Download 11 BALANCING CHEMICAL EQUATIONS 1. 2 K + 1

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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
__
__
__
1
__
__
____________
2
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.
2
3
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
3
I.
Combustion of propane
4
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)
4
5 Name
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.
5
6
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
6
HNO3
H3PO4
H3C6H5O7
H2CO3
HCO2H
7
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.
7
8
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
8
9 Name
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 carbon
9 dioxide.
10
____________ ___
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
10
11
9 IONIC COMPOUND NAMING CHART
Directions:
Write the formala name of each compound.
F
ClSO42CO32NO3-
NH4+
PO43-
Ammonium
Flouride
CrO42-
CH3CO23Ammonium
Acetate
(vinegar)
K+
Na+
Ag
Ca 2+
Mg
2+
Ba 2+
Al
3+
Fe 2+
Fe 3+
Iron III
Flouride
Iron III
Phosphate
9 IONIC COMPOUND FORMULA CHART
Directions:
NH4+
Write the chemical formula of each compound. Make sure the oxidation number add up to zero.
ClSO42CO32NO3PO43CrO42CH3CO23FNH4 F
K+
Na+
Ag+
Ca2+
Mg2+
Ba2+
Al3+
Fe2+
Fe3+
Fe3 (PO4)2
FeCl3
11
12
9 IONIC REACTION LAB CHART
Directions:
1) Write the entire chemical formula of each anion & cation below to be used (look at NaCl/AgNO3).
2) Put one drop of each chemical on the plastic grid sheet. Record your observations below.
Anions
Cations !
A AgNO3
F-
ClNaCl
White
ppt
SO42-
3
4
CO32-
NO3CaNO3
PO43-
CrO42
CH3CO23
-
-
8
9
No (NR)
Reaction
B
C
D
E
F
G
H
I
J
1
2
5
6
7
10
11
Directions:
1) Pick one reaction which made a Precipitate from each column and write the ionic reaction.
2) Use the solubility rule to determine which product formed the precipitate & which was soluble.
3) Cross out the products which were soluble because they’re spectators as reactants & products.
column
A
2
Reactants
Products
AgNO3 + NaCl AgCl + NaNO3
Ag++NO3- + Na++Cl- AgCl +Na++NO3Ag++
Cl- AgCl
B
C
D
E
F
G
H
I
J
12
Rule # states that Chlorides are soluble
except with Ag, Pb & Hg.
Total ionic equation
13
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
13
14
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
14
15
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_______________________ 15
16
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: 16
First Last Name___Per__ Cornell Question & Ans
Directions: Make 5 questions
& answers that are different
than the Anticipatory Response
1. 2. 3. 4. 5.