a) To perform the analysis of carbonates (lab 9) .

     b) To continue with part 1 one of Test 2.

 Period 2: 

1. Continue with part 1 of test 2.                                                                                                                     

Period 3/4: 

1.   Lab 9 – Analysis of Carbonates Complete all calculations and hand in (No conclusion).   

2.  Lab 8 & Lab 9 salt visual comparisons. Can we determine differences in the macro based on the micro.

3.  Continue with Test 2.  You will be able to continue at home with part 2 of the test.   

     a) To Complete Part 1 of Test 2

     b) To begin Part 2 of Test 3

Period 2/3: 

1.  Collect part 2 – question 1

2.  Complete Part 1 of Test 2 

3. Gave back both precipitation quizzes. (The best out of the 2 went into Power School)                                                                                                Reviewed 2nd quiz (2nd one after the Golden Arches Quiz)

Stoichiometry 4c – Precipitation – limiting reagent key p .pdf
View Download

Golden Arches Quiz:
Stoichiometry 4a – Precipitation – limiting reagent Key p .pdf
View Download

4. Begin Part 2 of Test 2                                                                                                         

Period 4: 

1. Collect part 2 – question 1                                                                                                         

     a) To complete the Part 2 of the test

     b) To Review Concepts of Keq value and law of mass action

Period 2: – After today you will have one more class period for the test (you may come in the rest of the week on your time to complete.)

1.  Continue with test 2, question 3 begins.                                                                                                                

Period 3/4: – Last day to work on the test in class. 

     a) To begin our discussion of acid/base chemistry –

     b) To identify strong acids, weak acids, strong bases, and weak bases and relate these strengths             with Coulombs Law

Period 2/3: 

1.  Complete the last period of in class testing of Test 2. Place everything in your folders of fun.

2.  Acid/Basics intro lesson – We will continue our tour of Stoichiometry through acid/base chemistry                                                                                                              

Period 4: 

1.  Acid/Basics intro lesson – We will continue our tour of Stoichiometry through acid/base chemistry   

Acid/Basics intro lesson notes:

 

                Demos – magnesium hydroxide, electrolyte 

                                        a) Strong Bases – weak bases Table F

                                             Coulombs Law!

 

                                        b) Acid and base definition introduction

                                                Why acids are dangerous? – what is the action of H⁺

                                                Why bases are dangerous?  – What is the action of OH^–

                                                Neutralization reaction –  example :  OH- from Mg(OH)₂

                                        c) Conductivity of metals – mobile electrons

 

                                        d) Electrolyte definitions – mobile ions

                                                Strong ACids and Bases are strongest electrolytes

                                                Salts that are soluble are electrolytes in (aq) and (l) phases only

                                                Stiochiometry is with Strong Acids or Strong Bases – (completion reactions)

                                                Weak acids/Weak bases do not completely dissociate.

                                                Vinegar (organic acid) weak acid = structure

 

                                          e)   Strong Acids – from Halogens – why HF is weak and why HCl, HBr, HI are strong?

                                                Coulombs LAW!!!!       

 

                                        Milk of Magnesia = Mg(OH)_{2                                                                   Drano = NaOH}

Both produce OH- ions but one is dangerous why?

NaCl (s)

Ionic solids  – NOT Electrolytes! (positive and negative ions locked in a crystal)   They are never electrolytes because the do not conduct electricity in solution or as a  liquid.  The ions ARE NOT FREE and thus cannot move.  It is the movement of ions that will enable them to conduct a charge.  All ionic compounds are a solid at STP due to STRONG COULOMBIC Attractions between the positive and negative ions.  Each ion is actually surrounded by 6 other oppositely charged ions that keep the ions in a very stable (low energy) structure. THUS IONIC Compounds in a solid state NEVER conduct a charge!

Ionic liquids – Electrolytes  These liquids require very high temperatures to occur as the ions would want to attract to each to form a crystal at lower temperature BUT at these high temperatures these liquids (of negative and positive ions) can conduct because the ions are free to move!

NaCl (s)     —–>      Na+(aq) + Cl– (aq)

Ionic solutions –  Electrolytes (dissolved ions) – must be soluble!  These solutions ARE electrolytes!  The ions although surrounded by water, are free to move and thus charge can be conducted through. the solution. IF the ionic solid is insoluble then it will not make a solution and the ions will still be locked in a crystal which will result in no charge being conduced

Sucrose (s)

Molecular compounds – NOT Electrolytes! Make molecules not ionic crystals These are made from nonmetals (small atoms) with a high attraction for electrons. These compounds make bonds by fighting for electrons between atoms since they all have high attraction for electrons. Each bond — is a pair of electrons between these atoms.  Because of the “tug of war” for electrons between these compounds, these electrons are not free to move and conduct a charge.  In fact because the electrons are held so tightly these compounds are so poor at conducting we call them insulators. Molecular compounds NEVER conduct as a solid or in a solution (even if they dissolve). Molecule compounds NEVER conduct in a solution because they are molecule with NO charge and thus are not electrolytes! Even if they are dissolved in solution there are no ions as theses are only atoms (Neutral!)

Metallic compounds – Fe (s)

Metallic compounds  – NOT electrolytes  These compounds do conduct in the solid state because they are made of metals (large atoms with a low attraction for their electrons) and thus allow the electrons in their outer most shell to “roam” throughout the crystal.  They unlike molecular compounds have loosely held electrons and thus these electrons are allowed to move freely.  Free moving charges conduct electricity!! We say that metallic compounds have a sea of mobile electrons in a crystal of positive nuclei.  Do not confuse the positive circles with ions as they are the nuclei of the atoms.

     a) To review concepts of an electrolyte with acid and bases and their relative strengths.

     b) To define and review the ACID /Base guys.

 Classwork:
Acid and Bases Intro packet new.pdf
View Download

Period 2:  – 

1.   A quick review of the electrolyte concepts (free ions), strong and weak base and acid.

2.   Acid/Base definitions – beginning of the acid/base packet       

3.   Weak acid/base equilibria, Conjugate acid, Conjugate base                                                                                       

Period 3/4: – 

1.   A quick review of the electrolyte concepts (free ions), strong and weak base and acid.

2.   Acid/Base definitions – beginning of the acid/base packet       

3.   Weak acid/base equilibria, Conjugate acid, Conjugate base       

Notes for today:

This is the mechanism of how CO₂ acts an acid by the the Lewis Definition.

The most complete definition is the Lewis acid base definition because there are acids and bases that DO NOT HAVE protons to donate or possibly accept BUT create acidic conditions or Basic Conditions.

 

In table K they list CO₂ an acid but it had no protons to donate?  It is an acid because when we bubble CO₂ in water the conditions in water become more acidic.  

 

                    CO₂  +   H₂O             ——>              intermediate                  ——>             H₂CO₃

                                                                                                                                                                                      _then…..

                                                    H₂CO₃   +   H₂O  <——>  H₃O⁺  +   HCO₃ ^-1

 

CO₂ can accept a pair if electrons (JUST LIKE a proton!!!) so the best and most complete definition of acids and bases is the LEWIS acid base definitions! Lewis acids like CO₂ are electron acceptors while bases like water in the example are electron donators!!

 

4. Demo with straw and pH probe.

CO₂ acts an acid by the the Lewis Definition.

The most complete definition is the Lewis acid base definition because there are acids and bases that DO NOT HAVE protons to donate or possibly accept BUT create acidic conditions or Basic Conditions.

 

In table K they list CO₂ an acid but it had no protons to donate?  It is an acid because when we bubble CO₂ in water the conditions in water become more acidic.  

Back to the pumpkin Stoichiometry from last week:

C2H2 (g)  +   5/2O2 (g)    —> 2CO2 (g)   +  H2O (g)                                                                                                               0r   2C2H2 (g)  +    5 O2 (g)    —> 4CO2 (g)   +  2H2O (g)

The chemical reaction that exploded the pumpkin was combustion or redox but the reaction the made fuel, C₂H₂ was?

What kind reaction is this?

 

                       CaC2 (s)   +   2H2O (l)           —–>                C2H2 (g)    +    Ca(OH)2

The Arrhenius definition although a good start to defining acids and bases is not complete because we have chemicals that do not have any hydroxide ions in their structure (like NaOH) but will create acidic or basic conditions in water.  In the case above,  the hydroxide ion (OH^–) was produced by the action of the  carbide ion (C₂^-2).   So the Bronsted-Lowry definition is a more complete definition because it includes those chemical species that Produce the Basic or Acidic conditions by Accepting a proton or donating a proton.                                                                                                                                                                                     

In the case above the carbide ion (C₂^-2) ion is the Bronsted-Lowry base (the carbide ion accepted the proton.) and the water is the Bronsted- Lowry acid (because water DONATED A PROTON) (

 

*Notice that acids must have electron deficient hydrogen to donate protons (H⁺).

 *Notice that Bases must have an ability to accept protons (H⁺).  Having a lone pair of electrons or having a negative           charge helps attract the protons!

 

                  The result of this acid base reaction is that acetylene C₂H₂ was produced.