Periodic table

The periodic table is a very much needed tool in chemistry. It organizes the elements along with their properties. The table originally started with French scientist, Antoine Lavoisier. He had created a list of elements to keep organized and it basically grew from there. In today's periodic table there are 116 elements. Each element has its own box containing elements name, symbol, atomic number, and atomic mass. Boxes are arranged in order of increasing atomic number into columns called periods. There are three classifications for the elements, metals, metalloids, and non metals. Metals are shiny, solid at room temperature, and good conductors.  Non metals are usually gasses or brittle or dull looking solids. They aren't good conductors. Metalloids have both chemical and physical properties of both non metals and metals. All in all the periodic table is very useful in science.

Conductivity

Conductivity

A good conductor carries lose ions easily. For example metal is a good conductor.  Metal wires are used for electricity since they are good conductors.

To learn about conductivity we did a lab. In this lab we were to test a variety of elements. To do this we choose six diffrent substances: lactose hydrate, collsium cloride, sodium acctate, corn syrup, molloscc, and citric acid. Then we put a little of each substance into six diffrent cups and tested there conductiviy. To test the conductivity we had a conductive meter. The conductive meter determined the level of conductivity on how bright the light shown. (1-not really conductive, 2-kinda conductive, 3-conductive, 4-very conductive)

Results:

According to the results lactose hydrate, sodium acetate, and molosses are very conductive, meaning they all have lose ions which carry easily. 

In conclusion conductivity is a form of conducting electric current, heat or sound. 

Reaction lab

Reactions  lab
   In this lab we experienced 7 different types of reactions. We observed and discovered characteristics  of these different reactions and even wrote formulas for these reactions.

Reaction 1:
        What we used: hydrochloride acid, magnesium metal, test tubes, match
         What we did: we took a test tube and filled it up about half way with hydrochloride acid. Then we put in a piece of magnesium metal and covered it with anther test tube.  The magnesium started bubbling and it made the tube foggy.  Once the magnesium metal stopped bubbling, we lit a match and stuck it in the tube that was covering the acid. The reaction there seemed to make a mini explosion, it even made a noise that made some people jump.
          The formula: 2HCI + Mg---->MgCI2+ H2
                  (single replacement)

Reaction 2:
        What we used: Bunsen burner, magnesium, tongs,
        What we did: we lit the burner and then held a strip of magnesium over the burner till the reaction took place. The magnesium made a really bright white light.
         The formula: 2Mg + O2----> 2MgO
                     (single replacement)
Reaction 3:
         What we used:  copper wire, sand paper, tongs, Bunsen burner,
         What we did:  we took the copper wire and shined it up with sand paper. Then we held the wire over the burner for a couple of minutes. The reaction seen was that the wire started to glow.
           The formula: 2Cu(s)+ O2(g)----> 2Cu(s)
                    (double replacement)

Reaction 4:
         What we used: ammonium carbonate, test tubes,  burner
         What we did: we added a little ammonium carbonate into a test tube and then we heated the test tube. And then we waft the smell of the gas and it smelt like baking powder.
           The formula: (NH4)2+CO2----> Co2+ H2O +2NH3
                     (combustion)

Reaction 5:
        What we used: hydrogen peroxide, manganese dioxide, test tube, match
        What we did: we filled half way a test tube with hydrogen peroxide and then added a little bit of manganese dioxide. There seemed to be a separation, like two different layers. When we put in the glowing match the top layer seemed to explode into flames.
         The formula: 2H2O2MnO2-----> 2H2O+O2
                 (single replacement)

Reaction 6:
       What we used: potassium iodine, test tube, lead(II)nitrate
       What we did: we poured potassium in one test tube and lead(II)nitrate into two different tubes. They were two different colors. Then we mixed them together and the solution got turned yellow.
        The formula: 2KI+Pb(NO3)2---> 2KINO3+ PbI2
               (double replacement)

Reaction 7:
       What we used: copper(II) carbonate, test tube, test tube holder, match
        What we did: we poured a little copper(II) carbonate into a test tube and then we heated it up while cover it with anther test tube. After that we lit a match and put it in the test tube and the smoke formed out.
      The formula: CuCo3--->CuO+CO2
             (decomposition)

In this lab we seen many reactions and learned how mixing or adding heat will cause a reactions.