1. Warm-Up 10/17/16
Name the difference between an ionic and covalent compound that you learned Friday.

2. Schedule Until Thanksgiving Break
Monday
Tuesday
Wednesday
Thursday
Friday
10/17
Ionic Bonding
10/18
Same
10/19
PSAT
Chill Day
10/20
Covalent Bonding
10/21
Naming Both Types
10/24
Shapes
10/25
Molecular Model Kit Lab
10/26
10/27
Lab Prep
10/28
Ionic vs. Covalent Lab
10/31 Halloween!!!
11/1
Intermolecular Forces
11/2
11/3
DNA
11/4
Follow-Up
11/7
Review
11/8
Exam
11/9
11/10
Go Over Exam
11/11
Begin Unit 4
11/14
Lecture
11/15
Sub
11/16
11/17
11/18
Practice
Schedule Until Thanksgiving Break

3. Essential Question: How are ionic compounds created?
Me on no Starbucks.
Topic: Ionic Bonding
Essential Question: How are ionic compounds created?

4. Ionic Bonding
Pyrite, also known as Fool’s Gold, looks like gold but is actually made of iron cations and sulfur anions. Since opposites attract, the positive cations will be attracted to the negative anions and form an ionic bond. In the case of pyrite, the iron cations are attracted to the sulfur anions and create an ionic bond.

5. Gaining and Losing
Sodium loses 1 valence electron when it becomes a cation, creating Na+. Since chlorine has 7 valence electrons, it acquires the electron from sodium to become stable and create the anion Cl-.
Since these ions are opposite charges, they attract one another and create an ionic bond to form sodium chloride. Sodium chloride is a salt, which is a term used for many ionic compounds.

6. Attracting one another
All salts are neutral ionic compounds and are held together in simple, whole-number ratios of cations and anions. These attractions do not just stop with just one single cation and a single anion. Each can attract several of the opposite charge and they are pulled together into tightly packed crystal structures.

8. Energy
Recall that ionization energy is the energy required to remove an electron.
Na + energy  Na+ + e-
Some elements release energy because they can accept extra electrons, like chlorine.
Cl + e-  Cl- + energy

9. More Energy
This energy released is less than that needed to remove an electron. Adding and removing electrons is just one part in forming an ionic bond. The rest of the process supplies enough energy so the overall process releases energy.

11. Lattice Energy
The release of energy is known as the lattice energy. Without this energy, the overall process would not be spontaneous. The same amount of energy released is needed to break these bonds. When sodium chloride dissolves in water, sodium cations and chlorine ions form.
Magnesium oxide, MgO, does not dissolve well in water because it has a higher lattice energy and requires more energy to break the bonds.

12. Ionic compounds
The ratio between cations and anions results in a neutral charge. Ionic compounds do not consist of molecules. Water is a molecule because it consists of 2 hydrogens and 1 oxygen. Sodium chloride is an ionic compound made of many Na+ and Cl- ions and form a crystal structure. There are no NaCl molecules.

13. Ionic compounds are made of a metal and a nonmetal and are not molecular compounds. For example, CaO would be an ionic compound because calcium is a metal and oxygen is a nonmetal. CO2 is not an ionic compound because it consists of two different nonmetals.

14. Repulsive and attractive forces exist in these compounds
Repulsive and attractive forces exist in these compounds. Na+ ions repel other Na+ ions and the same goes for the Cl- ions. Attractive forces exist between the positive nucleus of one ion and the electrons of another ion. They also exist between oppositely charged ions and involve more than one single cation and anion.

15. These attractive forces are greater when the ions form a crystal structure than when they are only in pairs. They are attracted to more than one single ion and create a stronger bond. Therefore, ionic bonds are strong.

16. Most ionic compounds have high melting and boiling points
Most ionic compounds have high melting and boiling points. A lot of energy is required to break these strong bonds.
For salts to conduct an electrical current, the ions must be able to move. As solids, ionic compounds are not conductors and require to be either melted or dissolved.

17. Most ionic compounds are hard and brittle
Most ionic compounds are hard and brittle. You can see this when looking at table salt, NaCl. These compounds are hard and brittle. These properties are due to the patterns of the cation and anion crystal structure.
All ionic compounds are solid at room temperature, they are hard to break apart, and have high boiling and melting points.

18. Salt crystals
Crystals of salts are made of simple repeating units. The repeating units are arranged in a salt to form a crystal lattice, the regular pattern in which a crystal is arranged.

19. The formula indicates the ratio of cations to anions
The formula indicates the ratio of cations to anions. For NaCl, there is a 1:1 ratio of sodium cations and chlorine anions. In that crystal, each Na+ ion is surrounded by six Cl- ions, and each Cl- ion by six Na+ ions.
Arrangement of these ions to form a crystal lattice depends on the size of the ions and the ratio of cations and anions.

21. How do we write these compounds though???