The Periodic Table and Periodic Trends Chapter 5 Standard #1: Atomic and Molecular Structure

Halogens Alkali Metals Alkaline Earth Metals Transition Metals Inner Transition Metals Noble Gases B Si GeAs SbTe At Metalloids/ Semi-metals THE FAMILIES OF THE PERIODIC TABLE Po

The Blocks of the periodic table s- block d-block p-block f-block The valence electrons spin in a sphere The valence electrons spin a figure 8 pattern The valence electrons spin in a four lobe pattern Too complex

RIDDLE: What does Sodium Oxide and Rihanna have in common? They both are called Oh Na Na

Some Facts about the periodic table: 18 vertical columns 7 Horizontal rows II.FAMILY /GROUP III.PERIOD

Can you do this?? Tom Lehrer the elements song pianist, musician and retired mathematician, UC Santa Cruz

Characteristics of METALS 1. GOOD Conductors of heat and electricity 2. Solid at Room Temperture 3.Malleable (to make into sheets) 4.Ductile (to make into a wire) Pure Copper Metal Except Mercury (Hg) Take out a sheet of paper

chemical properties of metals video

Characteristics of Non-Metals 1.Poor Conductors of heat and electricity 2.Mostly Gases 4. Texture Varies Chlorine Carbon Sulfur Bromine Iodine Carbon

chemical properties of non metals video

The Metalloids or Semimetals have some characteristics of both 1.Can be shiny or dull. 2.Some are malleable/ductile. 3.Some conduct heat and electricity. Silicon

Johann Dobereiner You can calculate the mass of the middle element by knowing the one above it an below it! Try Ni 59 Pd X Pt 195

John Newlands Law of OCTAVES Every 8 th element repeats in pattern He arranged the 62 known elements in order of increasing atomic weights

Dimitri Mendeleev 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 clipOrganizing the Elements Mendeleevs Table 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:. atomic radius:.152nmionic radius (1+ ion):.060nm e- 1.Cation: The distance from center of nucleus to valence electron for the ion. An atom that loses electrons (+) The cation is smaller than the original atom because it loses an electron and orbital.

F -1 anion 1.Anion: An atom that gains electrons (-) e The anion will be larger than the atom because it will have greater electron repulsion F atom

atom cation atom anion

C.Ionization Energy The amount of energy needed to remove an electron (to make a cation) 1.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? KJ/mol KJ/mol... 11,815.0 KJ/mol Li +1 (looks like He with 2 e-)

Li +1 (520KJ/mol) Li +2 ( KJ/mol) Li +3 (11,815.0KJ/mol)

Electronegativity : A.Going down a family: B.Going across a period: Reflects the atoms ability to attract electrons NOT attracting electrons….too big and wants to get rid of electrons Has a high attraction for electrons….small and needing electrons High electronegativity Low electronegativity

_____________is the most electronegative element and _______________is the least Fluorine Francium