1. Bellwork
Pick up a yellow Chemical Equations notes sheet and glue it into your comp book.
Pick up a pink sheet to SHARE with you and your shoulder partner.
Follow the directions on the Pink sheet to review what we learned on Tuesday about bonding. Complete this entire sheet with your partner, taking turns writing and looking up – you must work EQUALLY!

2. BONDING REVIEW & PRACTICE

3. Ionic Bonds Ionic bonds exist between a non-metal and a metal
When two atoms bond ionically, they gain/lose electrons
When an atom gains or loses an electron, it becomes an ion (an atom with a positive or negative electrical charge)

4. Ions +1 +1 +2 +3 +4 -3 -2 -1 +1 -2 +2 +3 +4 -3 -1 +1 -2 +2 +3 +4 -3 -1
Group 1 18 2 13 14 15 16 17 3 4 5 6 7 8 9 10 11 12 +1 +1 +2 +3 +4 -3 -2 -1 +1 -2 +2 +3 +4 -3 -1 +1 -2 +2 +3 +4 -3 -1 +1 +2 +3 +4 -3 -2 -1 +1 +2 +4 -3 -2 -1 +3 +1 +2

5. Cation Positive ion (a metal gives away electrons in ionic bonding and becomes positively charged)
Anion Negative ion
(a nonmetal takes electrons in ionic bonding and becomes negatively charged)

7. Covalent Bonds Covalent bonds exist between NONMETAL and NONMETAL.
Example: H2, H2O, NO3, CH4
Covalent bonds SHARE electrons.
Shared electrons don’t belong to either atom.

10. To Do Draw the bonds, as specified
Complete the “Bonding Basics” practice in your packet.
Draw the bonds, as specified
Write the chemical formula for each compound
Number 3 under Covalent Bonds is Optional. You can do the simpler bond of Hydrogen and Oxygen instead, or you can try the challenge.
Extra Challenge: Follow the instructions in your packet to try and write the correct names for each compound.

11. Bellwork: Happy Monday!
Please take out your Periodic Table, your Chemistry Packet and your Ch. 6 book packet
Complete the “Apply it!” on page 204 (reference figure 2 on page 202 for help)

12. Chemical Equation
The symbolic representation of a chemical reaction.

13. Reactants yield Products
Coefficient: Tells the amount of that compound in the equation. Multiply it through the whole compound.
Subscript: Tells the amount of the element that comes before it.

14. Reactants yield Products
Balanced or Not?
Does it follow the Law of Conservation of Mass/Matter?
Count the atoms on both sides!
Fill in your packet for the Law!

15. COUNTING ATOMS

16. Make an Inference How many atoms of each element are in this formula: 2H2O

17. RULES FOR COUNTING ATOMS
SUBSCRIPTS only refer to the atom that they are BEHIND. For example…
H2S
There are TWO atoms of HYDROGEN and only ONE atom of SULFUR.

18. COEFFICIENTS
COEFFICIENTS apply to the entire compound. You MULTIPLY the coefficients and SUBSCRIPTS.
2 H2S
ATOMS OF HYDROGEN:
ATOMS OF SULFUR: 4 2
IF THERE ISN’T A SUBSCRIPT BEHIND AN ELEMENT, ASSUME THERE IS ONLY ONE ATOM OF THAT ELEMENT!

19. PARENTHESES
3. If elements or compounds are inside of PARENTHESES, then the SUBSCRIPT behind the parentheses applies to everything inside.
Ba(OH)2
ATOMS OF BARIUM:
ATOMS OF OXYGEN:
ATOMS OF HYDROGEN: 1 2 2

20. LET’S PRACTICE! MgCl2 Atoms of Magnesium: Atoms of Chlorine: 1 2 Al2S3
Atoms of Aluminum:
Atoms of Sulfur: 2 3

21. PRACTICE 2 1 4 CH3OH Atoms of Carbon: Atoms of Hydrogen: 1
H2SO4
Atoms of Hydrogen:
Atoms of Sulfur:
Atoms of Oxygen: 2 1 4
CH3OH
Atoms of Carbon:
Atoms of Hydrogen:
Atoms of Oxygen: 1 4 1

22. THIS COULD BE A LITTLE TRICKY…
Ca3(PO4)2
Atoms of Calcium:
Atoms of Phosphorus:
Atoms of Oxygen: 3 2 8
Al2(SO4)3
Atoms of Aluminum:
Atoms of Sulfur:
Atoms of Oxygen: 2 3 12

23. What about this BAD BOY??? 2Ca3(PO4)2 Atoms of Calcium:
Atoms of Phosphorus:
Atoms of Oxygen: 6 4 16