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0
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Unit 8
tions
Chemical
Textbook Chapte
5
January 4
Student Holiday /
Teacher Work Day
Friday
Thursday
Wednesday
Tuesday
Monday
7
6
Nomenclature
Review
Chem Rxn
Day 3: Balancing
Reactions
Law of
Conservation of
Mass Lab
HW: pg 8
HW: pg 10 - 11
Day 2: Writing
Day 1:
Day 4: Redox
HW: pg 14
HW: pg 5
11
12
Day 5: Types of
Day 6: Single
Redox
Replacement
Reactions
15
Day 8: Double
Day 7:
Single
Compound
Formation Lab
Replacement
Replacement
Continued
HW: pg 17
14
13
HW: pg 27
HW: pg 21
Chalk Labÿ(ÿU ÿ2-)
Hwk: pg 24
18
Celebrate
Review
No School
STUDY GUIDE
DUE (pg 30-33)
MLK
Name:
22
20
19
Test: Chemical
"" Reactions
Period:
Day 1: Nomenclature Review!!!!!!!!!!
Before naming/writing any formula,
Identify the type of compound.
• Ionic --> Metal and a Nonmetal
If Ionic: Does the metal need roman numerals in the name?
If Ionic: Does the compound have a Polyatomic Ion?
• Molecular -) Only Nonmetals (Use Prefixes in the name)
Ionic Compounds
Ionic bonds are formed between a metal and a nonmetal OR ;ÿ cation + anion.
Naming ionic compounds
* First name the cation and then the anion.
(metal)
(nonmetal)
* Change the ending of the anion to -ide.
Example:
MgCI
Prefixes used for naming
magnesium chloride
2
Covalent Compounds
Wdting Fom]ulas for Binary Ionic Compounds
*znmber
indicated
USE THE CRISSCROSS METHOD
+ÿ
-2
Example: Li O
1
\'>(
If yotlr£aÿ,,qn is a transition metal,
then you must specify the charge
with a ÿ,
dl-
2
tt:i-
B
telmaL-
4
laeÿta_-
5
heÿa-
6
7
Exemple : iron (llr) Sulfide
Fe ÿ+ Sÿ- ÿ:ÿUse crisscross method to predict chemical formula"
,oc, ta;-
g
IlOiqiÿ-
9
Fe2Sa
EXCFPTIONS: These four metals DO NOT require a roman numeral!
AIa+, Zn2+, Cd2÷and Ag+
10
A polyatomic ion are groups of atoms that behave as one unit.
They are treated like single ions in formulas, but use parenthesis ( ) when more than one is used in a formula.
Ba(OH)2
Barium hydroxide
CaSO4 Calcium sulfate
(NH4)3P
Ammonium phosphide
Covalent Compounds
To name a covalent compound, name the first element, then name the second one and change its ending to
-ide. Use prefixes to show how many atoms of each element you have.
P205
CCI4
diphosphorus pentoxide
carbon tetrachloride
To write the formula of a covalent compound, simply translate the prefixes and element names.
Dinitrogen dioxide
Diphosphorus heptoxide
N202
P207
Let's Practice Nomenclature
,ire the formula for the following compounds.
1. Fe3+andNO3-
Name the following compounds.
ÿ--ÿ(°ÿJ0ÿ)ÿ
6. HgO ÿJÿ(jL]ÿrÿ 'ÿ
2. sodium oxide
7. LiBr
3. dinitrogen trioxide
ÿNJÿ Oÿ
8. SOÿ Sÿ/ ÿ'lJ'fÿ P'lOÿ}d'ÿ
iron(III) chloride
,
.
Law of Conservation of Mass Experiment
Problems:
1. How can the law of conservation of mass be verified?
2. How can we determine if a chemical change occurred?
Background:
Antoine Lavoisier formulated the Law of Conservation of Mass, which states that matter cannot be created or
destroyed, During a chemical reaction, the bonds of the reactants are broken, and the atoms are rearranged to
form new substances. Because matter must be conserved, the mass of the products, must be the same as the mass
of the reactants. In this lab you will verify the law of conservation of mass using the following reaction.
2NaOH (aq) +
CuSO4 .... ")
Na2SO4 (aq)
÷ Cu(OH)2 (s)
Pre-Lab Questions:
2S (s) + 302 (g)
1.
ÿ 2SO3
In the above reaction, 2.6g of S reacts with 2.0g 02. How many grams of SO3 are recovered.
:
,
2HCI + Mg ") MgCI2 + H2
In the above reaction, 5.0g of HCI react with 2.0g Mg. 3.0g of MgCI2 are recovered, how many grams of H2
werelost.
.
-1 ÿ- ÿ-3r-')/,ÿ
X= Lÿ.-ÿ 01ÿ ÿL
What arÿ the four indications of a chemical change?
a.
C.
d
Form he l+
Procedure:
1. Pour 10.0 ml of CuSO4 into a plastic measuring cup and label it.
2. Pour 10.0 ml of NaOH into a second plastic cup and label it. Carefully put each solution on the balance and
record the mass in the data table,
3, Pour the NaOH into the CuSO4. Use the stirring rod to mix the solutions. Describe what happens in your
qualitative observation section.
4. Put both containers (including the empty NaOH cup!) back on the balance and record the new mass. Did
the mass change? Record your answer in the observation section. Dispose of chemicals as teacher directs.
Data Table 1 :
Mass of cup 1
Mass of cup 1 and NaOH
Mass of NaOH
Mass of cup 2
Mass of cup 2 and CuSO4
Mass of CuSO4
Mass of cup 1 and 2 after mixing
Calculations:
Calculate the total mass of the reactants. (Add 3. And 6. From data table)
Post-Lab Questions:
.
The mass before the reaction is calculated above. The mass after the reaction is 7. in your data table. Do
your values for the total mass before and after each reaction verify the Law of Conservation of Mass?
Explain in complete sentences.
2. What indicators of a chemical change were observed? Which indicators were not observed?
4
Day 1: Homework
Na + CuS -ÿ NaÿS + 2 Cu
In the above chemical reaction; you reacted 25.0g Na with 15.5g CuS. What is the total mass of your
,
,
The reaction for the burning of 15.O a of ethanol (CH3CH2OH) looks like this:
2 CH3CH2OH (I) + 7 02 (g) -) 4 CO2 (g)+ 6 H20 (I)
The mass of the products is 30.Og. How much oxygen was consumed in the reaction?
3. A solid has a mass of 35 g. When it is mixed with a solution, a chemical reaction occurs. If the final total
mass of products is 85 g, what was the mass of the solution that the solid was mixed with?
4, The word equation for the following reaction is as follows:
vinegar + baking soda -ÿ sodium acetate + water ÷ carbon dioxide
The chemical equation for the reaction is:,
C2H3OzH + NaHCO3 -ÿ NaC2H.ÿO2 + H20 + COz
Use the data table below to find the answers to the three ?.
Mass of Weigh Boat
2.0 9
17.09
Mass of Weigh Boat and baking soda (NaHCO3)
?iq
Mass of Baking soda
Mass of 9raduated cycliner
Mass of Wÿ and vinegar (CzH302H)
Mass of vinegar (C2H3OzH)
Mass of NaC2H302
Mass of H20
Mass of COz
,
50.09
lO0.Og
40.09
15.09
? ioo
A full, unopened bottle of Dr. Pepper® has a mass of 1,250.0 grams. After opening the bottle
(but before taking a sip!)- the beverage now weighs 1050.0 grams. In your own words, explain why
the soda seemed to have lost mass.
5
Day 2:
Nomenclature Review: Write the formulas for the compounds below.
aluminum oxide
/ÿ12ÿ.0ÿ
nitrogen trioxide
ÿJ 0ÿ
sodium carbonate
ÿ
lead(IV) oxide
copper(II) nitrate CÿLÿ ÿ'ÿ1%ÿ (ÿ Lÿ)'2ÿ
So now let's write some chemical equations!
Summary'.
,
6
Wÿhen lormore ÿ ÿ0ÿl ÿ aÿ ÿaC tÿd to pÿodÿcÿ toÿaÿ ÿy ÿw co ÿpouÿdÿ that have
chemical ÿd physfÿaÿ 1 ÿÿÿ than they did before.
A chemical reaction is represented by writing a Cÿh ÿ iÿ{)j ÿ tÿ,(ÿ L) CZ[ÿ
1 U ÿ ÿ ÿg chemical formulas, symbols, and Cÿ ÿ iÿ ÿ ÿ
An equation represents the identities and relative amounts of what are called ÿ-ÿ(,ÿ ÿITLÿ
and
products in a chemical reaction.
- rÿiÿ)ÿ
are the substances you start with in the reaction.
- ÿ2ÿ ÿ)0Jfÿ2
are the results of the reaction.
Ingredi
ts
called "reactants" "
toefhc{a
re.
:
.....
ÿ:ÿ;ÿ ;:ÿrÿ ÿrÿ,ÿ .ÿ,ÿ,ÿ ,ÿ ÿ;,ÿ-.-ÿ.ÿ
r
su ÷or r4-
• To know for certain a chemical rxn has taken place requires ÿL/{ÿ'ÿ/ÿ that 1 or more substances have
• Absolute proofofsuchachangecanonly'beprovidedbychemically
i
EVIDENCE OF CHEMICAL CHANGE
1. ÿ0ÿL)0ÿI[ÿ(] f)'ÿ ÿ0ÿ This is usually indicated by bubbles. Bubbles don't always mean a gas is being
produced (Air bubbles, bubÿ'les when something boils).
2. ÿ)(ÿqDÿlbÿfÿ 0Jr' ÿF'ÿ2ÿOJÿTÿis is called a precipitate (ppt). If 2 liquids are combined and a solid
substance suddenly appears, this means that a new substance has been formed.
3. C0 Iÿ/Y" ÿVIÿ2/
When a different color or odor appears suddenly, this means a new substance
with new properties has formed.
4. ÿ0(ÿJrv]0}ÿ'ÿdTÿ 0Jÿ hÿ-/ÿk
If a substance becomes warmer in temperature even though no
heat is being added, that is a clue that a chemical change is occurring. Substances can also get lower in
temperature due to a chemical change•
Writing and Balancing Chemical Reactions: Common Symbols in Reactions
:ÿ:ÿ :ÿiÿ!i :ÿ
Symbol 'ÿ
Meaning= !i:
z
"=
Separates Reactant from Reactant
%
or
Separates Product from Product
"Yields" (indicates result of reaction)
Separates Reactants from Products
solid
pure liquid
gas
dissolved in water or in solution
heat is added to the reaction
A catalyst is added to the reaction.
A gas is produced.
A solid is produced.
Common Substances in Chemical Reactions
=: i:=
.
.=
===
:=: Formui ( )ÿto
emo zeÿ
==
Diatomic Elements
Water
Ammonia
Key Words Used in Describing Chemical Reactions
Words used to separate reactants from
other reactants.
Words used to separate reactants from
- q leloL
- 0omjvoÿ.bÿJ,ÿ
products.
- Oecÿfoÿ
Class Practice
Vÿ q-t-o ÿ-
For each of tÿllowing examples write the correct chemical formulas and symbols.
1 Wheÿsolid tungsten metal reacts with oxygen gas to produce solid tungsten (VI) oxide.
+ -ÿ.
tÿ- Noÿ,--
Plÿÿ- 2: -
2. Solutions of sodium ioÿdide and lead (II) nitrate are mixed and form the precipitate, lead (II) iodide and
aqueous sodium nitrate.
A:I'ÿ OZ..
When
, solid a ummum oxide decomposes to form alumin/ÿuu }m metal and oxygen gas.
Day 2: Homework
Directions:
For each item in Column A, write the letter of the matching item in the word bank. Each
choice in Column B may be used once, more than once, not at all.
Column A
C 1
The new substances that are formed in a chemical reaction
A chemical reaction that involves one or more substances change into new substances
Shows the relationship between the reactants and products in a chemical reaction
States the mass is neither created nor destroyed during a chemical reaction
The starting substances in a chemical reaction
_Jÿz_6.
The substances appearing on the left side of the arrow
The substances appearing on the right side of the arrow
Word Bank
a. Chemical Change
jÿ€ Reactants
Products
.ÿtÿ. Chemical Equation
.ÿ.¢fLaw of Conservation of Mass
Directions:
For the following problems, write the chemical equation for each reaction. Answer the question
using the equation and the Law of Conservation of Mass. Show all work on your paper.
8. In a laboratory, !78.8g of water is separated in hydrogen gas and oxygen gas. The hydrogen gas has a
mass of 20.0g. What is the masÿs of oxygen gas pÿ
lqy,, ÿ
-
7/o
"ÿ'-ÿ'-ÿ
+
9. When calciu_=_m is placed in water, it reacts to form calcium hydroxide and hydrogen gas. A student reacts
2.3g of calcium reacts with 13.8g of water. After the reaction is completed, the student determines
that a total of 1.2g of hydrogen gas was produced. How much calcium hydroxide was produced in this
reaction?
2,3 .+
i ,gD
=
------
Directions: Answer questions #10-14 based on the reaction below.
HzSO4(aq) + NazCOs(s) -) CO2(g) + NazSO4(aq) + HzO(I)
11. What is the physical state of water in this chemical reaction?
12. What is the physical state of sodium carbonate in this chemical reaction? SO ilÿ
13. What sign of a chemical change is demonstrated by this reaction?_pÿOÿ d CÿOÿ
)
Day 3: Review / BALANCING CHEMICAL EQUATIONS
Chÿlom ilL oxÿd.g
Crz03
AgNoÿ
DJI¢ÿ Nÿbÿiÿ
P02
.ÿltJrnlntJm chll orld6
AICI3
Lÿ]0 i g Iÿtr
: He is the father of modern chemistry, and first described the "Law
of Conservation of Mass."
Antoine Lavoisier found that the mass of the reactants and the products are
tJÿ 'i , even when the states
of matter change. Matter is neither created nor destroyed
Vlÿr-Vÿ,h6ÿ D,ÿ 01]iÿ1€ÿ : The number of each type of atom on the reactants side of the
chemical equation MUST be equal to the number of each type of atom on the products side of the equation.
0 ÿ'ÿh Ol.ÿJÿJf"
tÿ I{)ÿcp--ÿ
: Represents the number of units of each substance taking part in the reaction.
ÿJhÿ J(-ÿ /
ÿ Jÿ'ÿ/-/ÿ : The same number of atoms of each
element on both sides of the equation.
Four Steps to Balance Equations:
2. coont 4hÿ, avarice,,, oÿ aÿ¢
il ol0eÿvrt- balmvÿoe.Is this chemical equation balanced?
N2 +
Guided Practice: Balance these equations:
.
Hz -)
ÿ NHs
d
Aÿzÿ
**How many oj= each element do we have? Are both sides equal?
.H2 +
4" 2..
,
i Mg +
ÿ HCI--)i
IH2+
-ÿ.f H '. 7-..
Na+
oÿÿNaCI +
-
,9-
z. 4-- -hÿ z.
Day 3 Homework
Writing and Balancing Chemical Equations
1.
2,
i N2 + ÿ'Oz ÷
2" NO z
Magnesium Nitrate + Calcium Hydroxide ÿ Calcium Nitrate + Magnesium Hydroxide **use polyatomic Ion list.
. __J_Hÿ ÷ i ,clÿ_. 2"HCI
4. Magnesium Chloride + Sodium Iodide ÿ Magnesium Iodide + Sodium Chloride
6.
i Ca+ ¢ÿHÿO-ÿ I
7. P- .c÷2_oÿ ÷ ÿ co
@
.
Sulfuric Acid(HzSO4) -ÿ Sulfur Trioxide + Water
10
lO ¢- Hc,+__LMg÷ i Mgci2+ÿl .2
II. "2. AU (ÿ) +
-ÿ
13 I S(s) +
02 (g) ->
ÿ AlÿO3
__ÿ____Ag +
I .02
$ Oz(g) >
i H20 (I) l> ÿ-" HNO3
14.ÿ1 NzO5 (g)
15.
ÿ S03
ÿ l II CaO (s)
+
I H20 (I) ÿ J ICa(OH)2
+
17.
I CH4 +
ÿ 02--)
ÿ- H20 + ÿ COz
18. i SrFz + I Na2SO4 --ÿ ---L- SrS04 + ÿ NaF
.19.
Pb
21 ÿ- KOH + )
22. ÿ___Fe +
3
2
+
Hÿ÷
i
H2SO4-->
i
Kÿ + ÿ" H20
I Fe2Sÿ3 +ÿ ÿ Hz
11
Day 4: Oxidation-Reduction Reactions (Redox Reactions)
Reaction Types are put into three categories:
All of the reaction types we've discussed can be placed into one of 3 categories:
*Acid- Base (Neutralization)
*Precipitate
*Oxidation-reduction (Redox)
In this unit we will be looking at Precipitate and Redox.
Ae
( Synthesis, Decomposition and Single Replacement reactions)In redox reactions the oxidation number for an element ÿtÿm ÿ
in a chemical reaction.
0ÿ14ÿ ÿVÿ Number: A number assigned to an element, based on the distribution of electrons. The
same element can have very different properties in different oxidation states.
Rules for Assigning Oxidation #s
Examples Oxidation #
0
1 The oxidation number of any uncombined ELEMENT is Na,
02
Na = O ,Oÿ = O
The ox. # of an ION equals the charge of Cl"
the ion
2
CJ= -I
3 The ox. # of elements in COMPOUNDS typically, but not always
(unless noted otherwise), folbw a trend on the periodic table:
Group I = +1 ÿ_ALWAYS
LiF
Li= +1
Group 3 = +3
CaC03
Ca = ,+ÿ
Group I5 = -3
HF
F= -I
H20
H° +1
Group 2 = +2 ......
Group "I6 = -2 (O usually -2)
Group t7 -= 4 (F ALWAYS -t)
Transition metals AND Group 14 = variable charges
Note: H has exceptions but we will use *1 in this course
4 The sum of ox.#s of all atoms in a NEUTRAL COMPOUND Js 0
LiF
+F=J-
0
CaC03
c-.t( j =
0-2 (x3)=.,-ÿ
0
The sum of ox. #s of all atoms in a POLYATOMIC ION equals the
charge of the ion
SO42`
+0 -2 (x4)='-ÿ;
-2
Note: Additional rules/exceptions to these rules do exisÿ but are beyond the scope of this course.
12
o06ti']2ÿ On
]ÿ"{'qOÿ is a reaction in which
which there is the gain of electrons.
there is the loss of electrons.
0
is a reaction in
0
+1
-1
Ex: CIz ÷ 2e- --> 2CI-
Ex: Na --> Na÷1 + e-
"OIL RIG"
"LEO the lion says GER"
Losing of Electrons is Oxidation
Gaining of Electrons is Reduction
Since oxidation is the
OR
i 0ÿ
Oxidation Is Loss (of electrons)
Reduction Is Gain (of electrons)
.of electrons and reduction is the ,ÿ1ÿ i i/1
electrons, they must occur simultaneouslylÿI
Lj
** Any chemical process in which elements undergo changes in oxidation number is an
oxidation - reduction reaction, or redox reaction for short.**
Practice determining whether the following elements have been oxidized or reduced and label
the reaction.
0 o
Example t:
4ÿ -2-
4Fe + 302 --> 2Fe203
TYPE of Reaction: SID!SR/DR
Element Ox,# Reactants side Ox,# Products side Lose/Gain e" OxidizedlReduced
Fÿ,
0
0
,-kÿb
0
- ÿ-
LOc.Dÿ S
a s in :z.
OXiotiÿ
ÿD,soÿA
0 +1-1 -i-z-i 0
Example 2:
Element.
Ox;# Reactants side
-t+
Q
TYPE of Reaction: S!D!SR!DR
Mg 4- 2HCi -Y MgCl2 ÷ H2
Ox.# Products side
0
+l
0
Element Ox.# Reactants side
r-&4uÿL
oj oilvÿ /
4-2.
oÿ <,-l.
-)
Example 3:
OxidizedlReduced
LosetGain e*
e_,,i.t4ÿ
+ NaOH -ÿ NaCI: .+ H20
vqÿ
TYPE of ReaÿDR
Ox.# Productsÿi e Lose!ÿ'ÿxidized/Reduced
/
ÿ-,J
¢04
Note: ALL of the reaction types we have teamed are tedox reactions EXCEPT for double
replacement reactions.
13
of
Day 4 Homework
.
Label the following as an oxidation or reduction reaction,
Ag ÷ Ag++ e-
oÿti4D2.ÿ
Fz + 2e-÷ 2F-
@<4octlon
Cu ÷ Cuz÷ + 2e-
OX i4 ottl ÿt,.,
2. Complete the tables below.
0 0
if 2-
1. 2Ag + S ÷ Ag2S
Circle. TYP
e: SIDiSRIDR
.
Element ! OX:#Reactants side
.......
• ÿ
Oxÿ# Products side Lose!Gain e" Oxidized/Reduced ...............
0
i+
i oÿ i
o×ÿ4 iÿ,ÿt
O Zÿrl- i4-1-" O
2Na + FeCi2 --) 2NaCi + Fe
Ox,# Reactants side
Circle_Type: SIDISÿDR
Ox.# Products side LosetGain e" Oxidized/Reduced
s,/- 0 0
3. 2AI0i3 ÷ 2AI + 3Cl2
Element Ox.# Reactants side
Dri
Circle Type: SIDISRdDR
Ox:# Products side ........ LoseiGaln e Oxld!zed/Reduced
ÿ,4-
....................................... I .......................................................................................... II ................................................................................................. t: ............................................................... ÿ .......................................................................
14
Day 5: Types of Redox Reactions
Synthesis (also called Combination or Composition)
Synthesis means" ÿDf -jÿOÿe,,.-lvÿ ÿ ,
2 or more elements/simple compounds combine to form I compound.
General form: A + B --) AB
Identifyincl feature: only one_ ÿ) ÿOgÿOÿ
Analogÿ: A boy and a girl come to the dance separately, but end up dancing together.
EX: 2Mg÷Oz÷2MgO
EX: The combination of iron and sulfur to form iron (II) sulfide: Fe + S ÷ FeS
EX: Burning Charcoal: C (ÿ ÷ Oz ÿ --) COz ÿ
2. Decomposition
Decomposition means" ÿ0 K'ÿ ÿ( OL? ÿ ÿ1"
"
1 compound is broken down into 2 or more simpler elements/compounds.
General form: AB --) A + B
Identifying feature! only one (ÿÿJÿ
(opposite of Synthesis!)
Analogy: A boy and a girl are a couple, but they had an argument. This resulted in the boy and the girl
staying apart for the rest of the night.
k
z
Examples: 2 NaCI ÷ 2 Na + CIÿ
2 KCIOz ÷ 2 KCI + 30z
EX: The electrolysis of water to make oxygen and hydrogen gas: 2HzO 0) ÷ 2Hz ÿ + Oz ÿ
3. Combustion
Always follows the some form: Iÿ0ÿqÿ0b/Vÿ
Compound containing C and H (& sometimes O) + Oÿ ÷ CO2 ÷
15
HÿO
Note: In a combustion reaction, the compound always burns in ÿ gas and always releases
carbon dioxide and water.
During incomplete combustion (a limited amount of Oz), carbon monoxide (CO) is also produced.
Examples:
CH4 + 2Oz÷ COz + 2H20
2C3H6 + 902 ÷
6CO2+ 6HzO
**Trick for balancing tough combustion reactions:**
Balance from right to left,
1. Balance the H first by placing a coefficient in front of the water.
2. If that coefficient is ODD, double it and proceed with balancing C, then O.
3. If even, leave it alone and proceed with C, O.
4. Always balance oxygen last!!!
Exam..12ÿ.: ÿ"
2..-ÿ
1. ,ÿ C7H14 + ÿO2 -)'
ILÿ
jÿ
.ÿCO2 + .,.,ÿ H20
In class practice for balancing combustion.
1.
i
04H8 +
ÿ 02 --)'
Iÿ
CO2 +
@H20
2. i CÿH,2+ (ÿ O2--> ÿ" CO2+ b H20
3..-"ÿ C9H18+$O2--'> ÿCO2+ ÿ H20
2-2.
2-2,-
4. ÿ C,IH22+ ÿ 02-> ÿ4fCO2+
16
ÿ'H20
Day 5: Types of Reactions Homework
Balance and Identify the following:
synthesis = S
decomposition = D
combustion = C
Find Oxidized and Reduced Elements in 1., 3, and 5.
Reaction Type
Ox# Reactants
Element
AIz03
o2 (g)
1. ÿ AI (s)
Pri
Ox# Products
Lost/Gain e-
34-
0
0
0
Oxid/Red
:e:.,Ioÿ
Use Cu1+
Element
Ox# Reactants
04
0
ÿ i+
0
4. J soÿ(g) +
Element
Lost/Gain e-
ÿ-
:2-
Ox# Products
ÿÿ
Lost/Gain e-
0
0
iÿ- o2
-ÿ Mr C02 +
Oxid/Red
oxÿjzeÿL
IH=oo) ÿ i H=SO.
Ox# Reactants
__. CoH6÷
Ox# Products
:ÿ JÿS
Oxid/Red
uÿoL
OX IoIÿ ÿoL
H20
C
12-
C
,
.
i
17
Day 6: Single Replacement
Single Replacement
1 element takes the place of another in a compound ("like replaces like")
General forms: A + BC ÷ B + AC
D+BC÷C÷BD
(metaJ repJacement)
(halogen replacement)
Identifying feature: I element + 1 compound on each side of the arrow
Analogÿ: A boy and a girl are dancing, but then another boy '*cuts in" and dances with the girl, Jeaving
the first boy alone. Or a boy and a girl are dancing, but then another girl *ÿcuts in" and dances with the boy, leaving the first girl
alone. "Like" must replace "like"
Examples:
Metal replacement: 2 Na + CuCI2 ÷ 2 NaCI + Cu
Halogen replacement: F2 + 2 KCI ÷ 2 KF ÷ CI2
BUT the boy/girl will not always be able to "cut in." Sometimes the other boy/girJ will not let them!
Rules for Reactions Including: Metals with Metals/Metals with Acids
We must use the 0ÿVÿ
to predict whether or not the
replacement will occur.
A= Metal
B= Cation
C= Anion
18
ST AE
You can use the activity
series to predict whether
or not certain reactions
will occur. A specific
metal can replace any
metal listed below it
This is what it
looks like! You
Hetal
that is in a compound. It
[itNum
cannot replace any metal
:Potassium
listed above it. For
example, copper atoms
Barium
replace silver atoms in a
Cal:dum
can find this on
the BACK of the
Periodic Table of
the Elements.
solution of silver nitrate.
Sodium
However, if you place a
Nagnesium
silver wire in aqueous
Aluminum
copper (II) nitrate, the
Nanganese
silver atoms will not
replace the copper. Silver
Zinc
is listed below copper in
Chromium
Metals found higher up
in the activity series
means the metal is
MORE REACTIVE.
the activity series, so no
Iron.
reaction occurs. The
Cobÿtt
letters NR (no reaction)
Nickel
are commonly used to
indicate that a reaction
Tin
will not occur.
Lead
(Nydroÿlen)
Copper
**This applies to the
Nercury
nonmetal halogens as well.
Silver
They increase as you move
Platinum
up the family.
Predicting Sin qle Replacement Reactions
**Important Reminder: A metal can only replace another ÿ'ÿi
Rule #1: Metals will replace metals that are j#ÿf"
themselves on the Activity Series. ( The substances willswitch partners)
A and B are metals, and X represents a negative ion.
-Will the reaction proceed? If yes, what are the products?
A + BX-->
(Higher) (Lower)
A + BX->
(Lower) (Higher)
19
ÿ4-
or
than
Using your Activity Series, predict which reactions will occur:
2. FeCl2(aq)+ Cu(s) -> NO ÿ2_.iÿJ#'wxÿ
3. Sodium + Lithium Chloride -> [ÿ0 ÿ,ÿ (tÿ
!Z 4. Silver Nitrate + Zinc -> ÿ-'lm(_., ÿl'ÿtZÿ'ÿ-ÿ Jrÿ ÿilVÿ-,'r
Predicting the Products (meta/s and metals):
1. ÿ_ÿ_MÿAICIs(aq) ÷ 'ÿ/ÿi
2. Silver Nitrate+ Zinc ->
ÿ _
2./%ÿ] ÿOz + ÿn ---ÿ
<_j"
I
Rule #2: Any metal above
ÿ?ÿ
will react with an acid to
produce a compound + Hiÿ. Put Hÿ at the end of your arrow.
Example:
M= metal
X= negative ion
Using your Activity Series, predict which reactions will occur:
1. Zn+HCI-> ÿ/ÿ1.
2. Cu ÷ Hÿsoÿ ÷ gO i
Predicting the Products (metals andacids):
1. ÿ.zn + ÿ Hct ÷ 7ÿ bl
#
2. Calcium + Phosphoric Acid ->
2O
Day6: Homework
,
Circle any reactions that will NOT occur.
Ba + NaNO3
Fe + Pb(CzH3Oz)z
M9 + HCI
,
Cu + AgNO3
Using your activity series, determine if the reactions below will occur. If the reaction
will not occur, write no reaction. If the reaction will occur, predict the products of the
reaction and write a balanced chemical reaction.
a.
C°
Ag + Cu(NO, k ÷
zÿ ÷ ,ÿHcl ÷
140
'Z4n d3. +
d. 2--- A I + ÿ Cu(NO3)z -->
e. Au +
HBf ÷
21
Day 7: Redox Reactions continued...
Rule #3: Any metal that is ÿ0ÿiÿ ÿ)ÿ
will react wit!
water.
Help_ÿHÿLnÿt: Think of water as ÿ --
0
ff
Using your Activity Series, predict which reactions will occur:
2. Calcium metal is placed in water. Veÿ 1,
3. A sample of cadmium is placed in a test tube of water.
Predicting the Products (metals and water):
2. Calcium metal is placed in water.
Using your Halogen Activity Series, predict if the following reactions will occur:
2. Chlorine gas is bubbled through a solution of sodium iodide.
3. Liquid bromine is mixed with a solution of potassium chloride. ÿ) 1
4
Predicting the products (halogensÿ.
1.
,
Chlorine gas is bubble through a solution of sodium iodide.
22
Experiment on the Types of Reactions (Chalk Lab)
Purpose
How do you identify the various types of reactions?
Procedure
1. Obtain a small piece of white chalk, which is basically calcium carbonate.
2. Holding the chalk with a set of tongs, heat a piece of chalk in the hottest part of the Bunsen burner for
three to five minutes.
3. While heating, add lOOmL of water to a 15OraL beaker.
4. Add 2-3 drops of phenolphthalein to the water. Record the initial color of the solution.
5. After heating the chalk, place the chalk into the water solution.
6. Using a stirring rod, stir the mixture in the beaker. Note any change in color of the solution.
Initial Color of the Solution
Final Color of the Solution
Analysis Questions
1. When the chalk or calcium carbonate is heated, it forms solid calcium oxide and carbon dioxide gas. Write
the balanced chemical equation. Be sure to indicate the physical state of each substance and show how you
can represent the heat of the Bunsen burner.
2. What type of reaction is being described in question #1?
3. In order to decompose the chalk, you relied on the combustion of methane as your source of heat, Write
the balanced chemical equation for the combustion of methane, CH4.
.
The solid calcium oxide, which is produced while the chalk is being heated, undergoes another reaction when
it is placed in the water. The solid calcium oxide reacts with water to produce aqueous calcium hydroxide.
Write the balanced chemical equation for this reaction. Be sure to include the physical states of all
reactants and products.
5. What type of reaction is being described in question #4?
ANSWER IN COMPLETE SENTENCES!!
23
Day 7: Homework
1. Circle any reactions that will NOT occur.
LiCI + F2
Na + H20
.
H20 + Fe
Using your activity series, determine if the reactions below will occur. If the reaction
will not occur, write no reaction. If the reaction will occur, predict the products of the
reaction and write a balanced chemical reaction.
b. H20+ _Pb->
e.
I2 +
NO ÿ.ÿ2ÿ ÿ112ÿ
NaF--)
24
Day 8: Precipitate or Double Replacement Reactions
Ions from 2 ionic compounds switch places.
AB + CD ÷ CB + AD
+ÿ
+
* A and C (the cations from each compound) switch places *
*Combine inner ions with outer ions*
Identifyinq feature: 2 compounds on each side of the equation
Analogÿ: 2 boy-girl pairs are dancing, and they switch partners.
Example: FeCI2 + Na2CO3 --} 2 NaCI ÷ FeCO3
An insoluble compound
A soluble compound
,.¢ olidl or- (ÿ) lvl 64
How to determine if a substance is
soluble?
You will use this chart
Soluble
compounds contain
Cÿ!-IÿOÿ, CH< CO0NH+
Common eX¢ÿDIIOIIS
None
None
NOÿ
None
CN-
None
ClO-
None
Nonÿ
clo7
c]o;
None
Nÿne
Compounds of Ag+, Pbÿ+, and HOÿ÷
CI-
Compounds of Ag÷, Pbÿ+, and Hgÿ+
I-
Compounds of Ag+ÿ Pbÿ÷r and Hgÿ.÷
soI-
Compounds of SI'ÿ+ Baÿ% Pbÿ+, ÿnd Hÿÿ
l.soluble
compounds cÿntal.
Common ex:eptiorls
COÿ-
Compounds of NHÿ and the alkali metal cations
Foÿ-
compounds of NHÿ and the alkali meÿ! cations
CrOÿ-
Compounds of NHÿ- and [he alkali metal cations
compounds of NHÿ- and the alkali metal cations
OH-
Cempounds of NHÿ, ÿ:he alkali metal cations,
Caÿ% S]'=+ÿ and Baÿ+
25
Compounds of NHÿ, the alkali metal cations,
i
Caÿ+ÿ Srÿ+, and Ba2+
!
Determine if the following compounds are soluble or insoluble
by using the solubility table.
A) Sr(NO3)ÿ (45)-->
B) AgOH (S) ÷
C) PbCI2 (ÿ) -->
Tu, lsoJubl
D) Na3PO4 ÿ ->
80i@1 .
Predicting the Products of Double Replacement Reactions
A
Fr o FJ o
is a solid that forms when two solutions are mixed.
NaCl(aq) + AgNO3 (aq)-> AgCl(s) + NaNO3(aq)
I I
pr'gc ItOl,ÿ,f-#..
TIPS FORÿDOUBLE REPLACEMENT
REACTIONS
I
rUIII I
° Don't use the activity series.
• Determine if a precipitate will form.
o Precipitate will be an insoluble product!
o It should be marked as a solid (s).
- If a precipitate forms, a reaction occurs.
o If a precipitate does not form, then no visible reaction will occur.
General Formula
AX + BY "-ÿ BY + AX
ions should switch places!
Examples
1 (aq) ->
°
Nÿaq) ->
.+ s r4o faq)
° 3 I(Oÿe(NOa)3(aq) ->
°
ÿ04(aq) -->
r4
26
Day 8: Precipitate Homework
1. Predict if the following compounds are soluble (aq) or insoluble (s). Label with (s) or (aq).
a. Kc,(oÿ Solulole,
Q
e. NH4OH(O.ÿ DOIÿIÿiÿ,
Determine if the following pairs of solutions willÿÿrecipitate.
• If they do form a precipitate, write thÿeaction.
• If they do not form a precipitate, write NVR for no visible reaction.
a. ÿAgNTa(aq) + CÿCI2(aq)-) ÿÿJOÿ)2_ (ÿ r6L)
F"
I
b. Pb(NO3)2(aq) +
i
-)
C,
d4
|
V
N&3PO4(aq) + FeCI3(aq) ->
tL
l
eQ
27
%1
Day 9: Compound Formation Lab
Objectives
• Predict the products of the double replacement reactions.
° Identify the formation of a precipitate experimentally.
Backqround
In chemistry there are four signs that indicate that a chemical change has most likely taken place.
1. A Change in Color
2. Formation of a Gas (bubbles)
3. Release or Absorption of Energy (temperature change)
4. Odor
5. Formation of a Precipitate (solid)
A precipitate is a solid that is formed when two aqueous solutions are mixed. It usually separates from the mixture
by settling to the bottom of the container. Precipitates often appear to be cloudy, milky, gelatinous or grainy.
Pre-Lab Questions
1. In the following equation, circle the precipitate.
BaCI2(aq) + Na2SO4ÿoq) ÷ 2 NaCl(aq) + BaSO4(s)
.
Write the chemical equation for the following double replacement reactions. Predict the products of the
reactions, and using your solubility chart identify which product is the precipitate (insoluble), if there is
one. If no precipitate is formed, then write NO VISIBLE REACTION (NVR) as your product.
a. A solution of ammonium hydroxide is mixed with aqueous iron (III) chloride.
b. Ammonium hydroxide dissolved in water reacts with a solution of zinc (II) chloride.
c. Aqueous lead (II) chloride is mixed with aqueous ammonium hydroxide.
d. A solution of sodium hydroxide is mixed with aqueous zinc (II) chloride.
e. Aqueous sodium hydroxide reacts with iron (III) chloride.
28
f. A solution of lead (II) chloride is mixed with aqueous sodium hydroxide.
g. A solution of sodium iodide reacts with aqueous copper (II) chloride.
Procedure
1. Follow the directions on the Reaction Surface Chart.
2. Be sure to place all pipettes tip up to prevent contamination! ©
3. Record the appropriate data in your data table below.
4. To clean up, soak up your solutions using a paper towel. Dispose of the paper towel in the trash can.
5. Wash your overhead with water.
6. Dry your overhead completely!
Data
In each box, record the precipitate (insoluble, orsolid, compound) produced by the reaction, and the color of the
precipitate if one is formed. Record "NVR" for no visible reaction if no precipitate is formed.
ZnCI2
FeCI3
PbCI2
NaI
NH4OH
NaOH
CuCI2
Analysis
**WRITE IN COMPLETE SENTENCES**
1. If a product is soluble, why do you think we don't see a precipitate?
2. If a product is insoluble, why do you think that a precipitate is visible?
3. Predict the products (and circle the precipitate) if a solution of sodium sulfate is mixed with calcium
nitrate. (Be sure to write the BALANCED chemical equation!)
2g
CHEMICAL REACTIONS STUDY GUIDE
If completed in its entirety is +5 on TestJ
Nomenclature Practice:
What symbols represent the
Write the correct formula
1. Aluminum chloride ÿi//1¢
3. Sulfur dioxide
following terms?
ÿ0ÿ
A reaction is heated:
4. Sulfurous acid
A catalyst is used:
5. Copper (II) oxide
6.
Dinitrogen tetroxide ÿ9_0ÿi _
7.
Calcium sulfate ÿ tÿ01¢w
8. Hydrofluoric acid
%
A soJution of:
A precipitate:
"hLF
9. Barium phosphate ÿ0iÿ (lg01ÿ)
Gaseous:
lo. HN19
Vapor:
11. Write a balanced chemical equation for each worÿ
appropr'taÿe symbols,, formulas,.W7__ÿ, and balancinÿ!ÿ i zÿ
a. Soÿuÿm reÿ-cts with wafer
- - ÿzÿ
ÿ'
form to
hydrogen
gas and
IÿOLO':ÿf
sodium hydroxide.
b. Solid lead (IV) oxide is heated, decomposing to lead metal and oxygen gas.
p <,"+j +- (I)
c. In the presence of a catalyst, nitrogen and hydrogen gases react to form gaseous
ammonia.
12. Complete the Single Replacement reactions. Then use the activity series of metals
and Halogens :,to determine which of the below reactions will occur. If a reaction will
occur, write the balanced equation.
a. A u(s) + KNO3(aq)--) ÿxl ÿ2ÿ
b. Zn (s) +oÿAgNO3(aq) -)
3O
C. ÿ AÿSO4(aq)
d.
MgBrz+ Ez->
e.
Cu(s) +
HzO(0
f. ÿ Alÿs)+ _ÿCuSO4(aq) "-ÿ hi .ÿ, C-ÿq )ÿ2 '+ ÿ) Cÿ
.,o<T'. _.t-'ÿ-,
g,
,°
NaCI +
Br2 ÷ÿÿ. ÿ
#.HÿO+ ÿ,No÷ ÿr4ÿOÿ ,+ ÿ.
13. Balance the following combustion reactions.
b. ÿCsHm +'ÿOz ->iÿ COz +lÿHzO
14. Predict the products in the following double replacement reactions. Identify the
precipitate formed when solutions of these ionic compounds are mixed. If there is NO
PRECIPITATE (no insoluble solid), write NVR!
a.
Cÿlz ->
÷
d. CaCIz + Pb(NO3)z ->
e.
+ Fbcl;ÿ 8)
Ca(NO3)z + NaBr l>
31
15. Write a balanced equation and identify its type.(Combustion: C, Decomposition: D,
Synthesis: S, Double Replacement: DR, Single Displacement: SR)
And by Category ( ppt, redox)
b
of- DJuPrÿ
C,S,D,
Balance the following
SR,DR
S
o. 2Hf ÷ 2-Nÿ ÷_1HfÿNÿ
0
c. CzH6 + __ 02-> ÿ COz + ÿ HzO
d. ZHg(NO3)z +__7-" NH4OH->
ppt, acid-base,
redox
ÿ1 Hg(OH)z +
ÿ ÿ NH4NO3
b
'
,4/
16. Based on the oxidation numbers known for the other element(s), determine the
oxidation number of the underlined element.
a. NaSO4 "q-ÿ
c. _KcJ
d.ÿ
+1
e. CaO
g.ÿo
Jr
+1
b) i<jCrOÿ
0
--;Z-.
18. In an oxidation-reduction reaction, reduction is defined as the --
C loss of electrons.
DIoss of protons.
32
19. Which changes occur when Ptz÷ is reduced?
he Pt2+ loses electrons and its oxidation number decreases.
he Pt2÷ gains electrons and its oxidation number decreases.
C The Pt2+ gains electrons and its oxidation number increases.
DThe Pt2÷ loses electrons and its oxidation number increases.
20. The ionic chemical equation below is balanced.
Zn(s) + Cu2+(aq) ÿ ZnZ+(aq) + Cu(s)
Which equation represents the oxidation half-reaction?
AZn(s) -ÿ Zn2÷(aq) ÷ 2 eB CuZ+(aq) + 2 e- ÿ Cu(s)
CCu2÷(aq) -ÿ Cu(s) + 2 eDZn(s) + 2 e- -ÿ Zn2+(aq)
21.
The chemical equatio belo r pres n s a re ox reaction.
4ÿC1+ MnO2-+ MnClÿ-+ 2 H20 + Cÿ
What occurs during this reaction?
AThe manganese is oxidized, and its oxidation number changes from +2 to +4.
he manganese is reduced, and its oxidation number changes from +4 to +2.
C The manganese is oxidized, and its oxidation number changes from +4 to +2.
DThe manganese is reduced, and its oxidation number changes from +2 to +4.
22. Which half-reaction correctly represents oxidation?
AFe(s) + 2 e- ÿ FeZ÷(aq)
e(s) -ÿ Fe2÷(aq) + Z e-
C Fe2+(aq) + 2 e- lÿ Fe(s)
DFe2÷(aq) -ÿ Fe(s) + 2 e-
18
..... ÿ--i
.I
i H
He i
i LChÿ
Ne
&ÿ141
Na
Kr
g&oÿ>
5
Rb
31.g9 I
INLOofi
z
Fr
..Z'LU2Pÿ:z'&.
-" ,,"qÿTq ÿ,ÿ I ÿo [ oi [ÿ.4T"T"'ÿ I a I ÿ,ÿ
Lÿnlharÿide, ÿbnÿs
ActinVulo Soriÿ
ÿ l-"'ÿv"%"°'ÿi;''F'"lÿT"l-"":Fÿ-"Tÿiÿ`n
o
Ionic Compounds: Name the metal unchanged, Name the nonmetal with "ide" on the end.
Q
Ionic with multivalent metals: Name the metal unchanged and write the roman numeral for the oxidation of
the metal, Name the nonmetal with "ide" on the end.
Roman
Numeral
I
II
III
IV
V
VI
VII
VIII
Oxidation
#
i+ 2+
3+
4+
5+
6+
7+
8+
- Covalent/Molecular Compounds: Use the prefixes listed below to name the compounds
1"
2
3
4
5
6
7
8
9
Mono-
Di-
Tri-
Tetra-
Penta-
Hexa-
Hepta-
Octa-
Nona-
10
Deca-
• Ionic Compounds with polyatomic Ions: Write both the metal and the polyatomic ions AS IS.
o Acids: Use the chart below
ION TYPE
ION ENDING
ACID NAME BEGINNING
34
ACID ENDING
il
8A
i
iA
I
2
4
13
3A
M
4A
ÿ5
5A
16
6A
17
7A
Be
12
Mg
98
4
4B
5
5B
t9
ÿ20
21
22
K
Ca
So
TJ
V
• 39#98
4&178
40
41
Zr
Nb
24,
i
ÿ8
9
8B
iO ÿ
II
ÿ,
ÿB
12
ÿ.ÿ
B
ÿImmrÿ
27
ÿo
2,3
30
31
32
33
34
36
Fe
Co
NI
Ca
Zn
Ga
Ge
As
Se
Br
43
44
45
4ÿ
47
48
49
50
51
To
Ru
Rh
Pd
Ag
Cd
Iÿ
Sa
Sb
52
"re
25
26
Or Mn
79¢.ÿ4
7
Rb Sr
B&458
2,3
6
7
6ÿ 7B
42
ÿo
12&ÿ24
112412 114.ÿ1ÿ ÿ18,7ÿt ÿ2ÿ.7ÿ
87.e2
55
56
TJ
72
73
74
75
76
77
78
79
80
Cs
Ba
Lÿ
Hf
Ta
W
Re
0ÿ
Tr
Pt
Au
Hg
ÿ1
£2
TI
Pb
ÿ °
Bi
t4
At
Po
{ran
Pÿ>krRlJm
87
88
Fr
Ra
Lr
Rf
Db
Sg
Bh
59
Lanthanide Sefieÿ
La
Ce
Pr
89
Zÿ
ÿ)1
Acÿinida Series
Ac
Th
Pa
Hs
MI
Ds
Rg
80
ÿ1
82
ÿG
ÿ4
Nd
Pm
Sm
Eu
Gd
92
O
93
Np
N
Pu
95
Am
Mÿ numbers in ÿ rÿnlbermÿ m'ÿ3 &me el
$5
Tb
68
Dy
67
He
86
97
9B
99
Cm
Bk
Of
Es
68
9
Er
Tm
Fm
Md
70
Yb
102
No
Nsÿ
N#bÿl{ÿ,1}
REFERENCE MATERIALS
i Acetate
CmHOÿ-, CH3CO0'-
Se lub te
comlmuld s conrail
i Ammonium
i
FN4
Uÿium
CzHÿOÿ, CHsCOO-
NO.Iÿ
None
col
• Chlorate
C10ÿ
Chlo rile
CIOÿ
Cÿ rom aÿ:e
Cr 0ÿ-"
Nofle
CN-
None
cm2
None
None
None
cl%Cyanide
DI ÿhrea'iat e
CN ....
C rÿOÿ-
Hydrogen carbonate HCOÿ
Hydroxide
OH-
i Hypochledte
CtO-
4
N#ÿlce
• Nitrite
Perchlora te
Permanganate
, Phosphate
NOÿ
NOÿ-
CIOÿ
cÿ
None
Br-
Compmÿndsof Ag"ÿ , pbz+, and Hÿ+
CF
CompoundsoF Ag÷, Pbÿ*, and Hgÿ÷
F'
Compoÿndsof Ag% Pbzÿ', and Hÿ ÿ'ÿ
Compound e of Srÿ+, Baÿ*, Pbÿ, and Hgÿ"
In sol u role
compounds coÿtaln
Corn moÿ excepÿon s
Calcium
Sodi um
Magn esh m
AIu mÿn um
Hang anese
Zinc
Chroml Lrn
Iron
Cobal[
ill Nickel
Compounds of NHÿ' and lÿe alkali mÿal calms
po -
Compound s of NHÿ and ÿe alkali me[al catJms
Lea d
CrOÿ-
Compound s of NHÿ and ÿe alkali mer.alcalms
{Hydrogeÿ )
Compound s of NH: and ÿe alkali metal calms
Copper
Mn04
POÿ ....
tota ssiu m
Bariu m
Compound s of NHÿ, ÿe alkali meta ca{bns,
OH ....
52-
35
Mercuqÿ
Ca:z*, Srÿ*, and Baÿ+
Sliver
Compoundsof N;--ÿ, ÿhe alkali metal catbns,
P/atintÿm
Ca2+, Srÿ, and Baÿ"
Gold
!