2nd Three Questions

1. The tasks I have completed are how to find empirical formulas, molecular formulas, and how to do stoich properly.
2. What I can understand is the stoich conversions, and empirical/molecular formulas. I am still alittle fuzzy on the metric conversions.
3. What I plan to do is to study the metric conversions so I know them right off the top of my head, that way stoich will come a lot easier to me.

Electrolyzing Water Lab

Balanced chemical equation: 

The qualitative evidence to support the balanced chemical reaction is the fact that you could visually observe both gases and which was which gas by the amount in the tubes, and the pH indicator showed the difference. You could collect quantitative data to prove the balanced reaction by justifying whether the reaction gained electrons or lost electrons. The reduction and oxidation equations show that.

Particle Diagram

Hydrate Explore Lab

    A mixture is different from a pure substance because a pure substance is only one type of atom/molecules, whereas a mixture is a number of different pure substances mixed together. The Hydrate lab uses the technique heat to extract water molecules from the hydrate. Because all that is taken away from the hydrate is the water molecules, we can conclude that hydrate is a pure substance. You can support your conclusion mathematically by finding the percent composition. To find the percent composition, you need to divide the difference between the hydrated hydrate and the dehydrated hydrate, divided by the difference of the evaporating dish and hydrate, then multiply by 100. To evaluate the validity of your results, first you need to divide the part by the whole, then multiply it by 100. That number is going to be the ideal percent composition. Then you use stoichiometry to evaluate how close your results are.

Exothermic reaction in the Hydrate

 Percent composition equation

Stoichiometry equation

Three Questions

1. The tasks I've completed are the chromatography lab and the online homework and the atomic mass online worksheet.
2. I am starting to understand relative atomic mass and the inter/intramolecular forces, and I'm getting back the hang of nomenclature. I think what I could work on is calculating atomic mass and figuring out atomic isotopes, and I could use a bit of practice on polyatomic ions.
3. What I am going to do to understand or remember what I don't get or forgot is to look back on my old notes from Chemistry and study my polyatomic ions. 

Chromatography Lab

This experiment is dealing with the separation of dyes using Chromatography. The multiple trials done with the dyes and the different solvents used conclude that this experiment follows the scientific method. The main solvent, the paper, is what the dye, or solute,  is attracted to. The other solvents (NaCl, Alcohol, and the Chromatography solution)  are what help the dye travel up the paper. If the dye is more attracted to the paper, it will stay either in the same place or barely move with the solvent up the paper. If the liquid solvents are more attractive to the dyes, the dye will travel with the solvent up the paper. Whether the dye moves up the paper depends on the polarity of the solvent. Also, since the dye is a homogeneous mixture, the dye will separate into its original forms depending on how polar the solvent is. The chemical composition is different in all solvents, making the dye move up the paper differently. All solvents have different molecular structures, therefore their attraction towards the dyes differentiate. With the NaCl solution, the dyes moved further up the paper and are separated into its separate colors. With the alcohol, the dyes moved together and didn't fade or spread as much as the NaCl solution. With the FDC solution, the dye didn't move at all. The FDC dyes were supposed to be the control of this experiment, however they did not work according to plan. The qualitative evidence is that the dyes were proven to be a mixture according to the chromatography paper.  The separate dyes used to make a new mixture was separated when in contact with certain solvents. 

Example:  

       The quantitative data is the distance of the component compared to the distance of the solvent line/mobile phase. The different dyes in the mixtures were obviously set apart when the solvent traveled up the paper.

Examples: 

Data for Rf

Vis-a-vis: NaCl

.8cm on the 10cm mark

original color - blue

 Data for Rf

Crazart: Alcohol

.8cm on the 3cm mark

                                                   

This is the particle diagram explaining dye travelling

The 3cm mark's dye has a strong attraction to the solvent because of the molecular structure and the polarity. The 2cm mark's dye is not as attracted to the solvent, and the 1cm mark's dye is not attracted to the solvent at all. This lab reinforced the idea of intramolecular and intermolecular forces, which one is chemical and which one is physical, and the idea of 'like dissolves like' due to the polarity and nonpolarity of a substance. It also established the difference between physical and chemical properties and changes by using a certain separation technique.