1. Catalyst: Complete the Chart
Element
Symbol
Group #
# Valence Electrons
Ion Formed
Lewis Dot Structure
Barium Ba
Ba2+
Phosphorous 15
Nitrogen 5
Hint: According to the octet rule, atoms lose or gain electrons, forming ions, in order to get a full outer shell with 8 electrons. If the atom loses electrons it is a positive cation and if it gains electrons it is a negative anion.

2. Catalyst: Answers
Element
Symbol
Group #
# Valence Electrons
Ion Formed
Lewis Dot Structure
Barium Ba 2
Ba2+
Phosphorous P 15 5
P3-
Nitrogen N
N3-
Hint: According to the octet rule, atoms lose or gain electrons, forming ions, in order to get a full outer shell with 8 electrons. If the atom loses electrons it is a positive cation and if it gains electrons it is a negative anion.

3. TODAY’S OBJECTIVE: BONDING
TODAY’S OBJECTIVE: BONDING!!!! SWBAT Differentiate between IONIC &COVALENT BONDS
A.K.A.: Why don’t you blow up when you eat sodium chloride since sodium is a highly reactive metal and chlorine is an extremely poisonous gas??

4. Agenda Catalyst/HW Check (10) HW Review (10)
Part 1: Ionic Compound Formula Review: Kris-Kross Method (20)
PART 2: Ionic vs. Covalent Compounds
Ionic vs. Covalent Notes (20)
Ionic vs. Covalent Lab (40)
Ionic vs. Covalent Conductivity Demo (10)
Closing (5)

5. Homework Answers
Having equal amounts of positive and negative charge is called electroneutrality.
An electrically charged group of two or more bonded atoms that functions as a single ion is a polyatomic ion.
Collections of cations are never found without a similar number of anions (or sometimes electrons) nearby to effectively neutralize the charges.
The names for cations come from the element from which they are formed.
When an element forms two or more positive ions, the ions are distinguished by using roman numerals to indicate the charge.
The name of a simple anion is formed by changing the ending of the element name to –ide.
A subscript is a whole number written below and to the right of an element’s symbol, and it is used to denote the number of atoms in a formula.
Any chemical compound that is composed of oppositely charged ions is called an ionic compound.

6. More HW Answers K+ + Br- → KBr
Ba2+ + F- → BaF2 (2 F- to balance 2+ charge)
Sn4+ + O2- → SnO2 (2 O2- to balance 4+)
Cs2+ + Br- → CsBr2 (2 Br- to balance 2+)
The rest of the problems are coming up as practice…

7. Writing Ionic Compound Formulas Notes

8. Kris Kross Method!
Ca2+As3-
Ca3As2

9. Just kris kross the positive and the negative charges
Na1+Cl1-
NaCl
Pb4+O2-
Pb2O4

10. Practice Problems What ionic compound is formed?
Cobalt (II) and Bromine
Mercury(I) and Sulfur
Aluminum and Iodine
Hints:
Periodic table groups tell us how many valence electrons
Draw Lewis structure
Metals lose electrons to form positive cations
Nonmetals gain electrons to form negative anions
Compounds must be neutral (equal # of + and – charges)

11. Part 2! Ionic vs. Covalent Bonds
Make a Chart in your notes that looks like this:
Ionic Bonds
Covalent Bonds

12. Ionic vs. Covalent Bonds
Bond Strength = the energy needed to break the bonds between atoms in a compound.

13. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Atoms in ionic compounds are held together by ionic bonds.
Atoms in covalent or molecular compounds are held together by covalent bonds.
Ionic bonds are stronger (more bond strength)
Covalent bonds are weaker (less bond strength)

14. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Transfer of electrons
Sharing of electrons

15. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Crystal Lattice
Molecules
Water (H2O) molecules
Lithium Chloride (LiCl) crystal lattice

16. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Metal and nonmetal
Nonmetal and nonmetal

17. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Solid at room temp.
Solid, Liquid or Gas at room temp.

18. Ionic vs. Covalent Bonds
Ionic Bonds
Covalent Bonds
Conducts electricity when dissolved
Does not conduct electricity

19. Investigation: Ionic vs. Covalent
You will work in groups of 4. (2 groups per table)
Lab WS is due at end of class
Safety! Do not put any test substances near your eyes or mouth.
Clean Up: Pour liquids down the sink and solids in the trash.
Objective: Conduct four tests on four substances. Predict whether they are ionic or covalent.
Ms. Boon will run the conductivity test.

20. Exit Slip What is the formula for a compound between: Ca & F?
Compare at least one difference between ionic & covalent compounds?
Does the compound MgBr2 share electrons or transfer them between the atoms?

21. 3 Types of Bonding **IONIC *COVALENT METALLIC METAL + NON-METAL
How are Bonds Formed?
ELECTRONS are transferred between ions (1 steals, 1 gives)
Electrons are shared between atoms.
“Sea of Electrons” Spread all over between atoms of the same element.
Type of Bond Formed
Solid Crystals with repeating patterns of (+) and (-) ions
Usually liquid or solid
Solid metal
Who’s Involved?
METAL + NON-METAL
NON-METAL + NON-METAL
METAL AND METAL
Special Properties
When dissolves in H20, conducts electricity
Does not conduct electricity
Very good conductors of electricity on their own!

22. Practice- Ionic or covalent?
SH6
MgCl2
KCl
NH3
H3C3O2
Li2S N2
Cl2
CsBr
H2O HF
Na3P
CaCl2
BaS H2