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Mastering Nomenclature: Naming Ionic and Molecular Compounds

Understanding the rules of nomenclature is essential for accurately naming compounds. Always refer to the periodic table while working. Learn the classification of ions which includes cations (positively charged) and anions (negatively charged). This guide covers naming binary ionic compounds, distinguishing between Type I and Type II metals, and proper use of Roman numerals. We’ll also explore how to name molecular compounds formed from nonmetals. Mastery of these concepts is crucial for chemistry students and can simplify your learning process!

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Mastering Nomenclature: Naming Ionic and Molecular Compounds

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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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