2. Types of Compounds Chapter 5

3. Objectives 5.1 5.1 Apply ionic charge to writing formulas 5.1 Apply formulas to name ionic compounds 5.1 Interpret the information in a chemical formula

4. Ionic “Bonds” Instead of Formula’s: Ratio’s Some atom’s want more electrons than the other wants to give up So they bind to two, or three Example: Li and O, Li wants to give up only 1 electron, but O wants 2 electrons

5. Practice Question What ratio of Mg and N are needed to make an Ionic compound that has a neutral charge? –Draw a Lewis electron dot diagram for N –Draw a Lewis electron dot diagram for Mg What ratio of Na and Br are needed to make an Ionic compound that has a neutral charge?

6. +1+2General Ionic Charges-2-3

8. Ionic Nomenclature Only use Ionic Nomenclature when dealing with Ionic compounds –A–An ionic compound is formed when a metal and a non metal come together and electrons are completely lost and gained

9. Fixed Oxidation State Some Metals will always lose the same amount of electrons. These metals have Fixed Oxidation States Alkali Metals = +1 Alkaline Earth Metals = +2 Aluminum = +3

10. Ionic Nomenclature Binary Compounds of Metals with Fixed Charges: Given Formula, Write the Name The order for names in a binary compound is first the cation, then the anion. Use the name of cation with a fixed oxidation state directly from the periodic table. The name of the anion will be made from the root of the element's name plus the suffix "-ide."

11. Practice Naming What is the name of the following? MgO Magnesium Oxide NaF Sodium Flouride CaS Calcium Sulfide

12. Ionic Nomenclature Given Name, Write Formula The order in a formula is first the cation, then the anion. You must know the charges associated with each cation and anion. The sum of the positive charge and the sum of the negative charges MUST add up to zero. You MAY NOT adjust the charges of the cations or anions to get a total charge of zero. You MAY adjust the subscripts to get a total charge of zero.

13. CATION + ANION ---> COMPOUND COMPOUND CATION + ANION ---> COMPOUND COMPOUND A neutral compound requires equal number of + equal number of + and - charges. A neutral compound requires equal number of + equal number of + and - charges. COMPOUNDS FORMED FROM IONS Na + + Cl - --> NaCl

14. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions     – Na  +  F :  Na + : F :  NaF     sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

15. Hint Cross the charges to find the amount you need. If it can be reduced, then do so –Ie if both are 2, then it is 1

16. Ionic Nomenclature What is the formula of the following? Potassium Oxide K 2 O Strontium Chloride SrCl 2 Magnesium Nitride Mg 3 N 2

17. Ionic Nomenclature Potassium Phosphide K 3 P Magnesium Sulfide MgS Radium Flouride RaF 2

18. Variable Charges The transition metals have variable charges, they are happy with losing a variety of electrons –This is because they can also lose some of there D electrons and be stable

19. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu +, Cu 2+ Fe 2+, Fe 3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

20. Variable Charges Formula to Name 1) Find the charge of the cation by –F–Finding total charge of anion and dividing by number of cations Example: FeCl 3 –W–We have 3 Chlorines, each has a -1 charge –T–The Fe needs to be +3 to balance it out 2) Say the cation with its Roman Numeral –I–Iron (III) Chloride

21. Variable Charges What is the name? AuF 3 Gold (III) Flouride AgF Silver (I) Flouride PbO 2 Lead (IV) Oxide

22. Variable Charges SnF 2 Tin (II) Flouride MnO 2 Manganese (IV) Oxide CrN Chromium (III) Nitride Sn 3 N 4 Tin (IV) Nitride

23. Variable Charges Name to Formula The Roman Numeral tells you the charge Balance the formula Iron (III) Oxide –F–Fe has a +3 charge as denoted by the III –O–Oxygen always has a -2 charge –C–Cross them (Balance) –F–Fe 2 O 3

24. Variable Charge What’s the formula? Lead (IV) Sulfide PbS 2 Copper (I) Chloride CuCl Silver (I) Nitride Ag 3 N

25. Variable Charge Gold (III) Arsenide AuAs Tin (II) Bromide SnBr 2 Cobalt (III) Oxide Co 2 O 3

26. Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl . Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl  Cl  3. Write the number of ions needed as subscripts BaCl 2

27. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 Sc) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

28. Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

29. Naming Compounds 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl  = chloride CaCl 2 = calcium chloride Binary Ionic Compounds:

30. Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

31. Learning Check Complete the names of the following binary compounds: Na 3 Nsodium ________________ KBrpotassium________________ Al 2 O 3 aluminum ________________ MgS_________________________

32. Mixed Review Given the name, write the formula Given the formula, write the name 1) Sodium Oxide 2) Lead (II) Nitride 3) Cesium Iodide 4) RbF 5) AuO

33. Mixed Review 6) SrCl 2 7) CoS 8) Ag 2 Se 9) Manganese (IV) Chloride 10) Radium Nitride

34. Answers to Review 1) Na 2 O 2) Pb 3 N 2 3) CsI 4) Rubidium Flouride 5) Gold (II) Oxide

35. Answers to Review 6) Strontium Chloride 7) Cobalt (II) Sulfide 8) Silver (I) Selenide 9) MnCl 4 10) Ra 3 N 2

36. Objectives 5.2 5.2 Apply organic nomenclature to name hydrocarbons 5.2 Distinguish among allotropes of an element. 5.2 Apply formulas to name molecular compounds

37. Naming Molecular Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl)

38. Molecular (Covalent) Nomenclature for two nonmetals Prefix System (binary compounds) 1.Less electronegative atom comes first. 2.Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3.Change the ending of the second element to -ide.

39. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

40. CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride Molecular Nomenclature: Examples

41. arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10 More Molecular Examples

42. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon _______________ PCl 3 phosphorus _______chloride CCl 4 carbon ________chloride N 2 O_____nitrogen _____oxide

43. Learning Check 1.P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2.Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

44. A flow chart for naming binary compounds.

45. Mixed Practice 1.Dinitrogen monoxide 2.Potassium sulfide 3.Copper (II) nitrate 4.Dichlorine heptoxide 5.Chromium (III) sulfate 6.Iron (III) sulfite 7.Calcium oxide 8.Barium carbonate 9.Iodine monochloride

46. Mixed Practice 1.BaI 2 2.P 4 S 3 3.Ca(OH) 2 4.FeCO 3 5.Na 2 Cr 2 O 7 6.I 2 O 5 7.Cu(ClO 4 ) 2 8.CS 2 9.B 2 Cl 4

47. NO 3 - nitrate ion NO 2 - nitrite ion Polyatomic Ions

48. You can make additional polyatomic ions by adding a H + to the ion! CO 3 -2 is carbonate HCO 3 – is hydrogen carbonate H 2 PO 4 – is dihydrogen phosphate HSO 4 – is hydrogen sulfate Polyatomic Ions

49. Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don’t show charges in the final formula. Overall charge must equal zero. –If charges cancel, just write symbols. –If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion. Use Roman numerals indicate the ion’s charge when needed (stock system)

50. Monatomic Ions

51. Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

52. Diatomic Elements Dr. HOFBrINCl These elements are found naturally as two elements and do NOT use a prefix O 2 is Oxygen, not DiOxygen

53. Allotropes Molecules of a single element that different in molecular structure or crystalline structure –Oxygen and Ozone –Diamond, Graphite, Charcoal, Fullerenes, Acetylenic

54. Hydrocarbons Composed of Carbon Chain and hydrogens (functional groups discussed later) MethaneHexane EthaneHeptane PropaneOctane ButaneNonane PentaneDecane