Daily+Lessons

=__Organic Functional Group Priority List__=

Here is a great website with the priority list. It even has pictures you can manipulate with your mouse! Some of these, the anhydrides, acid halides and sulphides, will not be encountered in this course but it's still pretty great. You will get this list on the exam. Thank you Prof. Hunt from the University of Calgary. [|functional groups page]

__Review Topics and Faraday's Constant Challenge! [[file:Faraday's Law Intro.ppt]]__
==__Daniell Cell animation and PowerPoint [] And the Onion myth is: []__==

November 17th, 2009 Properties of Acids and Bases Intro!
With your group, you will
 * //Give the definition//
 * //Give a GENERIC and SPECIFIC example//
 * //Give a diagram or picture if applicable//
 * //Create one question for the class to solve//
 * //Post all of this below and sign off with your names so people can ask questions in the discussion tab//
 * //Briefly present it to the class//

1. Physical Properties of Acids and Bases (big red) •in solution, turn blue litmus red •these hydrogen-containing substances are electrolytes •compounds ionize to produce H +(aq) ions •in solution, neutralize bases •H +(aq) ions react with OH–(aq) ions to produce water •Taste sour •pH is below 7 Eg. Sulfuric Acid (H2SO4)
 * __ Acid: __**

•in solution, turn red litmus blue •ionic hydroxides dissociate to produce OH–(aq) ions •are electrolytes •in solution, neutralize acids •OH– (aq) ions react with H+ (aq) ions to produce water • Taste Bitter • Slippery • pH is above 7 Eg. Sodium Hydroxide (NaOH)
 * __ Bases __**

Question: A sour candy is dissolved in water. Which type of litmus paper will it affect?

2. Arrhenius Theory (small red) The Arrnehius Theory states that acids are substances which produce hydrogen ions in solution and bases are substances which produce hydroxide ions in solution. Neutralization happens because hydrogen ions and hydroxide ions react to produce water. The Arrhenius equation

Here is the equation posted!

k=A*exp(-Ea/R*T)

Temperature, T (K) The gas constant, R (From pV=nRT) Activation energy, EA (Minimum energy needed for the reaction to occur (J))

Examples 1. Acid + Base à Water + Salt 2. The reaction: 2NO2(g) -> 2NO(g) + O2(g) has a rate coefficient of 1.0 x 10-10 s-1 at 300 K and an activation energy of 111 kJ mol-1. What is the rate coefficient at 273 K? (  Solution: calculate the value of A for a temperature of 300 K, then use the calculated value of A to calculate k at a temperature of 273 K. We generally assume that A and the activation energy Ea do not vary with temperature). Question What is the exception to the Arrhenius Theory? By: Mackenzie, Jenna and Candy

3. Bronsted-Lowry Theory (big orange) 4. Lewis Theory (big blue) In 1923 G. N. Lewis suggested another way of looking at the reaction between H+ and OH- ions. In the Brnsted model, the OH- ion is the active species in this reaction it accepts an H+ ion to form a covalent bond. In the Lewis model, the H+ ion is the active species it accepts a pair of electrons from the OH- ion to form a covalent bond.

In the Lewis theory of acid-base reactions, bases donate pairs of electrons and acids accept pairs of electrons. A **Lewis acid** is therefore any substance, such as the H+ ion, that can accept a pair of nonbonding electrons. In other words, a Lewis acid is an **electron-pair acceptor**. A **Lewis base** is any substance, such as the OH- ion, that can donate a pair of nonbonding electrons. A Lewis base is therefore an **electron-pair donor**. __Example__: In the Lewis theory, an acid is any ion or molecule that can accept a pair of nonbonding valence electrons. Al3+ ions form bonds to six water molecules to give a complex ion. Al3+(//aq//) + 6 H2O(//l//) Al(H2O)63+(//aq//) This is an example of a Lewis acid-base reaction. The Lewis structure of water suggests that this molecule has nonbonding pairs of valence electrons and can therefore act as a Lewis base. __Question__: Predict whether the following ions or molecules can act as either a Lewis acid or a Lewis base. (a) Ag+ (b) NH3 [] The Lewis Theory was brought to you by: Leigh, Catherine, and Saptarshi (YAY!) 5. How the molecular structure affects the strenght: Binary Acids (small blue) Questions: What are the strong binary acids?
 * hydrogen is combined with a non metallic element
 * generic example: H-X, where H is the hydrogen and X is the non metallic element
 * Examples: CH4, NH3, H2O, HF, HCl, HBr, HI
 * their strengths depend on the solvation of the initial acid
 * the H-X bond energy
 * the electron affinity energy of X
 * the solvation energy of X
 * the weaker the H-X bond, the stronger the acid
 * reacts more quickly because there are less bonds to break
 * HCl + NaOH à H2O + NaCl
 * HCl only has one bond because chlorine and hydrogen share one electron to have a full orbital, this means it requires less energy to break the bonds, so it can react with other substances
 * Acid strength also coreelates to electronegativty differences
 * Greater the difference, the more polar the bond, meaning the loss of H+ occurs more regularily (therefore the acid is stronger)

6. How the molecular structure affects the strenght: Oxy Acids (small yellow) Acids in which OH groups and possibly additional oxygen atoms are bound to a central atom are called // oxyacids. They are usually written in a formula with H(a)X(b)O(c) - with hydrogen bonded with oxygen and any other atom. // When X is a nonmetal, the bond to O is covalent in character, and the substance does not readily lose OH-. Instead, these compounds are either acidic or neutral. As a general rule, as the electronegativity of X increases, so will the acidity of the substance. therefore H2SO4 is stronger than H2SO3 because the number of oxygen atoms bonded to the central atom is more. Question !!! Which is more stronger, HBRO or HBRO4? Ahsan,Jennice,Zach 7. What is pH and how do you calculate it? (small green) pH is a measurement of the acidity or basicity of a solution. It is measured on a scale of 0 to 14, with 7 representing neutrality (water), values above 7 representing bases, and values below 7 representing acids. The pH scale is not absolute, but rather uses standard solutions to create a relative scale. To calculate pH when the concentration of H­+(aq) is known, take the negative logarithm of the concentration as follows: pH = -log H­+(aq)]
 * 1) //For oxyacids that have the same number of oxygen atoms, acid strength increases with increasing electronegativity of the central atom X.//
 * 2) //For oxyacids that have the same central atom X, acid strength increases as the number of oxygen atoms attached to X increases.//
 * Definition of pH **

Acids have a pH below 7. An example of a slightly acidic substance is milk, with a pH of 6.8. A strong acid is battery acid, which has a pH of -0.1. Bases have a pH above 7. An example of a slightly basic substance is 7.2, and a strong base is household bleach with a pH of 12.9.
 * Examples **

Determine the substance by calculating the pH of a solution with a hydrogen ion concentration of 3.7 x 10-11 mol/L.
 * Question **



Definition: The theory states that an acid is a proton donor and a base is a proton acceptor. General Example AH+ -> A + H+ A is an acid B + H+ -> BH+ B is a base. Specific Example H2O -> OH- + H+ Water is acting as an acid. H2O+ H+ -> H3O+ Water is acting as a base in this case.
 * __Bronsted-Lowry Theory (big orange)__**

Conjugate Acid: A conjugate acid is formed when a base gains a positive hydrogen Ion (H+), and thus, having the ability to lose, this ion becomes an acid. Conjugate Base: A conjugate base is formed when an acid loses a positive hydrogen Ion (H+), and thus, having the ability to gain, this ion becomes a base.

A substance that appears to act as a Bronsted-Lowry acid in some reactions and Bronsted-Lowry base in some reactions is called amphiprotic. Therefore water is considered amphiprotic. Question: HCO3(aq) - + S2(aq) -> HS(aq)- + CO3 2-(aq) In the above diagram, identify the base in the reverse reaction. -Ho Jun Eom, Stephanie Pataracchia, and Mike Vine-

October 20th, 2009 Hess' Law! [[file:hess-law.ppt]]
Here is a video that summarizes the basics nicely too...media type="youtube" key="ViMxvmcH6C8" height="344" width="425"

**__ October 6th, 2009 __**
Packing of Solids:
 * __​__**__**​**__

Wednesday, September 30, 2009

 Here is the ppt presentation slides with the videos and slides for VSEPR theory and hybridization.

Friday, September 18, 2009 **

 Here is the ppt presentation slides with the videos and slides for quantum numbers and the quantum mechanical model.