Periodic Table 1. The periodic table is a systematic arrangement of the elements by atomic number (protons) Similar properties fall into vertical columns.

Slides:



Advertisements
Similar presentations
The Periodic Table and Periodic Law
Advertisements

CHAPTER 6 NOTES: The Periodic Table
Chapter 6 Periodic Table and Periodic Law. The Periodic Table got its name because of the repeating pattern of chemical & physical properties. Mendeleev.
Chapter 6.
Periodic Table & Trends
The Periodic Table.
Intro To The Periodic Table
Chapter 12 The Periodic Table
Chapter 6 The Periodic Table and Periodic Law
Periodic Table Chapter 6.
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
Ch. 14: Chemical Periodicity Standard: Matter consists of atoms that have internal structures that dictate their chemical and physical behavior. Targets:
Periodic Trends.
The Periodic Table.
CHAPTER 6: Periodic Table
The Periodic Table and Periodic Trends
Chapter 13 Chemical Periodicity.
Periodicity Periodic Table Trends. Describing the Periodic Table periodic law: the properties of elements repeat every so often period: group (family):
Chapter 6 The Periodic Table and Periodic Law. The Periodic Table Periodic – means repeating pattern Remember: The Periodic Table is Your Friend!!
Video 4.1Video 4.1 Introduction and History of the Periodic Table.
Chapter 5 The Periodic Law
Organization of the Periodic Table
The Periodic Table History, Organization and Trends.
Chapter 4 Notes: The Periodic Table
Periodic Table.
Periodic Table Chapter 6. Periodic Table Many different versions of the Periodic Table exist All try to arrange the known elements into an organized table.
Chapter 5 The Periodic Table. Periodic Table Info.
The Periodic Table and Periodic Law Chapter 6. History of the Periodic Table’s Development Late 1790s: Lavoisier compiled a list of the 23 known elements.
The Periodic Table Chapter 6. A quest for accurate reproduction J.W. Dobereiner – published his triad classification system (ex. Cl,Br,I similar chemical.
Chapter 6: The Periodic Table and Periodic Law. Development of the Periodic Table 1790s –Antoine Lavoisier composed a list of the 23 known elements –Included.
Groups (families)  Vertical columns  Group # = # of valence electrons (# of electrons in outer shell)  18 groups or families  Some properties repeat.
Periodic Relationships Among the Elements Chapter 5 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
The Periodic Table. ( very ) Brief History 1869 Mendeleev* & Meyer published similar tables * First to be recognized at international convention – Elements.
Periodic Law History of the Periodic Table Periodic Trends.
Unit #4: Periodic Table Chapter 5. The Periodic Table Origin of the Table Origin of the Table 1. J.W. Dobereiner (early 1800’s) German a. observed that.
Periodic Table Notes Topic Two. Dmitri Mendeleev is credited as the first scientist to start organizing the known elements. He began this process by looking.
Ch. 14: Chemical Periodicity Standard: Matter consists of atoms that have internal structures that dictate their chemical and physical behavior. Targets:
Trends in the Periodic Table. Organization Mendeleev: atomic mass but some problems Moseley: atomic number Periodic Law: when elements are arranged with.
Periodic Table And the Periodic Law. Dmitri Mendeleev Russian chemist Created a table by arranging elements according to atomic masses Noticed that chemical.
Periodicity Unit Part 3. Periodic Law When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical.
The Periodic Table Chapter 5. Dmitri Mendeleev Dmitri Mendeleev developed the periodic table in 1869 Dmitri Mendeleev developed the periodic table in.
Chapter 6 The Periodic Table. J. W. Dobereiner In organized elements into “triads” (a group of 3 elements with similar properties)
Unit 6: The Periodic Table
Unit 4: The Periodic Table History and Trends Chapters 6 & 7 Test - October 31, 2008.
Periodic Properties Periodic Table with f-block included A.Electron Configurations.
PERIODIC TABLE. Essential Question: What were Mendeleev and Mosley contributions to the development of the periodic table? History: Dmitri Mendeleev (1869)
The Periodic Table trends. History of the Periodic Table 1871 – Mendeleev arranged the elements according to: 1. Increasing atomic mass 2. Elements w/
Formation of the Periodic Table Mendeleev: arranged the periodic table in order of increasing atomic MASS (didn’t know about protons) –Started new rows.
Glencoe Chapter 6 Bryce Wolzen.  Dmitri Mendeleev: ◦ Developed the first “modern” periodic table (1869) ◦ Arranged elements according to increasing.
Find the Missing Alien 1. Study the 17 pictures of aliens. 2. Organize the pictures based on patterns. 3. Identify and draw the missing alien.
The Periodic Table History Structure Trends. Part I: Attempts at Classification.
Periodic Table 1. History of the Periodic Table 3.
Periodic Table & Trends
Periodic Table & Trends
Periodic Table and Periodic Law
Unit 3: Periodic Table
Periodic Table.
Unit 3 Part 3: Periodic Trends
The periodic table.
Development of the Periodic Table
History Structure Trends
Periodic Properties.
PSC Chap. 4 The Periodic Table.
Periodic Table.
Chapter 6 The Periodic Table.
Periodic Table & Trends
The Periodic Table A few elements, including copper, silver, and gold, have been known for thousands of years There were only 13 elements identified by.
The Periodic Table & Periodic Law
Presentation transcript:

Periodic Table 1

The periodic table is a systematic arrangement of the elements by atomic number (protons) Similar properties fall into vertical columns 3

History of the Periodic Table Three men recognized patterns in the elements. They attempted to organize the elements according to these patterns.. 4

History of the Periodic Table Johann Wolfgang Döbereiner – Noticed patterns in atomic mass recurring in sets of three elements Became known as “Döbereiner's triads” 5

History of the Periodic Table John Newlands noticed every eighth element had similar properties. Known as 'law of octaves' : 6

History of the Periodic Table Dmitri Mendeleev developed the first periodic table Found the repeating pattern by atomic mass and arranged them so that groups of elements with similar properties fell into vertical columns in his table. Found a problem Some elements fell into the wrong column Examples: Te & I ; Co & Ni 7

Mendeleev’s Periodic Table 8

History of the Periodic Table Henry Moseley Fixed Mendeleev’s problem by rearranging the modern table by atomic number Used X-ray spectrometer to find the atomic numbers 9

Arrangement of Periodic Table Periodicity– trends of properties as you go across the table or down a column 10

horizontal rows there are 7 Period number tells which energy level holds the valence electrons Periods

Groups/Families vertical columns groups 1-18; elements in the same group share chemical properties Main group elements Groups 1,2 13, 14, 15, 16, 17, 18 12

Types of Elements Noble gases 13

Metals Found on the left side of table 1, 2 or 3 valence electronsHave 1, 2 or 3 valence electrons Lose electrons to form positive ions (cations) Most are silver, shiny, solid, malleable, ductile & good heat/electrical conductors

Nonmetals Found on the right side of table Have 5, 6, or 7 valence electrons Gain electrons to form negative ions (anions) Brittle, dull, non-conductors, and exist in all three states (solids, liquids, gases)

Metalloids Elements found along the stair-step between metals and nonmetals, NOT Al Properties are in between metals & nonmetals Silicon (Si) is probably the most well- known metalloid.

Noble Gases odorless, colorless, monatomic gases low chemical reactivity.

Color Groups of the Periodic Table Alkali Metals Alkaline Earth Metals Transition Metals Lanthanide Series Halogens Noble Gases Actinide Series Inner Transitional Metals Also called inert gases because they do not react Metalloids 18

Properties and Electron Configuration Look- each group (column) ends with the same electron configuration. That determines many of the physical properties that the group share. 19

Group 1 Based on the video Alkali Metals with WaterAlkali Metals with Water 1.What properties of Alkali metals are observed? 2.What trend is observed as samples are tested with water? 3.Why weren’t hydrogen and francium tested? 20

Group 17 1.What are some of the physical properties of the halogens? Halogen 21

Group 18 Note: In the video “Group 0” is an old name for Group Why are the noble gases un-reactive? 2.If all neon signs were made of pure neon gas, what colors would we have? 3.What are uses for noble gases other than in neon lights? 4.How can a physical property be used to tell the difference between noble gases? 5.Radon was not tested. Predict what a balloon filled with Radon would do when dropped from the roof and why. Noble Gases 22

Summary of Groups, Props. & Electrons NOVA Video 1.What is the relationship between electron configuration and group number on the periodic table? 2.Why are halogens and alkali metals highly reactive, but not the noble gases? NOVA Video 23

Periodic Table Trends Patterns on the periodic table – Atomic Radius – Ionic Radius – Electronegativity – Ionization Energy – Reactivity 24

Periodic Trends- similarities of elements based on where they are in the table Depend on two things: Effective Nuclear Charge- The attraction the valence electrons have for the protons in the nucleus. Electron Shielding Effect- Inner shell electrons blocking valence electrons from the nucleus. 25

Effective Nuclear Charge Watch this video And this Effective Nuclear Charge is abbreviated Zeff Smart folks have noticed that the zeff for each group is equal to the number of valence electrons. 26

Atomic Radius Atomic radius is half the distance between the centers of two atoms measured in angstroms. The more energy levels, the ________ the atomic radius. (larger/smaller) The higher the effective nuclear charge, the ________ the atomic radius. (larger/smaller) larger smaller 27

Atomic Radius Trend Atomic radius increases as you move down a group Atomic radius decreases as you move from left to right in a period Down the group the number of energy levels increase so the number of shielding electrons increase. The nucleus cannot pull in the valence electrons. That makes a bigger atom. Across the period the number of protons increases while the number of shielding electrons stays the same. This make the nucleus pull in the valence electrons. That makes a smaller atom. 28

Ions Cations Form from metals Lose electrons Metal have low effective nuclear charge holding on to the valence electrons. Anions Form from nonmetals Gain electrons Nonmetals have high effective nuclear attraction on the valence electrons 29

Ions Metals lose electrons to form cations Li Li + F F-F- Nonmetals gain electrons to form anions Ionic radius is smaller than atomic radius energy level is lost or “shed” Ionic radius is larger than atomic radius because the electrons outnumber the protons. The nucleus has less control of the valence electrons. 30

Electronegativity Electronegativity s a measure of how strongly atoms attract bonding electrons to themselves An assigned number “rates” the electronegativity (from 0.7 to 4.0) – Low electronegativity = cannot attract valence electrons – High electronegativity = can attract valence electrons

Electronegativity Trend Electronegativity values increase as you move from left to right in any period. Within any group, electronegativity values decrease as you go down. Biggest IE = Fluorine Smallest IE = Francium 32

Electronegativity- EN- the tendency of an atom to pull shared electrons to itself. High EN= Big pull F9pF9p Li 3p Be 4p B 5p C 6p N 7p O 8p Factors affecting Electronegativity -Size of the atom/distance- small size/distance the nucleus has a stronger attraction for electrons Why does the trend decrease down a group? 33

Ionization Energy Ionization Energy – the energy needed to remove the outermost electron in an atom. How hard is it to steal an electron Increases as you go right in a period Larger nuclear charge – more protons pulling on the electrons Atom is smaller – outer electrons are closer to the nucleus; easier to pull in electrons Decrease as you go down in a group More energy levels – Radius is larger; outer electrons are farther from the nucleus; more difficult to gain electrons 34

Ionization Energy Pattern 35

Ionization Energy Decreasing ionization energy Increasing ionization energy 36

Metal Reactivity Trend Metal Activity depends on the attraction the metal has for the nonmetals electrons. Trend Increases as you move down a group Decreases as you move from left to right in a period *The most reactive metal is francium decreasing metal reactivity increasing metal activity

Nonmetal Activity Trend Non-Metal Activity refers to how easily nonmetals gain e- to form anions Trend Decreases as you move down a group Increases as you move from left to right in a period *The most reactive nonmetal is fluorine increasing nonmetal activity decreasing nonmetal activity