February 11th 2014

HONORS CHEMISTRY PERIOD 4

 * We walked in and showed Mrs. Friedmann our completed Pre- Lab questions

* Then our tests were returned and we went over certain questions that we had

* After we went over our tests, we started the lab

LAB

* During the lab, you must first weigh the metal rod
* Then you fill up the beaker with 600 ml of water
* Put 100 ml of water into the calorimeter (styrofoam cup) and measure the temperature of the water
* Boil the water and put the metal rod in there (carefully)
* Hold it up with the tongs and make sure that it does not touch the bottom
         - This is because you want the metal rod to have the same temperature as the water, not the hot plate
* Hold it there for 1 minute and then carefully transfer the rod into the calorimeter
* Stir and measure the final temperature of the water

MY DATA:

Weight of the metal rod - 26.68 grams

Initial temperature of the water in the calorimeter - 22.6 degrees Celsius

Final temperature of the water in the calorimeter - 26.1 degrees Celsius

HOMEWORK

1.) Webassign due tonight by 11:59 p.m.
2.) Specific Heat Calculations (hand out that consists of two worksheets) due tomorrow
3.) Lab write-up due Friday (VALENTINES DAY)

Next Blogger Will Be: Bobby

Class Blog 2/10/2014

Today we had a substitute teacher named Ms. Reicher. We had time to work on a few things today.

We got a worksheet called "Heat vs Temperature...What's the difference?" We finished it and turned it in by the end of class.

Then we had time to work on homework:

1. WebAssign - Section 8.1 "Principles of Heat Flow" - due tomorrow @ 11:59 PM
2. Pre-lab for "Specific Heat of a Metal", refer to "notes on heat calculations" - due tomorrow

Now its time for chemistry jokes...or not.

Class Blog 2/6/14

Before Class:

-We showed Mrs. Friedmann our homework, which was the two IMF worksheets

-We picked up a packet titled “Physical Properties of Liquids Lab”

During Class:

-We reviewed the homework (here)

-Next, we finished the Liquids Lab, and filled out the packet that went along with it, but it will not be collected

Homework:

-TEST TOMORROW

-Finish review packet for extra help, will NOT be collected for points

-Key to review packet is located here.

Next Blogger:

Harish Rajan

Wednesday February 3rd

We had a late arrival!!

What we did in class:

1. Went over the homework that was due yesterday

2. Took notes on Intermolecular Forces

3. Stared working on the Hw worksheets

Intermolecular Forces:

 There are three kinds

1. London Dispersion Forces
2. Dipole Dipole Force
3. Hydrogen bonding

The london dispersion method is also known as the Van Der Waals forces.  It includes Dipole between non-polar molecules to create a temporary attraction. Electrons can flow more in one direction than another, eventually temporary dipole.  The attraction is weak and short lived

The dipole dipole force is in between polar molecules. It when the + of one molecule attracts the - of another.  The attraction is a permanent one.

Hydrogen Bonding is like dipole on steroids.  It only happens when the H of one molecule attracts a F, O, or N of another molecule. 

HW:

1. Webassign due tonight by 11:59pm

2. Two IMF worksheets that we picked up at the beginning of class

3. Start the review packet!!! The test is this friday!!!!

Tuesday, Feb 4 BLOG

Blog for Tuesday, February 4

• First we checked in homework & received the Unit 8 Review packet
• No video for this unit, unless one is found from last year
• Test is Friday

• Then we continued taking notes & watched a demo

*     *     *     *     *     *     *     *     *     *     *

Hybridization

ex. NH3 Molecule: Trigonal Pyramid

The number of hybrid orbitals produced is the SAME as the number of atomic orbitals that blended.

S PPP DDDDD FFFFFFF

4 atomic orbitals made 4 hybrid orbitals so... =(SP3 hybridized)

*     *     *     *     *     *     *     *     *     *     *

ex. CO2      16 valence electrons

=(SP hybridized)

*     *     *     *     *     *     *     *     *     *     *

ex. KrF4      38 valence electrons

=(SP3D2 hybridized)

*     *     *     *     *     *     *     *     *     *     *

Sigma and Pi Bonds

(Double + Triple Bonds...)

^ There are 4 electrons in this SP2 orbital.

• There are 2 in a SIGMA bond (2 single bonds)
• And 2 in a PI bond

ex. SO2

Pi bonds allow electrons to spread out over the whole molecule. They are the reason resonance is possible. (Delocalization) 

Need to know: 

1. Sigma bonds stuck

2. Pi bonds can move

3. Single bond = sigma

4. Double bond = 1 sigma + 1 pi

5. Triple bond = 1 sigma + 2 pi

Tomorrow: Are molecules more like magnets or marbles?

*     *     *     *     *     *     *     *     *     *     *

Homework for Tonight

• TWO Webassigns:
• One - due tonight
• Other - due tomorrow (Weds @ 12am)

- Allie Boland

NEXT SCRIBE: Marlye Jerva (we switched)

February 3, 2014 Class Blog

We picked up 3 handouts which should be found in the Handouts Folder

We graded and went over our quizzes in class

We continued the notes on Molecule Polarity:

Molecule Polarity:
1) Are the bonds polar?
2) Is the molecule symmetrical?
3) Is the molecule polar?

Ex: ClO3 with a negative 1 charge
      =26 valence electrons

Hybridization 
To be a blend of something

Different atomic orbitals (s,p,d,f) are mixed to form new identical orbitals

Ex: SP3 orbital                  } A blending of orbitals
      SP3D orbital                }

(Proposed by Linus Pauling, it solves a big bonding problem)

What's the problem?
-The valence electrons don't fill each properly

The shape of the orbitals (doing the bonding) should look like the shape of the molecule.
THEY DON'T.

Pauling suggested that when electrons bond they are going to form a hybrid orbital to form the shape that we expect.


Homework: 
Webassign Due TOMORROW at 11:59
2 Wks we picked up today are due in class tomorrow

Next Blogger is Marlye Jerva

Friday January 31st

We took a partner quiz that took a majority of the class period

And we started taking some notes about Polarity

There are 2 kinds of Polarity:

• Bond Polarity
• electronegativity differences between 2 atoms

ex. N  <---+ C

    3.0          2.5 

The arrow points to N because the electrons have a stronger pull toward it. 

And since 3.0-2.5 is 0.5 the bond is a POLAR covalent bond.

• Molecule Polarity

We didn't finish the notes in class

Homework:

We have a WebAssign due SUNDAY night. You'll need your textbook.

I will be blogging on Monday again.