Is it over yet? Mastering Chemistry Reading Exam #3 Proficiency #3

Slides:

Advertisements

Similar presentations

Spontaneous Decompositions n H 2 CO 3 (aq) -> H 2 0 (l) + CO 2 (g) n NH 4 OH (aq) -> H 2 O (l) + NH 3.

Advertisements

Happy Birthday Tommy Lee Jones (1946) Read for Thursday Read for Thursday Chapter 5: Sections 1-5 Chapter 5: Sections 1-5 HOMEWORK – DUE Thursday 9/17/15.

Chapter 8 Chemical Reactions.

Happy Birthday J.J. Abrams (1966)

Section 4.3 Net Ionic Equations

AP Chemistry Due Next Class: Upcoming Due Dates: Chapter 1-3 Notes

Solubility Guidelines and Predicting precipitates

Barium Hydroxide Sulfuric Acid Reaction

CaCl2 (aq) + Pb(NO3)2 (aq) a Ca+2 Cl-1 Pb+2 NO3-1 Ca (NO3)2 + PbCl2

Net Ionic Equations The formation of an insoluble solid (a precipitate) drives a chemical reaction. Chemists use 3 types of equations to represent aqueous.

I’ve Got Nothin’ (2017) READING FOR Monday: Chapter 8 sections 1 – 5

Which of the following aqueous solutions would conduct electricity?

Na+ S2– PO43– 2Ca2+ 3Cl– Al3+ 9.1Net ionic equations.

CHEMISTRY 161 Chapter 4.

Ionic Equilibrium in Solutions

Chemical Change Chapter 9

9.2 Reactions in Aqueous Solutions

AP CHEMISTRY UNIT 8 TYPES OF REACTIONS

4-3 General Types (Sections 7.6, 7.7)

Reactions of Aqueous Ionic Compounds

Solubility Rules and Precipitation Reactions

Non-redox Reactions/ Double Replacement Reactions

Non-redox Reactions/ Double Replacement Reactions

Polyprotic Acids and Bases Section 6.5 pg. 258

Chapter 4: Aqueous Reactions

ACIDS AND BASES Chapter 18.

Reactions in Aqueous Solutions

Chapter 14 Acids and Bases

Chapter 4 Stoichiometry of Chemical Reactions

Complete Ionic Equation Net Ionic Equations

Types of Chemical Reactions

Net Ionic Equations.

Ppt15, Net Ionic Equations (mainly) PS6 material, continued

Practice What type of reaction is described by the following equation?

Reactions in Aqueous Solutions

Net Ionic Equations For precipitates only.

Complete and Net Ionic Equations

Tro's "Introductory Chemistry", Chapter 7

Reactions in Aqueous Solution

Happy Birthday Johannes Diderik van der Waals (1837)

S2– PO43– Na+ 2Ca2+ 3Cl– Al3+ Net ionic equations.

S2– PO43– Na+ 2Ca2+ 3Cl– Al3+ Net ionic equations.

Na and PO4 Iron (III) and Chlorine

Net Ionic Equations HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)

Double Replacement & Acid Carbonate Reactions.

Total/Net Ionic Equations

Happy Birthday Jagdish Chandra Bose ( )

Chapter 4: Types of Chemical Reactions

Predicting Reactions – Double Replacement

Chapter 11 Chemical Reactions 11.3 Reactions in Aqueous Solution

Solubility Guidelines and Predicting precipitates

Chemical Reactions Quiz 1 Common Problems…..

S2– PO43– Na+ 2Ca2+ 3Cl– Al3+ Net ionic equations.

REACTIONS IN AQUEOUS SOLUTIONS

Double Replacement & Acid Carbonate Reactions.

Reactions in Aqueous Solutions

= cations (+) = anions (-) Ions in Aqueous Solution Pb(NO3)2(s)

Chapter 5: Introduction to Reactions in Aqueous Solutions

Achuta! Do Now… Finish gluing! HW… Read 8.2 #’s 3-7.

Unit 3: Chemical Equations and Stoichiometry

Chemical Equations Review

S2– PO43– Na+ 2Ca2+ 3Cl– Al3+ Net ionic equations.

Predicting Reactions.

Ionic and Net Ionic Equations

Reactions in aqueous solutions:

Neutralization.

4-3 General Types (Sections 7.6, 7.7)

Ch (Net Ionic Equations)

Chapter 4: Types of Chemical Reactions

Presentation transcript:

Is it over yet? Mastering Chemistry Reading Exam #3 Proficiency #3 New assignment will be posted later today Due Thursday by 11:59PM Reading Chapter 8, sections 1-4 Exam #3 Proficiency #3

Electrolytes Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) S-E S-E S-E W-E 3 H2SO4(aq) + 2 Fe(OH)3(s)  Fe2(SO4)3(aq) + 6 H2O(l) S-E W-E S-E N-E 2 LiCl(aq) + Hg2(C2H3O2)2(aq)  2 LiC2H3O2(aq) + Hg2Cl2(s) S-E S-E S-E W-E

Electrolytes 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) W-E S-E W-E N-E K2CO3(aq) + 2 HClO4(aq)  2 KClO4(aq) + H2O(l) + CO2(g) S-E S-E S-E N-E N-E 2 NaNO3(aq) + Mg(ClO3)2(aq)  2 NaClO3(aq) + Mg(NO3)2(aq) S-E S-E S-E S-E

A solution of chromium (III) sulfate is added to a solution of cesium phosphate. Give the net ionic equation for any reaction that happens. Step 1: Write a balanced chemical equation (molecular equation) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3 Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) + Cs3PO4  CrPO4 + Cs2SO4

Step 1: Write a balanced chemical equation (molecular equation) A solution of chromium (III) sulfate is added to a solution of cesium phosphate. Give the net ionic equation for any reaction that happens. Step 1: Write a balanced chemical equation (molecular equation) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) SE SE WE SE Step 2: Break STRONG ELECTROLYTES ONLY into ions 2 Cr+3(aq) + 3 SO42-(aq) 2 Cr+3(aq) + 3 SO42-(aq) + 6 Cs+(aq) + 2 PO4-3(aq)  2 CrPO4(s) + 6 Cs+(aq) + 3 SO42-(aq) 2 Cr+3(aq) + 3 SO42-(aq) + 6 Cs+(aq) + 2 PO4-3(aq) 2 Cr+3(aq) + 3 SO42-(aq) + 6 Cs+(aq) + 2 PO4-3(aq)  2 CrPO4(s)

Step 1: Write a balanced chemical equation (molecular equation) A solution of chromium (III) sulfate is added to a solution of cesium phosphate. Give the net ionic equation for any reaction that happens. Step 1: Write a balanced chemical equation (molecular equation) Cr2(SO4)3(aq) + 2 Cs3PO4(aq)  2 CrPO4(s) + 3 Cs2SO4(aq) SE SE WE SE Step 2: Break STRONG ELECTROLYTES ONLY into ions 2 Cr+3(aq) + 3 SO42-(aq) + 6 Cs+(aq) + 2 PO4-3(aq)  2 CrPO4(s) + 6 Cs+(aq) + 3 SO42-(aq) Step 3: Cross out all spectator ions N.I.E 2 Cr+3(aq) + 2 PO4-3(aq)  2 CrPO4(s) 2 Cr+3(aq) + 2 PO4-3(aq)  2 CrPO4(s)

A zinc acetate solution is combined with 3. 50 M perchloric acid A zinc acetate solution is combined with 3.50 M perchloric acid. Give the net ionic equation. Step 1: Write a balanced chemical equation (molecular equation) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) HClO4 + Zn(C2H3O2)2  HC2H3O2

Step 1: Write a balanced chemical equation (molecular equation) A zinc acetate solution is combined with 3.50 M perchloric acid. Give the net ionic equation. Step 1: Write a balanced chemical equation (molecular equation) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) SE SE WE SE Step 2: Break STRONG ELECTROLYTES ONLY into ions 2 H+(aq) + 2 ClO4-(aq) 2 H+(aq) + 2 ClO4-(aq) + Zn2+(aq) + 2 C2H3O2-(aq) 2 H+(aq) + 2 ClO4-(aq) + Zn2+(aq) + 2 C2H3O2-(aq)  2 HC2H3O2(aq) + Zn2+(aq) + 2 ClO4-(aq) 2 H+(aq) + 2 ClO4-(aq) + Zn2+(aq) + 2 C2H3O2-(aq)  2 HC2H3O2(aq)

Step 1: Write a balanced chemical equation (molecular equation) A zinc acetate solution is combined with 3.50 M perchloric acid. Give the net ionic equation. Step 1: Write a balanced chemical equation (molecular equation) 2 HClO4(aq) + Zn(C2H3O2)2(aq)  2 HC2H3O2(aq) + Zn(ClO4)2(aq) SE SE WE SE Step 2: Break STRONG ELECTROLYTES ONLY into ions 2 H+(aq) + 2 ClO4-(aq) + Zn2+(aq) + 2 C2H3O2-(aq)  2 HC2H3O2(aq) + Zn2+(aq) + 2 ClO4-(aq) Step 3: Cross out all spectator ions N.I.E 2 H+(aq) + 2 C2H3O2-(aq)  2 HC2H3O2(aq) 2 H+(aq) + 2 C2H3O2-(aq)  2 HC2H3O2(aq)

Net Ionic Equations Start with a balanced chemical equation: M.E. Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) Na2C2O4(aq) + CaCl2(aq)  2 NaCl(aq) + CaC2O4(s) S.E. S.E. S.E. W.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2Na+(aq) + C2O4-2(aq) + Ca2+(aq) + 2Cl-(aq)  2Na+(aq) + 2Cl-(aq) 2Na+(aq) + C2O4-2(aq) + Ca2+(aq) + 2Cl-(aq) 2Na+(aq) + C2O4-2(aq) + Ca2+(aq) + 2Cl-(aq)  2Na+(aq) + 2Cl-(aq) + CaC2O4(s) 2Na+(aq) + C2O4-2(aq)

C2O4-2(aq) + Ca2+(aq)  CaC2O4(s) Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2Na+(aq) + C2O4-2(aq) + Ca2+(aq) + 2Cl-(aq)  2Na+(aq) + 2Cl-(aq) + CaC2O4(s) Cross out every thing that is EXACTLY the same on both sides: 2Na+(aq) + C2O4-2(aq) + Ca2+(aq) + 2Cl-(aq)  2Na+(aq) + 2Cl-(aq) + CaC2O4(s) N.I.E. C2O4-2(aq) + Ca2+(aq)  CaC2O4(s)

Net Ionic Equations Start with a balanced chemical equation (including subscripts): M.E. 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba(OH)2(aq)  BaF2(s) + 2 H2O(l) W.E. S.E. W.E. N.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2 HF(aq) + Ba2+(aq) + 2OH-(aq)  BaF2(s) + 2 H2O(l) 2 HF(aq) + Ba2+(aq) + 2OH-(aq)  BaF2(s) 2 HF(aq) 2 HF(aq) + Ba2+(aq) + 2OH-(aq)

Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2 HF(aq) + Ba2+(aq) + 2OH-(aq)  BaF2(s) + 2 H2O(l) Cross out every thing that is EXACTLY the same on both sides: 2 HF(aq) + Ba2+(aq) + 2OH-(aq)  BaF2(s) + 2 H2O(l) N.I.E. 2 HF(aq) + Ba2+(aq) + 2OH-(aq)  BaF2(s) + 2 H2O(l)

Net Ionic Equations Start with a balanced chemical equation (including subscripts): M.E. Fe2(SO4)3(aq) + 3 PbCl2(s)  2 FeCl3(aq) + 3 PbSO4(s) Fe2(SO4)3(aq) + 3 PbCl2(s)  2 FeCl3(aq) + 3 PbSO4(s) Fe2(SO4)3(aq) + 3 PbCl2(s)  2 FeCl3(aq) + 3 PbSO4(s) Fe2(SO4)3(aq) + 3 PbCl2(s)  2 FeCl3(aq) + 3 PbSO4(s) Fe2(SO4)3(aq) + 3 PbCl2(s)  2 FeCl3(aq) + 3 PbSO4(s) S.E. W.E. S.E. W.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2Fe+3(aq) + 3SO4-2(aq) + 3PbCl2(s)  2Fe+3(aq) + 6Cl-(aq) + 3PbSO4(s) 2Fe+3(aq) + 3SO4-2(aq) 2Fe+3(aq) + 3SO4-2(aq) + 3PbCl2(s)  2Fe+3(aq) + 6Cl-(aq) 2Fe+3(aq) + 3SO4-2(aq) + 3PbCl2(s)

Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2Fe+3(aq) + 3SO4-2(aq) + 3PbCl2(s)  2Fe+3(aq) + 6Cl-(aq) + 3PbSO4(s) Cross out every thing that is EXACTLY the same on both sides: 2Fe+3(aq) + 3SO4-2(aq) + 3PbCl2(s)  2Fe+3(aq) + 6Cl-(aq) + 3PbSO4(s) N.I.E. 3SO4-2(aq) + 3PbCl2(s)  6Cl-(aq) + 3PbSO4(s) 3SO4-2(aq) + 3PbCl2(s)  2Cl-(aq) + 3PbSO4(s)

Net Ionic Equations Start with a balanced chemical equation (including subscripts): M.E. NaNO3(aq) + LiCl(aq)  NaCl(aq) + LiNO3(aq) NaNO3(aq) + LiCl(aq)  NaCl(aq) + LiNO3(aq) NaNO3(aq) + LiCl(aq)  NaCl(aq) + LiNO3(aq) NaNO3(aq) + LiCl(aq)  NaCl(aq) + LiNO3(aq) NaNO3(aq) + LiCl(aq)  NaCl(aq) + LiNO3(aq) S.E. S.E. S.E. S.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. Na+(aq) + NO3-(aq) + Li+(aq) + Cl-(aq)  Na+(aq) + Cl-(aq) + Li+(aq) + NO3-(aq) Na+(aq) + NO3-(aq) + Li+(aq) + Cl-(aq) Na+(aq) + NO3-(aq) Na+(aq) + NO3-(aq) + Li+(aq) + Cl-(aq)  Na+(aq) + Cl-(aq)

Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. Na+(aq) + NO3-(aq) + Li+(aq) + Cl-(aq)  Na+(aq) + Cl-(aq) + Li+(aq) + NO3-(aq) Cross out every thing that is EXACTLY the same on both sides: Na+(aq) + NO3- (aq) + Li+(aq) + Cl-(aq)  Na+(aq) + Cl-(aq) + Li+(aq) + NO3-(aq) No reaction

Net Ionic Equations Start with a balanced chemical equation (including subscripts): M.E. 2 HC2H3O2(aq) + Ba(OH)2(aq)  Ba(C2H3O2)2(aq) + 2 H2O(l) 2 HC2H3O2(aq) + Ba(OH)2(aq)  Ba(C2H3O2)2(aq) + 2 H2O(l) 2 HC2H3O2(aq) + Ba(OH)2(aq)  Ba(C2H3O2)2(aq) + 2 H2O(l) 2 HC2H3O2(aq) + Ba(OH)2(aq)  Ba(C2H3O2)2(aq) + 2 H2O(l) 2 HC2H3O2(aq) + Ba(OH)2(aq)  Ba(C2H3O2)2(aq) + 2 H2O(l) W.E. S.E. S.E. N.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2 HC2H3O2(aq) + Ba2+(aq) + 2 OH-(aq)  Ba2+(aq) + 2 C2H3O2-(aq) + 2 H2O(l) 2 HC2H3O2(aq) + Ba2+(aq) + 2 OH-(aq) 2 HC2H3O2(aq) 2 HC2H3O2(aq) + Ba2+(aq) + 2 OH-(aq)  Ba2+(aq) + 2 C2H3O2-(aq)

Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2 HC2H3O2(aq) + Ba2+(aq) + 2 OH-(aq)  Ba2+(aq) + 2 C2H3O2-(aq) + 2 H2O(l) Cross out every thing that is EXACTLY the same on both sides: 2 HC2H3O2(aq) + Ba2+(aq) + 2OH-(aq)  Ba2+(aq) + 2C2H3O2-(aq) + 2 H2O(l) N.I.E. 2 HC2H3O2(aq) + 2OH-(aq)  2C2H3O2-(aq) + 2 H2O(l) HC2H3O2(aq) + OH-(aq)  C2H3O2-(aq) + H2O(l)

Net Ionic Equations Start with a balanced chemical equation (including subscripts): M.E. H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l) H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l) H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l) H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l) H2SO4(aq) + 2 NaOH(aq)  Na2SO4(aq) + 2 H2O(l) S.E. S.E. S.E. N.E. Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2H+(aq) + SO4-2(aq) + 2Na+(aq) + 2OH-(aq)  2Na+(aq) + SO4-2(aq) + 2H2O(l) 2H+(aq) + SO4-2(aq) + 2Na+(aq) + 2OH-(aq) 2H+(aq) + SO4-2(aq) + 2Na+(aq) + 2OH-(aq)  2Na+(aq) + SO4-2(aq) 2H+(aq) + SO4-2(aq)

Net Ionic Equations Break ALL strong electrolytes into ions. Leave non and weak electrolytes alone: I.E. 2H+(aq) + SO4-2(aq) + 2Na+(aq) + 2OH-(aq)  2Na+(aq) + SO4-2(aq) + 2H2O(l) Cross out every thing that is EXACTLY the same on both sides: 2H+(aq) + SO4-2(aq) + 2Na+(aq) + 2OH-(aq)  2Na+(aq) + SO4-2(aq) + 2H2O(l) N.I.E. 2 H+(aq) + 2 OH-(aq)  2 H2O(l) H+(aq) + OH-(aq)  H2O(l)