Starter S-44 A. What is Lithium’s electron configuration? What column of the periodic table is it in? What is Sodium’s electron configuration?

Chapter 5 The Periodic Table

6.1 Organization of the Elements Chapter 6 6.1 Organization of the Elements

6.1 Organization of the Elements In ancient times the known elements were Gold, Silver, Copper, Iron, Lead, Tin, Mercury, Sulfur, Carbon Up until the 1700’s only 4 more had been discovered Arsenic, Antimony, Phosphorus, Zinc

6.1 Organization of the Elements 1829 JW Dobereiner – puts elements in triads Sets of 3 elements with similar chemical properties (Daniel is a Weenie)

6.1 Organization of the Elements 1864 John Newland – Law of Octets When elements are placed in order of atomic mass, properties seem to repeat every 8 elements

6.1 Organization of the Elements 1869 – Dimitri Mendeleev – arranged by increasing atomic mass and properties The table is periodic – properties repeat

6.1 Organization of the Elements 1913 – Henry Mosley – used atomic number instead of atomic mass

6.1 Organization of the Elements The Periodic Law – when elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

6.1 Organization of the Elements Period – row 7 rows

6.1 Organization of the Elements Group – column 18 groups (some have names) Noble Gases Alkali Metals Alkaline Earth Metals Transition Metals Halogens

6.1 Organization of the Elements Draw the zig-zag line on your periodic table and label the metals and nonmetals

6.1 Organization of the Elements Metals Good conductors, lusterous, ductile, malleable

6.1 Organization of the Elements Nonmetals Poor conductors, dull, brittle

6.1 Organization of the Elements Metalloids Sometimes behaves like a metal, sometimes like a nonmetal

6.2 Classifying the Elements Chapter 6 6.2 Classifying the Elements

6.2 Classifying the Elements Information on the periodic table Electron configuration is determined by the elements position on the periodic table s1 p6 s2 p1 p2 p3 p4 p5 d1 d2 d3 d4 d5 d6 d7 d8 d9 d10 f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

6.2 Classifying the Elements Remember 1st s is level one, 1st p is second, 1st d third 1st f fourth s1 p6 s2 p1 p2 p3 p4 p5 d1 d2 d3 d4 d5 d6 d7 d8 d9 d10 f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

6.2 Classifying the Elements Noble Gas Configuration Find the noble gas before the element Put that element in brackets [ ] Fill out the rest of the configuration using the pattern in the periodic table s1 p6 s2 p1 p2 p3 p4 p5 d1 d2 d3 d4 d5 d6 d7 d8 d9 d10 f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

6.2 Classifying the Elements For example Strontium (Sr) [Kr]5s2 s1 p6 s2 p1 p2 p3 p4 p5 d1 d2 d3 d4 d5 d6 d7 d8 d9 d10 Sr f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

6.2 Classifying the Elements Germanium (Ge) [Ar]3d104s24p2 s1 p6 s2 p1 p2 p3 p4 p5 d1 d2 d3 d4 d5 d6 d7 d8 d9 d10 Ge f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

Starter S-45 What are the names of the elements in Group 1 Group 2

Chapter 6 6.3 Periodic Trends

6.3 Periodic Trends Atomic Size – The size of an atom of a particular atom Increases down a group Decreases across a period Video

6.3 Periodic Trends Not always an exact pattern

6.3 Periodic Trends Ions – charged atoms Lost (+) or gained (-) electrons Cation – lost electrons Anion – gained electrons Ion Formation Table of ionic radii

Ionization energy video 6.3 Periodic Trends Ionization Energy The energy required to remove an electron from an atom 1st ionization energy – energy to remove the first electron Decrease down a group Increase across a period Ionization energy video

6.3 Periodic Trends 6.3 Periodic Trends Electronegativity Ability of an atom to attract electrons when the atom is in a compound Increases across periodic table Decreases down periodic table

6.3 Periodic Trends 6.3 Periodic Trends 5. Density

6.3 Periodic Trends 6.3 Periodic Trends 5. Melting Point

6.3 Periodic Trends 6.3 Periodic Trends Main reasons for patterns Increasing nuclear charge down a group and across a period more protons, larger positive charge Increased shielding down a group as energy levels increase, those electrons further out, are shielded by the inner ones