BC: F Orbital: Actinide and Lanthanide | Cerium, Samarium, Uranium, Thorium, Euporium | Lewis Dot Diagram | Bohr Model | 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f2 | 5 uses Cerium:permanent magnets Samarium:used for carbon-arc lighting for the motion picture industry Uranium: X-ray production Thorium:atomic-fuel source | Number of Protons/Electrons: 90 Number of Neutrons: 142 | 5 chemical and physical properities: Actinides are typical metals. Actinide Elements are soft and have a silvery color (but tarnish in air). Actinide elements are highly reactive with halogens and chalcogens. Lanthanides metals have a high luster, but tarnish readily in air. Lathanides have high electrical conductivity.
FC: My Family Album (periodic Table) Family comes first
1: Table Of Contents | 1. Family History 2. History Continued 3.Trends of the periodic Table 4.How to read The periodic table 5.The S orbital 6.The D orbital 7. P orbital 8. F orbital
2: Family history | Uncle Dimitri Mendeleev Uncle Dimitri devised a chart, which organized all of the elements into a grid of horizontal rows called periods and vertical columns called groups or families. | Uncle Antoine-Laurent de Lavoisier Uncle Antoine a textbook called Traité Élémentaire de Chimie which contained a list of elements, or substances that could not be broken down further, which included oxygen, nitrogen, hydrogen, phosphorus, mercury, zinc, and sulfur | Uncle Henery found a relationship between an element's X-ray wavelength and its atomic number (Z), and therefore resequenced the table by nuclear charge rather than atomic weight
3: Hisory continued | Uncle Glenn T. Seaborg Uncle Seaborg's actinide concept of heavy element electronic structure, predicting that the actinides form a transition series analogous to the rare earth series of lanthanide elements, is now well accepted in the scientific community and included in all standard configurations of the periodic table. | Uncle Alexandre-Emile Béguyer de Chancourtois was the first person to notice the periodicity of the elements — similar elements seem to occur at regular intervals when they are ordered by their atomic weights. | Uncle John Newlands Proposed an orginizational scheme for the elements
4: Trends Of the periodic table | Ionization physical process of converting an atom or molecule into an ion by adding or removing charged particles such as electrons or other ions | Atomic Radius a measure of the size of its atoms. A term used to describe a size of an atom | Electronegativity a measure of the tendency of an atom to attract a bonding pair of electrons.
5: Understanding the periodic table | The periodic table is organized by selected properties of their atomic structures. Elements are going by increasing atomic number, the number of protons in an atom's atomic nucleus. | Its also organized by vertical columns and horizontal rows. The vertical columns of the periodic table (there are 18) are called groups or families. Elements in the same group or family have similar but not identical characteristics.
6: Getting to Know your Family
7: S-Orbital ( Alkaline Metals and Alkaline Earth metals) | Hydrogen, Lithium, Beryllium, Sodium, Magnesium, and Calcium | The orbital Notation of hydrogen is 1s1 which means that one orbital will be filled with one arrow. | 5 uses Lithium: Batteries Sodium: Dietary Salt Beryllium: Space telescopes Magnesium:Chlorophyll Calcium:Fireworks | 5 Chemical and Physical properties: Alkaline Metals: have a silvery, metallic appearance. Soft enough to cut with a knife. Have low Melting Points. chemical reactivity of alkali metals increase as we move from the top to the bottom of the group. Ionization potential of the alkali metals is very low | 5 Chemical and Physical Properties: Alkaline Earth Metals: Silvery-white, metallic appearance. Harder and denser than many of the group one elements. Have higher Melting points and boiling points than alkali metals . Densities increase. They have low ionization energies | Number of Protons/Electrons: 1 Number of Neutrons: 0
8: D orbital: Transition Metals | Titanium,Iron,Chromium, Nickel, Copper | 5 Physical and Chemical properties: Generally good conductors of electricity and heat. They are ductile (they can be pulled into wires). They are Malleable (can be hammered into thin sheets). They can form compounds with variable oxidation states. They form coloured compounds. | Lewis Dot diagram | Bohr Model Of Chromium | 5 Uses Titanium- Building buildings Iron-The Earth's core which is made out of a solid iron sphere. Chromium-Paint pigments Nickel- magnets and rechargeable batteries. Copper-Used to pipe water supplies | 1s2 2s2 2p6 3s2 3p6 3d5 4s1 | Number of Protons/Electrons: 24 Number of Neutrons: 28
9: P orbital: Boron, Carbon, Nitrogen,Oxygen, halogens | 5 chemical and physical properties Of P orbital: Boron: A metalloid and have higher melting points then alkaline earth metals. Carbon: A Non-metal and Increases in metallic character going down the group. Nitrogen: Is a colorless and odorless gas, Boiling points and densities generally increase going down the group. Oxygen: It is a odorless gas at room temperature, and boiling points increase with increasing atomic number. Halogens: Fluorine and chlorine are gaeses at room temperature, Bromine is one of only the two elements that are liquid at room temperature | Boron, Silicon, Phosphorus, Oxygen, Fluorine | 5 Uses Boron: Detergent Carbon: Graphite Golf Shafts Nitrogen: Fixing Bacteria Oxygen: used in making methanol and ethene oxide | Bohr Model for Boron | Lewis Dot Diagram | Number of Protons/Electrons: 5 Number of Neutrons: 6 | 1s2 2s2 2p1