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Related Concept Videos

Bonding in Metals02:32

Bonding in Metals

Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”.
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions.
Metallic Solids02:37

Metallic Solids

Metallic solids such as crystals of copper, aluminum, and iron are formed by metal atoms. The structure of metallic crystals is often described as a uniform distribution of atomic nuclei within a “sea” of delocalized electrons. The atoms within such a metallic solid are held together by a unique force known as metallic bonding that gives rise to many useful and varied bulk properties.
All metallic solids exhibit high thermal and electrical conductivity, metallic luster, and malleability. Many...
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Molecular Orbital Theory II

Molecular Orbital Energy Diagrams
Chemical Bonds02:40

Chemical Bonds


Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
An ionic bond is formed due to electrostatic attraction between cations and anions. Often, the ions are formed by the transfer of electrons from...
Electron Configuration of Multielectron Atoms03:26

Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the 3s orbital, giving a 1s22s22p63s1 configuration. The electrons occupying the outermost shell orbital(s) (highest value of n) are called valence electrons, and those occupying the inner shell orbitals are called core electrons. Since the core electron shells correspond to noble gas electron configurations, we can abbreviate electron...

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Related Experiment Video

Updated: Jun 3, 2026

Hydrogen Charging of Aluminum using Friction in Water
07:50

Hydrogen Charging of Aluminum using Friction in Water

Published on: January 28, 2020

The bonding electron density in aluminum.

Philip N H Nakashima1, Andrew E Smith, Joanne Etheridge

  • 1ARC Centre of Excellence for Design in Light Metals, Monash University, Victoria 3800, Australia. philip.nakashima@eng.monash.edu.au

Science (New York, N.Y.)
|March 26, 2011
PubMed
Summary
This summary is machine-generated.

Investigating aluminum

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Related Experiment Videos

Last Updated: Jun 3, 2026

Hydrogen Charging of Aluminum using Friction in Water
07:50

Hydrogen Charging of Aluminum using Friction in Water

Published on: January 28, 2020

Facile Preparation of Ultrafine Aluminum Hydroxide Particles with or without Mesoporous MCM-41 in Ambient Environments
05:50

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Published on: May 11, 2017

Indirect Fabrication of Lattice Metals with Thin Sections Using Centrifugal Casting
08:32

Indirect Fabrication of Lattice Metals with Thin Sections Using Centrifugal Casting

Published on: May 14, 2016

Area of Science:

  • Solid-state physics
  • Materials science
  • Quantum chemistry

Background:

  • Aluminum is often modeled as an ideal free electron gas.
  • Determining electron redistribution in aluminum's chemical bonding is challenging.
  • Experimental and theoretical results for electron distribution have differed.

Purpose of the Study:

  • To experimentally determine the bonding electron distribution in aluminum.
  • To correlate electron distribution with aluminum's elastic properties.

Main Methods:

  • Quantitative convergent-beam electron diffraction (qCBED).
  • Density functional theory (DFT) calculations.

Main Results:

  • Experimental electron distribution closely matches DFT calculations.
  • Established an accurate quantitative correlation between elastic properties and electron/electrostatic potential distributions.

Conclusions:

  • The study provides a precise experimental measurement of electron distribution in aluminum.
  • The findings link electronic structure to macroscopic elastic behavior.