1. Entry Task: Nov 5-6 th Block 2 Provide the name and formula for the following: MgP and Lithium nitride

2. Agenda: Sign off on Binary compounds 1 ws Notes Formula mass, # of elements and compounds HW: Formula mass and elements ws

3. I can… Create binary ionic formulas Count the # of elements in a compound. Check my formula with the given formula mass Describe the properties of ionic substances

4. Clear off Desks HAVE OUT: Binary compound ws Periodic table Writing utensil CALCULATOR

6. Ion Formation Review Provide the ions for the following atoms. Al____Si_____S_____ Cu(II)_____P_____Mn(V)____ Na____F_____Pb(IV)____ Cd(II)____Rb_____O______ Ca_____Cl_____Ag(I)_____ Al +3 Si +4 S -2 Cu +2 P -3 Mn +5 Na +1 F -1 Pb +4 Cd +2 Rb +1 O -2 Ca +2 Cl -1 Ag +1

7. Ion Formation Review Provide the ions for the following atoms. Se____K____Ba____ N_____In____Sr_____ I_____Au(III)_____Br_____ Te_____V(VI)_____Be_____ F_____Mg____Li_____ Bi(III)____Sc (II)_____Cs______ Se -2 K +1 Ba +2 N -3 In +3 Sr +2 I -1 Au +3 Br -1 Te -2 V +6 Be +2 F -1 Mg +2 Li +1 Bi +3 Sc +2 Cs +1

8. Ionic Bonding Basics Describe what happens to the electrons (cation/anion) when an ionic compound is formed. What type of elements are involved? What is the point of ionic bonding? Cations transfer their valence electron(s) to the anion. Metals and nonmetals The cation gives up its ve- to drop to a filled orbit and the anion gets the ve- to fill it orbit to be stable.

9. F/Mg Na/Ca Cs/F As/Sr O/N O/Ba Mg/Fr Ionic Bonding Determine if the following will form ionic compounds? If yes, write the correct ionic formula. Mg +2 F -1 MgF 2 Na +1 Ca +2 NO formula Cs +1 F -1 CsF Sr +2 As -3 Sr 3 As 2 O -2 N -3 No Formula Ba +2 O -2 BaO Mg +2 Fr +1 No Formula

10. Li/Cl At/Rb S/K N/Fe(II) Se/Be Br/Cs Ne/Ca Cl/S Ionic Bonding Determine if the following will form ionic compounds? If yes, write the correct ionic formula. Li +1 Cl -1 LiCl At -1 Rb +1 RbAt K +1 S -2 K2SK2S Fe +2 N -3 Fe 3 N 2 Be +2 Se -2 BeSe Cs +1 Br -1 CsBr Ne Ca +2 No Formula Cl -1 S -2 No Formula

11. 1. ZnCl 2 2. MgF 2 3. FeO 4. CoCl 2 5. VCl 5 6. AgCl 7. PbS Cl -1 (2) = -2 F -1 (2) = -2 Iron II oxide Cobalt II chloride Vanadium V chloride Silver I chloride Lead II sulfide Zinc II chloride Magnesium fluoride Zn = +2 Mg = +2 O -2 (1) = -2 Fe = +2 Cl -1 (2) = -2 Co = +2 Cl -1 (5) = -5 V = +5 Cl -1 (1) = -1 Ag = +1 S -2 (1) = -2Pb = +2

12. 11. MnO 2 12. NiCl 3 13. V 4 C 5 14. FeN 15. Co 2 S 3 Mn = +4 Nickel III chloride Vanadium V carbide Cobalt III sulfide Iron III nitride Iron III sulfide Aluminum oxide Gallium bromide 8. Fe 2 S 3 9. Al 2 O 3 10. GaBr 3 S -2 (3) = -6 Fe = +6/ (2)= +3 O -2 (3) = -6 Al = +3 (2)= +6 Br -1 (3) = -3 Ga = +3 O -2 (2) = -4 Manganese IV oxide Cl -1 (3) = -3 Ni = +3 C -4 (5) = -20 V = +20/4 = +5 N -3 (1) = -3 Fe = +3 S -2 (3) = -6 Co = +6/2 = +3

13. 16. Barium nitride 17. Nickel (II) iodide 18. Iron (II) sulfide 19. Chromium (III) chloride 20. Copper (I) oxide 21. Manganese (IV) nitride 22. Iron (III) sulfide 23. Germanium arsenide = Ba 3 N 2 = NiI 2 = FeS = CrCl 3 = Cu 2 O = Mn 3 N 4 = Fe 2 S 3 Ba = +2 N = -3 Ni = +2 I = -1 Fe = +2S = -2 Cr = +3Cl = -1 Cu = +1 O= -2 Mn = +4 N= -3 Fe = +3 S= -2 = Ge 3 As 4 Ge = +4 As= -3

14. 24. Zinc (II) oxide 25. Aluminum oxide = ZnO = Al 2 O 3 26. Cobalt (II) fluoride 27. Zinc (II) carbide 28. Nickel (III) selenide 29. Manganese (IV) arsenide 30. Copper (II) bromide Zn= +2 O = -2 Al = +3 O= -2 = CoF 2 = Zn 2 C = Ni 2 Se 3 = Mn 3 As 4 = CuBr 2 Co = +2 F = -1 Zn = +2 C= -4 Ni = +3 Se= -2 Mn = +4 As= -3 Cu = +2 Br= -1

15. Clear OFF Desk! I’ll provide a periodic Table for the Quiz

17. Properties of Ionic Compound 1. Ions are packed together tightly alternating positive and negative charges in a crystal lattice.

18. What effect does a strong bond have on boiling and melting points of a chemical compound? 2. Ionic Compounds have HIGH boiling points and have HIGH melting points

19. What happens when an ionic compound is placed in water? 3. The ions (cation/anion) separate in water because water is polar (having +/-) ends and ions are +/-.

20. Summary of Ionic Substances High melting/boiling point Dissolves in water Conduct electricity Solids at room temperature (think salt) Brittle – NOT malleable

21. Energy and Ionic Compounds WHY do Ionic compounds have these properties? 5. Ionic bonds are STRONG due to the repeated positive-negative lattice pattern.

23. Polyatomic ions Polyatomic ions: it’s a group of atoms that are covalently bonded that carry a charge and are dealt with just like monatomic ions. FLIP your Periodic Table Over- Use your common ion sheet to provide the formula and charge of the following polyatomic ions. Chloride________Nitride________ Chlorite ________Nitrite________ Chlorate________Nitrate________ Cl -1 ClO 2 -1 ClO 3 -1 N -3 NO 2 -1 NO 3 -1

24. Polyatomic ions Polyatomic ions: it’s a group of atoms that are covalently bonded that carry a charge and are dealt with just like monatomic ions. FLIP your Periodic Table Over- Use your common ion sheet to provide the formula and charge of the following polyatomic ions. Phosphide________Sulfide _________ Phosphite________Sulfite__________ Phosphate________Sulfate__________ P -3 PO 3 -3 PO 4 -3 S -2 SO 3 -2 SO 4 -2

25. Polyatomic ions What is the difference between –ites and –ate endings? What is up with Hydronium and Ammonium ion? acetatecarbonate cyanide dichromate borate hydroxide permanganateselenite Ions with –ites and –ates have oxygen's attached. The –ites have less oxygen compared to –ates. Hydronium (H 3 O + ) and ammonium (NH 4 + ) ions are positive polyatomic ions. C 2 H 3 O 2 -1 CN -1 BO 3 -3 MnO 4 -1 CO 3 -2 Cr 2 O 7 -2 OH -1 SeO 3 -2

26. When bonding with other ions, more than 1 polyatomic ion maybe needed to balance the charge. 2 chlorate ions 3 hydroxide ions 2 ammonium ions (ClO 3 ) 2 (OH) 3 (NH 4 ) 2 There are no charges because they bonded.

27. When dealing with polyatomic ions, treat them just like monatomic ions K +1 Potassium nitrate NO 3 –1 KNO 3 Barium sulfate Ba +2 SO 4 –2 BaSO 4 PO 4 –3 Iron III phosphate Fe +3 FePO 4

28. When dealing with polyatomic ions, treat them just like monatomic ions NaCN Sodium cyanide Ag 2 SO 3 Silver I Sulfite CuNO 2 Copper I nitrite

29. Use ( ) to group polyatomic ions Al 2 (SO 3 ) 3 Aluminum sulfite Ba(NO 2 ) 2 Barium nitrite Cu 3 (PO 4 ) 2 PO 4 -3 -6 Cu +? +6 Cu +2 Copper II phosphate

30. In-Class for credit!!

31. Polyatomic ions- Practice Silver Oxid e O -2 Ag +1 Ag 2 O K +1 CO 3 -2 K 2 CO 3 Potassium Carbonate Lithium Li +1 Sulfate SO 4 -2 Lithium sulfate Sodium Na +1 Bromide Br -1 NaBr

32. Polyatomic ions- Practice