1. Ch 7 PowerPoint Notes

2. Section Ions
OBJECTIVES:
Determine the number of valence electrons in an atom of a representative element.

3. Section Ions
OBJECTIVES:
Explain how the octet rule applies to atoms of metallic and nonmetallic elements.

4. Describe how cations and anions form.
Section Ions
OBJECTIVES:
Describe how cations and anions form.

5. Why do some elements react to form compounds and others do not
Why do some elements react to form compounds and others do not? Is there any way to predict if atoms might react with each other? Is there any way to predict what chemical formulas might be formed?

6. Ionic and Metallic Bonding
Na 1+, Na +1 or Na+ = cation , missing 1 e-
O2- = anion, gained 2 e-
(the number is the charge on ion, not # of e- gained or lost,, i.e., +1 means 1 electron lost, not 1 gained.)

7. Ion definitions
Valence electrons: Outermost electrons. The s and p electrons in the outer energy level. The highest occupied energy level.
Core electrons: are those in the energy levels below.
Ion: An atom that has lost or gained an electron. Ions have a + or - charge.
(Atoms are always neutral, # of p+ = # of e-)
Cation: Positive Ion or metals, gained e-.
Anion: Negative Ion or non-metals, Lost e-.

8. Valence Electrons are…?
The electrons responsible for the chemical properties of atoms, and are those in the outer energy level.
Valence electrons - The s and p electrons in the outer energy level
the highest occupied energy level
Core electrons – are those in the energy levels below.

9. Keeping Track of Electrons
Atoms in the same column (group)...
Have the same outer electron configuration.
Have the same valence electrons.
The number of valence electrons are easily determined. It is the group number for representative.
Group 2A: Be, Mg, Ca, etc.
have 2 valence electrons
Group 8A, Noble gases has 8.

10. Electron Dot diagrams are…
DEF: Shows the 8 valence electrons as dot pairs around the chemical symbol.
A way of showing & keeping track
of valence electrons.
How to write them?
Write the symbol - it represents the nucleus and inner (core) electrons
Put one dot for each valence electron (8 maximum)
They don’t pair up until they have to (Hund’s rule). Do 4 singles before pairs. X

11. Electron Dot diagrams Single dots can be on any side.

12. Valence e- highest electron energy level of an atom (ns np…where n is the same number) Nitrogen 1s2 2s2 2p Valence e-

13. e- dot structures show only valence e- (single per side/then pair up) 2 dots Mg –[Ne]3s2 3p0

14. Need to Memorize!! EASY!

15. valence e- determine the chemical properties of an element Alkali metals (1 ve-) - ns1 np0

16. Remember s, p, d, f blocks S p 1 2 3 4 5 6 7 1 2 3 4 5 6 7 1S1 1S2
2p1 2p2 2p32p4 2p5 2p6

17. Write the e dot structures O = 1s2 2s2 2p4 Ne = Na =

18. Write the e dot structures O = 1s2 2s2 2p4. Ne = 1s2 2s2 2p6
Write the e dot structures   O = 1s2 2s2 2p4   Ne = 1s2 2s2 2p6   Na = 1s2 2s2 2p6 3s1 3p

19. e dot structures – show valence e- as dots O = 1s2 2s2 2p4
e dot structures – show valence e- as dots   O = 1s2 2s2 2p4   Ne = 1s2 2s2 2p6   Na = 1s2 2s2 2p6 3s1 3p

20. octet rule – ions tend to have pseudo noble gas configuration (8 valence e-) full s and p orbitals

21. Formation of Cations
Metals lose electrons to attain a noble gas configuration.
They make positive ions (cations)
If we look at the electron configuration, it makes sense to lose electrons:
Na 1s22s22p63s1 1 valence electron
Na1+ 1s22s22p6 This is a noble gas configuration with 8 electrons in the outer level.

22. Electron Dots For Cations
Metals will have few valence electrons (usually 3 or less); calcium has only 2 valence electrons Ca

23. Electron Dots For Cations
Metals will have few valence electrons
Metals will lose the valence electrons Ca

24. Electron Dots For Cations
Metals will have few valence electrons
Metals will lose the valence electrons
Forming positive ions
Ca2+
This is named the “calcium ion”.
NO DOTS are now shown for the cation.

25. Electron Configurations: Anions
Nonmetals gain electrons to attain noble gas configuration.
They make negative ions (anions)
S = 1s22s22p63s23p4 = 6 valence electrons
S2- = 1s22s22p63s23p6 = noble gas configuration.
Halide ions are ions from chlorine or other halogens that gain electrons

26. Electron Dots For Anions
Nonmetals will have many valence electrons (usually 5 or more)
They will gain electrons to fill outer shell. 3- P
(This is called the “phosphide ion”, and should show dots)

27. Stable Electron Configurations
All atoms react to try and achieve a noble gas configuration.
Noble gases have 2 s and 6 p electrons.
8 valence electrons = already stable!
This is the octet rule (8 in the outer level is particularly stable). Ar

28. ATOM Na = 1s2 2s2 2p6 3s1 3p0 ION Na+1 = 1s2 2s2 2p6

29. a. What is the charge of an e-. b. What is the e- config for N 3- ion
a. What is the charge of an e-? b. What is the e- config for N 3- ion? c. How many e- does (B) have? d. how many valence e- does (B) have?

30. Common IONIC CHARGES OF REPRESENTATIVE ELEMENTS Add to periodic table
Common IONIC CHARGES OF REPRESENTATIVE ELEMENTS
Add to periodic table 1 +1 2 +2 13 +3 14 15 -3 16 -2 17 -1 Li Na K Rb Cs Be Mg Ca Sr Ba Al N P As O S Se F Cl Br I

31. Why don’t the noble gases form ions?

32. When writing S2-, what does the 2- indicate
When writing S2-, what does the 2- indicate? Does this ion have more or less e than the original atom?

33. Section 7.2 Ionic Bonds and Ionic Compounds
OBJECTIVES:
Explain the electrical charge of an ionic compound.

34. Section 7.2 Ionic Bonds and Ionic Compounds
OBJECTIVES:
Describe three properties of ionic compounds.

35. Ionic Compounds – compounds formed from cations and anions Usually a metal and a nonmetal (the charges always cancel) Na+, Cl- = NaCl

36. Ionic Bonding
Anions and cations are held together by opposite charges (+ and -)
Ionic compounds are called salts.
Simplest ratio of elements in an ionic compound is called the formula unit.
The bond is formed through the transfer of electrons (lose and gain)
Electrons are transferred to achieve noble gas configuration (Octet Rule).

37. Ionic Compounds
Also called SALTS
Made from: a CATION with an ANION (or literally from a metal combining with a nonmetal)

38. Ionic Bonding Na Cl
The metal (sodium) tends to lose its one electron from the outer level.
The nonmetal (chlorine) needs to gain one more to fill its outer level, and will accept the one electron that sodium is going to lose.

39. Ionic Bonding
Na+
Cl -
Note: Remember that NO DOTS are now shown for the cation!

40. Chemical formula = number of atoms in a formula unit of an ionic compound (and not the charges on the ions) Formula unit = NaCl

41. Ionic Bonding
Lets do an example by combining calcium and phosphorus: Ca P
All the electrons must be accounted for, and each atom will have a noble gas configuration (which is stable).

42. Ionic Bonding Ca P

43. Ionic Bonding
Ca2+ P

44. Ionic Bonding
Ca2+ P Ca

45. Ionic Bonding
Ca2+
P 3- Ca

46. Ionic Bonding
Ca2+
P 3- Ca P

47. Ionic Bonding
Ca2+
P 3-
Ca2+ P

48. Ionic Bonding Ca
Ca2+
P 3-
Ca2+ P

49. Ionic Bonding Ca
Ca2+
P 3-
Ca2+ P

50. Ionic Bonding
Ca2+
Ca2+
P 3-
Ca2+
P 3-

51. = Ca3P2 Ionic Bonding Formula Unit
This is a chemical formula, which shows the kinds and numbers of atoms in the smallest representative particle of the substance.
For an ionic compound, the smallest representative particle is called a: Formula Unit

52. Chemical formula = number of atoms in a formula unit of an ionic compound (and not the charges on the ions) Formula unit = NaCl

53. Ionic compounds are usually brittle solids at room temperature, with repeating internal 3-D crystal patterns, that have high melting points

54. Ionic bonds – electrostatic force that holds compound together

55. What number of each ion do you need to make an ionic compound
What number of each ion do you need to make an ionic compound? Na, F Na, S Al, N

56. What number of each ion do you need to make an ionic compound. Na, F
What number of each ion do you need to make an ionic compound? Na, F NaF Na, S Na2S Al, N AlN

57. Metal bonds valence electrons of metal atoms can be modeled as a sea of electrons Metallic bonds = free-floating valence electrons attracted to the positively charged metal ions

58. Alloys are mixtures composed of two or more elements, at least one of which is a metal

59. Quick review questions
Can have everyone stand up and answers following q’s to sit down.

60. An ionic compound is usually formed between a metal and a __?

61. How many dots around a sodium atom?

62. How many dots around a sodium atom?

63. What is the charge on a sodium atom?

64. What is the charge on a sodium ion?

65. What are some ionic compounds formed with sodium?

66. What is the charge on an aluminum ion?

67. What are some ionic compounds formed with Aluminum?