2. What are Compounds? Compound: combination of two or more atoms held together by a chemical bond

3. Three Types of Compounds Metallic: (Metal compounds) metal atoms of a single element bonded together (Li, Au, Ag, Mg) Covalent: compounds formed by sharing electrons between nonmetal atoms. Example: H 2 O, CO 2 Ionic: Compounds made of Ions Metals + Nonmetals NaCl, KBr, Fe 2 (SO 4 ) 3

4. What are ions? An atom or a group of atoms that have charge because of the loss or gain of electrons. Anion: A negative ion (Cl - ) Cation: A positive ion (Na + ) Examples: Na +, Cl -, Ca 2+, O 2-

5. How to predict ion charge Metals lose electrons and have pos. charge Non-metals gain electrons to have neg. charge. Why do they do this? In order to have a stable amount of (8) valence electrons.

6. How to predict ion charge Metals lose electrons and have pos. charge Non-metals gain electrons to have neg. charge. Why do they do this? In order to have a stable amount of (8) valence electrons.

7. Na then has 11p and 10 e - Cl then has 17p and 18 e -

8. Formation of Ionic Compounds Combination of a metal and a non-metal. Electrons are transferred to the non-metal. Both atoms take on the electron configuration of the closest noble gas. –Na + [Ne] and Cl - [Ar] Their charge comes from an imbalance of electrons to protons

9. Predicting Charge +1 +2Transition Metals Varying Positive Charges More than 1 Charge +3 -2-3 0

10. How do ions make ionic compounds? When ions combine to balance out charges. –Anions and cations attract Na + + Cl -  Mg 2+ + O 2-  K + + P 3-  Sr 2+ + Br -  Al 3+ + S 2- 

11. How do ions make ionic compounds? When ions combine to balance out charges. –Anions and cations attract Na + + Cl -  NaCl Mg 2+ + O 2-  MgO K + + P 3-  K 3 P Sr 2+ + Br -  SrBr 2 Al 3+ + S 2-  Al 2 S 3

13. Polyatomic Ions Some Ions are entire molecules (like Phosphate and Ammonium). They have more or less electrons giving the whole molecule a charge. Phosphate PO 4 3- Ammonium NH 4 +

14. They combine using the same method as with Binary compounds However you will need to use (parentheses) if there are more than one Polyatomic Ion. Li + + NO 3 -  K + + PO 3 3-  Mg 2+ + OH -  Al 3+ + SO 4 2- 

15. They combine using the same method as with Binary compounds However you will need to use (parentheses) if there are more than one Polyatomic Ion. Li + + NO 3 -  LiNO 3 K + + PO 3 3-  K 3 PO 3 Mg 2+ + OH -  Mg(OH) 2 Al 3+ + SO 4 2-  Al 2 (SO 4 ) 3

16. Naming Ionic Compounds For binary compounds that are typically in the “s” and “p” blocks: –Give the name of the metal followed by the name of the non-metal with an “ide” ending. BaBr 2 = Na 2 O = AlCl 3 =

17. Naming Ionic Compounds For binary compounds that are typically in the “s” and “p” blocks –Give the name of the metal followed by the name of the non-metal with an “ide” ending. BaBr 2 = Na 2 O = AlCl 3 = N= NitrideP= PhosphideBr=Bromide O= OxideS= SulfideI= Iodide F= FluorideCl= Chloride

18. Naming Ionic Compounds For binary compounds that are typically in the “s” and “p” blocks –Give the name of the metal followed by the name of the non-metal with an “ide” ending. BaBr 2 =Barium Bromide Na 2 O = Sodium Oxide AlCl 3 =Aluminum Chloride N= NitrideP= PhosphideBr=Bromide O= OxideS= SulfideI= Iodide F= FluorideCl= Chloride

19. Naming Ionic Compounds Any type of ion combined with a polyatomic ion: –Follow the same rules above, however… –Do not make any changes to the name of the polyatomic ion. Use the “special sheet” NH 4 Cl = CaSO 4 = AlPO 4 = Ba(NO 3 ) 2 =

20. Naming Ionic Compounds Any type of ion combined with a polyatomic ion: –Follow the same rules above, however… –Do not make any changes to the name of the polyatomic ion. Use the “special sheet” NH 4 Cl =Ammonium Chloride CaSO 4 =Calcium Sulfate AlPO 4 =Aluminum Phosphate Ba(NO 3 ) 2 =Barium Nitrate

21. Naming Ionic Compounds If a metal has more than one charge such as the transition metals (d block) then you need to state the charge using roman numerals. See the “special sheet” Fe 2+ is Iron II Fe 3+ is Iron III Cu + is Copper I Cu 2+ is Copper II Ag+ is Silver –(No Roman Numeral because there is only one charge).

22. Name the following FeCl 2 = FeCl 3 = PbS = PbS 2 = Au(NO 3 ) 3 = ZnO= Cu 3 PO 4 =

23. Name the following FeCl 2 =Iron II Chloride FeCl 3 =Iron III Chloride PbS =Lead II Sulfide PbS 2 =Lead IV Sulfide Au(NO 3 ) 3 =Gold III Nitrate ZnO=Zinc Oxide Cu 3 PO 4 =Copper I Phosphate

24. Name to Formula: Find the charges of the Ions 1 st Magnesium Oxide Sodium Bromide Copper I Chloride Copper II Chloride Lead II Sulfate Gold I Carbonate

25. Name to Formula: Find the charges of the Ions 1 st Magnesium Oxide Sodium Bromide Copper I Chloride Copper II Chloride Lead II Sulfate Gold I Carbonate 1.Find the formula for each ion 2. Write the formula Mg 2+ O 2-

26. Name to Formula: Find the charges of the Ions 1 st Magnesium Oxide=MgO Sodium Bromide=NaBr Copper I Chloride=CuCl Copper II Chloride=CuCl 2 Lead II Sulfate=PbSO 4 Gold I Carbonate=Au 2 CO 3

27. Properties of Ionic Compounds High melting point. Brittle, Solid Crystals at Room Temperature Dissolve in water and form aqueous solutions.Dissolve in water and form aqueous solutions. Aqueous solutions Conduct Electricity Why?

28. Demo with NaCl How do the ions form a structure? How do they balance charge? Discuss Water

29. Sites Dissolving Water Bonds More Dissolving

30. –What is an ionic compound? –List 3-4 rules to name ionic compounds –Name: AuC 2 H 3 O 2, HgF 2 –Formula: Sodium Permanganate, Iron III Phosphide