1. Chapter 9, Naming Chemicals Underlined are WOD

2. The first big use of chemical weapons was during WW1, when chlorine gas was used in Chlorine killed or maimed its victims by burning the lungs; it also caused panic among soldiers who were totally unprepared for gas war.

3. Oddly, although the chemical poisons killed tens of thousands of soldiers, they were of little military consequence because they often drifted back toward the perpetrators. Nonetheless, they caused enough international revulsion to spark the Geneva Protocol of 1925 which banned the use of chemical weapons.

4. What two things do you NEVER mix when cleaning?

5. 1. Bleach 2. Ammonia Why? They release Chlorine Gas!

6. Chlorine is an effective and cheap disinfectant
Chlorine is an effective and cheap disinfectant. It has been used in US water treatment for about hundred years to kill bacteria, like those of typhoid and cholera.

7. REVIEW: Can you identify these on the following periodic table?
Groups
Periods
Metals
Nonmetals
Alkali metals
Common ionic charges
Halogens
Noble gases
Chemical symbols
Names of the first 20 elements
Electron dot structures
Electronegativity values

8. Electronegativity Most Reactive Element Biggest Radius
Least Reactive Element, Smallest Radius
Electronegativity
Most Reactive Element
Biggest Radius

9. Show periodic table b rainpop.

11. Chemical Formulas Shows the kinds and numbers of atoms
Molecular formula = molecules (CO, CO2)
Formula unit = ionic compounds (NaCl)

12. Can a chemical compound be bad?

13. Ban Dihydrogen Monoxide!
Dihydrogen monoxide is colorless, odorless, tasteless, and kills uncounted thousands of people every year. Most of these deaths are caused by accidental inhalation of DHMO, but the dangers of dihydrogen monoxide do not end there. Prolonged exposure to its solid form causes severe tissue damage. Symptoms of DHMO ingestion can include excessive sweating and urination, and possibly a bloated feeling, nausea, vomiting and body electrolyte imbalance. For those who have become dependent, DHMO withdrawal means certain death. Highly addictive, anyone who has ever tasted it had to have it or they died.

15. Show water brainpop.

16. Start Notes

17. Chemical Formulas Shows the kinds and numbers of atoms
Molecular formula = molecules (CO, CO2)
Formula unit = ionic compounds (NaCl)

19. IONIC CHARGES OF REPRESENTATIVE ELEMENTS
Review: Change anion names to end with ide. Chlorine => Chloride ion.
IONIC CHARGES OF REPRESENTATIVE ELEMENTS 1A 1 +1 2A 2 +2 3A 13 +3 4A 14 5A 15 -3 6A 16 -2 7A 17 -1 Li Na K Rb Cs Be Mg Ca Sr Ba Al N P As O S Se F Cl Br I

20. Previous Slide was Representative or A elements
Previous Slide was Representative or A elements. Group B can have different rules than group A elements for naming and making IONS.

21. Start Notes 9.1 Varying charges roman numeral = number of positive charges on the ion These are the ones you need to know!
Copper I and Copper II Cu1+ Cu2+
Iron II , III Fe2+ Fe3+
Tin II , IV Sn2+ Sn4+

22. Common names
Water is a very common chemical compound. The problem is that the name “water” tells you nothing about the structure of a water molecule. Scientists needed a better way to communicate with each other.
Show Ch 9 naming video from Pearson Website.

23. Ionic compounds metal and non-metal ions that attract like magnets and form crystals.
Show model of crystal made from refridgerator magnets.

24. Ionic Compound Names, “How to” 1. Put the cation or metal 1st. 2
Ionic Compound Names, “How to” Put the cation or metal 1st. 2.List the Non-metal 2nd. 3. Use the charge on the non-metal to name the metal’s Roman Numeral.
To the second element, drop the suffix and add –ide (Only use –ide for anions and all binary compounds, ionic or covalent (molecules).)
Chlorine = Chloride
Magnesium chloride

25. Ionic Compound Names 1. Cation (metal) 1st. 2. Anion (Non-metal) 2nd. 3. Add Roman Numeral to B Metal. (Add Rom# when metal is in the B group.)
CuCl (chloride -1)
CuCl (2X chloride -1)

26. How do you find the charge on the metal?
CuCl Copper I chloride
(chloride -1)
CuCl2
(2X chloride -1)

27. How do you find the charge on the metal?
CuCl Copper I chloride
(chloride -1)
CuCl2 Copper II chloride
(2X chloride -1)

28. Examples of B metals names and possible charges: Look at page 266 Remember: Ionic compounds are always a metal and a non-metal that are acting like magnets and form crystals.

29. Polyatomic ions
Are tightly bound groups of atoms that behave as a single ion and carry a charge. They act like a single atom in an ionic bond. They can act like the Copper or Chlorine in the previous slide but MOST ACT LIKE THE NON METAL. They have fooled themselves and the world into thinking they are a single element. They walk like duck, talk like duck, act like duct, sound like a duck, look a duck, but are not a duck.
Polyatomic ions form ionic bonds

30. Polyatomic Ions
groups of atoms that behave as a single ion (in an ionic bond).
See examples on page Table 9.3.
Acetate is the same thing as Ethanonate.
You need to memorize all of them in the Table for the quiz this week: their names, charges, and formulas.
Draw out SO4 from the next slide and show it bonding and then adding 2 electrons. See next slide for answer. Remember Octet Rule

31. Polyatomic ions
Are tightly bound groups of atoms that behave as a unit and carry a charge
Polyatomic ions form ionic bonds

32. These are the polyatomic ions you will need to know p.268
C2H3O2- acetate NH4+ Ammonium
NO2- nitrite CO32- carbonate
NO3- nitrate
CN- cyanide
OH- hydroxide
HSO3- hydrogen sulfite
HSO4- hydrogen sulfate
SO32- sulfite
SO42- sulfate

33. Binary compounds are composed of any combination of two elements
Binary compounds are composed of any combination of two elements. (can be ionic or covalent.)
These are all binary compounds
NaCl, MgO, MgCl2
CH4
CF4
C2H2
NOTE: Not 2 atoms,
But 2 types of elements.

34. How do you know type of bond?
Ionic is Metal and NonMetal; Crystals.
Covalent is 2 non-metals: Molecules.
The rules for naming these 2 are different.

35. Naming binary ionic compounds (metal/nonmetal) (cation first)
MgCl2
Leave the first atoms name alone
Magnesium
To the second element, drop the suffix and add –ide (Only use –ide for anions and all binary compounds, ionic or covalent (molecules).)
Chlorine = Chloride
Magnesium chloride

36. Try these
NaCl
Na2S
Al2O3

37. Try these NaCl = sodium chloride Na2S = sodium sulfide
Al2O3 = aluminum oxide

38. Write the formula
Aluminum sulfide
Calcium oxide
Sodium nitride

39. Write the formula Aluminum sulfide Al2S3 Calcium oxide CaO
Sodium nitride
Na3N

41. With IONIC bonds only. Use smallest atom ratio for formula.
Mg2O2 becomes
MgO Magnesium oxide because it is an ionic bond.
BUT H2O2 stays H2O2 because it is a molecule.

42. The total charge of a compound will always equal ZERO!
MgO Magnesium oxide
Mg3N2 Magnesium nitride
MgCl2 Magnesium chloride

43. Ternary ionic compounds (polyatomic ion)
Contain atoms of three different elements or more
Don’t change either name just put them together. DO NOT USE –ide.
Na+ C2H3O2-
NaC2H3O2
Sodium acetate

44. Try these
NaNO3
NaNO2
Ca(C2H3O2)2

45. Try these NaNO3 NaNO2 Ca(C2H3O2)2 Sodium nitrate Sodium nitrite
Calcium acetate

46. Write formula
Calcium sulfate
Ammonium sulfate
Copper II cyanide

47. Write formula Calcium sulfate CaSO4 Ammonium sulfate (NH4) 2SO4
Copper II cyanide
CuII(CN) 2

48. Review: How do you know type of bond?
Ionic is ___ and ___
Covalent is ___ ___
The rules for naming these 2 are different.

49. Review: How do you know type of bond?
Ionic is Metal and NonMetal (crystal)
Covalent is 2+ non-metals (often gas or liquid)
The rules for naming these 2 are different.

50. Review: -ide -ide: 1.) Change the end of anions to end their name with ide (all negative mono ions). Fluorine becomes Fluoride ion. Iodine becomes Iodide ion. 2.) For all binary compounds (binary only) ionic and covalent, change the second element to end in -ide.

51. ide ending: 1.) monatomic anions 2.) binary compounds

52. naming binary molecular compounds

53. You will use Greek Prefixes to name binary molecular compounds Remember that molecules do not contain metals.

54. Memorize these: Greek Prefixes See pg 281
Number
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10

55. NAMING BINARY COVALENT COMPOUNDS 1st Element: 1
NAMING BINARY COVALENT COMPOUNDS 1st Element: 1.) Add a number prefix to the first element, in a molecule, if there is more than one. Do not put MONO in front of the first element if only one. 2nd Element: 2.)Always add a prefix to the second element in a compound 3.) and change the suffix to –ide.

56. H2O There are 2 H atoms dihydrogen The O has 1 atom monoxide
dihydrogen monoxide H 1p H 1p O 8p

57. SO4 there is only one S there are 4 oxygen atoms listed 2nd
Do not start with Mono.
sulfur
there are 4 oxygen atoms listed 2nd
-Put together tetra oxygen ide
-tetraoxide (optional, some people drop the a to spell as tetroxide.)
sulfur tetraoxide

58. Name these
C2S6
PCl3 NO

59. Name these C2S6 Dicarbon hexasulfide PCl3 phosphorus trichloride NO
Nitrogen Monoxide

60. Write the formula Dinitrogen trioxide Chlorine monofluoride
Carbon tetrachloride

61. Write the formula Dinitrogen trioxide N2O3 Chlorine monofluoride ClF
Carbon tetrachloride
CCl4

62. Naming common acids (ACID = the molecule starts with H)

63. What is an acid. Acid: Proton donor. Produces an positive or H+ ion
What is an acid? Acid: Proton donor. Produces an positive or H+ ion. Base: Proton acceptor or produces a negative or OH- ion. Water: Is it an acid or base? Vote.

64. Water: Is it an acid or base. Answer: Both
Water: Is it an acid or base? Answer: Both. It produces an H+ and OH- H20 => H+ + OH- So some scientist argue it should be named HOH instead of H20.

65. Naming common acids (ACID = the molecule starts with H) Look at the suffix on the anion. -ide hydro-x-ic acid -ite x-ous acid -ate x-ic acid example H2SO4 Sulfuric Acid

66. HCl
H2CO3
HCN

67. HCl = Chloride Ion
-ide hydro-x-ic acid
Hydrochloric acid
H2CO3 = Carbonate becomes
-ate x-ic acid
Carbonic acid
HCN = Cyanide
Hydrocyanic acid

68. sulfurous acid
acetic acid

69. sulfurous acid
-ite x-ous acid
HSO3
acetic acid
-ate x-ic acid
HC2H3O2