Class Blog 9/30

Beginning of Class

We started class by checking our homework. We checked the mole workshop correction and the Pre-Lab questions. Then we got our Beverage Density lab handed back. Mrs. Friedmann also attached a correction for the lab behind our Beverage Density Lab then we went over our lab. We went over getting density, percentage error, and writing conclusion. When writing the conclusion, we should always be thinking what was the point of our lab? Did we meet the goal of the lab?

Labs

Next we talked about Pre-Lab that was suppose to be done for homework. Some safety rules were…

1. Goggles

2. Tie long hair back

3. Light match 1st

But today, instead of match, we used something called flinch that will create a spark if squished together with two hands. When the Bunsen burner is fired up, put the test tube that has crystals in it side way and put it near the fire, so we can burn it off. Finally, we tried not to overheat the white stuff, it will produce poisonous gas. Never point the heating test tube to yourself nor your partner. After checking our pre-lab calculations, we started our lab.

(See the procedures on the hand-outs)

Mass of Test tube	32.15g
Mass of Test tube + hydrates	34.995g
Mass of burned hydrates in Test tube	34.09g

Homework:

-Finish the Lab Write up by Friday

-Quiz tmrw

Next Scribe:  Conrad M

Class Blog 9/27

Beginning of Class:

- Checked in  Homework (The problem we were assigned yesterday for the Mole Workshop activity)

- Picked up 3 handouts: Percent Sugar in Gum- An Introduction to “Percent Composition”, Lab: Formula of a Hydrate, and  Lab Write-Up

Bubble Gum Activity:

-If you were not in class today, check Moodle in the Notes folder to see what we did for the activity.

Mole Workshop:

- We spent 10 minutes with our group going over the 4 problems.

- There will be a key posted on moodle so you can correct your answers

Homework:

- Go on Moodle in the Keys folder and look at the key for all 4 problems on the Mole Workshop activity. Mark corrections in red pen on ALL 4 problems.

- 2 WebAssigns are due Sunday night at 11:59 pm

- Do the Pre-Lab Questions. Look on Moodle in the Unit 2 Lab and Activities Folder for critical information that will be needed for the lab.


Next Blogger: Kevin Jeon

Class Blog 9/26

Beginning of Class:

1. Picked up 1 handout: Mole Workshop. This can be found on Moodle in the Unit 2 Handouts Folder.

2. Checked in homework from last night (The 3 worksheets on Moles)

3. Quizzes from Monday were handed back.

Important Info:

• Mrs. Friedmann will be tutoring in the TLC next week on Monday and Wednesday
• Unit 2 Test will be next Thursday. There will be a study session before school again just like there was when we took the last test.

Homework:

• 2 new WebAssings were assigned. They are due Sunday at 11:59 PM
• Complete the problem you were assigned today from the Mole Workshop if you did not finish it in class. We will continue to work on it tomorrow in the first 15 minutes of class.

I will be the blogger again tomorrow because there was not much to blog about today.

Class Blog 9/25/13

Before Class:

1. Homework assignment “Calculating Molar Mass” was checked in.

2. “Moles 1” (2 Sheets), “Mole Conversions”, “Mole Worksheet #1” were all picked up at the start of class (These can be found on Moodle).

3. Mole Calcs Worksheet (there are two sheets in the one file) are homework due tomorrow (Unit 2 Handouts on Moodle).

4. “Moles 1” can be used as extra practice.

Answers to “Calculating Molar Mass” (which was Homework)

Equation Parenthesis represent subscripts Fe(2)= 2 Irons	Molecular or Ionic	Name of Compound	Molar Mass in g/mol (Go to 2 decimal places)
CaCO(3)	Ionic	Calcium Carbonate	100.09
N(2)O(6)	Molecular	Dinitrogen Hexoxide	124.02
Na(2)SO(4)	Ionic	Sodium Sulfate	142.05
C(8)H(18)	Molecular	Octane (OK if you didn’t know)	114.30
Fe(3)(PO(4))(2)	Ionic	Iron(I) Phosphate	357.50

****Remember the differences between ionic and covalent bonds while completing this****

Note: Grades for Beverage Lab, Non-metal vs Metal Lab, and Chapter 1 Quiz will be entered in the next few days. Class Dojo grades for Chapter 1 and 2 homework will be entered after Chapter 2.

Class:

1. Remember, a mole contains 6.022×1023 items!

2. This grams to moles to molecules conversion factor was used to solve problems on notes sheet “Moles 1” which can be found here with all the work shown. As you can see, the grams to moles to molecules was applied to solve a variety of problems.

3 . More practice with moles and using molar mass as conversion factor (see “Moles 1”).

Notes for “Moles 1” were filled out, can be found on Moodle again here, the rest is extra practice, NOT extra credit!

Next Blogger: Brant

Blog 9/24/2013

First we went over a few questions on the 3.1-3.2 reading sheet. Number 9 is confusing. You are expected to be confused… On question number 13, we will be learning how to do these calculations tomorrow.

We started and finished the first day of learning about the mole.

---

NOTES

Atoms

• Very small
• We work with them in large amounts so we can measure them in the lab
• Atoms are far too tiny to count

Moles

• No, not the animal
• No, not the thing on your face
• 6.02 * 1023
• This number is also known as avogadro's (avocado’s) number
  
  
  
  
  
  
  
  
  
• This is the amount of atoms in a mass
• Just like 2 is a par and 12 is a dozen, 6.02*1023 is a mole
• EXAMPLES:
• A dozen bowling balls is heavier than a dozen ping pong balls
• A mole of Li weighs less than a mole of Rn
• 1 atom of Co weighs 58.93 amu
• 58.93 g of Co is a mole of it

Molar Mass for Elements

• This is the average atomic mass
• The weight of one mole of the element
• EXAMPLES:
• 12.01 g C = 1 mole C
• 30.97 g P = 1 mole P
• 65.39 g Zn = 1 mole Zn
• 22.99 g Na = 1 mole Na

Molar Mass for Molecules

• (mass of element 1 + mass of element 2 + …)
• Find the mass of the WHOLE molecule
• EXAMPLES:
• H2O
• Mass of H = 1.01 g
• Mass of O = 16.00
• Since there are 2 H’s in H2O, when calculating the molar mass you must multiply the molar mass of an individual H by 2
• (2 * 1.01 g H) + (1 * 16.00 g O) = 18.02 g H2O
• 1 mole of H2O = 18.02 g

Size of the Mole

• An enormous number
• 6.02 * 1023
• 602,000,000,000,000,000,000,000
• Just to give you a better idea…
• 1 mole of watermelon would be found inside a melon larger than the size of the moon
• 1 mole of donut holes would cover the earth to a depth of 5 miles
• One mole of pennies would make at least seven stacks that reach the moon
• By the way, if you spent $1,000,000 a day, you would still have 99% of your wealth by the time you die

MOLES ARE REALLY BIG

Atoms are really small

HW: Calculating molar mass worksheet

Next blogger - FRANKIE SULEJMANI (to finish up from the first day which was the day of the quiz)

Class Blog 9/23/13

Class Blog 9/23/13

Beginning of Class:

-Three worksheets were checked in the were handed out Friday named "Names and Formulas of Ionic Compounds", "Classification of Elements", and "Naming Practice Covalents". Also notes from the 3 ChemThinks were also checked in

-These worksheets are available on Moodle

-Worksheets were reviewed, and questions were taken class

-The rest of the class was used for a quiz on everything we have learned from Chapter 2

Homework:

-Reading sheet for sections 3.1 and 3.2 in textbook

-This takes the place of WebAssigns, which we ARE NOT using as of now unless stated otherwise by Ms. Friedmann because of technical difficulties.

Class Blog 09/20/2013

PERIOD 4 HONORS CHEM CLASS 09/20/2013

The beginning of Period 4

In the beginning of class there were handouts on Classification of Elements.

First we went over the Ionic Bonding Chart handout that we got the other day in class.

Some major ideas that were brought up during the discussion were:

- Polyatomic ion Cyanide and Hydroxide are the only polyatomics that end in -ide

- Metals are never negative  

- How to make a compound neutral is by making sure the charges cancel out

Notes:

You can find the notes taken on Moodle to paste into your journal!

Properties of the Periodic Table Groups

Alkali Metals Alkaline Earth Metals

- Group 1 - Group 2

- +1 ions - +2 Ions

- Most reactive metals - Reactive Metals

Transition Metals Halogens

- Groups 3-12 - Group 17

- A Variety of ions - -1 Ions

- Use Roman Numerals when - Most reactive nonmetals

naming structural metals

Noble Gases Inner Transitions    

- Group 18 - supposed to slide in with

- NO IONS! (No charge!) the transition metals

- Used in “neon” lighting. - Aka Lanthanides and
Actinides

aka “Rare Earths”

- Group along the bottom

Naming Acids Handout

- Refer to the handout as you read these notes

- You can find this handout on Moodle under Unit 2

*Naming acid is going to be on the quiz (1 question or so)*

Patterns we see in the first column of names of the acids:

- They contain a single element anion (Cl⁻, Br⁻)

- Their names end in “-ic”

- Start with “hydro-”

- They do not contain oxygen

Patterns of the names of the acids in second and third column:

- The ones with more oxygens end with “-ic”

- The ones with fewer oxygens end with an “-ous”

To determine if a compound is an acid it must be in water and must start with “hydro” (H)

Acids that DO not contain the element oxygen have the prefix “hydro” in the front and the ending of the anion has to be changed to “-ic”

Acids that DO NOT contain the element oxygen:

If the anion ends with “-ate”, the ending of the acid is changed to “-ic”

If the ending of the anion is “-ite”, it has to be changed to “-ous”

Examples:

HF = Hydrofluoric Acid

H₂CO₃ = Carbonic Acid

HCIO₂ = Chlorous Acid

Naming Covalent Compounds Handout

Prefixes:

Mono - 1, Di - 2, Tri - 3, Tetra - 4, Penta - 5, Hexa - 6, Hepta - 7, Octa - 8, Nona - 9, Deka - 10

Some major notes:

- If you see a metal it’s IONIC.

- If you see no metals, and no ammonium, it is COVALENT

- The first element named in each compound is a nonmetal

- The second element named in each compound is a nonmetal

- The bonding holding these two compounds together is covalent (aka molecular)

RULE FOR NAMING COVALENT COMPOUNDS

Say the name of the first element and a prefix that says how many there are. Then say a prefix and name of the second element. End with and “-ide”

Example:

SiO₂ = Silicon Dioxide

HOMEWORK!

1.) Names and Formulas of Ionic Compound handout due Monday

2.) Classification of Elements also due Monday

3.) Naming Practice handout due Monday

4.) Three ChemThinks - Take notes on the tutorials and answer questions (12 Points for completion online and 3 points for notes)   

Take notes on:

- Ionic Bonding

- Ionic Formulas

- Covalent bonding

5.) Quiz on Monday - Everything we talked about starting from unit two until now is fair game!

Our next blogger will be....

Frankie Sulejmani!!!!! :)