1. Nomenclature Chemical Names & Formulas

2. Introduction to Chemical Bonding §Two types of Bonding l _____________________ - transfer of electrons l _____________________ - sharing of electrons

3. §Bonding takes place at the __________ energy level, ____ and ____ sublevels. §If there are less than half the electrons between the s and p sublevels, the atom will _________ the electrons. §If there are half or more electrons between the s and p sublevels, the atom will __________ electrons.

4. §Know the trends on the periodic table for how many electrons will be gained or lost.

6. Ionic Bonding §Because there is a ____________ of electrons, elements will lose or gain electrons. §If an element loses or gains electrons, it will then become a charged particle - _________. l Positive ion - ________________ l Negative ion - _______________

7. Cations §Substance that has ________ electrons. §The charge is equal to the number of electrons that are transferred. §Ca 2+ - calcium that has transferred two electrons to another substance (anion). §Mg 2+ - magnesium that has transferred two electrons to another substance (anion).

8. Anion §Substance that has ________ electrons. §The charge is equal to the number of electrons that are transferred. §F 1- - fluorine that has accepted one electron from another substance (cation). §O 2- - oxygen that has accepted two electrons from another substance (cation).

9. Ionic Size §______________ is a charged particle. §All atoms are _________________ – the protons and electrons are equal to one another. §The only way an atom becomes a charged particle is if it _______________ or ________________ electrons.

11. Ionic Size §_______________ – positively charged ions l Lost electrons – more _________________ than ______________________ l ____________________ tend to lose electrons §________________ – negatively charged ions l Gained electrons – more _________________ than ______________________ l _______________________ tend to gain electrons

12. Ionic Size - Cations §Cations are ___________ than their parent atoms. l The outermost electron is removed and repulsions are reduced.

13. Ionic Size - Anions §Anions are ___________ than their parent atoms. l Electrons are added and repulsions are increased.

14. §Ions _____________ in size as you go down a column. l Due to increasing value of the energy levels.

15. Ionic Bonding §Ionic bonding is the _______________ or _______________ of electrons. §Metals are _______________. §Nonmetals are _____________. §Hence, ionic bonding will occur between ___________ and _________________.

16. Oxidation Numbers §Possible _______________ on an element. §Any single element, by itself, has a charge of ____________. §An element takes on a charge when put with other elements.

17. Basic Rules of Oxidation Numbers §Group 1 elements are always 1+. §Group 2 elements are always 2+. §Group 3 elements are always 3+ §Group 17 elements will be 1-. §Group 16 elements will be 2-. §Group 15 elements will be 3-.

18. Other Elements §Ag = 1 + §Zn = 2 + Cd = 2 + §Al = 3 + Ga = 3 + In = 3 +

19. Other Elements with Multiple Charges §Cr 2+ and Cr 3+ §Fe 2+ and Fe 3+ §Co 2+ and Co 3+ §Ni 2+ and Ni 3+ §Cu + and Cu 2+ §Sn 2+ and Sn 4+ §Pb 2+ and Pb 4+

20. Writing Formulas from Ions §The total overall charge of a compound is ___________________ §Use subscripts to balance the charge to zero.

21. §Ca 2+ and S 2- l CaS §Na + andCl - l NaCl §Ba 2+ andN 3- l Ba 3 N 2

22. Writing Ions from Compounds §Go with what you know.

23. §MgCl 2 l Mg 2+ andCl - §CuBr 2 l Cu 2+ andBr - §FeCl 3 l Fe 3+ andCl -

24. Polyatomic Ions §Many atomed charged particle that acts as a single unit. §Polyatomic ions have specific names. Use the names. §Common polyatomic ions include: l Nitrate ____________ l Sulfate ____________ l Phosphate ____________ l Carbonate ____________ l Hydroxide ____________ l Chlorate ____________

25. Other Polyatomic Ions §AmmoniumNH 4 + §PermanganateMnO 4 - §BromateBrO 3 - §IodateIO 3 - §AcetateC 2 H 3 O 2 - §ChromateCrO 4 2- §DichromateCr 2 O 7 2-

26. Changing the Oxygen §Per - _____ - ate § _____ - ate § _____ - ite §Hypo - _____ - ite § _____ - ide  Move down – lose 1 oxygen each step  Move up – gain 1 oxygen each step

27. §Ba 2+ andSO 4 2- l BaSO 4 §Na + andClO 3 - l NaClO 3 §Fe 2+ andCO 3 2- l FeCO 3

28. §KNO 3 l K + andNO 3 - §CoSO 4 l Co 2+ andSO 4 2- §LiClO 3 l Li + andClO 3 -

29. More than one of the Polyatomic Ion Needed to Balance the Charge  If more than one of the polyatomic ions is needed to balance the charge, you must use parentheses ( ) around the ion. §Ba(NO 3 ) 2 l Ba 2+ andNO 3 -

30. §Mg 2+ and ClO 3 - l Mg(ClO 3 ) 2 §Fe 3+ and SO 4 2- l Fe 2 (SO 4 ) 3 §Co 3+ and NO 3 - l Co(NO 3 ) 2

31. Naming Ionic Compounds §Binary Ionic Compounds - Types 1 & 2 l A compound that contains a positive ion (______________) and a negative ion (_______________). l Bi- means two l Positive ion is written ___________, negative ion is written ______________ in a chemical formula.

32. Type 1 - Binary Ionic Compound §The cation of a Type 1 has only ________ possible charge. §Name the first element (cation) as is. §Name the second element (anion) as is with an ending of “-ide”. §Example:CaCl 2 l Calcium chloride

33. More Examples: §NaBr- ________________ §MgO- ________________ §KBr- ________________ §BaS- ________________

34. Type 2 - Binary Ionic Compounds §The cation has multiple charges - copper can have a charge of 1+ or 2+. §Determine which charge is being used. Use the anion as the guide. §Name the element as is. §Use a Roman numeral to indicate the charge being used.

35. §Name the anion as is, using an ending of “-ide” as with Type 1 compounds. §Example:CuCl 2 l Copper (II) chloride l MnO 2 - Manganese (IV) oxide l NiO- Nickel (II) oxide

36. Naming Type 1 & 2 with Polyatomic Ions §Form compounds called ______________ compounds - compound that contains atoms of three different elements. §______________________ - many atomed charged particle acting as a single unit. l poly - many l atomic - atom l ion - charged particle

37. Type 1 & 2 Compounds with Polyatomic Ions §N§Name the cation using the rules for Type 1 or Type 2 compounds. §N§Name the polyatomic ion as is - use the name on the chart. §E§Examples: lNlNaNO 3 -______________ lBlBaSO 4 -______________

38. Name these: §LiOH-________________ §Mg(NO 3 ) 2 -________________ §CrCl 3 -________________ §Al 2 O 3 -________________ §CoBr 2 -________________ §Fe 2 O 3 -________________

39. Covalent Bonding §C§Covalent bonding involves the ________________ of electrons between substances. §_§________________ - smallest neutral unit of a substance that still has the properties of the substance. §_§________________ - shows the kinds of numbers of atoms present in a molecule of a compound. §O§Occurs between ________________ and ________________.

40. §Because these are molecules and are covalently bonded, ions are ________________ - there is no transferring of electrons to form ions. §Prefixes are used in naming nonmetal-nonmetal compounds.

41. Prefixes §mono-1 §di--2 §tri--3 §tetra--4 §penta--5 §hexa--6 §hepta--7 §octa--8 §nona--9 §deca--10

42. Prefixes: §Only used for nonmetal-nonmetal compounds. §Mono- is never used on the first element. §Second element always has a prefix.

43. Naming Molecular Compounds §Name the first element as is. If there is more than one of the first element, you must use a prefix. §Name the second element with a prefix to indicate how many atoms there are and add the ending “-ide”. §Example: l CO 2 -carbon dioxide

44. Name these: §N§N 2 O- ____________________ §P§PCl 3 - ____________________ §S§SF 6 - ____________________ §P§P 4 O 6 - ____________________ §S§SO 2 - ____________________ §N§NO 3 - ____________________ §S§SO 4 - ____________________

46. Naming Acids §When dissolved in water, certain molecules produce ____________________ - H+. §These substances are called ____________________. §An acid can be viewed as a molecule with one or more H+ ions attached to an anion. §The rules for naming acids depend on whether the anion contains ____________________.

48. Naming Acids §Identify the compound as being an acid - the first element is hydrogen (two exceptions are H 2 O and H 2 O 2 ) §Find the anion on the chart. §Name the anion. §Following across to the name of the acid. §Name the acid.

49. Naming Acids §If you move up the chart, you ____________________ oxygen. §If you move down the chart, you ____________________ an oxygen. §Start with what you know - usually the -ate group.

50. Examples: §HCl l The chloride ion (anion) is a single element and ends in “- ide”. l It is at the bottom of the chart. l Move across and the name of this acid is hydrochloric acid.

51. §H 3 PO 4 l The anion is phosphate. l Move across to the acids and the name of this acid is phosphoric acid. §H 2 SO 4 l The anion is sulfate. l Move across to the acids and the name of this acid is sulfuric acid.

52. §HClO 2 l Identified as an acid. l The anion is ClO 2 1-, which is one less oxygen than chlorate, ClO 3 1-. l Lose an oxygen, move down the chart. l Move down the chart and the name of the anion is chlorite. l Move across to the acid and the name of this acid is chlorous acid.

53. Name these: §HNO 3 - ________________ §H 2 CO 3 - ________________ §H 2 SO 3 - ________________ §HNO 2 - ________________ §HC 2 H 3 O 2 - ________________ §HClO 4 - ________________

54. Name these Compounds §LiOH ___________________ §CuBr 2 ___________________ §H 2 S ___________________ §Na 2 SO 3 ___________________ §KI ___________________ §CCl 4 ___________________

55. Na 2 SO 4 Cu(ClO 4 ) 2 N 2 O 5

56. MgI 2 Sr(NO 2 ) 2 HgCl 2

57. CaCO 3 PbC 2 O 4 Cr 2 (Cr 2 O 7 ) 3

58. Iron (III) chromate Potassium hydroxide Triphosphorus hexaoxide

59. Potassium thiocyanate Silver nitrate Aluminum sulfite

60. Carbon disulfide Ammonium sulfate Nickel (II) chromate

61. Xenon tetraoxide Phosphorus trihydride Potassium carbonate

62. Disulfur dichloride Lithium oxide Cobalt (III) hydroxide

63. Sodium hydroxide Dinitrogen monoxide Ammonium nitrate