1 type of cation • ex. Li  Li+ • Type 2 • The metal can form 2 or more cations • ex. Cu  Cu+ or Cu2+

  7. Naming Binary Ionic Compounds • How can you tell if it is a Type I or Type II? • Type I: Group 1 and 2, Al, Zn, Cd, and Ag, • Transition metals are almost always Type II

  8. Binary Ionic CompoundsType I Rules for Naming Type I Ionic Compounds • Cation (metal) is named before the anion (non-metal). • Cation (metal) is the name of the element. • Anion (non-metal) is the “root” of the element + ide • Combine the Cation and Anion

  9. Binary Ionic CompoundsType I Ex. NaCl • Cation is named before the anion. • we know that Na is first because it’s a cation • Cation is the name of the element. • Na is Sodium • Anion is the “root” of the element + ide • Cl is Chlorine, root is Chlor + ide = Chloride • Combine the Cation and Anion • Sodium Chloride is the name!!

  10. Lets try one on our own: NaI Ex. NaI • Cation is named before the anion. • we know that Na is first because it’s a cation • Cation is the name of the element. • Na is Sodium • Anion is the “root” of the element + ide • I is Iodine, root is Iod + ide = Iodide • Combine the Cation and Anion • Sodium Iodide is the name!!

  11. Lets try another: CaO Ex. CaO • Cation is named before the anion. • we know that Ca is first because it’s a cation • Cation is the name of the element. • Ca is Calcium • Anion is the “root” of the element + ide • O is Oxygen, root is Ox + ide = Oxide • Combine the Cation and Anion • Calcium Oxide is the name!!

  12. Binary Ionic CompoundsType I • Notice: • The formula doesn’t show the charges of the individual ions. • Ex. NaCl means Na+ is present with Cl- • Ex. CaS means Ca2+ is present with S2-

  13. Let’s try some!! • CsF • AlCl3 • MgI2

  14. Binary Ionic CompoundsType II • Some metals can form more than one ion. • This is what makes them Type II • Ex. Lead(Pb) => Pb2+ or Pb4+ • Ex. Iron(Fe) => Fe2+ or Fe3+ • Transition metals are almost always Type II

  15. Binary Ionic CompoundsType II • To name these we use the same naming method except we add a Roman numeral to the cation name. • The anion stays the same as before. It’s so easy…. even a caveman could do it.

  16. Binary Ionic CompoundsType II (the cation) EXTEMELY IMPORTANT!!! • The Roman numeral tells the charge, not the # of ions present. • Ex. Fe3+ => iron(III) and Fe2+ => iron(II) • Ex. Pb2+ => lead(II) and Pb4+ => lead(IV) You would be wise to remember this.

  17. Binary Ionic CompoundsType II (the anion) • The anion will be named the same way as with Type I (using ide for the ending) • Anion is the “root” of the element + ide • Ex. O is Oxygen, root is Ox + ide = Oxide • Ex. Cl is Chlorine, root is Chlor + ide = Chloride

  18. Binary Ionic CompoundsType II • All together: • FeCl2 => iron(II) chloride • PbO2 => lead(IV) oxide • How do we know it’s iron(II) and not iron(III) • How do we know it’s lead(IV) and not lead(II) • Lets take a closer look.

  19. FeCl2 • We are given FeCl2 • We know the overall charge has to be natural. • We know: • Cl is going to have a 1- charge. • there are 2 Cl • Cl2 has an overall charge of 2- • There is only one Fe atom • Therefore the one Fe has to have a charge of 2+ • Draw out on board iron(II) chloride

  20. PbO2 • We are given PbO2 • We know the overall charge has to be natural. • We know: • O is going to have a 2- charge. • there are 2 O • O2 has an overall charge of 4- • There is only one Pb atom • Therefore the one Pb has to have a charge of 4+ • Draw out on board lead(IV) oxide

  21. Remember!!! • The Roman numeral in a name indicates the charge of the ion, not the subscript in the formula. • Ex. Iron(II) oxide => FeO • Ex. iron(II) chloride => FeCl2

  22. Let’s try some!!! • CuCl • HgO • Fe2O3

  23. Naming Molecular Compounds All are formed from two or more nonmetals. CO2 Carbon dioxide Ionic compounds generally involve a metal and nonmetal (NaCl) BCl3boron trichloride CH4 methane

  24. Binary Covalent Compound Rules for naming: Prefix System • The first atom is the element name. • The second atom is named like an anion. • Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Ex. PCl3 => phosphorus trichloride

  25. Binary Covalent Compound • These are the prefixes that are used to indicate the number of atoms in a compound. • Mono is never used for the first atom.

  26. Binary Covalent Compound:I207 • The first atom is the element name. • I becomes iodine • The second atom is named like an anion. • O is Oxygen, root is ox + ide = oxide • Prefixes are given to each atom to tell the number of atoms present. • di = 2, hepta = 7 • so… di + iodine = diiodine • and… hepta + oxide = heptoxide • Answer: diiodine heptoxide

  27. Binary Covalent Compound:CF4 • The first atom is the element name. • C becomes carbon • The second atom is named like an anion. • F is fluorine, root is fluor + ide = fluoride • Prefixes are given to each atom to tell the number of atoms present. • mono = 1, tetra = 4 • so… mono + carbon = monocarbon • and… tera + fluoride = tetrafluoride • Answer: carbon tetrafluoride • REMEMBER!!! Mono is never used for the first atom.

  28. Let’s try some!!! • BF3 • NO • N2O5

  29. Naming Binary Compounds Review

  30. Review Practice • AsF3 • Al2S3 • SnBr4 • CS2 • CdS • silver chloride • dinitrogen pentaoxide • iron(III) chloride • phosphorus pentaoxide • manganeses(IV) oxide

  31. More Complex Compounds!!

  32. Polyatomic Ions • Polyatomic Ions • Charged entities composed of several atoms bound together • Assigned special names • No system, must be memorized • (don’t worry you don’t have to, just know how to use it) • Ex. CN-, NH4+, NO3-

  33. Polyatomic Ions (pg 109)

  34. Polyatomic IonsOxyanions • Some of these polyatomic ions are called Oxyanions • They contain an atom and different #’s of oxygen atoms. • Ex. NO3-, ClO2-, PO43-

  35. Polyatomic IonsOxyanions • Some of these oxyanions, form in a series. • The smaller # O, ends with ite • The larger # O, ends with ate • Ex. NO2- => nitrite • Ex. NO3- => nitrate

  36. Polyatomic IonsOxyanions • If there are more than 2 then… • The smallest # O, begins with hypo • meaning less than • The largest # O, begins with per • meaning more than • Ex. ClO- => hypochlorite • Ex. ClO4- => perchlorate

  37. Polyatomic IonsOxyanions • All combined • smallest = hypo => ClO- = hypochlorite • Small = ite => ClO2- = chlorite • Large = ate => ClO3- = chlorate • largest = per => ClO4- = perchlorate

  38. Now back to the naming complex compounds • Need to do one thing. • Recognize common polyatomic ions

  39. Now when you see NH4C2H3O2 you can break it down. • NH4- => ammonium • C2H3O2 => acetate • It’s name is ammonium acetate

  40. NH4- => ammonium • C2H3O2+ => acetate • NH4C2H3O2 • Notice that it’s separate parts have a charge but together they are neutral • Just like binary compounds.

  41. Also like Type II, Binary Compounds, you may need Roman numerals • Ex. FeSO4 => iron(II) sulfate • Ex. Mn(OH)2 => manganese(II) hydroxide

  42. FeSO4 • What are the two parts? • We know the overall charge has to be natural. • We know: • SO4 is going to have a 2- charge. • There is only one Fe atom • Therefore the one Fe has to have a charge of 2+ • So the name is iron(II) sulfate • Draw out on board

  43. Mn(OH)2 • What are the two parts? • We know the overall charge has to be natural. • We know: • OH is going to have a 1- charge. • There are 2 OH • (OH)2 has an overall charge of 2- • There is only one Mn atom • Therefore the one Mn has to have a charge of 2+ • So the name is manganese(II) hydroxide

  44. Lets practice some!! • Na2(SO)4 • KH2PO4 • Fe(NO3)3

  45. Naming Acids!!

  46. Acids • Is a molecule with one or more H+ ions attached to an anion. • Translation: • A molecule with H+ and non-metals • Ex. HCl, HCN, H2S

  47. Naming Acids • Two types: • Ones that contain oxygen • Ones without oxygen

  48. Those with oxygen • Start with the root of the anion. • Add the prefix hydro • Add the suffix ic Ex. hydrochloric acid Ex. hydrofluoric acid

  49. HCl • Start with the root of the anion. Cl is chlorine, root => chlor • Add the prefix hydro hydro + chlore = hydrochlore • Add the suffix ic hydrochlore + ic = hydrochloreic Answer: hydrochloreic acid

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