1. Naming Chemical Compounds Nomenclature-naming system

2. Naming Ionic Compounds Positive ions are first, then negative ions –Ex: sodium chloride NaCl The metal keeps it’s name The nonmetal gets a suffix of –ide –MgCl 2 –K3P–K3P –Al 2 O 3 –BeS

3. Stock SystemNaming Some metal elements can form two or more cations with a different charge. The stock system denotes the specific ion by putting the charge in ( ). Examples: –Iron (II) has a + 2 charge –Iron (III) has a +3 charge

4. Possible Charges Roman Numeral –I–I –II –III –IV –V–V –VI –VII Charge –+1 –+2 –+3 –+4 –+5 –+6 –+7

5. Practice Write Names for the following: CuSO 4 –Copper (II) Sulfate Fe 2 O 3 –Iron (III) oxide ZnS –Zinc (II) sulfide VCl 4 –Vandium (IV) chloride Co(NO 3 ) 3 –Cobalt (III) Nitrite MnSO 4 –Manganese (II) Sulfate

6. Practice a)Radium chloride b)chromium(II)chloride c)Aluminum phosphate d)copper(I)sulfate e)Magnesium sulfate f)nitric acid g)Sodium oxide http://www.quia.com/jg/65800.html -

7. Compounds containing Polyatomic ions Always put polyatomic ion in parentheses if there are more than 1 of them Example: ammonium chloride –NH 4 Cl Practice Barium Nitrate –Ba(NO 3 ) 2 FeSO 4 –iron (II) sulfate

8. Naming Molecular Compounds Use prefixes when naming simple molecular compounds (memorize these) 1 = mono 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deca

9. Naming Binary Molecular Compounds: Compounds with 2 elements –The least EN Atom goes first C,P,N,H,S,I,Br,Cl,O,F –The first element is given a prefix if it contributes more than one element to the molecule. –The second element: Combine a prefix with the root of that element with -ide at the end. Dioxide, pentoxide This is true for most molecules containing 2 elements –The o or a at the end of a prefix is usually dropped when the name of the element begins with a vowel

10. Practice 1.CO –Carbon Monoxide 2.CO 2 –Carbon Dioxide 3.CCl 4 –Carbon TetraChloride 4.SiF 4 - –Silicon Tetraflouride 5.Nitrogen Monoxide –NO 6.N 2 O 3 –Dinitrogen Trioxide 7.Phosphorus Trichloride –PCl 3

11. Using Chemical Formulas Subscript indicates how many moles of that atom or polyatomic ion are in 1 mole of that compound. KNO 3 Na 2 SO 4 Ca(OH) 2 (NH 4 ) 2 SO 3

12. Using Chemical Formulas Formula mass -sum of all the average atomic masses of all elements in compound. Ex: H 2 SO 4 2 Hydrogen 2 x 1.01 = 2.02 1 Sulfur 1 x 32.07 =32.07 4 Oxygen 4 x 16.00 =64.00 total = 98.09 OR EX: NaCl 1 sodium ion 22.99 1 Chloride ion 35.45 to tal= 58.44

13. Practice (NH 4 ) 3 (PO 4 ) Al 2 O 3 Na 2 O

14. Molar Mass as a Conversion Factor Converting between moles and grams with compounds. –1 st calculate formula mass of given compound. (unit gram/mole) –2 nd convert either by multiplying or dividing by the formula mass moles  grams (x) by formula mass Grams  moles (divide) formula mass

15. Practice What is the mass of 4.5 moles of Ca(CO 3 )? –4.5 x 10 2 g Ca(CO 3 ) What is the mass of 2.0 moles of Na(NO 3 )? –1.7 x 10 2 g Na(NO 3 ) How many moles are contained in 25.0 grams of AgCl? –.174 mol AgCl How many moles are contained in 5.0 grams of ZnCl 2 ? –.037 mol ZnCl 2

16. Percent Composition Gives the percent by molar mass of each element in a compound. 1 st calculate the total molar mass of the compound H 2 SO 4 2 H x 1.01 = 2.02 1 S x 32.07 = 32.07 4 O x 16.00 = 64.00 98.09

17. continued 2 nd Divide each individual atoms mass by the total mass. 3 rd Multiply each by 100 (or move decimal two places to the right) 2 H x 1.01 = 2.01/98.16 = 0.0205 =2.05% 1 S x 32.07 = 32.07/98.16 = 0.327 =32.7% 4 O x 16.00 = 64.00/98.16 = 0.652 =65.2% Check to make sure % adds to 100 (or close to 100) More Practice Pg 244 Practice Problems ZnSO 4 7H 2 O –42.85%

18. Determining Chemical Formulas Empirical formula-symbols of elements in compound showing the smallest whole number ratio. Convert percents of elements in a compound into formula.

19. How to: 1 st change % to grams 2 nd convert grams to moles 3 rd divide each by the least Ex: Determine the formula of a compound made up of the following percents: 32.38 % Na 22.65 % S 44.99 % O

20. Practice problems 1-3 p.247

21. Molecular formulas Actual formula of a molecular compound C 2 H 4 simplifies to CH 2 C 3 H 6 simplifies to CH 2 C 2 H 4 (ethene) and C 3 H 6 (cyclopropane)

22. How the empirical formula relates to the molecular formula: EF = empirical formula MF = molecular formula X( EF) = (MF) 1 st solve for x X= (MF)/(EF) HINT-BIG NUMBER ALWAYS GOES ON TOP Multiply (EF) by x to get the molecular formula

23. Example The empirical formula of a cpd of phosphorus and oxygen was found to be P 2 O 5. the molar mass of this cpd is 283.89g/mol. What is the cpd’s molecular formula?

24. Practice Problems 1-2 p. 249

25. Give the formula for the following: 1. potassium oxide 2. lithium phosphide 3. aluminum chloride 4. calcium bromide 5. iron(II)oxide 6. iron(III)oxide 7. tin(IV)fluoride 8. copper(II)chloride 9. lead (II) sulfide 10. magnesium chloride

26. Determine the molecular formula: 1. Emperical formual = CH, molar mass = 78 g/mole 2. Emperical formula = NO 2, molar mass = 92.02 g/mol 3. Mesitylene has an empirical formula of C 3 H 4. What is the molecular formula(mass 121)?