Iron Chloride Lab

On day 1 of the of the lab we did very simply steps. We simply had to get the mass of our equipment and mix together 50mL of water with approximately 7.50g of Copper(2) Chloride in a baby jar. We placed our nail in this mixture overnight and we will wait to see what happens.

Quiz

Today we had our quiz over this unit and I found it particularly challenging. The conversions seemed harder than the notes we did in class.

To help me do batter for the unit test I found some websites with practice problems and more in depth notes.

More Notes

Practice Problems

Tutorial

Day 2 Stoichiometry

There are 2 approaches to this lecture. Personally, I liked the second approach better. It was more compact and it was all one step. I did not understand the part of subtracting from the original to find excess reactants. 

Even More Notes

Day 1 Stoichiometry

Must always start with a balanced chemical equation and if in doubt convert to moles! 

How to get Stoichiometry

What even is it?

Reactivity Lab

Today's lab was easy and so was the pre-lab quiz. Out of all the solids Calcium reacted the most while Lead never reacted with and of the liquids. I do not think my lab group waited long enough for all reactions to occur and we may have missed some:(

Redox Reactions

-driving force is electrons transferred
-losing electrons=oxidation(reducing agent)
-gaining electrons=reduced(oxidizing agent)

OIL RIG
(oxidation is lost, reduction is gain)

ELEMENTS REPLACE LIKE ELEMENTS, so non-metals to other non-metals and metals to metals

Synthesis- 2 or more reactants combine making 1 product

Decomposition- 1 reactant making multiple products

Combustion- oxygen as reactant, producing carbon dioxide and water

Redox for DUMMIES

Single Replacement

Unit Quiz

All together I thought this was a very easy quiz. Looking back I know realize I made at least one mistake. On question 6 you had to balance the equation then add the coefficients. You needed to put in two 3's to balance the equation, so the answer I choose was 6. However, I forgot to add the coefficients of one that were in front of the other products and reactants. Oh well, better luck next time.

Getting over it

Balancing chemical equations

How to improve

Practice Balancing

Acid/Base Reactions

•driving force is production of water 

•produces a salt and water

Strong acids

•produce H+

•HCl, HBr, H and when oxygen a outnumber the hydrogen a by two or more

Strong bases

•contain OH- anion

•all group 1 and 2 metals

Chemical Symbols

Anything above and arrow is a catalyst

All reactions must have diving force such as; formation of solid,water, or gas or transfer of electrons

Unit test

I feel that this test was a good judge of who worked hard and who didn't...those that complain that this test was to hard should try harder for the next test. This test may very well bring my grade down but I cannot blame the test for my lack of competence, only myself. I have been sick and did not put forth my best effort, however there will be other reset and I cannot dwell on the past or make excuses for myself(although I kinda just did with the sick thing)  Better luck next time!

Chemical Reactions

Clues that chemical reaction occurred 

-change in color

-solid forms

-bubbles form(aqueous solutions)

-heat/flame produced 

Molecular Formulas

1)calculate empirical formula mass

2)divide EF mass into gram formula mass and get whole number

3)distribute whole number to the empirical formula 

Quiz

I was very unprepared for this quiz. I spent hours studying the night before and still had no concept of the questions. I definetly need to look over my notes again before this next test. Did any of you have these problems? And do you have any advice? I want to understand this unit, I enjoy the simplicity of calculations but it is hard to find what data to use in a word problem.

Chemical Composition

Mole= 6.02x10^23

Moles to Grams

Grams to Moles

Average Atomic Mass

Molecular Weight

Molar Mass

Unit=grams/mole

Gram molecular mass

-covalent compound(no metals)

Gram formula mass

-ionic compounds(metals)

Calculate

The Mole and Molar Mass

Unit Pre-Test

We took this units pretest today...and I am quite worried. I did not know any of the subject material and I guessed in the entire test. However, all of the questions I didn't know were very similar. Hopefully, with some slight instruction I will understand. My grade in chemistry has slowly been rising and I do not want this unit to be what brings me down. I will try my best, and I can only hope it will be good enough!

Meal Conversion Project

I have rather enjoyed this project. It involves good food and it isn't overly complicated. The dish I am planning on bringing is gooey butter cake. This recipe is rather simply for being so delicious and dosent have many conversions to be made. This project has ingrained in my mind that 1cup=.473dL. Also, teaspoons=.203 mL. If I am ever in a different country and they ask me these metric conversions, now I have the answer. I hope that the rest of the class brings in even better treats!

Unit Test

After 2 weeks of learning information, both new and old, I successfully completed the test. I haven't received my grade yet but I am quite nervous. Although this chapter was easier compared to most, I'm worried I might have messed up my conversion rounding. Hopefully I didn't but being the realist that I am I expect the worst. I need to prepare more for these tests . Our class should have study sessions after school. There's always next chapter to improve!

Uncertainty in Measurement

Accuracy=proximity to true value(equipment)

Proximity=proximity of several measurements to each other(human)

Significant rules

RULES

0.004004500

-before decimal(insignificant)

-zeros before numbers hold place(insignificant)

-all non-zero integers(significant)

-trailing zeros(significant)

-zeros between integers(significant)

All numbers written in scientific notation are significant
how scientific notation works

Addition/subtraction 

Number of significant figures in the result is same as in the measurement with the smallest decimal places

Multiplication/division

Number of significant figures in the result is the same as in the measurement with the smallest number of significant figures

Matter notes

Whats the Matter with you?
•solids have lowest Kinetic energy; gases have highest

•CHANGE IN STATE IS PHYSICAL CHANGE

•change in temperature=change in Kinetic energy

•no temperature change=potential energy change

Classifying Matter

•Mixtures are homogenous(cannot see different components)or heterogenous(different components)

•pure substances are compounds(can be separated into similar substances) or elements(cannot be separated)

Changes of Matter

•changes either physical(no changes of matter) or chemical(change make new substance)

Seperating

•filtration

•distillation

•chromotgraphy

What Chromatography is?

Measurement pre-test

Today we took our pre-lab quiz for this unit. It consisted mostly of significant numbers and how to correctly find mass/volume. This chapter seems easy enough and relatively self explanatory, with it being centered around correctly reading measurements, something we've already learned. Hopefully, with a lesson on significant numbers and a formula worksheets I will easily be able to do well on the end of quarter test.

Mass and Volume Formulas

Measuring Tips

Beanium Lab

Beans after separated into color groups.

Beans before separated into color groups.

In trying to determine Isotopes of a "new" element, we counted the total number of beans, and the number of each color. We calculated the average mass of the isotopes by dividing the total mass by number of beans in that certain color. Also, calculated % abundance by dividing the number of beans in certain color by total of overall beans.

Influential Scientist

Dalton's 5 postulates Postulates

• elements composed of atoms
• atoms of one element are identical
• atoms of different elements are different
• compounds consist of the atoms of different elements
• atoms indivisible and are not created/destroyed in chemical reactions

how postulates are wrong

JJ Thompson(chocolate chip) JJ Thompson animation/information

• used cathode tube to show the atoms of any element emit particles with -charge



julieanngaleo.wikispaces.com

• electrons placed randomly in positive matrix

chemistry.tutorcircle.com

Rutherford(gold foil) Gold foil animation

• proved positively charged center in atom
• area of + was small and dense when compared to whole atom

www.daviddarling.info

Current Model

Atomic Structure and Radioactivity pre-test

This pre-test was very difficult for me, in reality I guessed on all of the questions. I did not know how to find the rate of atomic decay or half-life. I remembered very little about the difference between fission and fusion from physical science freshman year. I hope to master the sections from this unit, and with some instruction I believe I will be able to.

How to guess successfully

Types of Binary Compound Naming

tips for naming

Type 1

Characteristics

• contain metal and non-metal
• cation(+) and anion(-)
• metal has constant charge

                        Metals                                                                                  Non-Metal

name of metal does not change                                           take ending off and replace with -ide
no changes to end                                                                ions written with negative charge
ions are written with + charge          

Type 2

Characteristics

• metal from transitional block
• roman numerals

Type 3

Characteristics

• no metals
• prefixes used

1 Mono-

2 Di-

3 Tri-

4 Tetra-

5 Penta-

6 Hexa-

7 Hepta-

8 Octa-

9 Nona-

10 Deca-

Polyatomic Ions

practice naming

Polyatomic

Characteristics

• cannot alter form
• use () when using more than one ion

The memorization for the polyatomic ion test was stressful. Trying to remember the charges was the hardest part. Each ion has a different number with different names. The Chlorate family was most difficult because they were all so similar.