Chemistry: The PERIODIC TABLE of Elements.pptx

Periodic Table

1. The PERIODIC TABLE of Elements FC 103 Inorganic and Analytical Chemistry

2. PERIODIC TABLE

3. The periodic table is made up of rows of elements and columns. An element is identified by its chemical symbol. The number above the symbol is the atomic number. The number below the symbol is the rounded atomic weight of the element. A row is called a period . A column is called a group . Periodic Table of Elements

4. Chemists used the properties of elements to sort them into groups. Johann Wolfgang Döbereiner grouped elements into triads. A triad is a set of three elements with similar properties. * React with other elements (such as sodium) to make similar compounds Organizing the Elements

5. In 1869, a Russian chemist and teacher published a table of the elements. Mendeleev arranged the elements in the periodic table in order of increasing atomic mass. Mendeleev’s Periodic Table

6. In 1913, through Henry Moseley’s work with X-rays, he determined the actual nuclear charge (atomic number) of the elements. He rearranged the elements in order of increasing atomic number. Moseley’s Periodic Table

7. According to the Periodic Law, when elements are placed in ascending order of atomic number, their physical and chemical characteristics continue in a predictable and organized manner . This arrangement leads to a periodic repetition of their properties. The Periodic Law

8. The elements can be grouped into three broad classes based on their general properties: Metals, Nonmetals , and Metalloids Across a period, the properties of elements become less metallic and more nonmetallic. Metals, Nonmetals and Metalloids

9. good conductors of heat and electricity are shiny are ductile (can be stretched into thin wires) are malleable (can be pounded into thin sheets) a chemical property of metal is its reaction with water which results in corrosion Solid at room temperature except Hg (mercury) Properties of Metals

10. poor conductors of heat and electricity are not ductile or malleable solid non-metals are brittle and break easily are dull many non-metals are gases Properties of Non-Metals Sulfur

11. Metalloids (metal-like) have properties of both metals and non-metals. They are solids that can be shiny or dull. They conduct heat and electricity better than non-metals but not as well as metals. They are ductile and malleable. Properties of Metalloids

12. Groups vs Periods GROUPS PERIODS Columns of elements are called groups or families. Each horizontal row of elements is called a period. Elements in each group have similar but not identical properties. The elements in a period are not alike in properties. For example, lithium (Li), sodium (Na), potassium (K), and other members of group IA are all soft, white, shiny metals. The properties change greatly across even given row. All elements in a group have the same number of valence electrons (outer shell electrons that can form chemical bonds with other atoms). The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

13. * The hydrogen square sits atop group A1, but it is not a member of that group. Hydrogen is in a class of its own. H*

14. Alkali metals are located in group 1 on the left side of the Periodic table. Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb), Cesium (Cs) and Francium (Fr) Form a strong base (alkalis or alkaline solution) on reacting with water, are known as alkali metals. Group 1: Alkali metals group

15. Alkaline earth metals are found in the 2nd group of the Periodic table. Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba) and Radium (Ra) When these metals react with water, they form hydroxides which are alkaline in nature (or basis in nature). Group 2: Alkaline earth metals group

16. The elements lying from group 3 to 12 and two bottom rows on the periodic table are named as Transition metals and Inner transition metals. any of various chemical elements that have valence electrons—i.e., electrons that can participate in the formation of chemical bonds Group 3-12: Transition and Inner transition metals group

17. Boron element is in group 13 and period 2 of the Periodic table. Boron is the p-block element (have their outermost electrons in the p-orbital) and it is a metalloid. Boron (B), Aluminum (Al), Gallium (Ga), Indium (In), Thallium (Tl) and Nihonium (Nh) Group 13: Boron group

18. Carbon element is in group 14 and period 2 of the Periodic table. Carbon is the p-block element and it is classified as a nonmetal. Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), Lead (Pb) and Flerovium (Fl) Group 14: Carbon group

19. Nitrogen element is in group 15 and period 2 of the Periodic table. Nitrogen is the p-block element and it belongs to the category of Nonmetals. Nitrogen (N), Phosphorus (P), Arsenic (As), Antimony (Sb), Bismuth (Bi) and Moscovium (Mc) Group 15: Nitrogen group

20. Oxygen group is the group 16 on the periodic table. Oxygen (O), Sulfur (S), Selenium (Se), Tellurium ( Te ), Polonium (Po) and Livermorium ( Lv ) Group 16: Oxygen group

21. Halogens are located in the 17th group of Periodic table (exactly to the left of Noble gases). Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At) and Tennessine (Ts) Group 17: Halogen group

22. Noble gases are located in the right most group of the Periodic table at group 18 They are called noble gases because they normally do not react with any other elements. Helium (He), Neon (Ne), Argon ( Ar ), Krypton (Kr), Xenon (Xe), Radon (Rn) and Oganesson (Og) Group 18: Noble gases group Periodic table Groups Explained !! (With 1-18 Group Names)