Unit 1 - Avon Community School Corporation / Web view · 2013-01-25_ c2h4o2 + _ o2 (...

Unit 1 Name _______________________________ # ________

Section 1: Parts of Equations

Use the equation below to answer the questions.

Energy + 6H2O (l) + 6CO2 (g) C6H12O6 (aq) + 6O2 (g)

1. What are the reactants? _________________________________

2. What are the products? __________________________________

3. What information do the symbols in parenthesis give you about each

compound? __________________________

4. What does the (aq) mean after glucose (C6H12O6)? ___________________________________________________________

5. Why does water have an (l) instead of (aq) after it? __________________________________________________________

Section 2: Writing Chemical Equations

Write chemical equations from the description of each reaction. Be sure to include symbols for states of matter when possible. Remember that some elements are diatomic.

1. Sodium chloride and fluorine gas react to form sodium fluoride and chlorine gas.

2. Methane (CH4) and oxygen gas react to form carbon dioxide and water.

3. Solid magnesium metal reacts with oxygen gas to form magnesium oxide.

4. Lithium hydroxide and sulfuric acid (aqueous hydrogen sulfate) react to form lithium sulfate and water.

5. C6H12O6 and oxygen react to form carbon dioxide and water.

6. Calcium bromide is separated into its elements, calcium and liquid bromine.

7. Copper (II) nitrite reacts with solid lithium to form lithium nitrite and solid copper.

8. Hydrogen and oxygen react to form water.

Section 3: Balancing Chemical EquationsList how many atoms there are of each element in the problems below

1. 3 NaCl

2. 4 Na3PO4

3. 2 Fe2S3

4. 8 AlCl3

5. 5 N2O5

Balance the following equations by changing the coefficients to make the number of atoms on each side of the equation the same.

6. ___ NaNO3 + ___ PbO ___ Pb(NO3)2 + ___ Na2O

Na= Na=

Pb= Pb=

7. ___ AgI + ___ Fe2(CO3)3 ___ FeI3 + ___ Ag2CO3

Ag= Ag=

Fe= Fe=

8. ___ C2H4O2 + ___ O2 ___ CO2 + ___ H2O

9. ___ ZnSO4 + ___ Li2CO3 ___ ZnCO3 + ___ Li2SO4

Zn= Zn=

Li= Li=

10.___ V2O5 + ___ CaS ___ CaO + ___ V2S5

Ca= Ca=

Did you realize that… if you see a polyatomic ion that is on both sides of the equation, you can (almost always) write it like it is one element.

11.___ Mn(NO2)2 + ___ BeCl2 ___ Be(NO2)2 + ___ MnCl2Mn= Mn=

NO2= NO2=

Be= Be=

Cl= Cl=

12.___ AgBr + ___ GaPO4 ___ Ag3PO4 + ___ GaBr3

Ag= Ag=

Br= Br=

Ga= Ga=

PO4= PO4=

13.___ H2SO4 + ___ B(OH)3 __ B2(SO4)3 + ___ H2O

SO4= SO4=

OH= OH=

This one (above) doesn’t have OH on the right. OR does it?! Sometimes it is helpful to think of water as H(OH).

14.___ S8 + ___ O2 ___ SO2

S = S=

15.___ Fe + ___ AgNO3 ___ Fe(NO3)2 + ___ Ag

Fe= Fe=

Ag= Ag=

NO3= NO3=

Section 4: Balancing Equations

Fill in the blanks with the correct coefficient to balance the equation.

1. _____ Fe + _____ S _____ FeS

2. _____ H2 + _____ Cl2 _____ HCl

3. _____ Mg + _____ O2 _____ MgO

4. _____ O2 + _____ H2 _____ H2O

5. _____ HgO _____ Hg + _____ O2

6. _____ Ca + _____ H2O _____ Ca(OH)2 + _____ H2

7. _____ CH4 + _____ O2 _____ CO2 + _____ H2O

8. _____ Na2O2 + _____ H2SO4 _____ Na2SO4 + _____ H2O2

9. _____ N2 + _____ H2 _____ NH3

10. _____ Al + _____ O2 _____ Al2O3

11. _____ KMnO4 _____ K2O + _____ MnO + _____ O2

12. _____ Na + _____ H2O _____ NaOH + _____ H2

13. _____ H2SO4 + _____ NaOH _____ Na2SO4 + _____ H2O

Section 5: Balancing Equations

Place the proper coefficient in the blanks provided to correctly balance the following chemical equations.

1. _____ PCl3 + _____ H2O _____ H3PO3 + _____ HCl

2. ____ As2O3 + ____ KI + ____ HCl ____ AsI3 + ____ KCl + ____ H2O

3. _____ MnS2 + _____ O2 _____ MnO2 + _____ SO2

4. _____ Cr + _____ S8 _____ Cr2S3

5. _____ WO3 + ______ H2 _____ W + ______ H2O

6. _____ PdCl2 + ______ HNO3 _____ Pd(NO3)2 + _____ HCl

7. _____ RbBr + _____ AgCl _____ AgBr + _____ RbCl

8. _____ HfCl3 + _____ Al _____ HfCl2 + _____ AlCl3

9. ______ Zn + _____ CrCl3 _____ CrCl2 + _____ ZnCl2

10. ____ BaCO3 + ____ C + ____ H2O ____ CO + ____ Ba(OH)2

11. ____ Cu + ____ H2SO4 ____ CuSO4 + ____ SO2 + ____ H2O

12. ____ Pb(CH3COO)2 + _____ K2CrO4 ____ PbCrO4 + ____ KCH3COO

13. _____ RbCl + _____ O2 _____ RbClO4

14. _____ SiF4 + _____ H2O _____ H2SiF6 + _____ H2SiO3

15. _____ Sn + _____ KOH _____ K2SnO2 + _____ H2

16. _____ C6H12O6 + _____ O2 _____ CO2 + _____ H2O

17. _____ MoS2 + _____ O2 _____ MoO3 + _____ SO2

18. _____ NiS + _____ O2 _____ NiO + _____ SO2

19. _____ CaC2 + _____ H2O _____ Ca(OH)2 + _____ C2H2

20. _____ H2O2 _____ H2O + _____ O2

21. ____ Na2B4O7 + ____ H2SO4 + ____ H2O ____ H3BO3 + ____ Na2SO4

Section 6: Reaction Types

Balance each equation. Identify each as combustion, synthesis, decomposition, single replacement, or double replacement.

1. Na + H2O NaOH + H2

2. CO + O2 CO2

3. FeS + HCl FeCl2 + H2S

4. NaNO3 NaNO2 + O2

5. CH4 + O2 CO2 + H2O

6. Fe + CuNO3 Cu + Fe(NO3)2

7. KI + Cl2 KCl + I2

8. Al + S Al2S3

9. KClO3 KCl + O2

10. C4H10 + O2 CO2 + H2O

11. BaCl2 + Na2SO4 BaSO4 + NaCl

12. C2H2 + O2 CO2 + H2O

13. KOH + HCl H2O + KCl

14. NH3 + H2CO3 (NH4)2CO3

15. LiHCO3 Li2CO3 + H2O + CO2

Section 7: Predicting ProductsFor each of the reactants below, predict the products that would occur. Make sure to write the correct formulas for them. Name the reactants and the products. Balance and classify the equations.

1. FeCl3 + KOH a. Names of reactants

___________________________________________________

b. Names of Products

__________________________________________________

c. Classification ____________________________________

2. CH4 + O2 a. Names of reactants

_________________________________________________

b. Names of Products

__________________________________________________

3. Ag + H2S a. Names of reactants

_________________________________________________

b. Names of Products __________________________________________________

4. Cl2 + KI a. Names of reactants

_________________________________________________

5. Mg(NO3)2 + KOH a. Names of reactants

_________________________________________________

6. HF + NaOH a. Names of reactants

_________________________________________________

7. Mg + H2S a. Names of reactants

_________________________________________________

8. AgNO3 + NaCl a. Names of reactants

_________________________________________________

c. Classification ___________________________________

9. TiCl4 + Na a. Names of reactants

_________________________________________________

10. H3PO4 + LiOH a. Names of reactants

_________________________________________________

11. C2H6 + O2 a. Names of reactants

_________________________________________________

12. LiOH + Fe(NO3)2 a. Names of reactants

_________________________________________________

13. (NH4)2S + ZnCl2 a. Names of reactants

_________________________________________________

Section 8: Activity Series

1. Will chromium replace lead in a single replacement reaction? _________

2. Will bromine replace fluorine in a single replacement reaction? _________

For each of the following reactions, determine if they reaction will go forward. If it does, predict the products that will form and balance the equation. If it will not, write no reaction after the arrow.

3. Ca + FeCl3

4. Ag + H2SO4

5. F2 + AlCl3

Section 9: Molecular, Ionic, and Net Ionic Equations

Show the total ionic and net ionic forms of the following equations. If all species are spectator ions, write no reaction for the net ionic equation. Note: Make sure the molecular equation is balanced before proceeding. 1. AgNO3 (aq) + KCl (aq) AgCl (s) + KNO3 (aq)

2. Mg(NO3)2 (aq) + Na2CO3 (aq) MgCO3 (s) + NaNO3 (aq)

3. strontium bromide (aq) + potassium sulfate (aq)

strontium sulfate (s) + potassium bromide (aq)

4. manganese(II) chloride (aq) + ammonium carbonate (aq)

manganese(II) carbonate (s) + ammonium chloride (aq)

5. chromium(III) nitrate (aq) + iron(II) sulfate (aq) chromium(III) sulfate (aq) + iron(II) nitrate (aq)

Please complete the following reactions, and show the total ionic and net ionic forms of the equation:

6. K3PO4 (aq) + Al(NO3)3 (aq)

7. BeI2 (aq) + Cu2SO4 (aq)

8. Ni(NO3)3 (aq) + KBr (aq)

9. cobalt(III) bromide + potassium sulfide

10. barium nitrate + ammonium phosphate

11. calcium hydroxide + iron(III) chloride

12. rubidium chloride + copper(II) sulfate

Section 10: Molecular, Ionic, and Net Ionic Equations

Write balanced molecular, ionic, and net ionic equations for each of the following reactions.

1. NaCl(aq) + Pb(NO3)2(aq) PbCl2(s) + NaNO3(aq)

2. Na2CO3(aq) + FeCl2(aq) FeCO3(s) + NaCl(aq)

4. K2CO3(aq) + CaCl2(aq) KCl(aq) + CaCO3(s)

5. (NH4)3PO4(aq) + Zn(NO3)2(aq) NH4NO3( ) + Zn3(PO4)2( )

6. LiOH(aq) + VCl3(aq) LiCl( ) + V(OH)3( )

7. Mg(NO3)2(aq) + Na2SO3(aq) NaNO3( ) + MgSO3( )

9. BaBr2(aq) + Na2SO4(aq)

10. AgNO3(aq) + MgI2(aq)

11. (NH4)2CO3(aq) + Al(ClO4)3(aq)

12. Ni(NO3)2(aq) + NaOH(aq)

Section 11: Oxidation Numbers

1. Give the oxidation numbers of all the elements in the following molecules and

ions:a. SO SO2 SO3 SO3

2- SO42-

b. ClO2 ClO- ClO2- ClO3

- ClO4-

c. N2O NO NO2 N2O4, N2O5 NO2-

2. Determine the oxidation number of the sulfur atom:

a. H2S

c. H2SO4

d. S2-

e. HS-

f. SO2

g. SO3

3. Indicate the oxidation number of phosphorus in each of the following compounds:

a. HPO3 _____ d. H3PO4 _____

b. H3PO2 _____ e. H4P2O7 _____

c. H3PO3 _____ f. H5P3O10 _____4. Give oxidation numbers for the underlined atoms in these molecules and ions:

a. Cs 2O

b. Pt Cl62-

c. Ca I2

d. Sn F2

e. Al 2O3

f. Cl F3

g. H3AsO3

h. Sb F6-

i. Ti O2

j. P 4

k. Mo O42-

l. Mn O4-

m. Pt Cl42-

n. O 2

Section 12: Redox Reactions

1. What is a redox reaction?

2. Can oxidation occur without reduction? Explain.

3. What is the oxidation number of any atom in the elemental state? __________

4. What is the oxidation number of any monatomic ion? _____________________

5. What is the sum of the oxidation numbers in a neutral compound equal? ______

6. What is the sum of the oxidation numbers in a polyatomic ion equal? _________

7. Determine the oxidation number of phosphorous in each substance.a. P4O8

b. P4O6

c. PO33-

e. H3PO4

f. PO43-

8. Determine the oxidation numbers of each element in each of the following compounds.

a. S2O3

b. KCl

c. Cl2

e. CO32-

f. NO2

g. NO3

h. NH3

9. If a substance is “reduced” does it gain or lose electrons? If a substance is “oxidized” does it gain or lose electrons?

10. Determine which substance is being oxidized and which is being reduced..

a. H2 + Cl2 2 HCl

Oxidized ___________ Reduced ___________

b. 2 O2 + N2 2 NO2

Oxidized __________ Reduced __________

c. 2 Li + F2 2 LiFOxidized __________ Reduced __________

d. 3 H2S + 2 HNO3 3 S + 2 NO + 4 H2OOxidized __________ Reduced __________

e. 2 PbSO4 + 2 H2O Pb + PbO2 + 2 H2SO4

Oxidized __________ Reduced __________

f. 2 Na + Br2 2 NaBrOxidized __________ Reduced __________

g. S + Cl2 SCl3Oxidized __________ Reduced __________

h. Mg + Cu(NO3)2 Mg(NO3)2 + CuOxidized __________ Reduced __________

11.Write the oxidation number above each element. Then, determine if each equation represents a redox reaction (circle yes or no).

a. 2 KClO3 2 KCl + 3 O2 yes / no

b. BaCl2 + 2 KIO3 Ba(IO3)2 + 2 KCl yes / no

c. HCl + NaOH H2O + NaCl yes / no

d. Mg + Br2 MgBr2 yes / no

e. NH4NO3 N2 + H2O yes / no

Section 13: Redox Reactions

In each of the following equations, indicate the element that has been oxidized and the one that has been reduced and give the oxidation state of each before and after the reaction.

1) 2 Na + FeCl2 2 NaCl + Fe

2) 2 C2H2 + 5 O2 4 CO2 + 2 H2O

3) 2 PbS + 3 O2 2 SO2 + 2 PbO

4) 2 H2 + O2 2 H2O

5) Cu + HNO3 CuNO3 + H2

6) AgNO3 + Cu CuNO3 + Ag

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Unit 1 - Avon Community School Corporation / Web view · 2013-01-25___ c2h4o2 + ___ o2 (...

Unit 1 - Avon Community School Corporation / Web view · 2013-01-25_ c2h4o2 + _ o2 (...