1. Ionic Compounds and Metals
Bonding and Properties
Chapter 7- pages

2. Ions & Ionic Bonding Section 7.1: Ion Formation; pg 206-209
Learning Goals:
I understand how positive ions (cations) and negative ions (anions) are formed.
I understand why ions form and can relate ion formation to the valence electrons of an element.
Understanding the above is crucial to understanding chemistry- how elements combine to form compounds and chemical reactions.

3. Ion Formation Review What is the octet rule?
Why do elements form ions?
Which electrons are involved when ions are formed?
What are positive ions called?
What are negative ions called?

4. Ion Formation
All elements are trying to become like a noble gas, in other words become more stable.
Elements achieve this stability by losing or gaining electrons to reach a full octet of valence electrons.
Some exceptions to the octet rule are:
Elements 1-5: H, He, Li, Be and B.
Transition metals

5. Ion Formation Atomic Model

6. Ion Formation Lewis Dot Structures:
a simple shorthand way to represent valence electrons.
Used as an alternative to electron configurations and drawing atomic models.
Example: •Na → Na
Other ways to show ion formation: electron configurations & orbital diagrams.

7. Lewis Dot Structures

8. Ion Formation A cation is a positively charged ion.
Formed when a neutral element loses electrons.
All group #1 (alkaline metals), group #2 (alkaline earth metals) and group #13 (boron group) form cations.
An anion is a negatively charged ion.
Formed when a neutral element gains electrons.
All group #15 (nitrogen group), group #16 (oxygen group) and group #17 (halogen group) form anions.
Because it has 4 valence electrons, the carbon group can form both cations and anions, although we generally consider them to have a charge of zero.

9. Ionic Bonds and Ionic Compounds
Section 7.2, pages

10. Ionic Bonding Learning goals:
Ionic bonds are formed when electrons are transferred from one atom to another.
Ionic bonds are held together by electrostatic attraction.

11. Ionic Bonding Chemical Bond- is the force that holds 2 atoms together.
There are 3 general types of bonding
Ionic: ex. NaCl, CaCl2, FeS
Metallic: ex. copper, iron, brass
Covalent: ex. CH4, C6H12O6

12. Ionic Bonding: The Formation of Sodium Chloride
Sodium has 1 valence electron
Chlorine has 7 valence electrons
An electron transferred gives
each an octet
Na 1s22s22p63s1
Cl 1s22s22p63s23p5

13. Ionic Bonding: The Formation of Sodium Chloride
This transfer forms ions, each with an octet:
Na+ 1s22s22p6
Cl- 1s22s22p6 3s23p6

14. Ionic Bonding
Ionic bonds are held together by electrostatic attraction. This is the force of attraction by opposite charges.
The atom is held together by the electrostatic attraction of electrons
(e-) and protons (p+).
Ionic compounds are held together by the electrostatic attraction of the cation (+) and anion (-).

15. Ionic Bonding
In general metals form cations and nonmetals form anions.
The oxidation state is the charge on a given ion.
Na+ oxidation state = +1
Ca+2 oxidation state = +2
Cl- oxidation state = -1
Some metals can form ions with multiple oxidation states.
Fe+2, Fe+3
Cu+, Cu+2

16. Naming Ionic Compounds
A cation retains the name from the element it was formed from.
Na+ sodium cation
Ca+2 Calcium cation
Al+3 aluminum cation
An anion is named by adding the suffix -IDE at the end of the name of the element it was formed from.
Cl- chloride anion
S-2 sulfide anion
O-2 oxide anion
N-3 nitride anion

17. Naming Ionic Compounds
Ionic compounds are named by combining the names of the cations and the anions.
NaCl sodium chloride
NaF sodium fluoride
CaCl2 calcium chloride
MgO magnesium oxide
FeS iron sulfide

18. Ionic Compounds Properties
The packing of these positively charged cations and negatively charged anions must balance the forces of attraction and repulsion between the atoms.

19. Ionic Compounds Properties
The repeating pattern
of particle packing in an
ionic compound is called
an ionic crystal.

20. Ionic Compounds Properties
A crystal lattice is the three-dimensional geometric arrangement of particles, and is responsible for the structure of many minerals.
Quartz, SiO2
Pyrite, FeS2

21. Ionic Compounds Properties
In a solid, ions are locked into position and electrons cannot flow freely—solid ions are poor conductors of electricity.
Liquid ions or ions in aqueous solution have electrons that are free to move, so they conduct electricity easily.
An ion in aqueous solution that conducts electricity is an electrolyte.

22. Physical Properties of Ionic Compounds
The properties of ionic compounds can be explained by the strong attractive forces between the cations and anions-electrostatic attraction.
Ionic compounds have very high melting and boiling points compared to most other solid compounds.
Ionic bonds are very strong compared to metallic and covalent bonds.

23. Physical Properties of Ionic Compounds
Ionic compounds are hard, rigid and brittle

24. Ionic Bonding
Positive and negative ions exist in a ratio determined by the number of electrons transferred from the metal atom to the non-metal atom.
Example:
NaCl
CaCl2

25. Names and Formulas for Ionic Compounds
Sodium + Chlorine
Sodium + Oxygen
Potassium + Iodine
Calcium + Oxygen
Calcium + Bromine

26. Ionic Compounds https://www.youtube.com/watch?v=c-nMmwfTV-w

27. Ionic Bonding

28. Oxidation or Charge States of Ions

29. Assessment
Explain how an ionic compound made up of charged particles can be electrically neutral.
Name 3 properties of ionic compounds.
Why are ionic compounds so strong?
4. How would you write the following ionic compounds:
Potassium and fluoride
Magnesium and chloride
Sodium and oxygen

30. Review on Ionic Bonding
Which elements/groups form cations? Why?
Which elements/groups form anions? Why?

31. Metals & Metallic Bonding
Section 7.4- pages
Learning Goals:
I can describe a metallic bond and I understand how a metallic bond differs from an ionic bond.
I understand the physical properties of metals and can relate these properties to their valence electrons.
I can define and describe what alloys are.

32. Metallic Bonding
Metals form crystal lattices in the solid state and can be modeled as cations surrounded by a “sea”of freely moving valence electrons.
A metallic bond is the attraction of a metallic cation for these delocalized electrons.

33. Metallic Bonding
The metal ions are tightly packed in the crystal and their “d” electron orbitals overlap.
The electron sea model proposes that all metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons.
The electrons are free to move around and are referred to as delocalized electrons.

34. Review from last week What are the 3 types of bonds? Why do ions form?
What interaction holds ionic bonds together?
Last week’s BIG IDEA: oppositely charged ___________ attract each other, forming electrically _________ ___________ ____________.
What ion does Ca form? What is its oxidation state?