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The Periodic Table and Periodic Trends Chapter 5 Standard #1: Atomic and Molecular Structure THE FAMILIES OF THE PERIODIC TABLE Alkaline Earth Metals Alkali Metals B Si Ge As Transition Metals Sb Inner Transition Metals Te Po Noble Gases Halogens Metalloids/ Semi-metals At The Blocks of the periodic table The valence electrons spin in a sphere sblock The valence electrons spin in a four lobe pattern d-block f-block Too complex The valence electrons spin a figure 8 pattern p-block RIDDLE: What does Sodium Oxide and Rihanna have in common? They both are called Oh Na Na Some Facts about the periodic table: II. III. FAMILY /GROUP PERIOD 18 vertical columns 7 Horizontal rows Can you do this?? Tom Lehrer the elements song pianist, musician and retired mathematician , UC Santa Cruz Take out a sheet of paper Characteristics of METALS 1. GOOD Conductors of heat and electricity 2. Solid at Room Temperture Except Mercury (Hg) 3.Malleable (to make into sheets) Pure Copper Metal 4. Ductile (to make into a wire) chemical properties of metals video Characteristics of Non-Metals 1.Poor Conductors of heat and electricity 2.Mostly Gases Iodine Chlorine 4. Texture Varies Carbon Bromine Sulfur Carbon chemical properties of non metals video The Metalloids or Semimetals have some characteristics of both 1. 2. 3. Can be shiny or dull. Some are malleable/ductile. Some conduct heat and electricity. Silicon Johann Dobereiner Try Ni 59 Pd X Pt 195 You can calculate the mass of the middle element by knowing the one above it an below it! John Newlands Law of OCTAVES He arranged the 62 known elements in order of increasing atomic weights Every 8th element repeats in pattern A.K.A The Father of Chemistry Gets credit for publishing the First Periodic Table Mendeleev’s Periodic table Henry Moseley Corrected periodic table by arranging it according to the atomic number. Video Organizing the Elements Mendeleevs Table clip Stop! Review of metals/Non-metals Video clips Review before the periodic trends Periodic Trends A.The Atomic Radius: The distance from the center of the nucleus to the valence electron. 1. Down a group Going down a group, the electron orbitals (shell) increase, causing the radius to get BIGGER! 2. Going Across the (period) There is a greater attraction which will cause the radius to get smaller. Ionic Radius:. The distance from center of nucleus to valence electron for the ion. 1. Cation: An atom that loses electrons (+) e- The cation is smaller than the original atom because it loses an electron and orbital. atomic radius: .152nm ionic radius (1+ ion): .060nm 1. Anion: An atom that gains electrons (-) F-1 anion - F atom e- - - - - - The anion will be larger than the atom because it will have greater electron repulsion anion cation atom atom C. Ionization Energy 1. The amount of energy needed to remove an electron (to make a cation) Going down a Family: Requires LESS Ionization Energy because valence electron is further away from the nucleus. 1. Going across a period: It takes MORE ionization energy because the electrons are held closer to the nucleus. Can Lithium lose more than 1 electron? . . . Li +1 (looks like He with 2 e-) 520.2 KJ/mol 7290.1 KJ/mol 11,815.0 KJ/mol Li+3 (11,815.0KJ/mol) Li+2 (7298.1KJ/mol) Li+1 (520KJ/mol) Electronegativity: Reflects the atoms ability to attract electrons A. Going down a family: NOT attracting electrons….too big and wants to get rid of electrons High electronegativity Low electronegativity B. Going across a period: Has a high attraction for electrons… .small and needing electrons Fluorine _____________is the most electronegative element Francium and _______________is the least