Atomic Bonding And Conductivity Presentation
| Introduction to Atomic Bonding and Conductivity | ||
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| • Atomic bonding refers to the interaction between atoms to form stable compounds. | ||
| • Conductivity is the ability of a material to conduct electricity or heat. | ||
| • The type of atomic bonding in a material determines its conductivity properties. | ||
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| 1 | ||
| Types of Atomic Bonding | ||
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| • There are three main types of atomic bonding: ionic, covalent, and metallic. | ||
| • Ionic bonding occurs when electrons are transferred from one atom to another, resulting in positively and negatively charged ions. | ||
| • Covalent bonding involves the sharing of electrons between atoms to form molecules. | ||
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| 2 | ||
| Ionic Bonding and Conductivity | ||
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| • Ionic compounds are typically poor conductors of electricity in solid form. | ||
| • In ionic bonding, electrons are tightly held by ions, limiting their mobility. | ||
| • However, when ionic compounds dissolve in water or melt, the ions become mobile and can conduct electricity. | ||
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| 3 | ||
| Covalent Bonding and Conductivity | ||
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| • Covalent compounds can be either conductors or insulators depending on their structure. | ||
| • In pure covalent compounds, electrons are shared equally, resulting in a lack of charged particles for conductivity. | ||
| • However, some covalent compounds can form a network structure, allowing electrons to move and conduct electricity. | ||
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| 4 | ||
| Metallic Bonding and Conductivity | ||
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| • Metallic bonding occurs when delocalized electrons move freely between metal atoms. | ||
| • This mobility of electrons contributes to the high conductivity of metals. | ||
| • Metals are excellent conductors of both electricity and heat due to their metallic bonding. | ||
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| 5 | ||
| Factors Affecting Conductivity | ||
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| • Conductivity is influenced by factors such as temperature, impurities, and crystal structure. | ||
| • Higher temperatures generally increase conductivity due to increased atomic vibrations and electron mobility. | ||
| • Impurities can disrupt the regular crystal structure, reducing conductivity. | ||
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| 6 | ||
| Conductivity in Semiconductors | ||
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| • Semiconductors have an intermediate conductivity between conductors and insulators. | ||
| • In semiconductors, conductivity can be controlled by adding impurities through a process called doping. | ||
| • Doping introduces extra electrons or electron deficiencies, altering the conductivity properties. | ||
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| 7 | ||
| Superconductivity | ||
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| • Superconductivity is a phenomenon where certain materials exhibit zero electrical resistance at extremely low temperatures. | ||
| • Superconductors are used in various applications such as magnetic resonance imaging (MRI) machines and particle accelerators. | ||
| • The exact mechanism behind superconductivity is still not fully understood. | ||
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| 8 | ||
| Applications of Conductivity | ||
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| • Conductivity plays a crucial role in numerous technologies, including electrical wiring, electronic devices, and power transmission. | ||
| • Conductive materials are also used in sensors, solar cells, and batteries. | ||
| • Understanding atomic bonding and conductivity is essential for advancing these technologies. | ||
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| 9 | ||
| Conclusion | ||
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| • Atomic bonding determines the conductivity properties of materials. | ||
| • Different types of bonding, such as ionic, covalent, and metallic, result in different conductivity characteristics. | ||
| • Conductivity is influenced by factors such as temperature, impurities, and crystal structure, and has various applications in modern technology. | ||
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