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Metals are good conductors of heat and electricity. This property is conferred by _______ bonds.
- a)metallic
- b)ionic
- c)covalent
- d)hydrogen
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
Metals are good conductors of heat and electricity. This property is c...
Explanation:
Metallic bonds are responsible for the good conductivity of heat and electricity in metals.
Metallic bonds:
- In a metallic bond, positively charged metal ions are surrounded by a "sea" of delocalized electrons.
- These delocalized electrons are free to move throughout the structure of the metal.
- This free movement of electrons allows metals to conduct heat and electricity efficiently.
- When a temperature gradient is applied, the free electrons can carry thermal energy through the metal by transferring it from one electron to another.
- Similarly, when a voltage is applied, the free electrons can move in response to the electric field, allowing for the flow of electric current.
In contrast:
- Ionic bonds involve the transfer of electrons between positively and negatively charged ions, which do not allow for the free movement of electrons required for good conductivity.
- Covalent bonds involve the sharing of electrons between atoms, which also do not allow for the free movement of electrons needed for conductivity.
- Hydrogen bonds are relatively weak intermolecular forces that do not contribute significantly to the conductivity of heat or electricity.
Therefore, metallic bonds are uniquely suited for providing metals with their characteristic high conductivity of heat and electricity.
Metallic bonds are responsible for the good conductivity of heat and electricity in metals.
Metallic bonds:
- In a metallic bond, positively charged metal ions are surrounded by a "sea" of delocalized electrons.
- These delocalized electrons are free to move throughout the structure of the metal.
- This free movement of electrons allows metals to conduct heat and electricity efficiently.
- When a temperature gradient is applied, the free electrons can carry thermal energy through the metal by transferring it from one electron to another.
- Similarly, when a voltage is applied, the free electrons can move in response to the electric field, allowing for the flow of electric current.
In contrast:
- Ionic bonds involve the transfer of electrons between positively and negatively charged ions, which do not allow for the free movement of electrons required for good conductivity.
- Covalent bonds involve the sharing of electrons between atoms, which also do not allow for the free movement of electrons needed for conductivity.
- Hydrogen bonds are relatively weak intermolecular forces that do not contribute significantly to the conductivity of heat or electricity.
Therefore, metallic bonds are uniquely suited for providing metals with their characteristic high conductivity of heat and electricity.
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Community Answer
Metals are good conductors of heat and electricity. This property is c...
Metallic bonds are formed between positive metal ions and the sea of delocalized electrons. This bond is stronger than covalent and ionic bonds. Due to the mobility of electrons, conduction of heat and electricity is feasible.
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Metals are good conductors of heat and electricity. This property is conferred by _______ bonds.a)metallicb)ionicc)covalentd)hydrogenCorrect answer is option 'A'. Can you explain this answer?
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