Period 3 element

Experiment 2: The Alkaline Earths and the Halogens: Two Families in the Periodic Table Lab Report By: YOU Introduction: The purpose of this lab was to find the relative solubilities of some salts of the Alkaline Earths and use that information to find the order which they appear in the periodic table; also use that information to efficiently find an unknown alkaline earth halide. Also to find the relative oxidizing powers of the Halogens given and using that information finding the order of

The 2nd half for the gel is our experiment compared to Anderson group 6. The 1st layer in all 3 pictures is the bound dye, the 2nd layer is the free dye. Fig1 shows on the right group one next to it, 1st half of our result on electrophroresis gel. The 2nd half for the gel is our experiment compared to Anderson group 6. The 1st layer in all 3 pictures is the bound dye, the 2nd layer is the free dye. Group 1, the gel picture and Andersons experiment are closely

For the progress monitoring assignment, I first reviewed the students’ assessments data provide for the assignment, and using the provided decision tree guide I determined the students’ levels based on the FSP (RC, Maze, and WA) scores. Once I had determined their level or “box results” I filled the decision tree form in by order of the box results column. I chose to order the results by that column to help make choosing student groups easier. Once all the students’ data was filled in the next step

[pic] LITT11234G - Graphic Novels: the invisible art Wired Comics: a Comic Casebook, or a Collaborative Comic This assessment opportunity is worth 20% of your final grade Collaborative Comic For this assignment, you are also welcome to create a short comic of your own. You may do this in a small group. Your comic should be in either black and white or in colour. Please consider the following for your group submission: ✓ Your work is a minimum of two A4 pages (at the very

Task 1a ELEMENT SYMBOL GROUP PERIOD BLOCK ATOMIC NUMBER ATOMIC MASS Sodium Na 1 3 S 11 23 Potassium K 1 4 S 19 39 Calcium Ca 2 4 S 20 40 Magnesium Mg 2 3 S 12 24 Carbon C 4 2 P 6 12 Oxygen O 6 2 P 8 16 Nitrogen N 5 2 P 7 14 Fluorine F 7 2 P 9 19 Chlorine Cl 7 3 P 17 35 Iron Fe Transition block 4 D 26 56 Hydrogen H Sits on top of group 1 1 S 1 1 Sodium S 6 3 P 16 32 The periodic table is a table that categorises and displays all of the chemical elements. It is made up of groups, periods and blocks

The elements are positioned on the periodic table based on their atomic number. Atomic number, or the number of protons in the nucleus, is what distinguishes each element on the chart. In the original design of the periodic table, elements were organized based on their atomic mass, however it was later discovered that placing the elements based on atomic number made more sense, as it created a pattern and allowed it to be known what elements are yet to be discovered. Generally, however, the atomic

forth. This is where the name ionization energy comes from. (Claim) Element #1, Li has a higher ionization energy than element #2, K. Element #1, Li has a higher first, second, and third ionization energy than element #2, K.

the known elements in an informative array. Just like when entering a grocery store similar items are grouped together which makes an item easier to find. Elements are arranged left to right and top to bottom in order of increasing atomic number. The different rows of elements are called periods. The period number of an element signifies the highest energy level an electron in that element occupies. An element is a substance that is made

Period 3 oxides: Examples of period 3 oxides: Na2O, MgO, Al2O3, SiO2, P4O10 The examples of the oxides shown above are the “highest oxides”. These oxides have the highest oxidation state. The melting point and boiling point for period 3 oxides is usually very high. This is because a large amount of energy is needed to break the covalent and ionic bonds in the period 3 oxides. Metallic oxides which are Magnesium, Sodium and Aluminium contain metallic and oxides ions. These therefore have a strong

of the nineteenth century. By 1860, more than 60 elements had been discovered. Chemists had to learn the properties of these elements as well as those of the many compounds that they formed a difficult task. And to make matters worse, there was no method for accurately determining an element’s atomic mass or the number of atoms of an element in a particular chemical compound. Different chemists used different atomic masses for the same elements, resulting in different compositions being proposed