2. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid Chemistry Chapter 7

3.  There are 3 forms bonding atoms:  Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)  Covalent—some valence electrons shared between atoms  Metallic– holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

4. 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. Na + + Cl - --> NaCl

5. Predicting Charges on Monatomic Ions OR USE ION CHART +1 +2 -3 -2 -1 0 Cd +2

6.  A metal atom can transfer an electron to a nonmetal.  The resulting cation and anion are attracted to each other by electrostatic forces.

7.  1. Cation first, then anion  2. Monatomic cation = name of the element  Ca 2+ = calcium ion  3. Monatomic anion = root + -ide  Cl  = chloride  4. MAKE A NEUTRAL COMPOUND with subscripts  CaCl 2 = calcium chloride Binary Ionic Compounds:

8.  NaF-  LiCl-  MgO-

9.  NaF-sodium fluoride  LiCl-lithium chloride  MgO-magnesium oxide

10. Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

12. Complete the names of the following binary compounds: Na 3 Psodium ________________ KBrpotassium________________ Al 2 O 3 aluminum ________________ MgS_________________________

13. Write the formula for the ionic compound for barium chloride It forms between Ba 2+ and Cl .

14. Write the formula for 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

15. Li + + N -3 Ca 2+ + I - ----> Li 3 N lithium nitride ----> CaI 2 calcium iodide

16.  How do we know how many atoms of each ion we need?  A simple crossing of the charges can answer that question about 90% of the time.  Example: Mg 2+ and N 3- Mg 3 N 2 Check the charges… 3 x (+2) = +6 2 x (-3) = -6  When they combined they cancel to yield a neutral compound.

17. 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

18. 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

19. Write the correct formula for the compounds : 1. calcium oxide a) CaO b) Ca 2 Oc) CaO 2 2. lithium nitride a) LiN 3 b) LiNc) Li 3 N 3. magnesium phosphide a) MgP b) Mg 2 P 3 c) Mg 3 P 2

20. Write the correct formula for the compounds : 1. calcium oxide a) CaO 2. lithium nitride c) Li 3 N 3. magnesium phosphide c) Mg 3 P 2

21. POLYVALENT: Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. Look at your ion chart…..do you see some?

22. 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

23. The ROMAN NUMERAL is the charge on the metal. If it’s NOT on the ion chart, you can still do the work! tin (IV) = Sn 4+ chromium (VI) = Cr 6+

24. These compounds REQUIRE Roman Numerals because they have metals that can have more than one possible charge: FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ )lead (II) chloride Fe 2 S 3 (Fe 3+ )iron (III) sulfide

25. How can you tell which one it is? FeCl 3 Is it iron (II) or iron(III) (Fe 2+ ) iron (II) chloride (Fe 3+ ) iron (III) chloride Work backwards from anion. Figure out both choices and match OR Inverse criss-cross (only works sometimes)

27. Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron (_____) bromide CuClcopper (_____) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S________________________

28. Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron ( II ) bromide CuClcopper (_____) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S________________________

29. Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron ( II ) bromide CuClcopper ( I ) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S________________________

30. Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron ( II ) bromide CuClcopper ( I ) chloride SnO 2 tin (IV) oxide exception to inverse criss-cross Fe 2 O 3 ________________________ Hg 2 S________________________

31. NO 3 - nitrate ion NO 2 - nitrite ion

32. NH 4 + Cl - ammonium chloride, NH 4 Cl More than one element in the ion! Only one element.

33. NH 4 + Cl - ammonium chloride, NH 4 Cl More than one element in the ion! Only one element. SPECIAL NAME for POLYATOMIC IONS: Can you see them on your ion chart?

34. Writing Formulas SAME:  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 equal to zero, use subscripts to balance charges.

35. 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.  EXACTLY as appear on ion chart.  POLYATOMIC may have subscripts.  If not equal to zero, use subscripts to balance charges.  Use parentheses to show more than one of a particular polyatomic ion.

36. Writing Formulas magnesium phosphate  Write each ion, cation first.  Overall charge must equal zero.  If charges cancel, just write symbols.  EXACTLY as appear on ion chart for polyatomic.  POLYATOMIC may have subscripts.  If not equal to zero: Use parentheses to show more than one of a particular polyatomic ion and use subscripts to balance charges.

37.  How do we know how many atoms of each ion we need?  A simple crossing of the charges can answer that question about 90% of the time.  Example: Mg 2+ and PO 4 3- Mg 3 (PO 4 ) 2 Check the charges… 3 x (+2) = +6 2 x (-3) = -6  When they combined they cancel to yield a neutral compound.

38.  The crossing technique does not work if the magnitude of the charges is the same  Example: Mg 2+ and CO 3 2- Mg 2 (CO 3 ) 2 This is incorrect since we want the lowest ratio possible which is 1:1 to yield MgCO 3

39. Sodium Sulfate Na + and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 –2 (NH 4 ) 2 CO 3

40. Cd(OH) 2 cadmium hydroxide Ca(ClO 2 ) 2 calcium chlorite AgCN silver cyanide Na 2 SO 4 sodium sulfate Na 2 SO 3 sodium sulfite KClO 3 potassium chlorate

41. 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOHb) Fe 3 OHc) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

42. Contains at least 3 elements There MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 sodium nitrate K 2 SO 4 potassium sulfate Al(HCO 3 ) 3 aluminum bicarbonate or aluminum hydrogen carbonate

43. Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2.Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

44. Name the following: 1. Na 2 O 2. CaCO 3 3. PbS 2 4. Sn 3 N 2 5. Cu 3 PO 4 6. HgF 2

45. Write the formula: 1. copper (II) chlorate 2. calcium nitride 3. aluminum carbonate 4. potassium bromide 5. barium fluoride 6. cesium hydroxide

46. 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)

47. A covalent compound is formed by sharing electrons between 2 nonmetals or metalloids. These compounds are usually molecular and are named using a prefix system. When naming these compounds name the element further to the left (in the periodic table) first, then the one on the right.

48. You name the first element using the exact element name. Name the second element by writing the root of the element’s name and add the suffix “–ide.” If there is more than one atom of any given element, you add the Greek prefix denoting how many atoms of that element are present. Use list of Greek prefixes. If only one atom of the second element is present it gets the prefix “mono”, but not for the first element.

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

50. Here are some examples of prefix names for binary molecular compounds. PF 5 phosphorus pentafluoride SO 2 sulfur dioxide SF 6 sulfur hexafluoride N 2 O 4 dinitrogen tetroxide COcarbon monoxide

51.  Prefix System (binary molecular compounds) 1. Add prefixes to indicate # of atoms. 2. Omit mono- prefix on the FIRST element. Mono- must be used on the SECOND element. 3. Change the ending of the second element to -ide. Do the reverse for writing formulas!

52. CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride

53. arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10

54. 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

55. 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

58. Name the following compounds: 1. CaO a) calcium oxideb) calcium(I) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachlorideb) tin(II) chloride c) tin(IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

59. Name the following compounds: 1. CaO 2. SnCl 4 3.N 2 O 3 a) calcium oxide c) tin(IV) chloride b) dinitrogen trioxide

60. 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

61. 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

62.  Acids  Compounds that form H + in water.  Formulas usually begin with ‘H’.  In order to be an acid instead of a gas, binary acids must be aqueous (dissolved in water)  Ternary acids are ALL aqueous  Examples:  HCl (aq) – hydrochloric acid  HNO 3 – nitric acid  H 2 SO 4 – sulfuric acid

63. No Oxygen  w/Oxygen An easy way to remember which goes with which… “In the cafeteria, you ATE something ICky”

65. HBr (aq)HBr (aq) H 2 CO 3H 2 CO 3 H 2 SO 3H 2 SO 3 2 elements, -ide2 elements, -ide 3 elements, -ate3 elements, -ate 3 elements, -ite3 elements, -ite  hydrobromic acid  carbonic acid  sulfurous acid

66. hydrofluoric acidhydrofluoric acid sulfuric acidsulfuric acid nitrous acidnitrous acid 2 elements2 elements 3 elements, -ic3 elements, -ic 3 elements, -ous3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2  H + F-  H + SO 4 2-  H + NO 2 -

67.  HI (aq)  HCl  H 2 SO 3  HNO 3  HIO 4

68.  Hydrobromic acid  Nitrous acid  Carbonic acid  Phosphoric acid  Hydrotelluric acid

69. Nomenclature Summary Flowchart