1. Draw a picture of an ionic bond for salt (NaCl)
Do Now
What is an ionic bond?
What is a covalent bond?
Draw a picture of an ionic bond for salt (NaCl)

2. Chemical Bonding and compound naming

3. Ionic Compounds Ionic compounds form crystals
What do you notice about the pictures?

4. Ionic Compounds
Strong attractions between ions of a compound cause it to have
High melting points
Highly brittle (breakable)
Very strong
Cation
anion

5. Speaking of ions
How do we form an ion?

6. Ions
Ions- an atom with either a positive (cation) or a negative (anion) charge caused by the addition or removal of an electron.
Why do we add or remove electrons?

7. Bonding ELECTRONS are the reason we have compounds!
All bonding is caused by either the transfer or sharing of electrons!
When electrons are shared it is _________ bonding.
When electrons are transferred it is _________ bonding.

8. All elements want to be stable
Do you like being unstable?
Think about standing on the side of a cliff….with a very strong wind. Would you be happy?
How do elements gain stability?

9. The octet rule
What is a valence electron?
What is the octet rule?

10. The octet rule
Compounds are most stable when they have eight (8) valence electrons.
Compounds will gain or give up electrons based on how easy it is.
Ionization energy- the amount of energy required to remove an electron.

11. Octet rule
In your notebook explain how ionization energy changes across the periodic table.
You have 3 minutes.
Use full sentences!!!!!!! (I’m serious…I will be checking!)

12. Care to share?

13. Homework 12/2/13 What ionic charge will Magnesium have?
When is an atom least likely to react?
Define ion, ionization energy, valence electron, octet rule, covalent bond, and ionic bond.
*Bonus* how many protons, neutrons, and electrons does Bromine have?

14. Do Now
You need to pick up a white board, dry erase marker, and eraser from the front left corner of the room.
You must be seated with these materials by the time the bell rings or points will be deducted from your grade today.

15. Do Now Continued Draw a water molecule. Chemical formula H2O.
Is water a compound, mixture, or element?
How many elements are in a molecule of water?
What’s an ionic bond, covalent bond?

16. Lets break it down Many water molecules together
Pure substance not a mixture

17. The word molecule is ambiguous. What does ambiguous mean???
You can have a molecule of an element
You can have a molecule of a compound
You can have a molecule of a substance
The word molecule does NOT always mean compound or element.
Ambiguous= more than one meaning.
Your book defines molecule as a neutral group of atoms joined together by one or more covalent bonds.

18. How can two atoms together be an element?
Tricky right?
There are elemental forms of all elements.
Air is made mostly of what element?

19. STABILITY rules the UNIVERSE!
Confused?
Just Remember!
STABILITY rules the UNIVERSE!
All chemical bonding is done to make an element stable.

20. You can make one covalent bond for every valence electron you have.
Covalent bonding
What is a covalent bond?
You can make one covalent bond for every valence electron you have.

21. Covalent bond
Covalent bonds are expressed as lines. Unlike ionic expressed as charges.
C O H

22. Non-polar covalent
The types of atoms in a molecule and its shape affect its polarity.
What do you see when you look in a mirror?

23. Non-polar covalent
For non-polar elements you look for equality in the molecule.

24. Polar covalent To be polar you should look for unequal sharing.
The unequal sharing will cause some charges on molecules
BUT due to the fact there is no electron transfer it is still a covalent bond.

25. Polar covalent
Unequal sharing causes slight charges.

26. Polarity and strength What is the strongest type of bond?
Polar molecules will attract to one another through intermolecular forces. Which makes polar substances stronger than non-polar.
Intermolecular forces

27. Bond strength
Ionic > polar covalent > non-polar

28. Practice
Draw these molecules in your notebook and label them as either polar or non-polar molecules.

29. 3. Draw a picture of an ionic bond for salt (NaCl).
Do Now
1. What is ionic bond?
2. What is a covalent bond?
3. Draw a picture of an ionic bond for salt (NaCl).
Today’s Lesson Topic: Chemical Naming

30. Do Now answer

31. Today’s Objective SWBAT name common mono-atomic and polyatomic ions.
Essential Questions: how do chemical compounds get their name?

32. Review..
Ionic Bond vs. Covalent Bond
Ionic bond is an electron transfer
Covalent Bond is electron sharing
Which is stronger? Why?

33. Let’s Check…
How many elements are in the following compound?
Na2CO3

34. Naming compounds There are so many ways to combine atoms.
We must give compounds names.
To do this there are rules….many many rules
Fortunately this is not organic chemistry (you’ll get that in college)
Fewer rules to follow for physical science (yay!)
But, you will need to memorize some rules.

35. A cation is an ion with a positive charge
Hold up…Review
What is a Cation? What is an Anion?
A cation is an ion with a positive charge
An ion an with a negative charge

36. Review
What are the ions of Na, C, N, O, Cl ?

37. Ionic compound naming In ionic bonding we join an anion with a cation.
The first step to naming is to determine which is which.

38. Identifying the anion 1. In NaCl which would be the anion?
2. In CaCl2 which would be the anion?
3. In LiS which would be the anion?
Sensing a pattern?

39. Ionic Compound naming
In ionic bonding the anion is usually listed second in the chemical formula.

40. Anion RULE THE ONLY RULE YOU NEED FOR ANION NAMING!
CHANGE THE ENDING OF THE CHIMICAL NAME TO –ide.
Example:
Fluorine = Fluoride ion (F-)

41. Practice 1: Name these
1. Cl-1
2. N-3
3. Br-1
4. O-2

42. 1. Sulfide ion 2. iodide ion 3. phosphide ion 4. Fluorine ion
Practice 2: Write these
1. Sulfide ion
2. iodide ion
3. phosphide ion
4. Fluorine ion

43. Cation Rule This rule is easy. Use the element name of the cation.
NaCl = sodium chloride
Sodium is the cation
Chloride is the anion

44. Practice 3: Name these
1. NaCl
2. CaCl2
3. MgO2

45. That naming system works for mono-atomic ions
To complicate things we have polyatomic ions.
What are they?
Multiple atoms in an ion.
Multiple atoms with a charge
Example: NH4+ ammonium
Unfortunately, these are ion names you must memorize. 

46. Copy these in your notes Put your pencil down when down and wait silently

47. Trends?
Any trends you see?
Elements ending in –ate?

48. Molecular compounds
Molecular compounds are named based on the number of atoms in a molecule.

49. What is the common name for CO2?
What about CO3?
Carbon Trioxide

50. Practice 4: Molecular Compounds
In order to name you just add the prefix to the elemental name (with –ide).
1. CO
2. PO5

51. You Try
3. PO3
4. SO4 (careful with this one)
5. N2O4

52. Final Review
Name the following compounds:
1. NaCl
2. NaO
3. H2O
4. LiF

53. Exit Ticket 1. What are anions? What are cations?
2. What is the name of CaCl2?
3. What is the name of NaCl?
4. What is the name of