'Electronic configurations' diaporamas de présentation

GROUP VII The Halogens A guide for i GCSE students

GROUP VII The Halogens A guide for i GCSE students. 2010 SPECIFICATIONS. KNOCKHARDY PUBLISHING. GROUP VII. INTRODUCTION

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Chapter 3: Electron Structure and the Periodic Law

Chapter 3: Electron Structure and the Periodic Law. PERIODIC LAW This is a statement about the behavior of the elements when they are arranged in a specific order.

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Chapter 3: Electronic Structure and the Periodic Law

Chapter 3: Electronic Structure and the Periodic Law. PERIODIC LAW. This is a statement about the behavior of the elements when they are arranged in a specific order. In its present form, the statement is:. 7 periods. PERIODIC TABLE.

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Electronic configurations

Electronic configurations. Remember the rules for adding electrons. 1. Fill the orbitals in order of increasing energy. 2. When there are more than one orbital of the same energy, these orbitals are first occupied singly by electrons. 3. Each orbital can hold a maximum of two electrons.

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Subshells & orbitals

Subshells & orbitals. The ionisation energy graph does not increase steadily across a period. The ionisation energy graph does not increase steadily across a period The small decreases are due to sub-shells or sub-energy levels.

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Lecture 27 Molecular orbital theory III

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Unit 4 Topic 1

Unit 4 Topic 1. SPDF. Principal Energy Levels. Electrons occupy principal energy levels around the nucleus of the atom These energy levels represent specific distances from the nucleus. Each energy level n = 1 to n = 7, is farther from the nucleus. Principal Energy Levels Cont.

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Molecules

e-. Molecules. 2 st excited state 1 st excited state ground state. Potential Energy Surfaces. A 2. U(r). A* + A. A + A. q a. LCAO-MO. e-. a. b. H 2 +. Secular equation. Bonding vs antibonding energies. Other LCAO. How about p orbitals. e-. e-. a. a. b. b. p orbitals.

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Access to HE Diploma

Access to HE Diploma. Pharmacy and Biomedical Science Introduction to Matter Lesson 1. Assessment Criteria. 1.1 Define an element giving examples. 1.2 Write the names and symbols of the first 20 elements.

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Chemistry Revision 3

Chemistry Revision 3 . Electronic configurations. State which block in the periodic table you find the following elements: Sulphur Vanadium Strontium. Electronic configurations. Sulphur = p Vanadium = d Strontium = s

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What is the molecular mass and identity of the metal M?

A 1.0 g sample of an alkaline earth metal M reacts completely with 0.8092 g of chlorine gas to yield and ionic salt with the formula MCl 2 . In the process 9.46 kJ of heat is released. . What is the molecular mass and identity of the metal M?. M + Cl 2 = MCl 2.

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The general properties of transition metals

The general properties of transition metals. L.O.: Understand definition of transition metal. Explain the characteristic properties of transition metals. Write electronic configurations of: Sc, Ti, Cu and Zn. To which block of the periodic table do Sc, Ti and Cu belong to? Why?

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Distribution of electrons in various shells.

Learning Objective:. Distribution of electrons in various shells. How are Electrons Distributed in Different Orbits (Shells)?. The distribution of electrons into different orbits of an atom was suggested by Bohr and Bury.

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Electron Configuration: Ions

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