catalyst – october 5 2, 2010 monday mystery element! 1. like most rare earth metals, used to make...
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Catalyst – October 52, 2010
Monday Mystery Element!
1. Like most rare earth metals, used to make phosphors in TVs
2. Ferromagnetic (attracted to magnets)
3. Tarnishes slowly, oxide flakes off
Catalyst – October 52, 2010
Monday Mystery Element!
1. Like most rare earth metals, used to make phosphors in TVs
2. Ferromagnetic (attracted to magnets)
3. Tarnishes slowly, oxide flakes off
GADOLINIUM (#64)
Today’s Agenda
CatalystNew GroupsDiving into Balancing Equations
PracticeExit QuestionTONIGHT’S HW: BALANCING
WORKSHEET
Today’s Objectives
SWBAT apply law of conservation of mass to chemical reactions by balancing chemical equations.
White Board Door into classL R
3rd Period
Group 4
Kendell, Tracy, Shawn, Sara
Group 3
Allesandro, Melvin, Paula,
Tashelle
Group 1
Ariel, Kiedra, Bao, Amber
Group 2
Chicobi, Corey, Marissa, Jamie
Group 5
Warren , Tigler, Quanetta, Jasmine, Waynell
Group 6
Ebony, Brandon, Kara,
Melvin
Group 8 Group 7Group 9
White Board Door into classL R
4th Period
Group 4
Stephanie, Kim, Lizzeh,
Eddie
Group 3
Jeremy, Roniece, Lyndon, Kourtney
Group 1
Kentrell, Khallid,
Rachel, Kim
Group 2
Caleb, Infinity, Dwanyetta,
Troy
Group 5
Jytte’, Jaron, Artrel, Nia
Group 6
Josh’shawn, Aaron, Jon,
Chelsie
Group 8
Rodrea, Lester, Chelsie
Group 7
Chelsie, Shannon, Sam,
Darreal
Group 9
REVIEW: Balancing equations RULES!
Key Point #1: When balancing equations, never, Never, NEVER change subscripts, only coefficients!
Coefficient
A coefficient is a whole number that comes in front of the compound formula, never in the middle!
You multiply the coefficient to all the numbers in the compound
2 AlCl3
REVIEW: L-C-M!!!
Key Point #2: Chemical reactions MUST follow the Law of Conservation of Matter.What is the LCM? Matter cannot be created or destroyed. If 3 carbons are in the reactants of a
reaction, then there darn well better be 3 carbons in the products of a reaction.
Independent Practice
Worksheet!
Balancing with diatomics…
Key Point #1: Sometimes with diatomics , you must be a little tricky.
C4H10+ O2 CO2 + H2O
Diatomics
If you reach the point in a balance problem where everything is balanced except the diatomic atom...
You can only get even numbers with diatomics… 2 O2 = 4 O atoms 3 O2 = 6 O atoms
And sometimes the other side is odd Use a fraction, then multiply by 2
Example: Work it out…
C4H10+ O2 CO2 + H2O
Your Turn…
1. C6H6 + O2 CO2 + H2O
2. C10H22 + O2 CO2 + H2O
Balancing with some hot sauce… What if you have some
polyatomic ions? WHAAAAAAAAT will
you do?? Key Point #2: When balancing equations that involve polyatomic ions, keep them together!
Work it out…
___ H3PO4 + ___ KOH ___ K3PO4 + ___ H2O
Which polyatomics are we using? PO4 – phosphate OH – hydroxide
Where is the OH on the other side? It’s OK – rewrite H2O as HOH – Trust me!
Work it out…
__ H3(PO4) + __ K(OH) __ K3(PO4) + __ H(OH)
Which polyatomics are we using? PO4
2- – phosphate OH1- – hydroxide
Your Turn!Write a blank before each formula…1. HCl + NaOH NaCl + H2O
2. NaOH + H2CO3 Na2CO3 + H2O
3. Al(OH)3 + H2CO3 Al2(CO3)3 + H2O
Class/Homework Time!
WORKSHEET!You must complete
24 problems for HW…extra points
for extra problems!
Exit Question
Balance one of the following equations:
1. __KClO3 ---> __KCl + __O2
2. __S8 + __O2 ---> __SO3
HOMEWORK: BALANCING WKSHT(24 Problems)