Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1.

Slides:



Advertisements
Similar presentations
Periodic Table Larry Scheffler Lincoln High School.
Advertisements

4th period d-block elements 4th Period. d-block elements  center block of periodic table transition elements d-sub level partially filled in one or more.
Created by C. Ippolito Nov The Periodic Table The Periodic Table Objectives: 1. describe the origin of the periodic table 2. state the periodic.
The Periodic Table and Trends SONG Please have a periodic table out.
Periodic Table Larry Scheffler Lincoln High School.
Periodic Properties of the Elements
Periodic Table Larry Scheffler Lincoln High School IB Chemistry
Chapter 6.
Organizing the Elements
Intro To The Periodic Table
Chapter 6 The Periodic Table and Periodic Law
Chapter 4 The Periodic Table.
INTRODUCTION OF D-BLOCK ELEMENTS. Why are they called d-block elements? Their last electron enters the d-orbital.
Midterm Review Chapter 4 Periodic Table. Dmitri Mendeleev Father of the periodic table.
Mullis1 The Periodic Table  Elements are arranged in a way that shows a repeating, or periodic, pattern.  Dmitri Mendeleev created the first periodic.
 is an arrangement of the elements according to their properties.  It enables chemists to classify the elements so that it is possible to identify patterns.
Electron Configuration and Periodicity
The Periodic Table.
The Periodic Table 1. Number the groups and periods on your table.
The Periodic Table and Periodic Trends
PERIODICITY (TOPICS 3 AND 13) IB Chemistry HL2. Review: Periodic table, Physical and Chemical Properties of elements (Topic 3) Describe the arrangement.
Chapter 5 Periodic Law Chapter 4 Periodicity.
Click a hyperlink or folder tab to view the corresponding slides.
 Russian chemist Dmitri Mendeleev placed the known elements in order of increasing atomic mass.  When he did this he noticed that the elements’ properties.
CHEMISTRY Matter and Change
Chapter 13 Chemical Periodicity.
(Honors) Intro to the Table (Honors) Intro to the Table Dan Radcliffe.
The Periodic Properties of the Elements By Lauren Querido, Chris Via, Maggie Dang, Jae Lee.
The Periodic Table Dobereiner Organized elements into groups of three with similar properties called triads.
Periodic Table of Elements. Bohr Model: and Valence electrons Bohr Model: and Valence electrons
The 19 th Century……The Good Life? Typical chemist’s responsibilities during the middle of the 19 th century: Learn the properties of more than 60 elements.
Organization of the Periodic Table
Topic 13 Periodicity HL.
Periodic Table.1. The Periodic Table-Key Questions What is the periodic table ? What information does the table provide ? ? How can one use the periodic.
Chapter 11 The Periodic Table. I. History of the Periodic Table Johann Wolfgang Döbereiner and triads John Newlands and the Law of Octaves Dmitri Mendeleev.
Periodic Table.
Chapter 6: The 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.
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 and Physical Properties SONG Topics and Get a periodic table out.
Periodic Relationships Among the Elements Chapter 5 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
© 2014 Pearson Education, Inc. Sherril Soman Grand Valley State University Lecture Presentation Chapter 8-3 Periodic Properties of the Element.
 Law of Octaves  John Newlands(1865)  noticed repeating pattern of properties every eight elements ▪reminded him of musical scale.
Originally constructed to represent the patterns observed in the chemical properties of the elements. First chemist to recognize patterns was Johann Dobereiner.
Periodic Law History of the Periodic Table Periodic Trends.
Periodicity Chapter 5 Element song (Tom Lehrer), with Daniel Radcliffe:
The Periodic Table and Periodic Law Chapter 6 1. History of the Periodic Table’s Development In the 1700s, Lavoisier compiled a list of all the known.
The Periodic Table J.W. Dobereiner J.W. Dobereiner The elements in the triad has similar chemical properties. The elements in the triad has similar chemical.
Chapter 5 : The Periodic Table. Objectives Be able to define and explain each periodic trend, including comparing two different elements. For example:
Ch. 14: Chemical Periodicity Standard: Matter consists of atoms that have internal structures that dictate their chemical and physical behavior. Targets:
CHAPTER 5 Electrons in Atoms. Development of Atomic Models Dalton – Remember atomic theory? – Atom considered indivisible Thomson – “plum pudding atom”
Mullis1 The Periodic Table  Elements are arranged in a way that shows a repeating, or periodic, pattern.  Dmitri Mendeleev created the first periodic.
TEKS 5 – The student understands the historical development of the Periodic Table and can apply its predictive power. (5 A-C) STAAR Chemistry Review Topic:
The Periodic Table I.History II.Arrangement of Elements III.Electron Configuration Trends IV.Periodic Trends V.Reactivity.
Topic 13 - Periodicity. Ionic properties High melting and boiling point Conduct electricity in molten and aqueous states Crystalline solids Soluble.
Dmitri Mendeleev (1834 – 1907) listed elements in vertical columns in order of increasing atomic mass noticed recurrence of their physical and chemical.
The order of filling sublevels as seen on the periodic table. LanthanoidsActinoids.
The Periodic Table History Structure Trends. Part I: Attempts at Classification.
Periodic Table Unit 4.  Discovery of Modern Elements –Antoine Lavoisier suggested that burning was actually a chemical combination with oxygen. –Lavoisier.
What is a trend? What do the terms group and period mean? What are synonyms for those terms? Who is considered the greatest contributor to the current.
Chapter 6 The Periodic Table Periodic table Elements are arranged based on similarities in their properties Dmitri Mendeleev is credited with our current.
Transition elements Introduction
Click a hyperlink or folder tab to view the corresponding slides.
Ch. 14: Chemical Periodicity
Chapter 6 The Periodic Table & Periodic Law
Click a hyperlink or folder tab to view the corresponding slides.
History Structure Trends
Topic 3 - Periodicity 3.1 – Periodic Table .1.
Transition elements Introduction
Click a hyperlink or folder tab to view the corresponding slides.
Presentation transcript:

Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1

The development of the periodic table brought a system of order to what was otherwise an collection of thousands of pieces of information. The periodic table is a milestone in the development of modern chemistry. It not only brought order to the elements but it also enabled scientists to predict the existence of elements that had not yet been discovered..2

 Dobreiner’s Triads (1827) Classified elements in sets of three having similar properties. Found that the properties of the middle element were approximately an average of the other two elements in the triad..3

 John Newland attempt to classify 62 known elements  He observed that when ordered by Atomic Mass, there was a an observable repetition every eighth element  Tried to correlate the trends with musical scales, was ridiculed, and eventually awarded for his findings..4

Dmitri Mendeleev is credited with creating the modern periodic table of the elements. He gets the credit because he not only arranged the atoms, but he also made predictions based on his arrangements His predictions were later shown to be quite accurate..5

 Mendeleev organized all of the elements into one comprehensive table.  Elements were arranged in order of increasing mass.  Elements with similar properties were placed in the same row..6

Mendeleev left some blank spaces in his periodic table. At the time the elements gallium and germanium were not known. He predicted their discovery and estimated their properties..7

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaSeTiVCrMnFeCoNiCuZnGaGeAsSeBrKr RbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXe CsBaLaHfTaWReOsIrPtAuHgTlPbBiPoAtRn FrRaAcRfDbSgBhHsMtDs CePrNdPmSmEuGdTbDyHoErTmYbLu ThPaUNpPuAmCmBkCfEsFmMdNoLr PERIODS - Similarities: The number of outer electron shells.

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaSeTiVCrMnFeCoNiCuZnGaGeAsSeBrKr RbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXe CsBaLaHfTaWReOsIrPtAuHgTlPbBiPoAtRn FrRaAcRfDbSgBhHsMtDs CePrNdPmSmEuGdTbDyHoErTmYbLu ThPaUNpPuAmCmBkCfEsFmMdNoLr GROUPS – Similarities: The number of electrons in the outer shell. Common reactivity, bonding, chemical and physical properties.

HHe LiBeBCNOFNe NaMgAlSiPSClAr KCaSeTiVCrMnFeCoNiCuZnGaGeAsSeBrKr RbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXe CsBaLaHfTaWReOsIrPtAuHgTlPbBiPoAtRn FrRaAcRfDbSgBhHsMtDs CePrNdPmSmEuGdTbDyHoErTmYbLu ThPaUNpPuAmCmBkCfEsFmMdNoLr METALIC PROPERTIES Similarities: An elements relative ability to conduct energy in the form of heat or electricity. the “stair” Metals Non metals Metaloids

 When the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

Atomic Radius: A measure of the distance from the center of the nucleus to the outer-most electron Electronegativity: An atoms ability or affinity to gain another electron. Ionization Energy: The energy required to lose the outer-most electron from an element. Reactivity: An atoms general ability to undergo a chemical reaction.

Atomic Radius Trend

Ionization Energy Trend

H He LiBe BCNOFNe NaMg AlSiPSClAr KCaSeTiVCrMnFeCoNiCuZnGaGeAsSeBrKr RbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXe CsBaLaHfTaWReOsIrPtAuHgTlPbBiPoAtRn FrRaAcRfDbSgBhHsMtDs CePrNdPmSmEuGdTbDyHoErTmYbLu ThPaUNpPuAmCmBkCfEsFmMdNoLr Electronegativity (F) & Ionization Energy (He) Atomic Radius (Fr) & Reactivity (Fr)

Electrons between the nucleus and the valence electrons repel each other making the atom larger, affecting the atomic radius!.17

.18

Boosts the effective nuclear charge!.19

Lowers the effective nuclear charge.20

Isoelectronic ions have the same number of electrons. The more negative an ion is the larger it is and vice versa..21

 The ions of the d block and the lower p block have unfilled d or p orbitals.  These orbitals can accept electrons either an ion or polar molecule, to form a dative bond. This attraction results in the formation of a complex ion.  A complex ion is made up of two or more ions or polar molecules joined together.  The molecules or ions that surround the metal ion donating the electrons to form the complex ion are called ligands..22

 Compounds that are formed with complex ions are called coordination compounds  Common ligands  Complex ions usually have either 4 or 6 ligands. K 3 Fe(CN) 6 Cu(NH 3 ) 4 2+

 The formation of complex ions stabilizes the oxidations states of the metal ion and they also affect the solubility of the complex ion.  The formation of a  complex ion often has  a major effect on the  color of the solution of  a metal ion..24

 In an isolated atom all of the d sublevel electrons have the same energy.  When an atom is surrounded by charged ions or polar molecules, the electric field from these ions or molecules has a unequal effect on the energies of the various d orbitals and d electrons.  The colors of the ions and complex ions of d block elements depends on a variety of factors including:  The particular element  The oxidation state  The kind of ligands bound to the element Various oxidation states of Nickel (II).25

 The presence of a partially filled d sublevels in a transition element results in colored compounds.  Elements with completely full or completely empty subshells are colorless,  For example Zinc which has a full d subshell. Its compounds are white  A transition metal ion exhibits color, if it absorbs light in the visible range ( nanometers)  If the compound absorbs a particular wavelengths of light its color is the composite of those wavelengths that it does not absorb.  It shows the complimentary color..26

 Paramagnetism --- Molecules with one or more unpaired electrons are attracted to a magnetic field. The more unpaired electrons in the molecule the stronger the attraction. This type of behavior is called  Diamagnetism --- Substances with no unpaired electrons are weakly repelled by a magnetic field.  Transition metal complexes with unpaired electrons exhibit simple paramagnetism.  The degree of paramagnetism depends on the number of unpaired electrons.27

 Many D block elements are catalysts for various reactions  Catalysts speed up the rate of a chemical reaction with out being consumed.  The transition metals form complex ions with species that can donate lone pairs of electrons.  This results in close contact between the metal ion and the ligand.  Transition metals also have a wide variety of oxidation states so they gain and lose electrons in redox reactions.28

 Examples of D block elements that are used as catalysts: 1. Platnium or rhodium is used in a catalytic converter 2. MnO 2 catalyzes the decomposition of hydrogen peroxide 3.V 2 O 5 is a catalyst for the contact process 4.Fe in Haber process 5.Ni in conversion of alkenes to alkanes.29

Although we are most familiar with the periodic table that Seaborg proposed more than 60 years ago, several alternate designs have been proposed..30

.31

.32

.33