Download 1 R R 1Ch Ro_ R___ + ____ ____ + _+ S ___y → +

1
Firrst Last N
Name P
Per_____
_ Score ____/____
_ 11Ch
hemical +1R
+ Rxn’s Æ
Æ1Ch11R
Rx
_______________
__________
___________
__________
__________________________________________________
om_______
____
Syntthesis or Co
Basic Pattern
R
Ro_
____
_+ S___
S __
Æ
A+B
BÆ
__________
________
_______
_______
____________________________________
Dec
compositio
on
R
R___
____
___y
y Æ
+
ABÆ
Æ
__________
________
_______
_______
____________________________________
Sing
gle Replacement
+
ÆB
Æ _______yy + R
R____
A + BC Æ
__________
________
_______
_______
____________________________________
Dou
uble Replac
cement
ÆR___
____+ B___
____ AAB + CDÆ
Æ
+
____
____________
___________
___________
___________
____________
___________
___________
___________
____________
_
Com
mbustion
+
O2 Æ
C ____
__
+ H ____
__
___
_______
________
_______
________
_______
_______
________
_______
_______
1
05_CTR_ch11 7/9/04 3:33 PM Page 265
2
Name ___________________________
11.1
Date ___________________
Class __________________
DESCRIBING CHEMICAL REACTIONS
Section Review
Objectives
• Explain how to write a word equation
• Describe how to write a skeleton equation
• List the steps for writing a complete chemical equation
Vocabulary
• chemical equation
• skeleton equation
• catalyst
• coefficients
• balanced equation
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
A chemical reaction can be concisely represented by a chemical 1.
1
. The substances that undergo a chemical change are the
2.
2
. The new substances formed in a chemical reaction are the
3.
3
. In accordance with the law of conservation of
4
,
4.
a chemical equation must be balanced. When balancing an
equation, you place
5
5.
in front of reactants and products so
6
that the same number of atoms of each
6.
are on each side of
7.
the equation. An equation must never be balanced by changing the
8.
7
in the chemical formula of a substance.
9.
Special symbols are used to show the physical state of a
substance in a reaction. The symbol for a liquid is
a solid,
9
; and for a gas,
in water is designated
11
10
. If a
8
10.
; for
11.
. A substance dissolved
12.
12
is used to increase
the rate of a chemical reaction, its formula is written above the arrow.
2
Chapter 11 Chemical Reactions
265
05_CTR_ch11 7/9/04 3:33 PM Page 266
Name ___________________________
3
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 13. In an equation, a substance is shown to be in the gaseous state by
placing an upward-pointing arrow after its formula.
________ 14. The symbol placed over the arrow in an equation means that heat is
supplied to the reaction.
________ 15. Atoms are destroyed in a chemical reaction.
________ 16. A skeleton equation is not a balanced equation.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. an equation in which each side has the same
number of atoms of each element
________ 18. skeleton equation
b. a substance that speeds up the rate of a reaction
________ 19. catalyst
c. a symbolic way of describing a chemical reaction
________ 20. coefficients
d. substances that undergo chemical change
________ 21. balanced equation
e. a chemical equation that does not indicate the
amounts of substances involved
________ 22. reactants
f. new substances formed in a chemical reaction
________ 23. products
g. numbers used to balance a chemical equation
Part D Questions and Problems
Answer the following in the space provided.
24. Write a balanced equation for each of these chemical reactions. Include
appropriate symbols from Table 11.1.
a. Aluminum reacts with aqueous hydrochloric acid to form hydrogen gas and
aqueous aluminum chloride.
b. Acetylene gas (C2H2) burns in a welding torch with oxygen to form carbon
dioxide gas and water vapor.
266
Core Teaching Resources
3
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
________ 17. chemical equation
05_CTR_ch11 7/9/04 3:33 PM Page 267
4
Name ___________________________
Date ___________________
Class __________________
TYPES OF CHEMICAL REACTIONS
11.2
Section Review
Objectives
• Describe the five general types of reactions
• Predict the products of the five general types of reactions
Vocabulary
• combination reaction
• decomposition reaction
• single-replacement reaction
• activity series
• double-replacement reaction
• combustion reaction
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
It is possible to
the products of some chemical
1.
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
reactions. In order to do this, you must be able to recognize at least
five general types of reactions. For example, in a
3
the reactants are two or more
4
there is always a
2
reaction,
and/or compounds and
5
3.
4.
reaction, a single
5.
compound is broken down into two or more simpler substances.
6.
In a
6
product. In a
2.
reaction, the reactants and products are an
7
element and a compound. The
7.
can be used to predict
8.
whether most single-replacement reactions will take place.
A
8
9.
reaction involves the exchange of ions between two
10.
compounds. This reaction generally takes place between two ionic
compounds in
9
combustion reaction is
solution. One of the reactants in a
10
11.
12.
. The products of the complete
combustion of a hydrocarbon are
11
and
4
12
.
Chapter 11 Chemical Reactions
267
05_CTR_ch11 7/9/04 3:33 PM Page 268
Name ___________________________
5
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 13. In a decomposition reaction, there is a single reactant.
________ 14. The activity series of metals can be used to predict products in doublereplacement reactions.
________ 15. Carbon dioxide and water are the products of the combustion of
hexane (C6H14).
________ 16. A nonmetal can replace another nonmetal from a compound in a
single-replacement reaction.
________ 17. One of the products of a double-replacement reaction is a gas that
bubbles out of the mixture.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. reaction in which atoms of one element replace
atoms of a second element in a compound
________ 19. decomposition reaction
b. a reaction in which two or more substances
combine to form a single substance
________ 20. single-replacement reaction
c. reaction of a compound with oxygen to produce
energy
________ 21. combustion reaction
d. reaction in which a single compound is broken
down into two or more products
Part D Questions and Problems
Answer the following in the space provided.
22. Identify the type of each of the following reactions.
a. 2C6H14(l ) 19O2(g) y 12CO2(g) 14H2O(g )
b. 2Fe(s) 3Br2(l ) y 2FeBr3(s)
23. Complete and balance the following equation. What must be true of one of the
products?
Li3PO4 Zn(NO3)2 y
268
Core Teaching Resources
5
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
________ 18. combination reaction
6
11 BALANCING CHEMICAL EQUATIONS
Directions:. Label decomposition, synthesis (combination), single displacement, double displacement (or
double replacement), combustion reaction or Neutralization (acid/base).
Balance the Chemical Equation
Reaction Type
1.
2 K + 1 Cl2 → 2 KCl
COMBINATION
2.
__SO2 + __O2 → __SO3
________________
3.
__KClO3 → __KCl + __O2
________________
4.
__CO2 + __C → __CO
________________
5.
__H2 + __O2 → __H2O
________________
6.
__MgCO3 → __MgO + __O2
________________
7.
__H2O + __Cs → __CsOH + __H2
________________
8.
__Fe2O3 + __Al → __Fe + __Al2O3
________________
9.
__PbCl2 + __Li2SO4 → __PbSO4 + __LiCl
________________
10. __NaOH + __H2SO4 → __Na2SO4 +__H-OH
________________
12. __Pb(OH)2 +__HCl Æ __PbCl2 +__H-OH
________________
13. __Na2CO3 + __HCl Æ__H2CO3 +__NaCl
________________
14. __AgNO3 + __Cu → __Ag + __Cu(NO3)2
________________
15. __CH4 + __O2 → __CO2 + __H2O
________________
16. __C2H6 + __O2 → __CO2 + __H2O
________________
17. __C3H8 + __O2 → __CO2 + __H2O
________________
18. __C4H10 + __O2 → __CO2 + __H2O
________________
19. __C5H12 + __O2 → __CO2 + __H2O
________________
Bonus: Don’t unless given permission. Use decimal method if needed, for example “1.5 O2.”
20. __C7H5N3O6 + __O2 → __ CO2 + __ H2O + __ N2
__
__
__
6
__
__
____________
7
How To Write & Balance
Chemical Reactions
Equations must be balanced
Atoms can be neither created nor destroyed in an ordinary chemical reaction, so
there must be the same number of atoms on both sides of the equation.
These numbers are found in a chemical equation
2H2 + O2
2H2O
Subscripts
Coefficients
The small numbers to the
lower right of chemical
symbols. Subscripts
represent the number of
atoms of each element in
the molecule.
The large numbers in front
of chemical formulas.
Coefficients represent the
number of molecules of the
substance in the reaction.
Balancing Equations By Inspection
1.
2.
3.
4.
5.
6.
Balance Metals
Balance Nonmetals
Balance Ions
Balance Oxygen
Balance Hydrogen
DOUBLE CHECK
DIRECT COMBINATION REACTIONS
A + B
AB
(also called “synthesis reactions”)
A.
In the Haber process, nitrogen gas and hydrogen gas are combined under
high temperature and pressure to form ammonia (NH3).
B.
One of the rare reactions among the noble gasses that have been
discovered is the formation of solid xenon tetrafluoride from the
combination of xenon and fluorine gas.
7
8
C.
Pure magnesium metal is burned to form magnesium oxide, a fine white
Powder.
D.
Sodium metal and chlorine gas react to form table salt.
E.
Iron nails rust to form ferric oxide.
F.
Phosphorus is mixed with chlorine gas to form phosphorus pentachloride
(PCl5)
G.
Water is added to ammonia to yield ammonium hydroxide.
DECOMPOSITION REACTIONS
AB
A + B
E.
Electricity is run through water, liberating oxygen gas and hydrogen gas.
F.
Hydrogen peroxide decomposes in the presence of a catalyst
(manganese), to liberate oxygen gas, leaving only water behind.
HYDROCARBON COMBUSTION
CnH2n+2 + O2
H2O + CO2
Methane
CH4
Hexane
C6H14
Ethane
C2H6
Heptane
C7H16
Propane
C3H8
Octane
C8H18
Butane
C4H10
Nonane
C9H20
Pentane
C5H12
Decane
C10H22
G.
Combustion of methane
H.
Combustion of butane
8
I.
Combustion of propane
9
SINGLE REPLACEMENT REACTIONS
A + BC
AB + C
J.
When Copper metal is added to silver nitrate, pure silver is deposited and
a blue solution of copper (I) nitrate remains.
K.
(find one in the book or internet)
L.
Lead (II) sulfide is heated in the presence of oxygen to form solid lead (II)
oxide and sulfur dioxide gas.
DOUBLE REPLACEMENT REACTIONS
AB + CD
AC + BD
M.
Solid carbon is added to aluminum oxide in order to form pure aluminum
metal and carbon dioxide gas.
N.
If solutions of potassium chromate and barium chloride are mixed, a bright
yellow solid called barium chromate is formed, leaving potassium chloride
in solution.
O.
Hydrochloric acid is added to sodium hydroxide to produce water and
sodium chloride.
P.
(find one in the book or internet)
9
10Name
Date
Period
________
11 Writing & balancing
Chemical Reactions
Here are some sample reactions. Can you write the unbalanced reaction?
What type of reaction is taking place? (advanced: balance the rx's)
1.
sulfur trioxide and water combine to yield sulfuric acid.
2.
lead(II) nitrate and sodium iodide react to yield lead iodide and sodium
nitrate.
3.
calcium fluoride and sulfuric acid yield calcium sulfate and Hydrofluoric
acid.
4.
Sodium metal and chlorine gas yield sodium chloride.
5.
ammonia gas, when bubbled into water, will yield ammonium hydroxide.
6.
ethane is burned in oxygen to yield carbon dioxide and water.
7.
zinc sulfide and oxygen yields zinc oxide and sulfur.
8.
Aluminum metal reacts with Calcium oxide to produce calcium metal and
aluminum oxide.
9.
aluminum hydroxide and sulfuric acid yields water and aluminum sulfate.
10.
Silver (I) nitrate reacts with copper metal to yield silver metal and
copper (I) nitrate.
11.
barium hydroxide and sulfuric acid yield water and barium sulfate.
12.
aluminum sulfate and calcium hydroxide react to form aluminum hydroxide
and calcium sulfate.
10
11
Combustion of Hydrocarbons
A hydrocarbon is formed when a central carbon atom (or chain of carbon atoms)
bond with hydrogen atoms. The simplest hydrocarbons are the alkanes, with a
general formula of ...
CnH2n + 2
For example, what is the formula for an alkane hydrocarbon with 3 carbons?
Solution: Fill in the above general formula with the new numbers as follows:
C3H(2 x 3) + 2 = C3H8
Alkanes are named as follows:
n=
Formula
Name
Acronym
New Acronym
1
CH4
methane
Mother
M__________
2
ethane
eats
E__________
3
propane
peanut
P__________
4
butane
butter
B__________
5
pentane
pizza.
P_________
6
hexane
Hence
H__________
7
heptane
her
H__________
8
octane
office
O__________
9
nonane
never
N__________
10
decane
dines
D__________
Most hydrocarbons, including all the alkanes undergo combustion (burning in
oxygen) to form Carbon dioxide and water. For example, write the formula for
the combustion of ethane:
C3H8 +
O2
CO2
+
H2O
3CO2
+
4H2O
Now, we just need to balance the reaction.
C3H8 +
5O2
COMMON ACIDS
Hydrochloric acid
Hydrobromic acid
Hydroiodidic acid
Hydrofluoric acid
Sulfuric acid
Acetic acid
HCl
HBr
HI
HF
H2SO4
HCH3CO
Nitric acid
Phosphoric acid
Citric acid
Carbonic acid
Formic acid
11
HNO3
H3PO4
H3C6H5O7
H2CO3
HCO2H
12
Name
Date
Period
Writing and balancing Chemical Reactions
Here are some sample reactions. First write the chemical reaction, then
determine the type of reaction taking place. Finally, balance the reaction.
1.
Carbon dioxide and water combine to yield carbonic acid.
CO2 + H2O
H2CO3
2.
Carbon disulfide reacts with oxygen to form carbon dioxide and sulfur
dioxide.
3.
When heated, calcium carbonate yields carbon dioxide and calcium oxide.
4.
Calcium fluoride reacts with sulfuric acid to form calcium sulfate and
hydrogen fluoride.
5.
Lithium oxide reacts with water to form lithium hydroxide.
6.
Pentane burns.
7.
When water is exposed to electricity, oxygen and hydrogen are formed.
8.
Aluminum reacts with iron (II) nitrate to form aluminum nitrate and iron.
9.
Hydrochloric acid reacts with ammonium hydroxide.
12
13
10.
Sodium reacts with bromine to form sodium bromide.
11.
Decane burns.
12.
When heated, potassium chlorate forms potassium chloride and oxygen.
13.
Magnesium burns to form magnesium oxide.
14.
Aluminum reacts with fluorine to form aluminum fluoride.
15.
Hydrochloric acid reacts with calcium metal to produce calcium chloride
and hydrogen gas.
Name the following compounds:
a.
C3H8
b.
H2PO4
c.
FeCl
d.
Cu(NO3)2
e.
SCl5
f.
(NH4)O
g.
C8H18
h.
Mg(OH)2
13
14Name
Period
Date
11 Writing and balancing Chemical Reactions II
Name the following compounds:
1.
C6H14
2.
HCH3CO2
3.
CuCl
4.
Al(NO3)3
5.
PF4
6.
NH4OH
7.
CH4
8.
Fe(OH)2
IONIC
COVALENT
Here are some sample reactions. First write the chemical reaction, then determine the type of
reaction taking place. Finally, balance the reaction.
9.
Sodium metal reacts violently in water to form hydrogen gas and sodium
hydroxide.
10.
Chlorine gas reacts with magnesium iodide to form magnesium chloride
and pure iodine.
11.
Iron reacts with copper (II) sulfate to form iron (III) sulfate and pure copper
12.
Hydroiodidic acid reacts with calcium hydroxide.
13.
Combustion of heptane.
14.
Solid iron reacts with chlorine gas to form iron (III) chloride.
15.
Carbon monoxide burns to form 14
carbon dioxide.
15
____________ ___
Predicting Reactions Worksheet 1
Combination Reactions - Predict the product and write balanced reactions for each of the following.
1. Hydrogen burned in oxygen.
___ H2 + ___ O2 Æ ___ H2O
2. Sodium plus iodine.
Æ
3. Calcium burned in chlorine.
Æ
4. Carbon burned in oxygen.
Æ
5. Hydrogen combined with nitrogen.
Æ
6. Sulfur burned in air.
Æ
7. Magnesium burned in hydrogen.
Æ
8. Zinc plus bromine.
Æ
9. Water plus carbon dioxide.
Æ
10. Sulfur dioxide plus water.
Æ
11. Sodium plus hydrogen.
Æ
12. Hydrogen burned in chlorine.
Decomposition (decombination) - Predict products (if needed) and write balanced reactions for each:
If you need to search the net to find the products, you can do that also with permission.
1. The heating of magnesium carbonate to
form Magnesium Oxide & Carbon Dioxide.
2. The heating of sodium chlorate to form
Sodium Oxide and Dichloro-oxide.
3. The electrolysis of water.
__MgCO3(s) Æ __MgO(s) + __ CO2(g)
Æ
Æ
4. The decomposition of calcium carbonate to
form Calcium Oxide and Carbon Dioxide.
5. The heated of mercuric oxide.
Æ
6. The electrolysis of sodium chloride.
Æ
7. Ferric hydroxide heated.
Æ
8. Aluminum hydroxide heated.
Æ
9. Sodium carbonate heated.
Æ
10. Barium hydroxide heated.
Æ
11. The electrolysis of calcium bromide.
Æ
12. The heating of carbonic acid.
Æ
15
16
WORKSHEET ON SINGLE & DOUBLE REPLACEMENT REACTIONS
Predict the products. Write formulas & balance each reaction. If there is no reaction, then just put NO RXN.
Single Replacement:
A + BC → B + AC or A + BC → C + BA (when A and C are negative ions)
1. Zinc + Hydrogen chloride Æ
2. Magnesium + Hydrogen Sulfate Æ
3. Copper (II) chloride + Flourine Æ
4. Silver + Sodium Hydroxide Æ
5. Potassium iodide + Bromine Æ
6. Calcium + Hydrogen hydroxide Æ
7. Iron IV oxide + Hydrogen Æ
Double Replacement: AB + CD Æ AD + CB
1. Barium chloride + Aluminum sulfate Æ
2. Calcium nitride + water Æ
3. Calcium hydroxide + Hydrogen phosphate Æ
4. Hydrogen sulfate + Sodium hydrogen carbonate Æ
5. Calcium hydroxide + Ammonium chloride Æ
6. Potassium iodide + Lead II Nitrate Æ
7. Sodium acetate + Calcium sulfide Æ
Complete each word equation, write formulas and balance the reaction equation. Then identify and place the type of
reaction (single replacement or double replacement) in the blank provided.
1. Zinc + Silver nitrate →
2. Aluminum + Hydrogen chloride Æ
3. Magnesium oxalate + Ammonium carbonate →
4. Calcium + Aluminum nitrate Æ
5. Potassium flouride + Lead (II) Nitrate →
6. Calcium bromide + Silver nitrate →
7. Ammonium phosphate + Barium acetate →
8. Sodium chloride + Potassium →
9. Magnesium nitrate + ammonium chloride →
10. Iron (III) chlorate + calcium →
11. Chlorine + Sodium bromide →
12. Potassium chloride + Silver nitrate →
13. Calcium hydroxide + Hydrogen nitrate →
14. Lead II nitrate + Potassium chloride Æ
15. Strontium carbonate + Hydrogen nitrate Æ
16. Gold + Potassium nitrate Æ
17. Zinc + Silver nitrate Æ
18. Aluminum + Copper II sulfate Æ
16
17
11-1 Comparing Synthesis and Decomposition Reactions Formative Assessment
1.
a.
An equation with the “A + B Æ AB” format is which of the following types of reaction?
combustion
b.
synthesis/combination
c.
c.
decomposition
2.
a.
b.
Which of the following reactions is an example of the above unbalanced reactions?
H2 + O2 Æ H2O
c.
CH4 + O2 Æ H2O + CO2
H2O2 Æ H2O+ O2 d.
Na + H2O Æ NaOH + H2
3.
4.
5.
Which above reaction in #2 is a decomposition reaction? ______________________
Which above reaction is a single replacement reaction? ________________
Which above reaction is a combustion reaction? ______________
Directions - Write the following reactions equation noting the states. For example, note a gas as (g). Then
balance the equation by placing coefficients in front of the formula. For example, 2 CO2.
6.
Hydrogen gas reacts with oxygen gas to form water vapor?
_________ _______
Æ ____________
Score ___/10
11-2 Chemical Reaction Formative Assessment
Approaching
1. Circle the letter of the reactions below that are balanced equations.
a.
2PbO2
b.
(NH4)2CO3
c.
PbO +
Pb(NO3)2
O2
2NH3 +
+
2NaI
H2O
+
CO2
PbI2
+
2NaNO3
+
H2O
Meets
2. Balance the following equations:
Fe3O4
a. Fe
+ O2
b.
C2H6
+
O2
CO2
Exceeds
3.
Write an equation of the chemical reaction when we burned Magnesium in Oxygen.
______ + _______ Æ _________
Score ___/10
11-2 Writing Equations- Formative Assessment
1.
Convert the following unbalanced equation into the written form (See number 2):
Methane_______________________________________
CH4 (g) + O2 (g) Æ H2O (g) + CO2 (g)
____________________________________________________________________________________
____________________________________________________________________________________
2.
Convert the following into a balanced chemical equation: Hydrogen peroxide is catalyzed by
Manganese IV Oxide decomposes to form water & Oxygen gas.
Æ
3.
Which is the correct balanced equation for the combustion of Methane?
a. CH4 (g) + O2 (g) Æ H2O (g) + CO2 (g)
c. CH4 (g) + 2O2 (g) Æ 2H2O (g) + CO2 (g)
b. C2H6 (g) + 3.5 O2 (g) Æ 3H2O (g) + 2CO2 (g) d. C3H8 (g) + 5O2 (g) Æ 4H2O (g) + 3CO2 (g)
4.
Balance the following equation by filling in the missing numbers and letters.
___BaO( ) +
____ O2 ( ) Æ ____ BaO ( )
Score ___/10
17
18
___________________________
First Name, Last ________
Period
SCORE: ___/10 pts
11 Chemical Naming Formative Assessment 1
Directions – Circle the best answer for each.
1.
2.
3.
Chemical Reaction occur when atoms are:
separated or joined
Which is correct:
rearranged
both correct
a.
Reactant 1 + Reactant 2 Æ Product 1 + Product 2
b.
Product 1 + Product 2
c.
None correct
Æ Reactant 1 + Reactant 2
Which must be written as “diatomic”, “double-atoms” or “Siamese Twins”?
a.
Br2 I2 N2 Cl2 H2 O2 F2
b.
H2 O2 F2 Br2 Au2
4.
Which is the correct skeleton equation considering the diatomic atoms above?
a.
H2 + O2 Æ H2 O
b.
H + O Æ H2 O
5.
In an equation how does one write a catalyst which speeds up the reaction?
a.
6.
MnO2
Æ
b.
∆
Æ
Which is correct for:
Fe (s) + O2 (g) Æ Fe2O3 (s)
a.
Solid Iron reacts with Oxygen gas to form solid Iron III Oxide
b.
Solid Iron reacts with Oxygen to produce Iron II Oxide.
Write True of False for each when using the below true equation:
Cu (s)
+ HCl
(l)
∆
Æ CuCl2 (s)
+
H2 (g)
7.
Copper metal reacts with liquid Hydrochloric Acid to form solid Copper (I)
Dichloride and Hydrogen Gas.
8.
Copper metal reacts with liquid Hydrochloric Acid to form solid Copper (II)
Chloride and Hydrogen Gas.
9.
This reaction was done without a catalyst but with added heat.
10.
A “2” in front of the __HCl would balance this equation.
18
19
Name _____________________
11 CHEMICAL REACTION LAB – DECOMPOSITION
Directions:
Make sure to balance all Chemical equations and fill in all boxes correctly for full credit.
Information: In this type of chemical reaction a compound decomposes into other compounds or
elements. Examples: AB → A + B. AB is the reactant; A and B are the products.
Sucrose (C12H22O11, decomposes into Carbon and Water
Procedure: Place two pinches of sucrose on one end of an aluminum foil scoop. Heat gently at
first. Hold a metal jar lid over the decomposing sugar to observe one decomposition product. The
charred carbon in the scoop is the other product. Wear goggles.
Word Equation
Chemical Equation
Physical Property
Blue Copper Sulfate Hydrate(CuSO4 h5H2O) Crystals produces Water and anhydrous CuSO4
Procedure: Heat two pinches of the crystal in aluminum foil 1cm above a candle flame to avoid
sooting. Wear goggles. Observe the color of the crystal and the product. Note any vapor (H20)
leaving. Then add a drop of water to the product to re produce the original substance.
Word Equation
Chemical Equation
Physical Property
Calcium (Ca) in Water produces Calcium Hydroxide [Ca(OH)2] and H2 Gas
Procedure: Fill a test tube half with water. Place a calcium turning into the water. To catch the
H2 gas, place another test tube upside down over the mouth of the first test tube until the
reaction is complete. To prove there was H2 gas produced place mouth of the upside down test
tube over the flame. The 2nd reaction is H2 gas & oxygen becomes water. (Write both RXNs)
Word Equation
Chemical Equation
Physical Property
Hydrogen Gas burns in Oxygen to Produce Water (Chemical Combination)
Word Equation
Chemical Equation
Physical Property
Poppers/Gun Powder Potassium Nitrate, Carbon and Sulfur produce Potassium Sulfide, Nitrogen & CO2
Procedure:
After balancing the below, inspect the color of a party popper. Then throw the party
popper on the ground. Observe the color difference. The grey is Potassium Sulfide. The explosion is
from the many molecules of Nitrogen gas and Carbon Dioxide gas produced.
Word Equation
Chemical Equation
Physical Propert
19
20
Name _____________________
CHEMICAL COMBINATION
Information: In a combination reaction, two chemicals combine to from a new compound.
Example: A + B → AB. Chemical A and B are the “reactants” and AB is the “product.”
Copper and Sulfur
Procedure: With all your strength quickly rub a pinch of sulfur powder on the copper
copper is not shiny. Observe color of copper and your fingers.
Word Equation:
until the
Chemical Equation:
Physical Property:
Copper and Oxygen
Procedure: Tie your hair back. Clean one end of copper wire with steel wool till shiny. Heat shiny
part of copper wire 1cm above candle flame until the copper is no longer shiny. Wear goggles.
Hold copper with small piece of paper to avoid burning fingers.
Word Equation:
Chemical Equation:
Physical Property:
Iron (Steelwool) and Oxygen produces Iron II Oxide and Fe3O4 Complex
Information: Iron reacts with oxygen in different combinations to form products such as FeO
grey, ferrous oxide, Fe2O3 reddish, ferric oxide; and Fe3O4 black, magnetic iron oxide. All are
forms of rust. You only have room below for 2 of the 3 products mentioned above.
Procedure: Burn steelwool by holding a small ball of it in the tip of a candle flame with a
paperclip. Wear goggles. Fill in the spaces below for the formation of FeO and Fe2O3.
Word Equation:
Chemical Equation:
Fe2O3
Physical Property:
Word Equation:
Chemical Equation:
Fe3O4
Physical Property:
20
21
Name _____________________
DOUBLE DISPLACEMENT (REPLACEMENT)
Lead II Nitrate and Sodium Hydroxide produce Lead II Hydroxide and Sodium Nitrate
Directions:
Add several drops of two ionic solutions in one container or well.
Read the solubility rules one through six and determine which two ions are
Soluble (dissolved) and which two are insoluble or precipitate (clump up).
Write the balanced reaction below:
Word Equation:
Chemical Equation:
Physical Property:
Write the net ionic reaction below canceling the spectators ions on both sides of the arrow
Na+ +
Example
NO3 - +
Pb2+ + 2OH- Pb(OH)2 + Na+ + NO3 -
Word Equation:
Chemical Equation:
Physical Property:
Word Equation:
Chemical Equation:
Physical Property:
SINGLE DISPLACEMENT
Silver in Silver Nitrate is Replaced by Copper and Lead
Directions:
Add enough drops of the solution to half cover the metal chunk. Observe
And then write the balanced reaction.
Word Equation:
Chemical Equation:
Physical Property:
Word Equation:
Chemical Equation:
Physical Property:
Conclusions:
1.
For your double displacement reaction, which Solubility Rule(s) predicts the precipitate?
2.
3.
Which predicts the ions which will be soluble in the double displacement reaction?
If the single replacement reaction, where on the activity chart series is the more
Reactive metal? Top middle bottom (circle one). Which metal is more valuable?
21
22
Jeopardy 9 & 111 1-10
00 equation which each side has the same # off atoms of ea
ach elementt
1-20
00 what is a new substa
ance formed in a chemic
cal reaction
Product
Reacttion
Ca
atalyst
e above
None of the
1-30
00 a starting
g substance in a chemic
cal reaction __________
_
________
1-40
00 A reactio
on in which oxygen
o
reactts with anoth
her substancce, often
producing heat or light
2-10
00 a reaction in which th
he atoms of one elemen
nt replace the
e atoms
of a seco
ond elementt in a compo
ound AB + CÆ
C
2-20
00 The ioniz
zation energy of which fo
ollowing grou
up is arrang ed from sma
allest to grea
atest. Explaiin
a.
Na,
N Si, Cl
b.
Na, K, Cs
2-30
00 How man
ny electrons does nitrogen gain in order to achie
eve a noble--gas electron
n configuratiion?
2-40
00 What typ
pe of ions alw
ways have names
n
ending in -ide? __
__________
___ like ____
_____ & ___
________
2-50
00 Which off the followin
ng are arrang
ged with all electronegat
e
tivities from greatest to ssmallest exp
plain
a.
K, Se, Kr
b.
Li, Na, Cs
33-10
00 What is the
t correct name
n
for the N ion?
3-20
00 When na
aming a trans
sition metal ion that can have more than one co
ommon ionicc charge, the
e numerical
value of the
t charge is
s indicated by
b a ____.
3-30
00 The electron configuration of a fluoride ion, F,
F is ____
3-40
00 Calculate
e the charge
e on each ion
n.
X2Y3
3-50
00 How man
ny valence electrons
e
doe
es each X & Y have?
4-20
00 In AlCl3 Al
A loses ___
___ electrons
s & Cl gains _____ elecctrons.
D.
1, 2
1, 3
E.
A.
3, 2
B.
3, 1 C. 2,
4-30
00 What is the
t balanced
d rxn betwee
en. (hint: sing
gle replacem
ment) __Br2 & ___NaI Æ
Æ___ ___ + _
___ ___
4-40
00 What is the
t formula unit
u of sodium nitride?
4-50
00 What typ
pe of bond would
w
the below two subs
stances form
m? Why?1s2
2 2s2 2p5 &1
1s2 2s2 2p6
6 3s2
5-10
00 What is the
t formula for
f sodium sulfide?
s
5-20
00 Which 2 of the follow
wing are NOT
T cations?
A. iron(III) ion c.
Ca
b. sulfate
s
d.
mercurous ion
3+
5-30
00 Which of the following
g compound
ds contains the
t Mn ion
n?
MnO b. MnBr2
d.
Mn2 O3
a. MnS c.
5-40
00 Which sh
hows correcttly an ion pa
air and the io
onic compou nd the two io
ons form?
5-50
00 Draw the
e electron do
ot structure for
f Hydrogen
n Sulfide?
6-10
00 What is th
he name of the
t ionic com
mpound form
med from lith
hium and bro
omine?
6-20
00 What is th
he correct fo
ormula for po
otassium sulfate? K2SO
O4 KSO4 K2SO3 Non
ne of the abo
ove
6-30
00 Which off the followin
ng is a binary
y molecular compound ((not ionic)?
b.
a.
BeHCO3
B
c.
AgI
PCl5 d. MgSO4
6-50
00 Sugar burrns under fire
e and salt do
oesn’t. Why
y?What type
e of bonds?
7-10
00 What is the
t name forr N2O5 Din
nitrogen Hex
xoxide Binittrogen Pento
oxide Dinitrrogen Pentoxxide None
7-20
00 Which on
ne has a sing
gle covalent bond?
CO2 O2
N2
F2
Na2S
7-40
00 What is th
he correct name for the compound CoCl2??
C
7-50
00 How man
ny Neutrons, Electrons & Protons do
oes Potassiu
um have in tthat order?
Which has the most?
8-10
00 What doe
es an -ite or -ate ending in a polyato
omic ion mea
an?
No
8-20
00 Which is correct Tin IV Flouride
e SnF4 Sodium Oxide NaO Bariium Nitride BaN
one
8-30
00 What kind
d of reaction
n is the follow
wing?
__H2O2 Æ _
__H2O
+ __O2
8-40
00 What kind of reaction
n is the follow
wing?__Fe + __Cl2 Æ _
__FeCl3 Th
hen Balance them with ccoefficient.
8-50
00
22
23
First Last Name Per 4 –11 & 25 Cumulative & Reteaching
Score ___/20
4 Atomic Structure
Problem Symbol Isotope Number Name 25 1. 12 Magnesium‐?__ ? Avg Atomic Mass # Mass 24.3 Atomic Number = ‐ Neutrons Electrons Protons = 2. From the above chart, Isotopes of the same element have different: 3. Elements are always Identified by the same: 4. Ions are formed because of a losing or gaining protons, neutrons, electrons protons, neutrons, atomic mass protons, neutrons, none correct 25 Nuclear Chemistry
5. Mass Letter Charge P 6. __________ He Fill missing numbers 7. Reaction type Radioisotope Beta Decay Oxygen Reactants 17
Reacts To Form Æ
O 8. How much material is left after 3 half‐lives: 100% 50% 25% Products ‐1 e Fission Or Fusion + 12.5% None correct 5&6 Electron Configuration
Element Electron Configuration 9. 1s2 2s2 2p6 3s2 3p3 Noble Gas Shorthand
Highest Energy Level with Electrons # electrons in highest level Lewis Dot 10. In “2s2 “, the 2 represents which 3 Æ (column, group, family, period, row or energy level). 7 Ions and Bonding
11. Which 2 have 3 valence electron? 12. Aluminums’ charge after reacting would be 13. Which formula is correct? (Aluminum, magnesium, Group 1A, Group 3A) (0, 1+, 2+ 3+) (AlCl, MgCl2, AlCl3) 8 Covalent Bonding
14. What type of bond is Aluminum Chloride? (covalent, ionic, metallic) Type 1
9 Naming
15. 16. 17. 18. Type II
Type III
What is the name of MgCl2? Magnesium Chloride Magnesium II Chloride Manganese Dichloride What is the name of Fe2O3? Iron Oxide Iron III Oxide Di‐Iron Tri‐oxide Nitrogen Iodide Nitrogen III Iodide Nitrogen Tri‐iodide What is the name of Nl3? From the above, Type I is (alkalis, transitions), Type II is (transitions, non‐metals) & Type III is (alkalis, nonmetals) 11 Reactions
19. The missing product in the reaction:__HCl +__ Ba(OH)2 Æ _ ___ + _ BaCl2 is: [H‐OH HBa Cl‐OH] 20. The above reaction is a: single replacement double replacement combustion 21. To balance the above reaction, the coefficients would be: (1,1,1,1 2,1,2,1 3,1,3,1) 10 Moles
22. 24 grams of Carbon is how many moles: 23. 24 grams of Carbon is how many molecules: 24. 8.0 grams of Hydrogen is how many liters: 25. Show work for the # 8 above. 0.5 1.0 3.01 x 10 23 22.4 44.8 2.0 4.0 6.02 x 10 23 12.04 x 10 23 none correct 89.6 none correct = Corrected by_______________________ 23
24
11CHEMICAL RXN’S __ /__ pts burns is a combustion? Y N 5.Double replacement reactions A + B ÆAB Anticipatory Response 1.Chemical reactions occur only when atoms are joined or rearranged? Y N 2. In the above equation, the the rt. side are reactants? Y N 3. Æ means “to produce”, “to make”, or “to yield”? Y N 4.Skeleton equations are not Balanced? Y N 5. Hydrogen can be written as “H” in an equation? Y N 6. Catalysts & heat are always written on the arrow? Y N 7. Aqueous (aq), liquid(l) & gas (g) should be written? Anticipatory Response 1. A + B ÆAB is the pattern for a decomposition reaction? Y N 2. H2 + O2 Æ H2O fits the pattern for synthesis? Y N 3. Photosynthesis is called so because chlorophyll combines CO2+H2O to makeÆsugar? Y N 4The reverse of #3 when sugar Involve cations & anions? Y N Summary Section: 24
First Last Name___Per__ Cornell Question & Ans
Directions: Make 5 questions
& answers that are different
than the Anticipatory Response
1. 2. 3. 4. 5.