Which one of the following is the reason why pure metals are good thermal and electrical conductors?The high melting and boiling points.The arrangement of metal atoms in layers.The movement of delocalised electrons.The strong force of attraction between metal ion and delocalised electron.
Question
Which one of the following is the reason why pure metals are good thermal and electrical conductors?The high melting and boiling points.The arrangement of metal atoms in layers.The movement of delocalised electrons.The strong force of attraction between metal ion and delocalised electron.
Solution
The reason why pure metals are good thermal and electrical conductors is due to "The movement of delocalised electrons."
Here's a step-by-step explanation:
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Metals have a unique atomic structure with a sea of delocalised electrons moving freely around a lattice of positive metal ions.
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These delocalised electrons are not attached to any particular atom and can move freely throughout the metal.
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When an electric current or heat energy is applied to the metal, these electrons can quickly carry and spread this energy throughout the metal, making metals good conductors of electricity and heat.
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The other options mentioned, such as high melting and boiling points, the arrangement of metal atoms in layers, and the strong force of attraction between metal ions and delocalised electrons, are properties of metals but they do not directly contribute to their ability to conduct heat and electricity.
Similar Questions
Match the correct explanation to the property of pure metals it explains. Electrical conductivitySolid at room temperatureHigh densityDuctileHigh boiling pointPossible AnswersA lot of energy is needed to overcome the weak electrostatic attraction between the metal atom and the delocalised electron.This is due to the high boiling and melting points.The delocalised electrons are free to move and can transferthermal energy.A lot of energy is needed to overcome the strong electrostatic attraction between the metal ion and the delocalised electron.The delocalised electrons are free to move and can carry anelectric current.The metal is in the solid state which means the particles are tightly packed together and held in a fixed positions.The layers of metal atoms can slide over each other when a force is applied.I DON'T KNOWRESETSUBMIT ANSWER
Which property of metals makes them good conductors of heat?A.Their mobile electronsB.Their hardnessC.Their melting pointD.Their ductilitySUBMITarrow_backPREVIOUS
Which one of the following is NOT a property of pure metals?High melting pointPoor electrical conductorSolid at room temperatureGood thermal conductor
Metallic bonding always occurs between:Noble gasesMetal atomsNon-metal atomsMetal and non-metal atoms2A metallic bond is the electrostatic attraction between:Positive ions and delocalised electronsNegative ions and delocalised electronsElectrons and delocalised negative ionsElectrons and delocalised positive ions3Which of these is a property of metals?Poor conductors of electricityLow boiling pointsMalleableLow melting points4Which of the following statements best describes why metals are good conductors of heat?Metallic bonds are very strongLayers of metal atoms can slide past one another easilyMetals have high melting pointsThe delocalised electrons can carry thermal energy through the substance5Which of the following is a metal alloy?AluminiumCopperSteelIron6Metal alloys are generally harder and stronger than the individual elements they are made from. This is because the atoms of each element are of a different size and therefore:Disrupt the regular layers of ions, making them less malleableIncrease the size of the latticeLead to an increase in boiling pointLead to an decrease in boiling point
Match the correct explanation to the property of pure metals it explains. High melting pointMalleableHigh densitySolid at room temperatureThermal conductivityPossible AnswersThe delocalised electrons are free to move and can carry anelectric current.When the metal is in the solid state the particles are tightly packed together and held in a fixed positions.A lot of energy is needed to overcome the weak electrostatic attraction between the metal atom and the delocalised electron.The delocalised electrons are free to move and can transferenergy.The layers of metal atoms can slide over each other when a force is applied.This is due to the high boiling and melting points.A lot of energy is needed to overcome the strong electrostatic attraction between the metal ion and the delocalised electron.I DON'T KNOWRESETSUBMIT ANSWER
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