Transcript Unit5NotesEquationsandStoich - PHA Science

C: 12 January 2012
Grab your green folder
 Objective: You will be able to:
 write correct formula equations for
chemical reactions
 Do now: Brainstorm: Write down as
many indications (signs) of a chemical
reaction as you can.

Agenda
Do now
II. Organize/stamp
III. Chemical reactions notes and demo
IV. Writing equations examples
V. Practice problems
Homework: Week 18 Homework #1-3, 7-9:
Fri.
Late work/Lab report rewrites by
Weds. Jan. 18
I.
10 min. to organize
Organize your folder/notebook.
2. Stack up and paperclip all Unit 3 materials
Put your tracking sheet on top.
3. Track your last Unit 3 Quiz.
4. Get stamps!
5. Put your papers in your green folder in the
bin.
**You must be in your seat unless you
are putting your folder in the bin.**
1.
Chemical Reactions
Demo

In your notebook, record your
observations.
Indications of a Chemical Reaction
1.
2.
3.
4.
Heat and Light
Production of a Gas (bubbles)
Formation of a precipitate
 A solid produced as a result of a
reaction between two solutions
Color change

chemical reaction: changing substances
to other substances by breaking bonds in
reactants and forming new bonds in
products.

http://www.youtube.com/watch?v=F54rq
Dh2mWA
Chemical Equations
How do chemists describe chemical
reactions?
 chemical equations: an expression
representing a chemical reaction

Word Equation

Hydrogen gas combines
(explosively!) with oxygen gas to
produce water vapor
reactants: hydrogen, oxygen
products: water
Formula Equations

H2(g) + O2(g)  H2O(g)
Reactants
Products
(s) – solid, (l) – liquid, (g) – gas
 (aq) – aqueous (dissolved in water)

Symbols
+ and, reacts with
  yields (to yield), produces (to produce),
forms (to form)

Diatomic molecules
7 elements make diatomic molecules:
 H2, N2, O2, F2, Cl2, Br2, I2
 “7 make a 7”
 HINClBrOF


You must be sure to write correct
chemical formulas for reactants and
products!
Write the word equation
Na2O(s) + H2O(l)  NaOH(aq)
 Solid sodium oxide reacts with water to
yield a solution of sodium hydroxide

Write the formula equation
Solid copper reacts with a solution of
silver nitrate to yield solid silver and a
solution of copper (II) nitrate.
 Cu(s) +AgNO3(aq)  Ag(s) +
Cu(NO3)2(aq)

C: 13 January 2012
Take Out Homework: Week 18 #1-3, 79
 Objective: You will be able to:
 write correct formula equations for
chemical reactions
 Do now: Write the word equation:
Zn(s) + HCl(aq)  ZnCl2(aq) + H2(g)

Agenda
Do now
II. Writing equations practice problems
III. Exit ticket
Homework: Week 18 Homework #4-6 and 1018: Wednesday
Late work/Lab report rewrites by
Weds. Jan. 18
I.
Practice
1.
Solid magnesium reacts with oxygen gas
to yield solid magnesium oxide.
Practice Worksheet

Complete pages 3-4 with your partner
Exit ticket
Homework
Week 18 Homework #4-6 and 10-18:
Wednesday
Late work/Lab report rewrites by
Weds. Jan. 18
A: 12 January 2012
Take Out Homework: Week 18 # 1-3,
7-9
 Objective: You will be able to:
 write formula equations for chemical
reactions
 Do now: Write correct formulas for:
a. iron (III) oxide
b. nitrogen dioxide

Agenda
Do now
II. Check homework and answers
III. Writing formula equations practice
Homework: Week 18 Homework #4-6 and
10-12
Late work/Lab report rewrites by
Weds. Jan. 18
I.
Writing Formula Equations

Complete pages 1-2 with your partner.
C: 18 January 2012
Take Out Homework: Week 18 #4-6,
10-12
 Objective: You will be able to:
 use the law of conservation of mass to
balance chemical equations
 Do now: Write the formula equation for:
 Solid magnesium reacts with oxygen gas
to yield solid magnesium oxide.

Agenda
Do now
II. Paperclip Mini-lab
III. Balancing Equations Examples
IV. Practice Problems
Homework: Finish paperclip mini-lab:
Thurs.
Week 18 Homework pages 5-6: Thurs.
I.
Midterm Exam
Wednesday, January 25
 10:15 am -12:05 pm
 Bring a calculator, pens/pencils
 You’ll get a periodic table and polyatomic
ions list

Midterm Exam
29 Questions, most with 2 parts
 A mix of multiple choice and short
answer/problem solving
 Some have tier III questions – at end of test
 On most objectives in Units 1-5
 Your review sheet will tell you which
ones.
 Very similar to quiz and homework
questions you’ve seen.

Paperclip Mini Lab p. 1-2
You and your partner share on bag of
paperclips.
 Follow the directions exactly.
 Be sure to record data as specified by the
directions.
 To bond, unlink paperclips completely
from the original compounds and then
relink them to form the new compound.
 Unlink all paperclips and return to bag when
you finish!

Law of Conservation of Mass
In a chemical reaction, matter is never
created or destroyed.
 The number of atoms and the mass of
each element of the reactants must be
equal to the number of atoms and the
mass of element of the products.


This is shown by placing a coefficient in
front of the formula for each compound.
OO
HH
OO
HH
OO
CC
HH
OO
CC
HH
OO
CC
HH
OO
CC
HH
CC
CC
O O
O O
O O
O O
O O
O O
H H
H H
H H
H H
H H
H H
O
CC
CC H
H
CC C
CHC
H
C
H
H
C
O
O
O
O
H
H
O
H
H
O
C
H
H
O
O
O
O
O
H2(g)


H2(g)
+ F2(g) 
+ F2(g)
2
HF(g)
HF(g)


H2O(l) 
H2(g) +
O2(g)
2H2O(l)  2 H2(g) +
O2(g)
Balancing Chemical Equations
Ca(s) +


8 Ca(s) +
S8(s)
S8(s)

8
CaS(s)
CaS(s)


Zn(s) + HCl(aq)  ZnCl2(aq) + H2(g)
Zn(s) +2HCl(aq)  ZnCl2(aq) + H2(g)
Balancing Equations
1.
H2 + O2  H2O
2.
ZnS + O2 
3.
Ag3PO4 +
KBr 
4.
H2SO3 +
O2 
5.
Na2SO4 + Fe(NO3)3  NaNO3 + Fe2(SO4)3
6.
AgNO3 + CaCl2 
ZnO + SO2
K3PO4 + AgBr
H2SO4
AgCl +
Ca(NO3)2
Now:
Finish the paperclip lab page 3
 Rank your studying priorities on pages 1-3
of the midterm review guide
 Both of these things are due tomorrow!

Assignment

Paperclip Mini-lab Handout
 with your partner
Homework
Finish paperclip mini-lab
 Week 18 Homework pages 5-6
 both due tomorrow

C: 19 January 2012
Take Out Homework: Paperclip Mini-Lab
and Midterm Review Packet
 Objective: You will be able to:
 balance chemical equations to satisfy the
law of conservation of mass and review for
the midterm
 Do now: Write and balance:
 Solutions of silver nitrate and calcium
chloride react to form solid silver chloride
and a solution of calcium nitrate.

Agenda
Do now
II. Homework answers
III. Writing and balancing equations practice
challenge!
IV. Unit 1 Review
V. Midterm review packet work time
Homework: Finish Unit 1 Review questions
AND Priority 1 and 2 Questions: Fri.
I.
On your Priorities Ticket
Write down your top three priority units.
 We’ll use these to make work groups
tomorrow and Monday.

Midterm Exam
Wednesday, January 25
 10:15 am -12:05 pm
 Bring a calculator, pens/pencils
 You’ll get a periodic table and polyatomic
ions list

Midterm Exam
29 Questions, most with 2 parts
 A mix of multiple choice and short
answer/problem solving
 Some have tier III questions – at end of test
 On most objectives in Units 1-5
 Your review sheet will tell you which
ones.
 Very similar to quiz and homework
questions you’ve seen.

Unlock the Code!
1.
2.
3.
4.
5.
With your partner, write and balance four
equations.
Place the correct coefficients into the
blanks at the top of the page.
Come up and try the lock!
Hand in your worksheet.
Start Unit 1 Review problems with your
partner.
Unit 1 Review
1.
2.
With your partner, complete the Unit 1
Review questions (p. 3-7)
When you finish, decide on your next priority
and begin those questions.
1. You will receive a class work grade out of 10
points for your work today.
2. Stay in your seat, work quietly, stay on task
Homework: Unit 1 Questions and your Priority
1 and 2 Questions due tomorrow.
A: 19 January 2012
Take Out Homework: Week 19 Homework
 Objective: You will be able to:
 review Unit 1 for the midterm exam.
 Do now: List the steps of the scientific
method.
 Then, write a hypothesis for the research
question: Will my jeans shrink more each
time I put them in the dryer?

Unit 1 Review
Unit 1 is a HUGE priority for this class!
 So, let’s review together.

Na2O2
+
H2O 
NaOH
+
O2
2Na2O2
+
2H2O 
4NaOH
+
O2
CaCl2 +
FeCl3
Fe2(SO4)3 
CaSO4 +
3CaCl2 + Fe2(SO4)3  3CaSO4 + 2FeCl3
Al2O3 +
HCl 
AlCl3 +
H2O
Al2O3 +
6HCl 
2AlCl3 +
3H2O
KClO3

KCl +
KClO4
4KClO3

KCl +
3KClO4
AgNO3 +
CaCl2 
AgCl +
Ca(NO3)2
2AgNO3 + CaCl2 
2AgCl + Ca(NO3)2
Na2SO4 + Fe(NO3)3  NaNO3 + Fe2(SO4)3
3Na2SO4 + 2Fe(NO3)3  6NaNO3 + Fe2(SO4)3
3Na2SO4 + 2Fe(NO3)3  6NaNO3 + Fe2(SO4)3
C12H22O11 +
O2 
CO2 +
H2O
C12H22O11 +
12O2  12CO2 +
11H2O
BaCl2 +
(NH4)2CO3  BaCO3 +
NH4Cl
BaCl2 + (NH4)2CO3  BaCO3 + 2NH4Cl

Liquid silicon tetrachloride reacts with
liquid water to produce solid silicon
dioxide and a solution of hydrochloric
acid.

SiCl4(l) + 2H2O(l)  SiO2(s) + 4HCl(aq)

Nitrogen gas reacts with oxygen gas and
water to produce a solution of hydrogen
nitrate.

2N2(g) + 5O2(g) 2H2O(l)  4HNO3(aq)
KOH +
H2O
Cl2 
KCl +
KClO3 +
6KOH + 3Cl2  5KCl +
3H2O
KClO3 +
Balancing Equations Practice
Worksheet
A: 18 January 2012
Grab your clicker! 
 Take Out Homework: Week 18 p. 5-7
 Objective: SWBAT classify reactions as one
of the five types of chemical reactions.
 Do now: Balance:
Na2SO4 + Fe(NO3)3  NaNO3 + Fe2(SO4)3

Agenda
Do now
II. Homework solutions balancing equations
III. Balancing Equations Exit Ticket
IV. Types of Reactions Notes
V.
Clicker Practice Problems
VI. Midterm Studying Survey
Homework: Week 19 Homework: Thurs.
Finish “Unlock the Code” Worksheet (optional)
I.
Midterm Exam
Wednesday, January 25
 10:15 am -12:05 pm
 Bring a calculator, pens/pencils
 You’ll get a periodic table and polyatomic
ions list

Midterm Exam
29 Questions, most with 2 parts
 A mix of multiple choice and short
answer/problem solving
 Some have tier III questions – at end of test
 On most objectives in Units 1-5
 Your review sheet will tell you which
ones.
 Very similar to quiz and homework
questions you’ve seen.

Exit Ticket

Balancing Reactions
Midterm Review!
What units are your studying priority?
 Complete by the end of the period
 You’ll be assigned groups working on
your top priorities based on this survey!
 Then, work on your 1st priority review or
the Week 19 Homework

Homework
Week 19 Homework: tomorrow
 “Unlock the Code” worksheet (optional)
 Start the Midterm Review packet
(optional)

A: 19 January 2012
Take Out Week 19 Homework
 Objective: You will be able to:
 review Unit 1 for the midterm!
 Do now: Fill in a Venn diagram:
phosphide phosphate

Agenda
Do now
II. Homework Answers
III. Unit 1 Review with a partner
IV. Begin your second priority unit review
Homework: Finish Unit 1 Review
questions
Finish your priority #2 review questions
Unlock the code = extra credit: tomorrow
I.
Extra Help
Today: 3:30-4:30
 Monday and Tuesday at lunch
 Tuesday: 3:30-4:30

Your grade

10 point class work grade:
 follow directions
 stay on task
 work quietly with only your partner
 stay in seat unless using a scavenger
hunt clue
A: 20 January 2012
Take Out: Midterm Review Packet
 Objective: You will be able to:
 review your second and third priority
units for the midterm!
 Do now: a. How many atoms are in a
mole of calcium?
b. How many atoms are in 0.50 moles of
calcium atoms?

Agenda
Do now
II. Today’s assignment and Groups
III. Check Unit 1 answers with group
IV. Check assigned unit answers with group
V.
Unit 4 Review as a class
VI. Begin 3rd priority review questions
independently
Homework: Complete your third priority
review questions (started in class)
 Then, complete the questions for one more
unit.
 You should have FOUR units complete!
 due Monday
I.
Your #2 Priority: Check answers

Unit 2a: Garlyn, Joey, Sophie,

Unit 2b: Larissa, Emily, Zuri

Unit 2c: Ricardo, Israel

Unit 2d: Trae, Marie, Julian

Unit 3: Loveng, Brunyr, Crystal

Unit 4: Karen, Hannah
Homework
Complete your third priority review
questions (started in class)
 Then, complete the questions for one
more unit.
 You should have FOUR units complete!
 due Monday

C: 20 January 2012
Take Out: Review Packet
 Objective: You will be able to:
 review your 2nd and 3rd priority units for
the midterm.
 Do now: Fill in Venn diagram:
phosphide phosphate

Agenda
Do now
II. Groups and Assignment
III. Check Unit 1 Answers
IV. Check Assigned Unit Answers
V. Complete 3rd priority review questions
Homework: Finish 3rd priority review
questions
Do one more unit: Due Monday.
I.
Groups

Unit 2a: Javier, Dyani, Lorreno

Unit 2b: Jackson, Nekeyla, Bryan

Unit 2c: Meryem, Martely, Carlheb

Unit 2d: Leslie, Patrick, Christine

Unit 3a: Devin, Jesse, Kenny

Unit 3b: Courtney, Obayanna, Daysia

Unit 5: Adley, Kendra, Carla
Today’s assignment
1.
2.
3.
With your group, check your answers to
the Unit 1 Review Questions (10 min.)
Then, with your group, check your
answers to review questions for your
assigned unit (10 min.)
Finally, work independently to complete
the review questions for your third
priority unit. (remaining time)
Class work grade

10 points possible:
 Stay in your seat unless you’re
scavenging.
 Talk quietly and only with members of
your group.
 Stay on task and complete the work!
Homework
Finish 3rd priority review questions
 Do one more unit: Due Monday.
 You will have FOUR units done by
Monday!

Extra Help
Today: 3:30-4:30
 Monday and Tuesday at lunch
 Tuesday: 3:30-4:30

A: 23 January 2012
Take Out: Midterm Review Packet
 Objective: You will be able to review
objectives for the midterm exam.
 Do now: Write an equation:
A solution of sodium nitrate and solid lead
(II) oxide react to form a solution of lead
(II) nitrate and solid sodium oxide.

Agenda
Do now
II. Questions?
III. Review work time
Homework: Check your review answers!
Study for midterm on Wednesday
Bring a calculator!
Extra help Tuesday, 3:15-3:45 pm
I.
Review Packet Answers

on the blog!
 I made a mistake on the second
balancing the equation problem – fix it
for bonus points. Give me your
correction tomorrow at the exam.
A review problem together!
A solution of sodium nitrate and solid lead
(II) oxide react to form a solution of lead
(II) nitrate and solid sodium oxide.
1. Write and balance the equation.
2. Calculate the molar mass of lead (II)
nitrate.
3. How many moles are equal to 10.0 grams
of lead (II) nitrate?
4. How many molecules is that?

On your own
Complete the review questions for any
unit you have left.
 You may quietly ask your partner if you
have questions, but are working on your
own.
 Raise your hand if you have questions!

Questions?
C: 31 January 2012
Take Out: Green folder, notebook, twopocket folder
 Objective: You will be able to:
 look through your midterm, ask
questions and correct answers
 Do now: Fill in the blanks; I thought the
midterm was __________ because
_________.

Agenda
Do now
II. Pass back work
III. Organize folders and materials
IV. Return midterm
V. Ask and answer questions about the
midterm
Homework: Be sure you have: chemistry
notebook, two pocket folder
I.
Organize – 10 min.



You should have no loose papers in your
notebook.
In your two pocket folder:
 “Homework:” Week 17 thru 19
 “Everything Else:”
 Unit 4/5 Objective Mastery Tracking Sheet
(on top)
 4.1/4.2 Quiz
 Writing Formula Equations
 Chemical Reactions Mini-Lab
Paperclip everything else and put it in your
green folder. Return your green folder.
Hand Back Exams





Your percent grade is circled on the top of the
paper Tracking Sheet
Number circled by each objective is your
objective mastery (0-4) for that objective.
3 = 95% unless there was no Tier III question,
then 3 = 100%
MCAS = that multiple choice question was
from an old MCAS question. Circled = you got
it right.
Your extra credit is added into your percent
already
Questions?
Homework
Notebook with no loose papers
 Cleaned out 2 pocket folder
 I’m checking these Wednesday for 5
homework points!

C: 1 February 2012
Take Out: Folder and Notebook
 Objective: You will be able to:
 identify reactions as one of the five types
of reactions
 predict the products of a single
replacement reaction
 Do now: Watch the demonstration. List
two signs of a chemical reaction.

Agenda
Do now
II. Five types of reactions notes with demos!
III. Practice Problems
IV. Predicting products of a single replacement
reaction
V.
Practice problems
VI. S’mores pre-lab questions
Homework: Week 21 Homework Part 0
Week 21 Homework page 1
read S’mores lab
I.
Types of Chemical Reactions
Reaction Type
Composition
Decomposition
Single
Replacement
Double
Replacement
Combustion
General
Equation
Definition Example
A: 1 February 2012



a.
b.
Take Out: Open your folder on your desk
Objective: You will be able to:
 identify reaction demos as one of the five
types of reactions
 predict the products of a single
replacement reaction
Do now: What type of reaction?
AX + B → A + BX
CaCO3(s) → CaCO(s) + CO2(g)
Agenda
Do now
II. Review five types of reactions with
demos!
III. Predicting products of a single
replacement reaction
IV. Practice problems
V. S’mores pre-lab questions
Homework: Week 21 Homework page 1,
read S’mores lab
I.
Composition Reaction
•
•
•
General Equation: A + X  AX
Definition: two or more substances
combine to form a new compound.
Example: Mg(s) + O2(g) → MgO(s)
Composition

Li
+
Li
O2

O
O
Li2O
Composition Example
Solid magnesium reacts with oxygen gas to
produce solid magnesium oxide.
Decomposition Reaction
•
•
•
General Equation: AX  A + X
Definition: a single compound breaks
down into two or more simpler
substances.
Example: 2H2O2(l)  2H2O(g) + O2(g)
Decomposition
KClO3
K
K
O
Cl
O
KCl

Cl
O
+
O2
O
O
Decomposition Example

Liquid hydrogen peroxide decomposes to
form liquid water and oxygen gas.
Single Replacement Reaction
General Equation: A + BX  AX + B
Definition: One element replaces a similar
element in a compound.
Examples:
Mg + 2HCl  H2 + MgCl2
2Al + Pb(NO3)2  3Pb + 2Al(NO3)3
Single Replacement

KI
+
K
Br2
Br
I
Br

KBr
+
I2
Single Replacement Example

Magnesium metal reacts with a solution of
hydrochloric acid to produce a solution of
magnesium chloride and hydrogen gas.
Double Replacement Reaction
General Equation: AX + BY  AY + BX
Definition: the ions of two compounds
exchange places in an aqueous solution to
form two new compounds.
Example:
2KI(aq) + Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq)
Double Replacement

CuCl2 + Na2S  2NaCl + CuS
Cl
Cl
Cu
Na
Na
S
Double Replacement Example

Solutions of lead (II) nitrate and
potassium iodide react to produce a
solution of potassium nitrate and solid
lead (II) iodide.
Combustion Reaction
General Equation:
CxHy(g) + O2(g)  CO2(g) + H2O(g)
Definition: a substance combines with oxygen and
releases a large amount of heat (exothermic) or
light energy
Example:
C2H6(g) +O2(g)  CO2(g) + H2O(g)
Combustion Example


Hydrogen gas reacts with oxygen gas to
make water vapor.*
*Yes, this is also a combination reaction
A + Y  AY
100%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
1
0%
0%
2
3
0%
0%
4
5
A + BX  B + AX
94%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
6%
0%
2
3
4
0%
5
AB  A + B
95%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
5%
1
0%
2
3
0%
0%
4
5
AB + XY  AY + XB
94%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
0%
2
6%
3
0%
4
5
A + O2  CO2 + H2O
89%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
6%
6%
0%
1
2
0%
3
4
5
2H2O  2H2 + O2
94%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
0%
2
3
6%
4
0%
5
2C + O2  2CO
94%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
2
6%
3
0%
0%
4
5
Mg + CdCl2  Cd + MgCl2
67%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
28%
6%
0%
1
0%
2
3
4
5
Al2(SO4)3 + 3Ca(OH)2  2Al(OH)2 + 3CaSO4
67%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
28%
6%
0%
1
0%
2
3
4
5
2C6H14 + 19O2  12CO2 + 14H2O + heat
89%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
6%
0%
1
6%
0%
2
3
4
5
BaO + H2O  Ba(OH)2
88%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
1
12%
0%
0%
2
3
0%
4
5
2NaNO3  2NaNO2 + O2
89%
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
6%
6%
0%
1
0%
2
3
4
5
AgNO3 + NaCl  AgCl + NaNO3
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
0%
0%
2
3
0%
0%
4
5
2Al + 3ZnCl3  3Zn + 2AlCl3
1.
2.
3.
4.
5.
Composition Reaction
Decomposition Reaction
Single Replacement Reaction
Double Replacement Reaction
Combustion Reaction
0%
1
0%
0%
2
3
0%
0%
4
5
What does a combustion reaction
require?
1.
2.
3.
4.
5.
Heat
Oxygen
Carbon dioxide
Love
Gasoline
0%
1
0%
0%
2
3
0%
0%
4
5
Which type of reaction?
1.
2.
3.
4.
5.
6.
7.
Al2(SO4)3 + 3Ca(OH)2  2Al(OH)2 + 3CaSO4
2C6H14 + 19O2  12CO2 + 14H2O + heat
BaO + H2O  Ba(OH)2
2NaNO3  2NaNO2 + O2
AgNO3 + NaCl  AgCl + NaNO3
2Al + 3ZnCl3  3Zn + 2AlCl3
What does a combustion reaction require?
Predicting Products
of Single Replacement Reactions
A + BX → B + AX
The lone element replaces one of the two
elements in the compound.
 It tries to replace the element it is most
similar to (metals replace metals,
non-metals replace non-metals)
 If the lone element is more reactive than
the element it’s trying to replace.
 Be sure to write correct formulas for each
new compound you make!

How do you know
which elements
replace other
elements?
Metals: Look at an
Activity Series
 Replace elements below
them on this list.

How do you know which elements
replace other elements?

Halogens (Group 17): replace elements
under them on the periodic table
F
Cl
Br
I
Examples
1.
Mg + HCl →
2.
Al + Pb(NO3)2 →
3.
KI
4.
Cu + AlCl3 →
+
Br2 →
Practice Problems!
1.
2.
3.
4.
5.
6.
7.
8.
9.
Mg + CdCl2 →
Al + ZnCl2 →
F2 + MgBr2 →
Zn + CuCl2 →
Cl2 + NaBr →
Ca + HCl →
I2 + NaCl →
Br2 + CaI2 →
Iron reacts with copper (II) nitrate…
(use Fe3+)
If you finish early, go back and balance each
equation.
Homework
Week 21 Part 0: tomorrow
 Week 21 Page 1: tomorrow
 If you don’t know the charge of a
transition metal (Sn, Cu, Fe, etc.) use 2+
 Zn is always 2+
 Ag is always +

A: 3 February 2012
Take Out: Week 21 HW p. 2
 Objective: You will be able to:
 explore mole ratios in a chemical reaction
by modeling the process with s’mores!
 Do now: 2H2(g) + O2(g) → 2H2O(g)
a. How many moles of hydrogen gas react
with 1 mole of oxygen gas?
b. How many moles of water vapor are
produced by the reaction of 10 moles of H2
gas?

Agenda
Do now
II. Check homework
III. S’mores lab instructions
IV. Carry out the lab
V.
Collect and analyze data, answer post lab
questions
VI. Mole ratios practice
Homework: Complete the S’mores lab packet:
Tuesday
Week 21 Homework p. 2-3
I.
Check homework
Lab Expectations
Stay at your station and with your group.
 Stay on task.
 Be thoughtful about the volume of your
voice; talk only with your group members.
 Be responsible and careful with the lab
materials and equipment.
 Clean up after yourself before you move
on to the post lab questions.

With your group…
1.
2.
3.
4.
5.
6.
Read p. 1 and complete page 2 through #3.
Send your supply monitor to the front to
pick up your supplies.
Continue with page 3. Be sure to use
waxed paper on the balance to keep your
ingredients clean!
Once you have completed p. 3 #7, eat your
s’more!
Then, clean up and begin the Post Lab
Questions on p. 3
Entire packet due Tuesday – lab grade!
Homework
Complete the lab packet: Tues.
 Go to the blog
www.phascience.wordpress.com
and click “10th Grade Chemistry”
Watch the YouTube video – first link on the
page. Do the “Your turn” questions in
your notebook: due Tuesday

C: 3 February 2012
Take Out Homework: S’mores lab
 Objective: You will be able to:
 use a balanced chemical equation to
calculate mole ratios in a reaction.
 Do now: 2G2 + M + 10C → G4MC10
How many s’mores could you make if you had 4
graham crackers (each one = G2), 5
marshmallows and 25 chocolate chips?
Explain how you got your answer.
What would you have left over?

Agenda
Do now
II. Mole ratio notes and examples
III. Practice problems
Homework: Week 21 Homework p. 2-3
due Mon.
I.
For one sandwich:
1 roll
1 slice
2 slices
1 leaf
2 slices
You have
2 rolls
5 slices
6 slices
4 leaves
8 slices
What is the limiting ingredient?
Which ingredients are in excess?
Mole Stoichiometry
How are quantities of reactants and products
related in a chemical reaction?
4Fe(s) + 3O2(g)  2Fe2O3(s)
SWBAT calculate mole relationships for chemical reactions.
4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of oxygen gas react with
4 moles of solid iron?
How many moles of iron (III) oxide are
produced by the reaction of 3 moles of
oxygen gas?
How many moles of solid iron are
required to react with 3 moles of oxygen
gas?
How many molecules of iron (III) oxide
are produced by the reaction of 4
molecules of solid iron?
SWBAT calculate mole relationships for chemical reactions.
4Fe(s) + 3O2(g)  2Fe2O3(s)
5.
6.
7.
8.
How many moles of O2 react with 8
moles of Fe?
How many moles of Fe2O3 react with
2 moles of Fe?
How many moles of Fe react with 12
moles of O2?
How many moles of O2 react with 16
moles of Fe?
SWBAT calculate mole relationships for chemical reactions.
Mole Ratio Practice
with your partner
 Page 1 #1-4


What if more than simple math is
involved?
SWBAT calculate mole relationships for chemical reactions.
4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of O2 react with 10
moles of Fe?
How many moles of Fe2O3 are
produced by the reaction of 20.0
moles of O2?
How many moles of Fe react with 1.2
moles of O2?
How many moles of Fe are required to
produce 7.0 moles of Fe2O3?
SWBAT calculate mole relationships for chemical reactions.
4Fe(s) + 3O2(g)  2Fe2O3(s)
5.
6.
7.
8.
How many moles of O2 react with 15
moles of Fe?
How many moles of Fe2O3 are
produced by the reaction of 8.0 moles
of O2?
How many moles of Fe react with 1.8
moles of O2?
How many moles of Fe are required to
produce 13.0 moles of Fe2O3?
SWBAT calculate mole relationships for chemical reactions.
Moles Ratio Practice
finish p. 1-2
 Begin your homework

Homework
Week 21 page 2-3: Tues.
 S’mores Lab: Tues
 Extra help:
Go to the blog
www.phascience.wordpress.com
and click “10th Grade Chemistry”
Watch the YouTube video – first link on the
page.

4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of oxygen gas react with
2 moles of solid iron?
How many moles of iron (III) oxide are
produced by the reaction of 1.0 mole of
oxygen gas?
How many moles of oxygen gas are
required to produce 0.35 moles of iron
(III) oxide?
How many moles of solid iron are
required to produce 0.5 moles of iron
(III) oxide?
SWBAT calculate mole relationships for chemical reactions.
4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of oxygen gas react with
10.5 moles of solid iron?
How many moles of iron (III) oxide are
produced by the reaction of 2.0 mole of
oxygen gas?
How many moles of oxygen gas are
required to produce 0.75 moles of iron
(III) oxide?
How many moles of solid iron are
required to produce 1.5 moles of iron (III)
oxide?
SWBAT calculate mole relationships for chemical reactions.
Homework
Week 21 Homework page
Need more help?
 search YouTube:
“phachemistry mole stoichiometry”
and watch the first video that comes up!

A: 7 February 2012



a.
b.
Take Out: S’mores lab
Objective: You will be able to:
 use mole ratios to calculate amounts of
reactants and products in a chemical reaction.
Do now: N2(g) + 3H2(g) → 2NH3(g)
How many moles of nitrogen gas react with 3
moles of hydrogen gas?
How many moles of ammonia (NH3) are
produced by the reaction of 5 moles of nitrogen
gas?
Agenda
Do now
II. More moles ratio examples
III. Practice problems
IV. Exit Ticket
V. Mass stoichiometry examples
VI. Practice problems
 Homework: Week 22 Homework p. 1: Fri.
Quiz on 5.3 through 5.6 Quiz: Fri.
I.
4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of oxygen gas react with
2 moles of solid iron?
How many moles of iron (III) oxide are
produced by the reaction of 1.0 mole of
oxygen gas?
How many moles of oxygen gas are
required to produce 0.35 moles of iron
(III) oxide?
How many moles of solid iron are
required to produce 0.5 moles of iron
(III) oxide?
4Fe(s) + 3O2(g)  2Fe2O3(s)
1.
2.
3.
4.
How many moles of oxygen gas react with
10.5 moles of solid iron?
How many moles of iron (III) oxide are
produced by the reaction of 2.0 mole of
oxygen gas?
How many moles of oxygen gas are
required to produce 0.75 moles of iron
(III) oxide?
How many moles of solid iron are
required to produce 1.5 moles of iron (III)
oxide?
SWBAT calculate mole relationships for chemical reactions.
What if…

we start with mass instead of moles?!
Homework
Week 22 Homework p. 1: Fri.
 Quiz on 5.3 through 5.6 Quiz: Fri.

A: 10 February 2012
Take Out Homework: Week 22 p. 1
 Objective: You will be able to:
 show what you know about objectives 5.3
through 5.6 on a quiz.
 use mole ratios to calculate masses of
reactants and products in a chemical
reaction.
 Do now: Predict the products:
I2(s) + CaCl2(aq) →

Agenda
Do now
II. Exit ticket statistics and self-assessment
III. 5.3 through 5.6 Quiz
IV. Mass stoichiometry practice!
Homework: Week 22 Homework p. 2-3:
Thurs.
I.
Percent of section C students
earning each score
1
2
6% 22%
3
61%
2.5
11%
Percent of section A students
earning each score
4 1
7% 7%
2
13%
2.5
13%
3
60%
Another statistic

60% of you didn’t use the correct number
of significant figures!
4Fe(s) + 3O2(g)  2Fe2O3(s)
Example 1:
How many grams of iron (III) oxide are
produced by the reaction of 10.0 grams of
solid iron in excess oxygen.

4Fe(s) + 3O2(g)  2Fe2O3(s)
Example 2
 How many grams of oxygen gas react with
5.00 grams of solid iron?

4Fe(s) + 3O2(g)  2Fe2O3(s)

1.
2.
3.
Your turn:
How many grams of iron (III) oxide are
produced by the reaction of 3.00 grams of
solid iron in excess oxygen?
How many grams of iron react with 50.0
grams of oxygen gas?
How many grams of oxygen gas are
required to produce 15.0 grams of
iron (III) oxide?
Challenge!

Solid calcium reacts with iron (III) nitrate.
How many grams of calcium are required
to produce 5.00 grams of iron as a
product?
Homework

Week 22 Homework pages 2-3: Tuesday
C: 9 February 2012
Take Out Homework: Week 22 p. 2-3
 Objective: You will be able to crack a code
by balancing equations and making mole
and mass calculations.
 Do now: C(s) + O2(g) → CO2(g)
a. Balance this equation.
b. How many grams of carbon are required to
produce 100.0 grams of carbon dioxide?
Round to the correct number of significant
figures.

Agenda
Do now
II. Check homework
III. Crack the code challenge!
Homework: Week 22 Homework p. 4-5
I.
Crack the Code!
At each station, work with your group (and only
your group) to:
1. Write and balance the reaction.
2. Identify the type of reaction.
3. Arrange the cards to show the work that solves
the problem at the station.
4. Copy down this work, calculate, and record
your answer to the correct number of sig. figs.
5.
Flip the cards over and record part of the code.
6. Use the code to figure out the message on p. 3

Your grade will be based on:
20 points for your work on the handout,
due at the end of the class.
 10 points for your citizenship:
 working with your group at the station
 staying on task and following directions
 maintaining a professional volume of
voice

10 minutes per station.
 Don’t move on until I tell you to!
 If you finish a station early, work on
homework problems.

Homework

Week 22 Homework p. 4-5
C: 17 February 2012
Take Out: CSI and Stoich lab
 Objective: You will be able to:
 determine the limiting reagent in a
chemical reaction.
 Do now: Describe in one complete
sentence why the confirmatory test was
required to make a good case against Omar,
your prime suspect.

Agenda
Do now
II. Collect CSI lab
III. Limiting Reagent examples and problems
Homework: Limiting Reagent Worksheet:
finish. Due Mon.
I.
H2 + 2O2 → 2H2O
Vocab
Limiting reagent: the reactant that limits
or determines the maximum amount of
product that can be formed in a reaction.
Excess reagent: reactant that is not
completely reacted; extra
Ex. 1
2Na(s) + Cl2(g)  2NaCl(s)
If 5 moles of sodium is reacted with 2 moles
of chlorine gas…
a. What is the limiting reagent?
b. How many moles of NaCl are
produced?
Ex. 1b
C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(g)
If 2.70 moles of C2H4 (ethylene) is reacted
with 6.30 moles of oxygen gas…
a. What is the limiting reagent?
b. How many moles of water are
produced?
Complete the front page of the handout.
Ex. 2
2Na(s) + Cl2(g)  2NaCl(s)
If 2.0 grams of sodium is reacted with 3.0
grams of chlorine…
a. What is the limiting reagent?
b. How many grams of NaCl are
produced?
Ex. 2b
C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(g)
If 5.00 grams of ethylene is reacted with
1.00 gram of oxygen gas…
a. What is the limiting reagent?
b. How many grams of water are
produced?
**c. How many grams of the excess
product are left?**
Complete page 2 of the handout
Homework

Calculating limiting reagents handout
back page
A: 17 February 2012
Take Out: CSI and Stoichiometry Lab
 Objective: You will be able to
 use reaction chemistry and
stoichiometry to solve a crime!
 Do now: Have you ever watched a crime
drama on tv? What chemistry have you
seen detectives and crime scene techs use?

Agenda
Do now
II. Lab intro and demo
III. Carry out lab part 3: Testing suspect
samples
IV. Lab part 4: Confirming your findings
Homework: Complete lab packet
I.
With your group

Summarize the article – 5 min.
As a class
Watch the demo, record observations and
discuss
 Complete the demonstration questions

With your lab group
Read the four suspect profiles
 Collect materials
 Carry out part 3: testing the suspect
samples and unknown
 Collect careful and complete data
 Clean up your materials and return them
to the kidney table
 Answer questions on page 7

Materials
We don’t have enough for each group.
Share with groups around you!
 Work really carefully and use only the
amount specified in the procedure.
 Make really complete observations about
color, transparency, pH, texture, gas
bubbles, etc!

Homework
CSI lab through page 8: Thursday
 Read pages 8-9 so you’re ready to go
tomorrow!

C: 16 February 2012
Take Out: CSI and Stoichiometry lab
 Objective: You will be able to:
 perform confirmatory tests to determine
the identity of the criminal!
 Do now: The unknown white substance is
_____________ because when I tested it
with ___________, I observed
_____________. Complete this TWICE.

Agenda
Do now
 CSI Stoichiometry lab part 4
 Post Lab questions
Homework: Complete CSI and
Stoichiometry lab: tomorrow
Quiz on 5.7: Mass to mass stoichiometry:
tomorrow

Confirmatory Tests!
What do we know so far?
 Why do a confirmatory test?
 How do we do a confirmatory test?

Massing
Use the same balance each time.
 Never mass a hot evaporating dish!
 Record your data as you collect it.


How will you know all the water has been
evaporated?
Clean up!
After you clean up
With your group, quietly, complete the
rest of the lab packet to show hard
evidence to prove the identity of the
unknown white solid.
 Check your lab packet for high quality
work and perfect completion.
 Turn it in.

Homework
Complete lab packet: tomorrow
 Quiz on 5.7 tomorrow
 You can use your note card or sticky
note.

C: 29 February 2012




Get out Homework: Metacog. Part 1
Objective: You will be able to:
 determine the limiting reagent and calculate
percent yield.
 review unit 5 objectives
Do now: Nitrogen monoxide gas reacts with
oxygen gas to produce nitrogen dioxide gas.
If 2.00 grams of nitrogen monoxide gas react
with excess oxygen gas, calculate the mass of
nitrogen dioxide gas formed.
Agenda
Do now
II. Review stoichiometry
III. A poem
IV. Limiting reagents
V.
Percent yield
VI. Review all unit 5 objectives
Homework: Week 24 Homework p. 1-3
Finish Unit 5 Review
Quiz on ALL of Unit 5 on tomorrow
I.
Limiting Reagents - Moles
2NO(g) + O2(g) → 2NO2(g)
1.
a. If 5.00 moles of nitrogen monoxide
react with 5.00 moles of oxygen gas,
which is the limiting reagent?
b. How many moles of nitrogen dioxide
gas are produced?
Limiting Reagents - Grams
2NO(g) + O2(g) → 2NO2(g)
1.
a. If 3.00 grams of nitrogen monoxide
react with 1.00 grams of oxygen gas,
which is the limiting reagent?
b. How many grams of nitrogen dioxide
gas are produced?
A: 1 March 2012
Take Out: Week 24 Homework p. 1-2
and Metacog. Worksheet
 Objective: You will be able to:
 review Unit 5 objectives for a quiz

Do now: 2NO(g) + O2(g) → 2NO2(g)
a. If 2 moles of NO are reacted with 2 moles
of O2, which is the limiting reagent?
b. How many moles of NO2 are produced?

Agenda
Do now
II. Track your exit ticket (5.7)
III. Limiting reagent homework
IV. Unit 5 Review sheet work time
Homework: Finish Unit 5 review sheet
Quiz on all Unit 5 objectives (except 5.9)
tomorrow
I.
10 Point Class Work Assignment

Criteria:
 Work with your assigned partner
 Stay on task
 Stay in your seat
 Use a professional volume of voice
 Ask for help when you need it!
Until the bell rings:
Week 24 Homework p. 1-2
 Unit 5 Review (skip #18)

Stay in seat
 Moderate the volume of your voice
 Don’t fall off!!

C: 1 March 2012
Take Out: Week 24 p. 1-2 and Unit 5 Review
 Objective: You will be able to:
 show what you know about Unit 5 objectives
 explain the difference between memorizing
and understanding
 Do now: Get your clicker!

Agenda
Do now
II. Review Unit 5
III. Quiz on Unit 5
IV. More metacognition: Memorization vs.
Understanding
V. Percent Yield
Homework: Week 24 p. 3 and
Metacognition Part 2 worksheet: Fri.
I.
2NO(g) + O2(g) → 2NO2(g)
a. If 3.00 moles of nitrogen monoxide react
with 1.50 moles of oxygen gas, which is the
limiting reagent?
b. How many moles of nitrogen dioxide are
produced?
2. a. If 100. grams of nitrogen monoxide react
with 50.0 grams of oxygen gas, which is the
limiting reagent?
b. How many grams of nitrogen dioxide are
produced?
Begin pages 1-2 of your homework.
1.
C: 2 March 2012
Objective: You will be able to:
 calculate percent yield
 explain the difference between memorizing
and understanding
 Do now: If you calculated that your
theoretical yield should be 4.00 grams, but
your experiment only produced 3.75 grams,
what is your percent yield?

Agenda
I.
II.
III.
Do now
Percent Yield
More metacognition: Memorization vs.
Understanding
Homework: Week 24 p. 3-4 and
Metacognition Part 2 worksheet: Mon.
Percent Yield
C2H4(g) + 3O2(g)  2CO2(g) + 2H2O(g)
If you calculate that the reaction of 5.00
grams of ethylene with 3.00 grams of
oxygen will yield 2.75 grams of carbon
dioxide, should you expect the actual
reaction to really yield exactly that much?
Why or why not?
Vocab
Theoretical yield: maximum amount of
product that could be formed given the
amounts of reactants.
(Calculated on paper.)
Experimental yield: the amount of
product that actually forms during an
experiment
(Determined by doing an experiment.)
Equation
Percent Yield is usually < 100%
Why?
• Reaction not going to completion
• Impure reactants
• Side Reactions: a product reacts with a
reactant
• Loss during filtration or pouring between
containers
Quicklime
Limestone (calcium carbonate) is heated
to 900oC to produce quicklime (calcium
oxide) and carbon dioxide gas.
 Quicklime is used to decrease the acidity
of fields to increase crop yield and to make
concrete and other industrial products.
 It was key for the rise of civilization in
Europe!

Ex. 1
CaCO3(s) → CaO(s) + CO2(g)
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You calculate that, with the masses of
reactants used, your experiment should
have yielded 3.00 grams of solid calcium
oxide. However, you only got 2.00 grams
of calcium oxide. Calculate the percent
yield.
Ex. 2
CaCO3(s) → CaO(s) + CO2(g)
a. What is the theoretical yield of CaO if
24.8 grams of CaCO3 is heated?
b. What is the percent yield if 13.1 g CaO is
actually produced?
Ex. 3
Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)
When 84.8 g of iron (III) oxide reacts with
an excess of carbon monoxide, 54.3 g of
iron is produced. What is the percent
yield?
Practice Problems!
Fe2O3(s) + 3CO(g)  2Fe(s) + 3CO2(g)
1.
2.
3.
You calculate that your reaction should have
produced 10.0 g of iron, but only 6.8 grams
were produced. What is the percent yield?
When 10.0 g of iron (III) oxide reacts with an
excess of carbon monoxide in an experiment,
only 6.45 g of iron is actually produced. What
is the percent yield?
When 5.00 g of iron (III) oxide is reacted with
1.00 g carbon monoxide, 1.20 grams of iron is
produced. What is the percent yield? (Hint:
Calculate the limiting reagent FIRST!)
Homework
Week 24 p. 3-4
 Metacog. worksheet part 2
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