The Element Symbol Group Period Block Atomic Number Atomic Mass

For the lesson observed the objectives was to explain the trends of the periodic table based on the elements’ valence electrons and atomic numbers. Additionally, students were responsible for applying their previous knowledge in calculating subatomic particles to review the Bohr Models and discus the relationship among families in the periodic table. Students will use the information from today’s lesson to make future judgments on reactivity and bonding created during chemical reactions in the next unit. Lastly, students were to connect the information on elemental properties to previous experiences with their health, commercial products, and everyday life.

Page 13 of The Disappearing Spoon ties into learning goal 22. Learning goal 22 ties into this page because the page discusses about how the periodic table is arranged by the different types of elements such as metals, metalloids, and nonmetals. On the western side and the middle part of the periodic table, you will find the metals which make up seventy five percent of the periodic table. On the eastern side, you will find the gases or

Relate your knowledge of the periodic trends to the chemical bonding exhibited by various elements.

Strontium is a chemical element with symbol Sr and atomic number (protons in nucleus) 38 and atomic weight 88.1 It is a soft, silver-gray metal, and has physical and chemical properties like to Calcium and Barium. It is available as four stable isotopes ubiquitously (Isotopes are differ in forms of an by number of protons in nucleus but possess a variable number of neutrons.) Strontium-88 is the most dominant among other forms, comprising 83% of natural strontium, where in additional three stable isotopes and their relative abundance are strontium-84 (0.6%), strontium-86 (9.9%), and strontium-87 (7.0%). Strontium is available ubiquitous vitally as as celestite (SrSO4) and strontianite (SrCO3), and it comprises about 0.025% of the earth’s crust. There are 16 major radioactive isotopes of strontium, but only strontium-90 has a half-life sufficiently long (29 years). In comparison with half-lives of remaining strontium radionuclides are fewer than 65 days. Strontium-90 decays to yttrium-90 by decaying a beta particle, and yttrium-90 decays by decaying a energetic beta particle with a half-life of 64 hours to zirconium-90. The key health concerns for strontium-90 are associated to the energetic beta particle from yttrium-90.2

In the Modern periodic table there are two disadvantages, the position of the Hydrogen atom and the position of the f-block elements. The Ato Circular Periodic Table easily provides the necessary aspects of the periodic table and allows them to understand the basic concepts of the periodic classification and the structure of atom.

Nonmetallic properties tend to predominate for elements at the far right portion of the table.

When metal atoms pack together in a specific and orderly fashion metals such as gold, silver, and copper are produced. Each metallic atom gave up its valence electron to form a common pool of electrons in the entire structure. The freedom of valence electrons to

By the year 1869, a collection of 63 elements had been revealed. As the number of known elements increased, scientists began to notice patterns in properties and formulate classification schemes. In 1862, a French geologist, A.E.Beguyer de Chancourtois, recorded a list of the elements on a cylinder regarding their individual atomic weights. He was the first to identify that elemental properties reoccur every seven elements.

Throughout history the periodic table of elements has been influenced and amended by multiple scientists. These scientists include Johann Dobereiner, A.E Beguyer de Chancourtois, John Newlands, and Glenn Seaborg. As well as Dmitri Ivanovich Mendeleev and Lothar Meyer the creators of the periodic table. There are many ways that the periodic table of elements was set out. For example the table can be organized using patterns between atomic numbers, electronegativity, ionization energy, structure (gas or solid) valence electrons and electron configuration (shells) as seen in the modern day periodic table.

Though there are over a hundred different elements, each one is unique in its complexity and properties. Helium has an atomic Number of two, that’s how you can tell it it has two positively charged atoms, or ‘protons’, in

Group 1- hydrogen: lightest element on the periodic table. lithium: lithium never occurs freely in nature. sodium:Sodium is the sixth most abundant element in the Earth's crust,. potassium:Potassium ions are necessary for the function of all living cells. rubidium: Rubidium has also been reported to ignite spontaneously in air. caesium:the element is only mildly toxic, it is a hazardous material as a metal and its radioisotopes present a high health risk if released into the environment. francium:Francium is the most unstable of the naturally occurring elements

Twenty-two is the atomic number of the chemical element titanium. Its value in roman numeral is XXII. Twenty-two is also the sum of the totient function for the first eight integers. Also twenty-two is the standard port number for the Secure Shell protocol for computing and technology. My number also is a pentagonal number and a centered heptagonal number. The number twenty-two in the game bingo is called or referred to as "Two Little Ducks". In American Football there are only 22 players on the field per game. Twenty-two is a master number. Lastly twenty-two can be reduced to the number 4.

One of the most impotent parts of this elements is the arrangement of the electrons. How the shells are arranged for copper.

The element I have chosen for our Atomic Structures And The Periodic Table Project is

In Fig 1 the reactivity of Non-Metals decreases every period and increases every group, the halogens lie on the end of the group of Non-metals causing them to be highly reactive. The alkali metals have a single electron in their outer electron shell, making it easy for them to become a noble gas and period down the periodic table the easier it is to get rid of the extra electron, causing the alkali metals to become more reactive the further down the periods. To become a noble gas a halogen must gain an electron, the farther away the outer shell is from the nucleus, the more energy that is required for an electron to enter the shell. Halogens need one more electron to become a noble gas, while alkali metals need to donate an electron to become a noble gas. (Johnsonburg High School, n.d.) Fig 1. This shows the trends of the reactivity of Metals and non-metals on the periodic table.