1. Chapter 7 Ionic and Metallic Bonding
Mr. Samaniego
Lawndale High School

2. Section Ions
When Mendeleev arranged his periodic table according to properties, he didn’t know that it was also due to the number of bonding electrons
The reason that certain elements were grouped together was because they have the same number of valence electrons
Valence Electrons – electrons in the highest occupied energy level of an atom
To find the valence electrons in an atom of the representative element, simply look at the group number

3. He
2 e-

4. Determine the Valence electrons in each of these elements
K Be
P Li
C He
O 9. Ne
N B

5. Electron Dot Structure
A diagram that shows valence electrons as dots around the element symbol
PRACTICE
1. K 6. Be
2. P 7. Li
3. C 8. He
4. O 9. Ne
5. N B

6. Valence Electrons
The reason that valence electrons are so important is that they are the only electrons involved in bonding

7. Octet Rule
Remember that all atoms want to be like the noble gases because their s and p orbitals are completely filled, which makes them unreactive and stable
The Octet Rule states that all atoms want 8 electrons in their valence shells, just like the noble gases (except He)

8. Satisfying the Octet Rule
In forming compounds, atoms want to achieve a noble gas configuration
In order for atoms to combine together to obtain 8 valence electrons, they transfer electrons (either gain or lose electrons)

9. Some atoms will gain electrons, while other atoms will lose electrons
Filling Order: 1s 2s 2p 3s 3p 4s 3d 4p
Draw the orbital diagram for Sodium
Draw the orbital diagram for Magnesium
Draw the orbital diagram for Fluorine
Draw the orbital diagram for Oxygen

10. Cation versus Anion
Remember that atoms are electrically neutral because they have the same number of protons and electrons

11. How are electrons transferred?
Metals lose valence electrons
Nonmetals gain valence electrons

12. Bonding
Once an atom has a stable octet, it is happy and does not want to react anymore
Atoms without stable octets are sad and want to react with other atoms to achieve a stable octet
Why don’t noble gases want to form bonds?

13. How do atoms become more stable and less reactive?
Why do atoms form bonds? 1. To have a full octet 2. To be more stable 3. To be less reactive
How do atoms become more stable and less reactive?
By having completely filled s and p
orbitals just like the noble gases

14. Charges on the Periodic Table

15. Practice What are the charges on the following elements? Calcium
Oxygen
Chlorine
Hydrogen
Cesium
Helium
Krypton
Aluminum

16. Section 7.2 – Ionic Bonds
Ionic Compounds are METAL cations and NONMETAL anions held together by electrostatic forces
Ionic compounds are formed through transferring or exchanging electrons

17. Example…
Sodium Chloride (Salt, NaCl) is an example of an ionic compound

18. Practice Which of the following are ionic compounds? LiCl NaS C2H4
MgBr2
H2O
SiC
Rb3P
CsI

19. Ionic Charges
Although they are composed of positive and negative charges, ionic compounds are overall electrically neutral because their charges will cancel out
For example…
Na+1 will bond with Cl-1
Mg2+ will bond with O2-
Al3+ will bond with N3-
Two K+1 can also bond with One S2-

20. Writing Chemical Formulas
Al2S3
The numbers on top are the charges, while the numbers on the bottom tell how many atoms there are

21. Practice Li+1 Ca2+ Al3+ N3- S2- Cl-1
Write as many compounds as you can with the following ions. Remember that the overall charge must be zero. There are 9 possible.
Li+1
Ca2+
Al3+
N3-
S2-
Cl-1

22. Salt
Salt crystals are repeating patterns of positive and negative ions held together by electrostatic attraction

23. Ionic Bonding
When cations and anions transfer electrons, a SALT is formed
Draw the electron dot structure for the following atoms
Li and Br
Mg and O
Two K and One S
One Sr and Two F

24. SALTS
When cations and anions form bonds with each other they are called SALTS
Example: Li
1s 2p F
Li+
LiF F-

25. Practice
Show how the following compounds bond with the use of orbital diagrams
NaF
MgO
Li2S
CaCl2
AlN

26. Properties of Ionic Compounds
Crystalline Solid at Room Temperature
High Melting Points
Can conduct an electric current when melted or dissolved in water

27. Section 7.3 – Bonding in Metals
Metal atoms are arranged in very compact and orderly patterns

28. Metallic Bond
A Metallic Bond is a bond between metal cations surrounded by a sea of electrons

29. Metallic Bond
The attraction of the free floating valence electrons holds them together

30. Crystalline Structure of Metals (Page 202)

31. Properties of Metals Good Conductors of electrical current
2. Ductile (ability to be stretched)
3. Malleable (ability to be shaped)

32. Alloys Very few of the metal objects you use everyday are pure metals
Alloys are a mixture of two or more elements, at least one being a metal
Alloys are important because the combination of metals are stronger than the single metal by itself

33. Examples of Alloy Combinations
Brass – copper and zinc
Sterling Silver – silver and copper
Bronze – copper and tin
Steel – iron, carbon, boron, chromium, manganese, molybdenum, nickel, tungsten, vanadium
Stainless Steel – iron, chromium, carbon, nickel
Cast Iron – iron and carbon

34. Homework Chapter 7 Assessment