MOLECULAR, (TOTAL) IONIC AND NET IONIC EQUATIONS 1.Sodium chloride and silver nitrate → sodium nitrate and silver chloride NaCl + AgNO 3 → NaNO 3 + AgCl(s)

Slides:

Advertisements

Similar presentations

Reactions in Aqueous Solutions

Advertisements

Double Replacement Rxn

Predicting the Products of Double Replacement Reactions

Writing Equations for Reactions in Solution Nia Gilliam 5/6 periods Chem. II, 3 rd tutorial.

Electrolytes Some solutes can dissociate into ions. Electric charge can be carried.

AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?

Net Ionic Equations.

Unit 3 – Chemical Reactions.  In many ionic reactions, not all of the chemical species undergo a change.  Those that do not change are called spectator.

Notes on Total and Net Ionic Equations. Ionic Compounds (Metal and Nonmetal) (Cation and Anion) If soluble these compounds will DISSOLVE and DISSOCIATE.

Net Ionic Equations mixing ionic compounds. Ionic interactions When you dissolve 2 or more ionic compounds in water some parts of it may react together.

Chapter 6: Chemical Reactions.  Determine if a compound is soluble.

Which day would you like OWL quizzes due (4 AM)

Solubility Rules.

Meghan Daniel Emily Spellmire Mandy Radulea

Solubility Rules and Precipitation Reactions. Not all ionic compounds dissolve! Instead of doing experiments all the time to see which ones will dissolve,

Objectives To learn more about some of the results of chemical reactions To learn to predict the solid that forms in a precipitation reaction To learn.

 The ability to dissolve or break down into its component ions in a liquid  Example:  NaCl is soluble  Completely dissolves in water  AgCl is insoluble.

Net Ionic Equations Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Net Ionic Equations.

Chemical Reactions 9.3: Reactions in Aqueous Solutions.

Chemical Reactions CHM 1010 PGCC Barbara Gage

Unit 2 - Chemical Reactions. Double displacement occurs between ions in aqueous solution. A reaction will occur when a pair of ions come together to produce.

Precipitates and Solubility

Chapter 11 Chemical Reactions 11.3 Reactions in Aqueous Solution

Objective:  write a formula equation, complete ionic equation, and net ionic equation that represent a reaction.

Reactions in Aqueous Solution

7.5 Aqueous Solutions and Solubility: Compounds Dissolved in Water A compound is soluble in a particular liquid if it dissolves in that liquid. A compound.

1 Ions in Aqueous Solutions and Colligative Properties Chapter 13 Modern Chemistry Sections 1 & 2 Compounds in Aqueous Solutions Colligative Properties.

Types of Reactions. In Chemistry, we can identify a lot of different types of chemical reactions. We can put these chemical reactions into groups, so.

 Determine the type of reaction and predict the products: NaOH  Li + Br 2  C 2 H 4 + O 2 

Some Terminology Soluble – Will dissolve in a solvent Insoluble – Will not dissolve in a solvent Solvent – The substance that dissolves the solute Solute.

Solubility Rules. The terms soluble and insoluble are relative terms. soluble insoluble solute Solubility: the maximum amount of solute needed to make.

Chapter 4; Reactions in Aqueous Solutions I.Electrolytes vs. NonElectrolytes II.Precipitation Reaction a)Solubility Rules.

Reactions. Ionic solutions can be identified by their ability to conduct electricity. If a large number of ions are present in a solution, the solution.

Net Ionic Equations And A Little Review.

Compounds in Aqueous Solutions When dissolved in water, ionic and molecular compounds behave differently.

4.5 Precipitation Reactions

Predicting solubility. Pb(NO 3 ) 2 (aq) + 2 KI(aq)  PbI 2 (s) + 2KNO 3 (aq) overall ionic equation, which separates all the ions out: Pb 2+ (aq) + 2.

Predicting solubility. Using the table of solubilities we can now predict which of the products of a double replacement reaction will be insoluble (form.

Reactions in Aqueous Solution:. Double Replacement Reactions AB + CD  AD + CB AB + CD  AD + CB.

Precipitation Reactions

1) C + H 2 → C 3 H 8 2) C 6 H 12 + O 2 → H 2 O + CO 2 3) NaI + Pb(SO 4 ) 2 → PbI 4 + Na 2 SO 4 4) HgI 2 + O 2 → HgO + I 2 5)List the 7 diatomic molecules.

Aqueous Solutions.

Precipitation Reactions

Ch (Net Ionic Equations)

Net ionic equations Na + Al 3+ S 2– 2Ca 2+ PO 4 3– 3Cl –

Double Displacement Reactions

Net Ionic Equations.

CH 8 Solubility Rules & Net Ionic Equations. Chemical Reactions Many chemical reactions take place in solution. This means that the ionic compounds are.

Chemical Equations Molecular, Total Ionic & Net Ionic Equations.

Reactions in Aqueous Solution Chapter 9 Section 3.

If 36.2 mL of M CaCl 2 solution is added to 37.5 mL of M Na 2 CO 3, what mass of calcium carbonate, CaCO 3, will be precipitate? CaCl 2 (aq)

11.3 Reactions in Aqueous Solution 1 > Chapter 11 Chemical Reactions 11.1 Describing Chemical Reactions 11.2 Types of Chemical Reactions 11.3 Reactions.

Pick up a Packet and write down the following Essential Question: How are precipitation reactions written and how is a compound determined to be soluble.

CHAPTER 7 – REACTIONS IN WATER SOLUTIONS Reactions in water solution involve dissolved ionic compounds and acids DISSOLVED IONIC COMPOUNDS When an ionic.

Precipitation Reactions & Solubility Rules Thursday, February 18 th, 2016.

Ch. 11.3: Chemical Reactions Writing Net Ionic Equations & Solubility Rules Honors Chemistry.

Ch. 11.3: Chemical Reactions Solubility Rules & Writing Net Ionic Equations Dr. Knorr Honors Chemistry.

Net Ionic Equations. Do All Double Replacement Reactions Occur? (DEMO) Sodium chloride + silver nitrate  Sodium chloride + potassium nitrate 

Representing Aqueous Ionic Reactions With Net Ionic Reactions.

Balancing Equations Interactive Bonding learner.org.

Jeopardy Parts of Equations Balancing equations Predicting products

Solubility Rules and Precipitation Reactions

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

And Net Ionic Equations

Friday Bellwork Predict the products of the following reactions and balance the equation. Ca + N2  Cl2 + Fe (iron III)  MgO + CO2.

Double Replacement Reactions

Solubility and Precipitation Rules

What happens when you put

Solubility Rules (Page 170)

Ch (Net Ionic Equations)

Presentation transcript:

MOLECULAR, (TOTAL) IONIC AND NET IONIC EQUATIONS 1.Sodium chloride and silver nitrate → sodium nitrate and silver chloride NaCl + AgNO 3 → NaNO 3 + AgCl(s) The AgCl is labeled with (s) because it is insoluble and forms a precipitate.

IONIC EQUATION Na + + Cl - + Ag + + NO 3 - → Na + + NO AgCl(s) All substance are dissociated except for the insoluble AgCl(s)

NET IONIC EQUATION The ions not involved in forming the precipitate (Na + and NO 3 - ) are called "Spectator Ions" and are eliminated to form the net ionic equation. Ag + + Cl - → AgCl(s) Any source of silver ions and chloride ions would result in the same net ionic equation. Sodium chloride substitutes contain potassium chloride.

2. Copper(II) chloride + sodium sulfide → copper(II)sulfide and sodium chloride CuCl 2 + Na 2 S → CuS + NaCl CuCl 2 + Na 2 S → CuS (s) + 2 NaCl Cu Cl - + 2Na + + S 2- → CuS(s) + 2Na + + 2Cl - The spectator ions are Na + and Cl - Cu 2+ + S 2- → CuS(s)

3. Calcium chloride + sodium carbonate  calcium carbonate and sodium chloride CaCl 2 + Na 2 CO 3 → CaCO 3 (s) + 2NaCl Ca Cl - + 2Na + + CO 3 2- → CaCO 3 (s) + 2Na + + 2Cl - The spectator ions are Na + and Cl - Ca 2+ + CO 3 2- → CaCO 3 (s)

4. Barium nitrate + sodium phosphate → barium phosphate and sodium nitrate Ba(NO 3 ) 2 + Na 3 PO 4 → Ba 3 (PO 4 ) 2 (s) + NaNO 3 3 Ba(NO 3 ) Na 3 PO 4 → Ba 3 (PO 4 ) 2 (s) + 6 NaNO 3 3Ba NO Na + + 2PO 4 3- → Ba 3 (PO 4 ) 2 (s) + 6Na + + 6NO 3 - The spectator ions are Na + and NO 3 - 3Ba PO 4 3- → Ba 3 (PO 4 ) 2 (s)

5. Chromium(III) chloride + silver nitrate → chromium(III) nitrate and silver chloride CrCl 3 + 3AgNO 3 → Cr(NO 3 ) 3 + 3AgCl(s) Cr Cl - + 3Ag + + 3NO 3 - → Cr NO AgCl(s) 3Ag + + 3Cl - → 3AgCl(s) Ag + + Cl - → AgCl(s)