Chapter 9, Naming Chemicals Underlined are WOD

1. Chapter 9, Naming ChemicalsUnderlined are WOD

2. The first big use of chemical weapons was during WW1, when chlorine gas was used in 1915. 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. Bleach2. AmmoniaWhy?They release Chlorine Gas!

6. 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. 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 REVIEW: Can you identify these on the following periodic table?

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

9. Show periodic table b rainpop.

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

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 9.1.

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

19. Review: Change anion names to end with ide. Chlorine => Chloride ion.

20. 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 9.1Varying chargesroman numeral = number of positive charges on the ionThese 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.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 Names1. 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) • CuCl2 (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 266Remember: 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 268. 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.(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 • Sodium nitrate • NaNO2 • Sodium nitrite • Ca(C2H3O2)2 • 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.