1. Ionic Bond’s Notes /

2. Ch. 4-1: p.p. 114-119 An atom that gains one or more electrons will have a ____________________ charge. An atom that loses one or more electrons will have a ____________________ charge. An atom that gains or loses one or more electrons is called an ____________. A positive ion is called a ______________ and a negative ion is called an _______________. ION “An-Eye-On” “Cat-Eye-On”

3. There are ____ types of bonds: 1.Ionic Bonds – Metals bond with ________ (electrons are taken, not shared) 2. _________ Bonds – Nonmetals bond with _____________ (share electrons) 3. Metallic Bonds – ______ bond with _____ (“positive ions in a sea of electrons” to describe metallic bonding)

5. ______ p 115 An atom or group of atoms that is ___________ _________.

6. What is an ionic _________? Atoms will transfer one or more ________________ to another to form the bond. Each atom is left with a ________________ outer shell. An ionic bond forms between a ___________ ion with a positive charge and a ________________ ion with a negative charge. * Ionic bonds attract ______________ charged ions. (_________ bonded with a ____________)

7. ion 11P - 10E = _____17P - 18E = ______ ____ __

8. - Ionic Bonds More _________ = ___________ Charge (+) whereas _________ Electrons = ____________ Charge (-)

9. - Ionic Bonds

11. ionic bond Na + Cl  Na + Cl - * The ionic bond is ____________.

12. Turn to page 116 and answer the following questions: Q. What is an ionic bond? A:_________________________________ ________________________________. Q. What is the overall charge on an ionic compound? A:_________________________________ ________________________________.

13. _________ ________ Number of ________ an atom _____, _____ or ______when it ____ a chemical bond. Also called ________.

14. Oxidation Number The ________of electrons an _____ will gain OR lose to be _______

15. Let’s complete the chart for each element (see Bonding Basic h/o)…

16. Now let’s complete each ionic bond!

17. Example 3: Sodium + Oxygen Example 4: Sodium + Chlorine Example 5: Calcium + Chlorine Example 6: Aluminum + Chlorine

18. atomic ion p.117 An ion that is made of ______ _____ one atom.

19. polyatomic ion

20. Carbonate ion: CO 3 2- Q. How many carbon atoms? A: ___ carbon atom Q. How many oxygen atoms? A: ___ oxygen atoms Q. What is the overall charge? A. overall charge of _____

22. Naming ionic compounds p.117 The name of the __________ ion comes FIRST The name of the __________ ion comes LAST The __________ ion is __________ the name of the ____________. If the name of the _________ ion is an element, the ______ of its name changes to -ide For example, MgO is… magnesium oxide Look at page 115, Fig. 2 for names of ions. Complete the following in your notes, page 119 #4:

23. Page 119 #4 NaF _________ __________ BeI 2 _________ __________ K 2 SO 4 _________ __________

24. Page 119 #4 CaO __________ H2SH2S MgCo 3 __________

25. _________ p.118 An ________, 3- dimensional ______ of _____ or _____ in a ______.

26. Crystals

27. Crystal ________ Look at Fig. 4 on p.118 What general characteristics of crystals can you observe in the photograph of halite?

28. Crystals have tight, ___________ bonds

29. Look at p.118 Na + Cl  Na + Cl -

30. ___________ of ionic compounds pages 118-119 The characteristic properties of ionic compounds include: 1.__________ ___________ 2.________ melting ________ 3.____________ conductivity

31. __________ Shape

32. High Melting Points Q. Why are ionic bonds so strong? Answer: Every ion is __________ to ions _________ it that have an ___________ ____________. *When exposed to high ________, the particles do ________ away from each ___________.

33. _________ Conductivity Q. Why do ionic compounds dissolve/separate in water?

34. Answer: ________ breaks ions ______, allowing the ions to move __________.

35. Ionic Bonding Activity http://www.learner.org/interactives/periodi c/groups_interactive.html