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Metallic Bond

 
5.6  Metallic Bond
 
The Purpose of Scientists to Classify Elements
  • Chemists try to develop and generalize elements by classifying them according to certain characteristics.

The image features a blue and white background with text in the center. The text is titled ‘Classification will allow scientists to:’ and lists four points: 1. Classify chemical and physical properties. 2. Predict the position of the element. 3. Identify and compare elements from different groups. 4. Predict chemical and physical properties. There is a hand holding a pen at the top right corner, and the logo ‘Pandai’ is at the bottom right corner. The corners of the image have red and blue triangular shapes.
 
Formation of Metallic Bond
  • Metal atoms are arranged closely packed and orderly in the solid state.
  • Valence electrons of metal atoms can be donated easily and delocalised although in the solid state.
  • Metal ions that are positively charged are formed when valence electrons are delocalised.
  • All delocalised valence electrons can move freely between the metal structure and form a sea of electrons.
  • Electrostatic attraction force between the sea of electrons and the positively charged metal ions forms the metallic bond as belows:

The image illustrates the structure of metallic bonding. On the left, it shows a regular arrangement of positively charged metal ions with valence electrons scattered among them. On the right, it depicts the same metal ions surrounded by a ‘sea of electrons,’ indicating the delocalized nature of electrons in metallic bonds. The electrons are free to move around, which explains the conductivity and malleability of metals.
 
Electron Conductivity of Metals
  • When the electrons of metal atoms are delocalised in the sea of electrons, the metal can conduct electricity.
  • Electrons that move freely in the metal structure carry the charges from the negative terminal to the positive terminal when electricity is supplied.
  • Electrical conductivity of metals is as below:

This diagram illustrates the flow of electrons in a metal conductor. On the left side, there is a negative terminal, and on the right side, there is a positive terminal. The metal conductor is depicted in the center, with positively charged ions (large blue circles) arranged in a grid. Electrons (small red circles) are shown moving from the negative terminal to the positive terminal, indicating the direction of current flow. The arrows indicate the movement of electrons through the metal.
 

 

 

 

 

 

The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.

Metallic Bond

 
5.6  Metallic Bond
 
The Purpose of Scientists to Classify Elements
  • Chemists try to develop and generalize elements by classifying them according to certain characteristics.

The image features a blue and white background with text in the center. The text is titled ‘Classification will allow scientists to:’ and lists four points: 1. Classify chemical and physical properties. 2. Predict the position of the element. 3. Identify and compare elements from different groups. 4. Predict chemical and physical properties. There is a hand holding a pen at the top right corner, and the logo ‘Pandai’ is at the bottom right corner. The corners of the image have red and blue triangular shapes.
 
Formation of Metallic Bond
  • Metal atoms are arranged closely packed and orderly in the solid state.
  • Valence electrons of metal atoms can be donated easily and delocalised although in the solid state.
  • Metal ions that are positively charged are formed when valence electrons are delocalised.
  • All delocalised valence electrons can move freely between the metal structure and form a sea of electrons.
  • Electrostatic attraction force between the sea of electrons and the positively charged metal ions forms the metallic bond as belows:

The image illustrates the structure of metallic bonding. On the left, it shows a regular arrangement of positively charged metal ions with valence electrons scattered among them. On the right, it depicts the same metal ions surrounded by a ‘sea of electrons,’ indicating the delocalized nature of electrons in metallic bonds. The electrons are free to move around, which explains the conductivity and malleability of metals.
 
Electron Conductivity of Metals
  • When the electrons of metal atoms are delocalised in the sea of electrons, the metal can conduct electricity.
  • Electrons that move freely in the metal structure carry the charges from the negative terminal to the positive terminal when electricity is supplied.
  • Electrical conductivity of metals is as below:

This diagram illustrates the flow of electrons in a metal conductor. On the left side, there is a negative terminal, and on the right side, there is a positive terminal. The metal conductor is depicted in the center, with positively charged ions (large blue circles) arranged in a grid. Electrons (small red circles) are shown moving from the negative terminal to the positive terminal, indicating the direction of current flow. The arrows indicate the movement of electrons through the metal.
 

 

 

 

 

 

The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.
Chapter : Chemical Bonds
Topic : Metallic Bond
Form 4 Chemistry
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