Dihydrogen Monoxide

1. Dihydrogen Monoxide • contributes to the Greenhouse Effect • may cause severe burns • contributes to the erosion of our natural landscape • accelerates corrosion and rusting of many metals • may cause electrical failures and decreased effectiveness of automobile brakes • has been found in excised tumors of terminal cancer patients Should we ban it?

2. Matching Activity Find your partner!

3. Review Ionic Bonds: metals and non-metals. Covalent bonds: non-metals and non-metals.

4. Ionic Bonds Draw: • Lithium and Fluorine • Oxygen and Sodium Remember: • Ion charge • Arrow showing electron movement If you finish early try making up one!

5. Ionic Lattice

6. Covalent bonds Draw: • Hydrogen and Chlorine • Carbon and Hydrogen Remember: • Overlapping shells • No charges If you finish early try making up one!

7. Molecule

8. Properties of Matter

9. Giving Explanations

10. Which is more reactive? H or He

11. Drawing Bohr Diagrams A) 9 Protons, 9 neutrons Period? Group? B) 12 protons, 13 neutrons Period? Group?

12. Drawing ions A) Period 2, Group 17 B) Period 3, Group 2 Make it stable! Full outer shell!

13. Labs • CaCl2 • CO2

14. Chapter 1-2 Test You will have a chance to re-do up to 3 questions I have circled questions you might want to redo to make the biggest impact on your grade If you want to sign up to redo questions – I must see your review sheet first! The redo questions will be the same topic but different!

15. What am I doing? • Looking at Test • Asking questions • Signing up for redo • Working on crossword • Chembook

16. Discovered vs. Invented Can you invent oxygen? Can you invent radioactivity?

17. Naming Compounds!

18. Learning Objectives I will be able to name ionic compounds and write their formulas I will be able to explain the difference between simple element ions, multivalent metal ions, and polyatomic ions.

19. Get out a piece of paper for practice problems!

20. Why name compounds? Universal language of chemistry! Salt: The International Union of Pure and Applied Chemistry (IUPAC) decides the rules for naming compounds.

21. Formulas and Names Formula • You write the chemical symbols and number of atoms Names • You write the full names of the elements in the compound

22. Ionic compounds Made up of a metal (positive ion) and a non-metal (negative ion). The non-metal “steals” electrons from the metal. One becomes positive, the other becomes negative.

23. The Rules for Naming • The metal (positive ion) comes first • The non-metal (negative) comes second • The non-metal’s name ends with “ide” Go to page 85 of your textbook to fill out the table of ions!

24. Test Yourself! • calcium and fluorine • lithium and nitrogen • potassium and bromine If it is too easy try drawing the ionic bonds between them!

25. Chemical Formulas Chemical formulas contain chemical symbols and subscripts that tell you the number of atoms in the compound. E.g. a) K2S b) Na2O c) Sr3P2

26. Test Yourself! Do question 1 a) to o) on page 86 in your textbook! Questions?

27. Writing formulas Ionic compounds do not have an overall charge. This is because the positive and negative charges cancel each other out.

28. The Rules • Find the charge of each ion • Calculate the total charges needed to balance (0 charge) • Write down how many of each ion you need • Write the chemical symbols and use subscripts if you need Remember: metal first, non-metal second!

29. Example a) zinc nitride b) aluminum chloride

30. Test Yourself Do #1 and #2 on page 87! If you want, use the colored squares to represent charges.

31. The Transition Metals Look at the “middle metals” of your periodic table! What do you notice about their ion charges?

32. Multivalent Metals Multivalent metals: metals that can form more than one ion. These elements have multiple ion charges. Find 3 examples of multivalent metals and their possible charges!

33. Roman Numerals • Fill out the table using pg 88!

34. Test Yourself! I IV III VI II V

35. Roman Numerals • Fe2+ = Iron II “Iron two” • Fe3+= Iron III “Iron three” • Pb4+= Lead IV “Lead four” • Cu+ = Copper I “Copper one”

36. Why Roman Numerals?

37. Writing Multivalent Formulas Same as before! • Find the charge of each ion • Calculate the total charges needed to balance (0 charge) • Write down how many of each ion you need • Write the chemical symbols and use subscripts if you need Remember: metal first, non-metal second!

38. Example iron (III) sulphide

39. Test Yourself Do #1 on page 89!

40. Rules for Writing Names • Find the metal • Check the periodic table to see if it is multivalent • Find the number of atoms • Find the charge of the non-metal(s) and balance it with the metal’s charge • Write the name using a Roman numeral

41. Examples Cu3P MnO2

42. Test Yourself! Do #1 on page 90!

43. Polyatomic Ions Polyatomic ions have a negative or positive charge. Since they are charged they attract ions of the opposite charge. Negative polyatomic ions attract positive ions. Positive polyatomic ions attract negative ions. Polyatomic ions don’t exist on their own, they are always paired with another ion.

44. Writing Polyatomic Formulas Same as before! • Find the charge of each ion • Calculate the total charges needed to balance (0 charge) • Write down how many of each ion you need • Write the chemical symbols and use subscripts if you need Use brackets if there is more than one polyatomic ion!

45. Example Notice that we put the polyatomic ion in brackets so that we know there are 3 OHs: Al(OH)3 DO NOT write: AlOH3 it is a different compound!

46. What if there are no metals? Then put the positive first!

47. Example Use page 92 of your textbook! iron (III) hydroxide ammonium carbonate

48. Naming Polyatomic Compounds Same rules as before, just look up the name of the polyatomic ion!

49. Test Yourself! Do #1 and 2 on page 91!

50. Chapter 1-3 Test Next Tuesday, March 5th Chapter 1.2 – 3.2 Friday – Review Day with Ms. Nickel