Periodic Table The how and why. History u 1829 German J. W. Dobereiner Grouped elements into triads Three elements with similar properties Properties.

Slides:



Advertisements
Similar presentations
Development of the Periodic Table
Advertisements

The Periodic Table and Periodic Law
The History and Arrangement of the Periodic Table
The Periodic Table Chemistry.
Periodic Table of the Elements. u These are called the inner transition elements and they belong here.
Lecture No.7 The Periodic Table and Some Properties of The Elements
U5: The History and Arrangement of the Periodic Table
The History and Arrangement of the Periodic Table
The Modern Periodic Table
Periodic Table Families
Chapter 3 The Periodic Table
Periodic Table of the Elements
Chemistry Chapter 6/7 Notes #1 Periodic Table LaVigne.
Chapter 6 - The Periodic Table and Periodic Law
The Periodic Table. Early Organization As early as the early Greeks, scientists wanted to organize. As early as the early Greeks, scientists wanted to.
PSC Chap. 4 The Periodic Table. In modern periodic table, elements in the same column have similar properties.
Unit 6 – The Periodic Table
Periodic Table.
Introduction to the Periodic Table. Dmitri Mendeleev The elements were first arranged in the periodic table in 1869 by Dmitri Mendeleev. By arranging.
Unit 3 Periodic Table James Hutchison ROHS. Development of the Periodic Table – By the mid-1800s, about 70 elements were known – Dmitri Mendeleev ordered.
PERIODIC TABLE ORGANIZATION How is the periodic table organized? What are the properties of each group?
Unit 5 The Periodic Table The how and why. Newlands u Arranged known elements according to properties & order of increasing atomic mass u Law of.
Periodic Table. History Antoine Lavoisier – Father of Modern Chemistry 1829 German J. W. Dobereiner Grouped elements into triads – Three elements with.
End Show Slide 1 of 28 Classifying the Elements 6.2.
Chapter 3 The Periodic Table The how and why. History u Dmitri Mendeleev - Russian scientist taught chemistry in terms of properties. u Mid 1800’s - molar.
The Periodic Table History, Organization and Trends.
Groups of the Periodic Table Ms. Beckham. Patterns in Element Properties (History) Elements vary widely in their properties, but in an orderly way. In.
The Periodic Table
Chapter 6 Periodic Table World of Chemistry Harry potterHarry potter sings the element song.
Chapter 5 (cont.) The Periodic Table. History of the Periodic Table Mendeleev (1860’s) –Developed the first periodic table –It was arranged by atomic.
Chem 11. History Russian scientist Dmitri Mendeleev taught chemistry in terms of properties. Mid molar masses of elements were known. Wrote down.
The Periodic Table The how and why….  Early in the 19th century, scientists began to seek ways of classifying elements.
Ch. 6 Notes-Pre AP Chemistry Periodic Table and Periodic Law John Newlands – when elements arranged by increasing mass, properties repeated every 8 th.
The Periodic Table chapter 6.
The Periodic Table An Introduction.
Chapter 6 The Periodic Table. J. W. Dobereiner In organized elements into “triads” (a group of 3 elements with similar properties)
The Modern Periodic Table Early Periodic Table – Atomic Number In 1913 Henry Mosley discovered that each element contained a unique number of protons.
. + ic. History u Russian scientist Dmitri Mendeleev taught chemistry in terms of properties. u Mid molar masses of elements were known. u Wrote.
The Periodic Table Chemistry 11. The Periodic Table’s History: We didn’t always have the periodic table! We didn’t always have the periodic table! by.
Tuesday, Oct 10  You have a CBA tomorrow!  Follow the power point to fill in your chart  Tape it on p. 30 when you are done  Work on your CBA review.
Periodic Table. Periodic Table - 1 A periodic table is an arrangement of elements in which the elements are separated into groups according to their properties.
The Periodic Table and Periodic Law Chapter 6. Section 6.1: Development of the Modern Periodic Table Late 1790’s- Lavoisier compiled a list of 23 elements.
Chapter 6 The Periodic Table.
THE PERIODIC TABLE.
Unit 3 Part 2 Chapter 5 Explain the trends of the periodic table based on the elements’ valence electrons and atomic numbers. (PS-2.3)
The Periodic Table SCH3U1.
The Periodic Table.
The History and Arrangement of the Periodic Table
Most Important tool in chemistry.
The Periodic Table: Metals, Nonmetals, and Metalloids
Periodic Table.
The Periodic Table and trends
Chapter 6 The Periodic Table
The Periodic Table Cl 35.5 Br 79.9 I History of the Periodic Table J.W. Dobereiner – elemental triads Elements in a triad have similar properties.
SCH3U Unit 1: Matter, Chemical Trends and Chemical Bonding
Development of the Periodic Table
Unit 2 lecture 2- Periodic Table Intro
The Periodic Table.
The Periodic Table Chemistry 11.
PSC Chap. 4 The Periodic Table.
Unit 2 lecture 2- Periodic Table Intro
Organizing the Elements
Periodic Table Families & Identifying
Periodic Table Families & Identifying
The Periodic Table.
Periodic Table Look for blue circles: these will tell you how to color periodic table!!
History of the Modern Periodic Table
Periodic Table The how and why.
Presentation transcript:

Periodic Table The how and why

History u 1829 German J. W. Dobereiner Grouped elements into triads Three elements with similar properties Properties followed a pattern The same element was in the middle of all trends Example: Ca, Ba, Sr u Not all elements had triads

u 1863 – John Newlands suggested another classification. u Put elements in order of increasing atomic masses. u Found repetition of similar properties every 8 th element. u He arranged the elements (known at that time) into 7 groups of 7. u Law of Octaves

u Russian scientist Dmitri Mendeleev taught chemistry in terms of properties u Wrote down the elements in order of increasing mass u Found a pattern of repeating properties u Difference – thought that similar properties occurred over periods (rows) of varying length.

Mendeleev’s Table u Grouped elements in columns by similar properties in order of increasing atomic mass u Found some inconsistencies - felt that the properties were more important than the mass, so switched order. u Found some gaps u Must be undiscovered elements u Predicted their properties before they were found

Predicted Properties - EkasiliconActual Properties - Germanium Atomic mass Melting Point high958 Density 5.5 g/cm g/cm 3 Dark gray metalGray metal Will obtain from K 2 EsF 6 K 2 GeF 6 Slightly dissolved by HClNot dissolved by HCl Will form EsO 2 Does form oxide (GeO 2 ) Density of EsO g/cm 3 Density of GeO 2 = 4.70 g/cm 3

The Modern Table u Elements are still grouped by properties u Similar properties are in the same column u Late 1800’s added a column of elements Mendeleev didn’t know about. u Henry Moseley recognized increasing nuclear charge was a better order for arranging elements

u Horizontal rows are called periods u There are 7 periods

u Vertical columns are called groups. u Elements are placed in columns by similar properties. u Also called families

1A 2A3A4A5A6A 7A 8A 0 u The elements in the A groups are called the representative elements

1A2A 3A4A5A6A7A 8A 3B4B5B6B7B8B 1B2B IAIIA IIIBIVB VB VIBVIIB VIIIB IIIAIVAVA VIAVIIA VIIIAIBIIB Other Systems

Metals

l Luster – shiny. l Ductile – drawn into wires. l Malleable – hammered into sheets. l Conductors of heat and electricity.

Transition metals l The Group B elements

Non-metals l Dull l Brittle l Nonconductors - insulators

Metalloids or Semimetals l Properties of both l Semiconductors

u These are called the inner transition elements and they belong here

u Group 1A are the alkali metals u Group 2A are the alkaline earth metals

u Group 6A is called the chalcogens u Group 7A is called the Halogens u Group 8A are the noble gases

u Alkali metals (group 1): Extremely reactive, soft metals with low density that form ions with a +1 charge. u Alkaline earth metals (group 2): Slighly less reactive than alkali metals, they are somewhat denser and less soft. They form ions with a +2 charge.

u Halogens (group 17): Highly reactive and electronegative nonmetallic elements that form ions with a -1 charge. They are diatomic, volatile, and very difficult to handle safely. u Noble gases (group 18): Very stable nonmetallic gases that react poorly with other elements.

u Transition metals (groups 3-12): Dense, hard metallic elements that usually form ions with more than one possible positive charge. u Lanthanides and actinides (the two rows at the bottom of the periodic table): The lanthanides are the top row and are reactive, dense metals. The actinides are the bottom row and include mainly radioactive elements that are produced artificially.

u Main group elements: These elements consist of groups 1, 2, and