1. Chemistry Matter and Change
Chapter 7
Ionic Compounds and Metals

2. Previous Ca: 1s22s22p63s23p64s2 Ar: 1s22s22p63s23p6
Draw the valence shell diagrams.
Ca is what element?
Ar is what element?
Compare Ca to Ar:

3. Calcium Argon
Both have 3 full shells of electrons, 1s, 2s and 2p, 3s and 3p.
Calcium has 2 more electrons in the 4s shell.

4. Previous Ca: 1s22s22p63s23p64s2 Ar: 1s22s22p63s23p6
Cl: 1s22s22p63s23p5
What element is Cl? Draw its valence shell diagram.
Compare Cl to Ar:

5. Previous Ca: 1s22s22p63s23p64s2 Ar: 1s22s22p63s23p6
Cl: 1s22s22p63s23p5
What will it take for calcium and chlorine to be like argon?
Why would calcium and chlorine want to be like argon?

6. Previous K: 1s22s22p63s23p64s1 Ar: 1s22s22p63s23p6
Draw the valence shell diagrams.
What element is K?
Compare and contrast:
Why is argon stable?
How can K become “Noble Gas” like?

7. Previous Ca: 1s22s22p63s23p64s2 Ga: 1s22s22p63s23p64s23d104p1
What element is Ga? Draw its valence shell diagram.
Compare and contrast:

8. Important
“Noble Gas Like” means to have a full octet of valence electrons in the s and p orbitals.
The atoms do not become Noble Gases.
Only the atomic number determines the name of the element. The only way to change to another element is nuclear decay, remember the proton and neutrons are in the nucleus not the electrons.

9. 7.1 Ion Formation
How do so many compounds form from the relatively few elements know to exist?

10. Chemical Bond
A chemical bond is the force that holds two atoms together.
One way is an attraction between the electron (-) on one atom and the nucleus of another (+).
Another way is the attraction between ions.

11. Valence Electrons Electrons in the s and p orbitals only Gp 1 2 13 1415 16 17 18

12. Cation Positively charged atom Lose 1 or more electrons
Groups 1, 2 and 13

13. Li1+ Group 1 Li: 1s22s1 or [He] 2s1
The outermost shell has 1 electron.
Remove 1 electron and lithium is like the Noble Gas helium, called lithium cation
Li1+

14. Na1+ Group 1 Na: 1s22s22p63s1 or [Ne]3s1
The outermost shell has 1 electron.
Remove 1 electron and sodium is like the Noble Gas neon, called sodium cation
Na1+

15. K1+ Group 1 K: 1s22s22p63s23p64s1 or [Ar]4s1
The outermost shell has 1 electron.
Remove 1 electron and potassium is like the Noble Gas argon, called potassium cation
K1+

16. Be2+ Group 2 Be: 1s22s12 or [He] 2s2
The outermost shell has 2 electrons.
Remove 2 electrons and beryllium is like the Noble Gas helium
Be2+

17. Mg2+ Group 2 Mg: 1s22s22p63s2 or [Ne]3s2
The outermost shell has 2 electrons.
Remove 2 electrons and magnesium is like the Noble Gas neon
Mg2+

18. Group 2 Write the Noble Gas electron configuration for Ca
Write the ion symbol.

19. Noble Gas Electron Configuration
Ca: [Ar]4s2
Ion Symbol Ca2+

20. B3+ Group 3 B: 1s22s2sp1 or [He] 2s22p1
The outermost shell has 3 electrons.
Remove 3 electrons and boron is like the Noble Gas helium
B3+

21. Group 3 Write the Noble Gas electron configurations for: Al Ga
Write the ion symbols.

22. Cations
Does removal of an electron from a neutral atom require or release energy?

23. Sodium atom Sodium ion

24. Formation of a Cation Notice Requires Energy Notice Smaller Cloud
Why?
Notice
“free” electron

25. Metals
Group 1 and 2 most reactive
Form cations easy

26. Transition Metals Have full s2 orbitals
Lose these 2 electrons and maybe one electron in the d orbital
Sometimes it is difficult to predict how many
Important to write cation symbol
Fe2+ and Fe3+

27. Anion Negatively Charged Ion Gain one or more electrons
Name is changed: __suffex becomes __ide
chlorine  chloride
nitrogen  nitride

28. Flouride F- Group 17 Flourine wants to be neon like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Flouride F-

29. Chloride Cl- Group 17 Chlorine wants to be argon like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Chloride Cl-

30. Bromide Br - Group 17 Bromine wants to be krypton like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Bromide Br -

31. Oxide O2- Group 16 Oxygen wants to be neon like
Has 6 valence electrons and wants 8
Gains 2 electron and has a -2 charge
Oxide O2-

32. Sulfide S2- Group 16 Sulfur wants to be argon like
Has 6 valence electrons and wants 8
Gains 2 electron and has a -2 charge
Sulfide S2-

33. Group 16 Write the Valance Electron Diagram for Selinium, Se
What noble gas does it want to be like?
How many electrons does it need?
Write the name and symbol for the anion.

34. Valence Electron diagram
Wants to be like Krypton, Kr
Needs 2 electrons
Ion Se2-

35. Group 15 Find the number of valence electrons.
What noble gas do these elements want to be like?
Draw the electron dot structure for each.
Name the anion and write its name.
Nitrogen, Phosphorus and Arsenic

36. Fluorine atom Fluoride (ion)

37. Formation of an Anion Notice “free’ electron Notice Energy Released
Smaller cloud
Now
Larger cloud

38. Compare
How do the energy changes accompanying positive ion and negative ion formation compare?

39. Questions p. 209
Compare the stability of a lithium atom with that of its ion, Li+.
Describe two causes of the force of attraction in a chemical bond.
Why are all of the elements in group 18 unreactive, whereas those in group 17 are very reactive?

40. Summarize ionic bond formation by correctly paring these terms: cation, anion, electron gain, electron loss.
Write out the electron configuration for each atom. Then predict the change that must occur in each to achieve a noble-gas configuration.
a. nitrogen b. sulfur c. barium d. lithium

41. 6. Draw models to represent the formation of the positive calcium ion and the negative bromide ion.

42. Fluorine Write out electron configuration
Calculate number of valence electrons
What ion forms? (symbol)
What is the name of the ion?

43. Each Student
Write 5 element symbols on a piece of paper with atomic number 54 or lower.
Switch papers
Write electron configuration for each element
Draw electron dot diagram
Determine what type of ion is most likely formed

44. Exit Ticket
Determine the ions formed for
Strontium
Aluminum
Sulfur