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Ionic Compound Nomenclature. Binary Ionic Compounds Nomenclature w/ oxidation numbers 1.The name of the cation (metal) is first. It will have its entire.

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Presentation on theme: "Ionic Compound Nomenclature. Binary Ionic Compounds Nomenclature w/ oxidation numbers 1.The name of the cation (metal) is first. It will have its entire."— Presentation transcript:

1 Ionic Compound Nomenclature

2 Binary Ionic Compounds Nomenclature w/ oxidation numbers 1.The name of the cation (metal) is first. It will have its entire element name. 2.The anion (nonmetal) will have its element name with its –ide ending For example NaCl Sodium chloride

3 Try these examples 1.ZnS 2.KCl 3.BaO 4.AlF 3 5.CaO 1.Zinc Sulfide 2.Potassium Chloride 3.Barium Oxide 4.Aluminum Fluoride 5.Calcium Oxide

4 Oxidation Numbers Group 1 (IA)+1 Group 2 (IIA)+2 Group 13 (IIIA)+3 Group 14 (IVA)±4 Group 15 (VA)-3 Group 16 (VIA)-2 Group 17 (VIIA)-1

5 Criss Cross/Swap & Drop Method 1.Write the symbol and charge for each element. 2.The anion’s charge becomes the # of cations 3.The cation’s charge becomes the # of anions 4.Reduce if necessary. (if there is a common factor)

6 For example Calcium chloride Ca 2+ Cl 1- cation anion CaCl 2

7 For example Barium sulfide Ba 2+ S 2- cation anion Ba 2 S 2 Reduce. BaS

8 Example potassium chloride K 1+ Cl 1- cation anion The charge of your anion = the # of cations K 1 The charge of your cation = the # of anions Cl 1 Reduce if necessary KCl

9 Try these examples 1.Lithium oxide 2.Potassium sulfide 3.Sodium iodide 4.Magnesium Nitride 5.Rubidium Phosphide

10 Writing Formulas without Oxidation Numbers

11 The charge of transition metals will be given in parenthesis. Iron (III) oxide Fe 3+ O 2- Use the criss cross method. Fe 2 O 3

12 Try these examples 1.Copper (II) iodide 2.Tin (II) chloride 3.Tin (IV) oxide 4.Chromium (VI) sulfide

13 Naming Binary Ionic Compounds without oxidation numbers

14 * Use your reference sheet to determine ions of different transition metals. 1.The cation (metal) will have its entire name with its charge in parentheses. 2.The anion will have its element name with its –ide ending. 3.You will need to reverse the criss cross method to find the cations charge.

15 Example CoI 2 Cobalt (?) iodide Use the criss cross method in reverse. Write the element symbols with their subscripts and the charge of the anion. Co X 1 I 1- 2 Set up an equation equal to zero using the charges and number of each element. The charge of the cation is x (unknown). Then solve for x. 1(x) + (1-)(2) = 0 1x - 2=0 X= 2+

16 Try these examples 1.Cu 2 Se 2.FeS 3.SnO 2 Copper (I) selenide Iron (II) sulfide Tin (IV) oxide

17 Tertiary Ionic Compound Nomenclature

18 Tertiary Ionic Compounds Composed of – positively charged Polyatomic ion + nonmetal (anion) –Metal (cation) + negatively charged polyatomic ion –Two polyatomic ions (one positive and one negative charge)

19 Writing Formulas with oxidation #s 1.Write symbol and charge for each element or polyatomic ion 2.Use the crisscross method. 3.Polyatomic ions must remain in parenthesis with the amount written outside as a subscript. i.e. 2 nitrate ions(NO 3 ) 2

20 Try these examples 1.Magnesium hydroxide 2.Potassium sulfate

21 Naming Must be able to recognize polyatomic ions. 1.Name the cation and (-) charge poly ion 2.Name the (+)polyatomic ion and name the anion. 3.Name both polyatomic ion.

22 Example 1.CaCr 2 O 4 2.KClO 3 Calcium dichromate Potassium chlorate

23 Naming Formulas without Oxidation Numbers Must include charge of the cation (transition metal). Will only include the tertiary ionic compounds with a cation (transition metal) and polyatomic ion. 1.Name the cation with its charge. May require using the criss cross method reversed. 2.Name the polyatomic ion.

24 Example: Sn 3 (PO 4 ) 2 1.The charge of your cation is the number of anions. Or Sn X 3 (PO 4 ) x + (3-)(2)=0 3x-6=0 3x=6 X=2+ Tin (II) phosphate

25 Try this One: 1.Pb(C 2 H 3 O 2 ) 2 Lead (II) acetate

26 Writing Formulas Without Oxidation Numbers 1.Write elements or polyatomic ions with charges 2.Use the criss cross method Chromium (III) nitrate Cr 3+ NO 3 1- Cr(NO 3 ) 3 (3+)(1) + (1-)(3)=0

27 Try these examples 1.Mercury (II) hydroxide 2.Iron (III) chlorate Hg(OH) 2 Fe(ClO 3 ) 3


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