'Ionization energy' diaporamas de présentation

Chapter 6 The Periodic Table

Chapter 6 The Periodic Table. The how and why. History. 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 Not all elements had triads. History.

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The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION

The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION. PHYSICAL SETTING CHEMISTRY. Jan 2015. Table. 1 According to the modern model of the atom, the nucleus of an atom is surrounded by one or more. electrons neutrons positrons protons. Table.

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Chapter 7 Periodic Properties of the Elements

Chemistry, The Central Science , 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 7 Periodic Properties of the Elements. John D. Bookstaver St. Charles Community College Cottleville, MO. Development of Periodic Table.

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The Periodic Table

The Periodic Table. Basic Concepts. What do the numbers mean?. This is the atomic number. It is the number of protons in a single atom of this element. It is also # of electrons. 11. Na. The symbol for this element.

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Section 6-1

Section 6.1 Development of the Modern Periodic Table. Trace the development of the periodic table. Identify key features of the periodic table. atomic number: the number of protons in an atom.

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Chapter 6

Chapter 6. Ionic Bonds and Some Main-Group Chemistry. Ions and Their Electron Configurations. Chapter 2 Metals lose electrons to form cations Main group elements tend to lose the same # of electrons as their group number Nonmetals when combined with metals gain electrons to form anions

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Chemical Periodicity? What?

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LCD Calorimeter Design Issues

LCD Calorimeter Design Issues. Gary R. Bower/Ron Cassell, SLAC Chicago LCD Workshop January 8, 2002. Calorimetry for jets. At NLC energies almost all physics events produce high mass particles (W, Z, t, H?,?)

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Periodic Trends/Patterns

Periodic Trends/Patterns. CH. 2. Nuclear charge atomic size or radius ionization energy electron affinity electronegativity metallic character. Reactivity bonding characteristics crystal configurations acidic properties densities. Periodic Trend. Quantum Mechanical Model.

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Ch 5.3 Electron Configuration and Periodic Properties

Ch 5.3 Electron Configuration and Periodic Properties. Atomic Size. }. Measure the Atomic Radius - this is half the distance between the two nuclei of a diatomic molecule. Radius. #1. Atomic Size - Period Trends. Going from left to right across a period, the size gets smaller .

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Ionization Energy

Ionization Energy. It requires more energy to remove each successive electron. When all valence electrons have been removed, the ionization energy takes a quantum leap. Trends in First Ionization Energies. As one goes down a column, less energy is required to remove the first electron.

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Periodic Trends

Periodic Trends. CA Standards. Students know how to use the periodic table to identify trends in ionization energy, electronegativity , and the relative sizes of ions and atoms. Atomic Radius. Definition: Half of the distance between nuclei in covalently bonded diatomic molecule .

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Sparks: An example of competing models

Sparks: An example of competing models. Bruce Sherwood & Ruth Chabay Department of Physics Presented at the August 2003 meeting of the American Association of Physics Teachers in Madison WI

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Chapter 8

Chapter 8. Relationships in the Periodic Table. A Brief Overview. A Series of Properties: ? Atomic Radius - one half the distance between the two nuclei in a covalent homonuclear molecules. Metals. Diatomic Molecules.

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CHEMICAL PERIODICITY

CHEMICAL PERIODICITY. Group Trends. Transition Metals Innertransition Metals Main Block Elements Hydrogen Alkali Metals Alkaline Earth Metals Halogens Noble Gases. Transition & Innertransition Metals. Innertransition Metals. Transition Metals.

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Periodic Table

Periodic Table. Bohr Model. Energy of Atomic Sublevels. Basic Premises. (1) Radius is dependent upon outermost electrons (2) Nucleus is positive (3) Electrons are negative (4) Opposites attract (5) Electrons can occupy only specific energy levels.

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Metals, Nonmetals and Metalloids

Metals, Nonmetals and Metalloids. Metals. Location: 2/3 of all elements, l eft of the ladder, most active lower left (Fr) Lose/gain: lose electrons to form positive ions (cations)

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Ionization Energy

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Bond Strength

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