Metallic Bonding and the Electron Sea Model, Electrical Conductivity - Basic Introduction

This chemistry video tutorial provides a basic introduction into metallic bonding and the electron sea model. The valence electrons in the metal are delocalized - they are free to move around stationary metal cations. This explains the electrical conductivity of metals. A substance with free flowing charge can conduct an electric current. The charge carrier in metals are valence electrons. The core electrons in metals atoms are localized - they are bound to their respective atoms and are not free to move from one metal atom to another.
Lewis Structures - Mega Review:
• Lewis Structures, Intr...
Sigma and Pi Bonding:
• Sigma and Pi Bonds Exp...
Hybridization of Atomic Orbitals:
• Hybridization of Atomi...
Molecular Orbital Theory:
• Molecular Orbital Theo...
Dipole Dipole Forces of Attraction:
• Dipole Dipole Forces o...
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Hydrogen Bonding:
• Hydrogen Bonds In Wate...
London Dispersion Forces:
• London Dispersion Forc...
Ion Dipole Forces:
• Ion Dipole Forces & Io...
Bragg's Equation For X-Ray Diffraction:
• Bragg's Equation For X...
Molecular & Network Covalent Solids:
• Ionic Solids, Molecula...
_______________________________
Metallic Bonding:
• Metallic Bonding and t...
Metal Alloys:
• Metal Alloys, Substitu...
Diamond Vs Graphite:
• Structure of Diamond a...
Semiconductors:
• Semiconductors, Insula...
Unit Cell Chemistry:
• Unit Cell Chemistry ...
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Final Exams and Video Playlists:
www.video-tuto...
Full-Length Videos and Worksheets:
/ collections
Chemistry PDF Worksheets:
www.video-tuto...

[@TheOrganicChemistryTutor]

Chemistry PDF Worksheets: www.video-tutor.net/chemistry-basic-introduction.html
Full-Length Videos & Exams: www.patreon.com/MathScienceTutor/collections

[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for a basic analysis into Metallic Bonding and the Electron Sea Model in AP/General Chemistry. The characteristics of metals are very important especially those that conduct heat and electricity. Melting points must also be considered in all types of metals.This is an error free video/lecture on RUclips TV with the Organic Chemistry Tutor.

[@theoretically_true151]

Summary:
Metallic Bonding:
-Basically covalent bonds but mobile delocalized/valence electrons can be shared with thousands of atoms
-Electron Sea Model:
-Fixed metal cations surrounded by a "SEA" of mobile valence electrons
-Mobile valence electrons are free to move, are shared among many metal cations, are random in motion (mobile), and is the reason for electrical conductivity
-Delocalized electrons: The valence electrons that are free to move and are shared among the many metal cations
-Localized electrons: Core electrons that are not free to move
-***Any object that has FREE-FLOWING CHARGES can conduct electricity (movement of electric charge)
-***Metallic bonds have free-flowing electrons, ionic bonds have free-flowing ions
-BATTERIES create an electric field that creates a voltage which forces the electrons to go in one way (instead of the random direction they normally move in), towards the positive terminal.
-Physical Properties of Metallic Bonds:
-Malleable: Can be hammered into shapes like thin sheets (ex: aluminum sheets)
-Ductile: Can be pulled into very thin wires (ex: Cu and Ag wires)
-Excellent Thermal Conductors: Mobile delocalized/valence electrons allows heat to be transferred from one part of the metal to the other part of the metal
-Excellent Electrical Conductors: Mobile delocalized/valence electrons that are free to move
-Luster: Creates a shiny appearance
-Melting points and boiling points in metallic bonds may vary greatly.

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HOLD ON!!! I absolutely love your videos and you are one of the GOAT but a battery does contribute electrons to the circuit. A voltage difference is created by reactions in the anode and cathode. There is a barrier in the battery that prevents the direct discharge of this voltage, and so the conductor wire provides a path for the discharge. Your explanation is correct that the wire/conductor's electrons move in one direction since they are experiencing the simultaneous repulsive forces from the freed electrons that are now being built up in the anode and the attractive forces towards the cathode (as the reaction in the cathode creates a high reduction potential in which the electrons want to get there).

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Valence and conduction band hybrid for conductors or metals.

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[@josephstar1883]

How are mettalic bonds covalent bonds? In chemistry lessons we are thaught that metallic bond is a separate type of bond? You're confusing me.

[@HessiDude]

I'm no expert, but I would guess it's closer to, but not the same as, ionic bonds because the cations and the free flowing electrons attract and create the bond, and the free flowing electrons never "attach" to the valence shell of the cations. Afaik the attraction between the cations and the free flowing electrons is known as electrostatic attraction (not the only form of it).

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4:30
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At 6:02, you say that electrons dont emanate from the battery but I have read that the oxidation reactions occurring at the negative end of the battery produce electrons which then flow to the positive terminal. Kindly clarify this. Thanks :-)

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[@Dazzletoad]

You said that electricity is the movement of electrical charge, and that sodium chloride in water can conduct electricity because of the free movement. You mean of ions in hydration shells?
If so, then if you pump electrons in wouldn't you have the implied flow of cl- ions, and not simply electrons? Or you mean electrons are delocalised from these ions in water?
I'm confused :D

[@Roarzan]

Yes, the meant the ions themselves. Whether it's electrons in a metal, or ions in a solution, what matters is that they're charged.

[@Dazzletoad]

@@Roarzan Thank you for your comment 👍🏻

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is malleable there means forged?

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