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Chapter 6 Nomenclature of Inorganic Compounds

Chapter 6 Nomenclature of Inorganic Compounds. Objectives: Distinguish between common and systematic names of compounds Review differences between elements and ions Be able to write formula from names of compounds Understand binary compounds Name compounds containing polyatomic ions

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Chapter 6 Nomenclature of Inorganic Compounds

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  1. Chapter 6Nomenclature of Inorganic Compounds Objectives: Distinguish between common and systematic names of compounds Review differences between elements and ions Be able to write formula from names of compounds Understand binary compounds Name compounds containing polyatomic ions Name and recognize acids

  2. Common and Systematic Names • Common Names • Arbitrary • Not based on chemical composition • Historically associated with a physical or chemical property • Not consistent among languages or disciplines • Systematic names • Identify the chemical composition • Devised by IUPAC

  3. Elements and Ions • Diatomic molecules • 2 atoms of same element • H2, O2, N2, F2, Cl2, Br2, I2 • Polyatomic • 3 or more atoms of same element • Sulfur (S8) and Phosphorus(P4) • Ion • Charged particle • Positive (cation) • Negative (anion)

  4. Elements and Ions • Naming cations • Same as element but add the word ion • Potassium ion • Naming anions • Stem of the parent name with ending changed to –ide • Add the word ion • Oxide ion • Commonly formed ions – figure 6.2 pg 107

  5. Writing Formulas from Names of Compounds • Chemical compounds must have a net charge of zero • Compare charges of ions formed from elements • “Trade” charges and rewrite as subscript on opposite ion • Write with lowest possible whole numbers

  6. Writing Formulas from Names of Compounds • Write formulas for • Sodium and chlorine • Aluminum and oxygen Na1+ Cl1- NaCl Al2O3 Al3+ O2-

  7. Writing Formulas from Names of Compounds • Write formulas for the following • Calcium chloride • Calcium will form Ca2+ • Chlorine will form Cl1- • Formula is CaCl2 • Magnesium oxide • Magnesium will form Mg2+ • Oxygen will form O2- • Formula is MgO

  8. Writing Formulas from Names of Compounds • Barium phosphide • Barium will form Ba2+ • Phosphorus will form P3- • Formula is Ba3P2 • Sodium sulfide • Sodium will form Na+ • Sulfur will form S2- • Formula is Na2S

  9. Binary Compounds • Contain only two different elements • Often metal with nonmetal (binary ionic compound)

  10. Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation • Name of cation is left the same • Name of anion is changed (-ide) • Write formulas for the following compounds • Strontium chloride • Strontium is Sr2+ and Chlorine is Cl- • Calcium sulfide • Calcium is Ca2+ and Sulfur is S2- SrCl2 CaS

  11. Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations • Metals in the center of the periodic table • Iron can be Fe2+ or Fe3+ • Stock System • Use Roman Numeral to designate charge of cation • Copper (II) Chloride is CuCl2 • Tin (IV) Oxide is SnO2 • -ous and –ic endings are also sometimes used

  12. Binary Ionic Compounds Containing a Metal That Can Form Two or More Types of Cations • Write the name for each of the following compounds • PbI2 • Fe2O3 • CuO • TiF4 Lead (II) Iodide Iron (III) Oxide Copper (II) Oxide Titanium (IV) Fluoride

  13. Binary Compounds Containing Two Nonmetals • Not ionic bonds - Molecular (covalent) • Different system of naming • Element that occurs first in the series below is written and named first • Si, B, P, H, C, S, I, Br, N, Cl, O, F • Usually given to you…first element listed always named first • Second element retains –ide ending

  14. Binary Compounds Containing Two Nonmetals • Prefix is attached to each element to indicate the number of atoms of that element in the molecule • Mono (1) never used for first element

  15. Binary Compounds Containing Two Nonmetals • Examples: • N2O is dinitrogen monoxide (drop “o”) • S2F10 is disulfur decofluoride • You try: • P2O5 • CBr4 • NH3 Diphosphorus pentoxide Carbon tetrabromide Nitrogen trihydride

  16. Acids Derived from Binary Compounds • Hydrogen compounds – form acids in water • Write symbol of H first, then the rest • Shows it is an acid • Naming • Take stem of nonmetal • Add prefix hydro- • Add suffix –ic • Add the word acid

  17. Acids Derived from Binary Compounds • H2S • Hydrogen sulfide (if not in water) • Hydrosulfuric acid • HCl • Hydrogen chloride (if not in water) • Hydrochloric acid Figure 6.4 on page 115 VERY HELPFUL FOR NAMING BINARY COMPOUNDS

  18. Naming Compounds ContainingPolyatomic Ions • Polyatomic ion • Must be able to recognize common polyatomic ions • Table 6.6 (pg 116)

  19. Naming Compounds ContainingPolyatomic Ions • Usually end in –ate or –ite (but not always) • -ate indicates • -ite indicates • Nitrate is NO3- • Nitrite is NO2- • Hypo- • (if more than two varieties) ClO- hypochlorite ClO2- chlorite ClO3- chlorate ClO4- hyperchlorate or perchlorate

  20. Naming Compounds ContainingPolyatomic Ions • Need to recognize polyatomic ions in Table 6.6 • Hydroxide (OH-) • Cyanide (CN-)

  21. Naming Compounds ContainingPolyatomic Ions • Naming follows binary compound rules

  22. Naming Acids • Oxy-acids • Inorganic compounds containing hydrogen, oxygen, and one other element • Change ending of polyatomic ion • Add the word “acid” • HC2H3O2 • Hydrogen & acetate ion • Acetic acid

  23. Homework • Questions #1,3,6 • Paired Exercises #7-25 odd • Additional Exercise #34 & 36 • Remember: Quiz next class 

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