Chemical Equations

Like a recipe: ReactantsProducts 2H 2 (g) + O 2 (g)  2H 2 O(l) Introduction

Symbols  Yields or Produces (s)solid (l)liquid (aq)aqueous (g) gas Introduction

The Difference between (l) and (aq) Liquid – Pure liquid.Nothing is in it. H 2 O(l) Aqueous – Dissolved in water. NaCl(aq) = Salt water (l) or (aq)?

Distilled water Tap Water Iced Tea Mouthwash Gasoline Paint (l) or (aq)?

Easy Examples: Hd 10 + Bu 8  HdBu Balancing

1. Must balance because of the Law of Cons. of Matter 2.Rules: Can only change the coefficient, never the subscript Coefficient multiplies every atom in a formula Balancing

S + O 2  SO P 2 (g) + H 2 (g)  PH 3 (g) Balancing

Al + Cl 2  AlCl 3 H 2 O + C  H 2 + CO C 3 H 8 + O 2  CO 2 + H 2 O Balancing

C 2 H 6 + O 2  CO 2 + H 2 O C 4 H 10 + O 2  CO 2 + H 2 O Na 2 SO 4 + Fe(NO 3 ) 3  NaNO 3 + Fe 2 (SO 4 ) 3 Balancing

Fe(OH) 3 + H 2 SO 4  Fe 2 (SO 4 ) 3 + H 2 O Sodium reacts with water to form sodium hydroxide and hydrogen gas Balancing

Magnesium hydroxide reacts with hydrochloric acid (HCl) to form magnesium chloride and water.

Calcium reacts with water to form hydrogen and calcium hydroxide Aluminum nitrate reacts with sodium hydroxide to form aluminum hydroxide and sodium nitrate

Copper(II) chloride reacts with iron(III) sulfate to form copper(II)sulfate and iron(III) chloride Phosphoric acid (H 3 PO 4 ) reacts with calcium hydroxide to form water and calcium phosphate Balancing

Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  MgSO 4 + AlPO 4 Fe 2 S 3 + O 2  Fe 2 O 3 + SO 2 Ru 2 O 3 + CO  Ru + CO 2 NaBr + Al(NO 3 ) 3  NaNO 3 + AlBr 3 Ba + AlCl 3  BaCl 2 + Al Propane (C 3 H 8 ) is burned in oxygen to produce carbon dioxide and water Iron(III)nitrate reacts with lithium carbonate to form iron(III)carbonate and lithium nitrate. Sodium Chlorate decomposes to form sodium chloride and oxygen gas

Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  3MgSO 4 + 2AlPO 4 2Fe 2 S 3 + 9O 2  2Fe 2 O 3 + 6SO 2 Ru 2 O 3 + 3CO  2Ru + 3CO 2 3NaBr + Al(NO 3 ) 3  3NaNO 3 + AlBr 3 3Ba + 2AlCl 3  3BaCl 2 + 2Al C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 2Fe(NO 3 ) 3 + 3Li 2 CO 3  Fe 2 (CO 3 ) 3 + 6LiNO 3 2NaClO 3  2NaCl + 3O 2

Sulfur trioxide reacts with water to form sulfuric acid (H 2 SO 4 ) Boron sulfide, B 2 S 3, reacts with water to form boric acid, H 3 BO 3 and hydrogen sulfide, H 2 S. Mercury(II)nitrate decomposes to form mercury(II) oxide, nitrogen dioxide, and oxygen Hydrogen sulfide reacts with iron(III)hydroxide to form iron(III)sulfide and water.

Mg 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  MgSO 4 + AlPO 4 Fe 2 S 3 + O 2  Fe 2 O 3 + SO 2 Ru 2 O 3 + CO  Ru + CO 2 a.Propane (C 3 H 8 ) is burned in oxygen to produce carbon dioxide and water b.Iron(III)nitrate reacts with lithium carbonate to form iron(III)carbonate and lithium nitrate. c.Sodium Chlorate decomposes to form sodium chloride and oxygen gas

Chemical Equations

Synthesis (Combination) Decomposition Combustion Single Replacement Double Replacement Dissolving Types of Reactions

1. Synthesis Two or more elements or compounds combine to form a new compound Examples Na(s) + Cl 2 (g)  NaCl(s) C(s) + O 2 (g)  CO 2 (g) CaO(s) + CO 2 (g)  CaCO 3 (s) Types of Reactions

2. Decomposition Opposite of synthesis One compound breaks down, usually requires heat energy Types of Reactions

Dima, a 40,000 year old frozen mammoth (Alaska)

Examples: HgO(s)  Hg(l) + O 2 (g) CaCO 3 (s)  CaO(s) + CO 2 (g) KClO 3 (s)  KCl(s) + O 2 (g) Types of Reactions

Duke: In loving memory.

3. Combustion Fast reaction with O 2 (Burning) Hydrocarbons burn to form CO 2 and H 2 O Types of Reactions

Examples: Mg(s) + O 2 (g)  MgO(s) C 8 H 18 + O 2  CO 2 + H 2 O C 6 H 12 O 6 + O 2  CO 2 + H 2 O Types of Reactions

4. Single replacement One element replaces another Not every element can replace every other element Types of Reactions

Zn + CuCl 2  Cu + ZnCl 2 Cr + Pb(NO 3 ) 2  Pb + Cr(NO 3 ) 3 Mg + HCl  MgCl 2 + H 2

5. Double replacement Two elements switch places ZnBr 2 + AgNO 3  Zn(NO 3 ) 2 + AgBr BaCl 2 + H 2 SO 4  BaSO 4 + HCl Na 2 CO 3 + CaCl 2  CaCO 3 + NaCl Types of Reactions

Acid/Base Reactions A special type of double replacement Acids a. produce H + b. Often start with H (HCl, H 2 SO 4, H 3 PO 4 ) Types of Reactions

Bases a. produce OH - b. Hydroxides (Drano, NaOH) NaOH + HCl  KOH + HCl  Types of Reactions

6. Dissolving A. Molecular Compounds 1) Contain all non-metals 2) Do not break up into ions in water 3) Some are still soluble: C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) Types of Reactions

B. Ionic Compounds (and acids) 1) Contain a metal 2) Break up into ions in water. 3) Examples: NaCl(s)  Na + (aq) + Cl - (aq) CaCl 2 (s)  Ca 2+ (aq) + 2Cl - (aq) KNO 3 (s)  K + (aq) + NO 3 - (aq) 4) Different than decomp. because ions are produced. Types of Reactions

What Ions are produced when these dissolve: AlCl 3 (s)  Na 2 CO 3 (s)  NH 4 Cl(s)  FeBr 2 (s)  (NH 4 ) 2 Cr 2 O 7 (s)  Types of Reactions

BaCO 3 (s)  BaO(s) + CO 2 (g) Ca(NO 3 ) 2 (s)  Ca 2+ (aq) + 2NO 3 - (aq) KOH + HBr  KBr + H 2 O N 2 + H 2  NH 3 BaCl 2 + MgSO 4  BaSO 4 + MgCl 2 Cr + Pb(NO 3 ) 2  Pb + Cr(NO 3 ) 3 C 5 H 12 + O 2  CO 2 + H 2 O Types of Reactions

Steps: 1.Identify the type of reaction 2.Break all elements into ions (generally keep polyatomic together) 3.Write the products 4.Balance the equation Predicting Reactions

K + O 2  Mg + O 2  Al + Cl 2  Na + N 2  K + F 2  Predicting Reactions

CH 4 + O 2  C 2 H 6 + O 2  C 3 H 8 + O 2  C 6 H 6 + O 2  Predicting Reactions

CuSO 4 + NaOH  BaCl 2 + AgNO 3  HNO 3 + LiOH  H 2 SO 4 + KOH  AgNO 3 + HCl  Predicting Reactions

K + Fe(OH) 2  Al 2 O 3 + Mg  Fe + CuCl 2  HCl + Al  Na + Ca(NO 3 ) 2 

CuCl 2 (s) (placed in water)  KNO 3 (s) (placed in water)  Mg(NO 3 ) 2 (s) (placed in water)  Na 3 PO 4 (s) (placed in water) 

K 2 CO 3 (s)  (Placed in water) HNO 3 + KOH  Pb(NO 3 ) 2 + K 2 SO 4  Al + O 2  FeCl 3  (Placed in water) H 2 SO 4 + NaOH  C 2 H 4 + O 2  Mg + CaCl 2  Types of Reactions

C 4 H 10 + O 2  Ga + Cl 2  Na + HNO 3  H 3 PO 4 + NaOH  Ba(NO 3 ) 2 (s)  (Placed in water) AgNO 3 + KCl  Li + O 2  C 6 H 12 O 6 (s)  (placed in water) Types of Reactions

Barium nitrate reacts with copper(II) sulfate Sulfuric acid (H 2 SO 4 ) plus lithium hydroxide Zinc metal reacts with lead(II)nitrate Propane (C 3 H 8 ) is burned in oxygen Aluminum metal reacts with bromine Magnesium phosphate dissolves in water

HCl + Ba(OH) 2  HClO 4 + LiOH  Pb(NO 3 ) 2 + KI  H 3 PO 4 + NaOH  H 3 PO 4 + Ca(OH) 2  Types of Reactions

2H 2 +O 2  2H 2 O 2 molecules 4molecules 7molecules 24 molecules

CH 4 +2O 2  CO 2 +2H 2 O 5 molecules 18 molecules 16 molecules Molecule to Molecule

2KBrO 3  2KBr+3O 2 2 molecules 4 molecules 6molecules 12 molecules 12 molecules 24 molecules Molecule to Molecule

H 3 PO 4 +3NaOH  Na 3 PO 4 +3H 2 O 12 molecules 75 molecules 18 molecs Molecule to Molecule

4Al +3O 2  2Al 2 O atoms 12 molecules 32 molecules Molecule to Molecule

a)P 2 + H 2  PH 3 b)B 2 H 6 + H 2 O  H 3 BO 3 + H 2 c)C 2 H 4 + O 2  CO 2 + H 2 O d)KBrO 3  KBr + O 2

Fe + CuSO 4  KI + Pb(NO 3 ) 2  NaCl (s)  C12H22O11(s)  HCl + NaOH C 3 H 7 OH + O 2  Mg + O 2  (NH 4 ) 2 CO 3 

19.2Al + 3H 2  2Al H 3 4Al + 3O 2  2Al 2 O 3 2Al + 3I 2  2AlI 3 2Al + N 2  2AlN 21.2SbF 5  2Sb + 5F 2 PtO 2  Pt + O 2 3BrF  Br 2 + BrF 3

23.2C 4 H O 2  8CO H 2 O H 2 SO 3  SO 2 + H 2 O 2Na + O 2  Na 2 O 2 2Cu 2 O  4Cu + O 2

25. Ca 2+ (aq) + 2ClO 3 - (aq) Cs + (aq) + Br - (aq) Al 3+ (aq) + 3Cl - (aq) 2Cs + (aq) + SO 3 2- (aq) 27.LiOH  Li + (aq) + OH - (aq) HI  H + (aq) + I - (aq) 56.Ca(OH) 2 + 2HI  CaI 2 + 2H 2 O H 2 SO 4 + 2LiOH  2H 2 O + Li 2 SO 4 2HClO 4 + Ba(OH) 2  2H 2 O + Ba(ClO 4 ) 2

Fe + CuSO 4  Pb(NO 3 ) 2 + KI  NaCl(s)  C 12 H 22 O 11 (s)  HCl + NaOH  C 3 H 7 OH + O 2  Mg + O 2  (NH 4 ) 2 CO 3 (heated) 

Al + F 2  C 2 H 6 + O 2  KCl(s) (in water)  H 2 SO 4 + KOH  Ba + N 2  KCl + AgNO 3  (NH 4 ) 2 CO 3 (s) (in water) 

C 6 H 12 O 6 + O 2  Na 2 CO 3 + FeBr 3  Fe(NO 2 ) 2 (s) (in water)  Li + S 8  K 2 S + FeC 2 O 4  Mg + I 2  HNO 2 + Mg(OH) 2  C 4 H 6 + O 2  HCl + Al 

3. a) 2121 b)2112 c)121 d)2313 5a)1212 b)1333 c)838 d)2343

7a) 1212 b)1211 c)1316 d)1415 9a)1212 b)1331 c)4143 d)1434

11 a) C 6 H 6 O + 7O 2  6CO 2 + 3H 2 O b) Ca(OH) 2 + SO 3  CaSO 4 + H 2 O c) 6Li + N 2  2Li 3 N d) 3Mg + 2Cr(NO 3 ) 3  2Cr + 3Mg(NO 3 ) 2 13Fe 3 O 4 + CO  3FeO + CO 2 17a) 2C 2 H 6 O 2 + 5O 2  4CO 2 + 6H 2 O b) 2B 6 H O 2  6B 2 O H 2 O c) C 6 H O 2  6CO 2 + 6H 2 O d) Pb(C 2 H 5 ) 4 +14O 2  PbO 2 +8CO 2 +10H 2 O

19.2Al + 3H 2  2AlH 3 4Al + 3O 2  2Al 2 O 3 2Al + 3I 2  2AlI 3 2Al + N 2  2AlN 21. SbF 5  F 2 + SbF 3 PtO 2  Pt + O 2 3BrF  Br 2 + BrF Ca(ClO 3 ) 2 (s)  Ca 2+ (aq) + 2ClO 3 - (aq) CsBr(s)  Cs + (aq) + Br - (aq) AlCl 3 (s)  Al 3+ (aq) + 3Cl - (aq) Cs 2 SO 3 (s)  2Cs + (aq) + SO 3 2- (aq)

Ca 3 (PO 4 ) 2 + Al 2 (SO 4 ) 3  3CaSO 4 + 2AlPO 4 2C 4 H O 2  8CO H 2 O 2Fe 2 S 3 + 9O 2  2Fe 2 O 3 + 6SO 2 Fe 2 O 3 + 3CO  2Fe + 3CO 2 3KBr + Al(NO 3 ) 3  3KNO 3 + AlBr 3 2HgNO 3 + Na 2 CO 3  2NaNO 3 + Hg 2 CO 3 3Ca + 2AlCl 3  3CaCl 2 + 2Al 2HgO  2Hg + O 2

2K + Br 2  2KBr 2Au 2 O 3  4Au + 3O 2 2C 6 H O 2  12CO 2 + 6H 2 O P F 2  4PF 5 H 2 SO 4  H 2 O + SO 3

Types of Reactions a)Doublej) Single b)Singlek) Combustion c)Combustionl) Synthesis d)Decompositionm) Decomposition e)Synthesisn) Double f)Combustion g)Decompostion h)Single i)Synthesis

Na 2 S(s)  2Na + (aq) + S 2- (aq) Li 2 SO 4 (s)  2Li + (aq) + SO 4 2- (aq) FeCl 3 (s)  Fe 3+ (aq) + 3Cl - (aq) NaNO 3 (s)  Na + (aq) + NO 3 - (aq) Ca(NO 3 ) 2 (s)  Ca 2+ (aq) + 2NO 3 - (aq) NH 4 Cl(s)  NH 4 + (aq) + Cl - (aq)

SET A 2Al + 3F 2  2AlF 3 3Na 2 CO 3 + 2FeCl 3  Fe 2 (CO 3 ) 3 + 6NaCl AlCl 3 + 3Na  3NaCl + Al 2C 4 H O 2  8CO 2 + 6H 2 O KCl(s)  K + (aq) + Cl - (aq) 2C 2 H 6 + 7O 2  4CO 2 + 6H 2 O Fe(NO 3 ) 2 (s)  Fe 2+ (aq) + 2NO 3 - (aq) 4Na + O 2  2Na 2 O H 2 SO 4 + 2KOH  K 2 SO 4 + 2H 2 O

Na 2 S + CuSO 4  Na 2 SO 4 + CuS 3Ba + N 2  Ba 3 N 2 Mg + CuCl 2  Cu + MgCl 2 KCl + AgNO 3  AgCl + KNO 3 2HNO 3 + Ca(OH) 2  2H 2 O + Ca(NO 3 ) 2 (NH 4 ) 2 CO 3  2NH CO 3 2- C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O

SET B 3K + AlCl 3  Al + 3KCl AgNO 3 + HCl  AgCl + HNO 3 C 3 H 8 + 5O 2  3CO 2 + 4H 2 O 2Al + 3Cl 2  2AlCl 3 NaNO 3 (s) (in water)  Na + (aq) + NO 3 - (aq) HCl + KOH  H 2 O + KCl Mg(NO 3 ) 2 + 2Na  Mg + 2NaNO 3 BaCl 2 + Na 2 SO 4  2NaCl + BaSO 4 CuSO 4 (s) (in water)  Cu 2+ (aq) + SO 4 2- (aq)

2Na + I 2  2NaI Ca(OH) 2 + 2HBr  2H 2 O + CaBr 2 2C 4 H O 2  8CO H 2 O Mg + CuCl 2  MgCl 2 + Cu 3K 2 CO 3 + 2Fe(NO 3 ) 3  6KNO 3 + Fe 2 (CO 3 ) 3

Set C 4Li + O 2  2Li 2 O Al(NO 3 ) 3 (s) (in water)  Al 3+ (aq) + 3NO 3 - (aq) 16Ga + 3S 8  8Ga 2 S 3 H 2 SO 4 + 2NaOH  2H 2 O + Na 2 SO 4 3Zn(C 2 H 3 O 2 ) 2 + 2Al  3Zn + 2Al(C 2 H 3 O 2 ) 3 2NaOH + CuCl 2  Cu(OH) 2 + 2NaCl Fe 2 (SO 4 ) 3 (s) (in water)  2Fe 3+ (aq) + 3SO 4 2- (aq) C 2 H 5 OH + 3O 2  2CO 2 + 3H 2 O

3Mg(OH) 2 + 2H 3 PO 4  Mg 3 (PO 4 ) 2 + 6H 2 O Sn + 2HCl  SnCl 2 + H 2 4Al + 3O 2  2Al 2 O 3 2AlBr 3 + 3Na 2 S  6NaBr + Al 2 S 3 2CH 4 O + 3O 2  2CO 2 + 4H 2 O (NH 4 ) 2 CO 3 (s) (in water)  2NH 4 + (aq) + CO 3 2- (aq) 8Mg + S 8  8MgS HNO 3 + LiOH  H 2 O + LiNO 3 2AgNO 3 + Pb  Pb(NO 3 ) 2 + 2Ag

CaCl 2 + Na 2 CO 3  NaCl + CaCO 3 CaCl 2 + NaOH  NaCl + Ca(OH) 2 CuSO 4 + NaOH  Na 2 SO 4 + Cu(OH) 2 NaHCO 3 + HCl  NaCl + H 2 O + CO 2

12 a) 612 b)132 c)2214 d)1632 e)3216 f)2112 g)494102

13.CaC 2 + 2H 2 O  Ca(OH) 2 + C 2 H 2 2KClO 3  2KCl + 3O 2 Zn + H 2 SO 4  H 2 + ZnSO 4 PCl 3 + 3H 2 O  H 3 PO 3 + 3HCl 3H 2 S + 2Fe(OH) 3  Fe 2 S 3 + 6H 2 O 14. SO 3 + H 2 O  H 2 SO 4 B 2 S 3 + 6H 2 O  2H 3 BO 3 + 3H 2 S Pb(NO 3 ) 2 + 2NaI  2NaNO 3 + PbI 2 2Hg(NO 3 ) 2  2HgO + 4NO 2 + O 2 Cu + 2H 2 SO 4  CuSO 4 + SO 2 + 2H 2 O

19. a)232synthesis b)1322combustion c)612synthesis d) 111decomposition e) 1874combustion 20. a) 2966combustion b) 112decomposition c) 1653combustion d) 132synthesis e) 112synthesis

Na 2 S(s)  2Na + (aq) + S 2- (aq) Li 2 SO 4 (s)  2Li + (aq) + SO 4 2- (aq) FeCl 3 (s)  Fe 3+ (aq) + 3Cl - (aq) 2K + Br 2  2KBr 2Au 2 O 3  4Au + 3O 2 2C 6 H O 2  12CO 2 + 6H 2 O P F 2  4PF 5 H 2 SO 4  H 2 O + SO 3

Fe + CuSO 4  Cu + FeSO 4 Pb(NO 3 ) 2 + 2KI  PbI 2 + 2KNO 3 NaCl(s)  Na + (aq) + Cl - (aq) C 12 H 22 O 11 (s)  C 12 H 22 O 11 (aq) HCl + NaOH  H 2 O + NaCl 2C 3 H 7 OH + 9O 2  6CO 2 + 8H 2 O 2Mg + O 2  2MgO (NH 4 ) 2 CO 3  H 2 O(l) + 2NH 3 (g) + CO 2 (g)