What is the primary reason for the high electrical conductivity in metals?
Mobile electrons
Arrange the steps in describing the structure of metals
1️⃣ Lattice arrangement of metal atoms
2️⃣ Sea of delocalized electrons
3️⃣ Metallic bonding by electrostatic attraction
Metals have high electrical conductivity because mobile electrons can carry electric charge.
True
Delocalized electrons in metals enable efficient transfer of heat and electricity.
True
Metals are good conductors of electricity because delocalized electrons can move freely to carry charge.
True
The luster of metals is due to the effective reflection of light by delocalized electrons.
True
Metals are excellent conductors of electricity because electrons are delocalized and move freely within a sea of electrons surrounding positively charged metal ions.
What determines how well a metal conducts electricity?
Mobility of delocalized electrons
Match the material type with its thermal conductivity:
Metals ↔️ High
Ionic compounds ↔️ Low
Covalent compounds ↔️ Low to moderate
The lattice structure in metals provides stability and density.
Metallic bonds have delocalized electrons, which leads to high conductivity and malleability.
True
Why are metals malleable and ductile?
Delocalized electrons allow layers to slide
Metallic bonding involves a lattice of metal cations surrounded by a "sea" of delocalized electrons
The high electrical conductivity of metals is due to the movement of delocalized electrons
What is the primary reason covalent compounds are poor conductors of electricity?
Localized electrons
The delocalized electrons in metals absorb and transfer thermal energy
Malleability and ductility in metals are due to the ability of metal layers to slide over each other without disrupting metallic bonds
What is the purpose of creating alloys by mixing two or more metals?
Improve specific properties
Adding chromium to iron in stainless steel creates a protective oxide layer, improving corrosion resistance.
True
Adding chromium to iron creates a protective oxide layer, improving corrosion resistance.
True
Match the alloy with its composition:
Stainless Steel ↔️ Iron + Chromium + Nickel
Brass ↔️ Copper + Zinc
Bronze ↔️ Copper + Tin
Why do metals have high electrical conductivity?
Delocalized electrons
What is the unique property of metals that allows them to be drawn into wires?
Ductility
Match the metallic property with its description:
Malleability ↔️ Can be hammered into thin sheets
Ductility ↔️ Can be drawn into wires
Luster ↔️ Shiny appearance
Ionic compounds conduct electricity only when molten or dissolved in water.
True
Ionic compounds conduct electricity only when solid
False
Match the material type with its thermal conductivity:
Metals ↔️ High
Ionic Compounds ↔️ Low
Malleability in metals is the ability to be hammered into thin sheets
Match the alloy with its improved properties:
Stainless Steel ↔️ Corrosion resistance, Hardness
Brass ↔️ Strength, Malleability
In covalent bonding, electrons are shared between atoms in localized bonds
Metallic bonding involves the electrostatic attraction between metal cations and delocalized electrons.
True
Metallic bonds are characterized by delocalized electrons, leading to properties like high conductivity and malleability
What unique feature of metallic bonding allows metals to be malleable and ductile?
Delocalized electrons
Compared to ionic and covalent bonds, metallic bonds are characterized by delocalized electrons, leading to unique properties like high conductivity and malleability
What are the two main factors that contribute to the unique properties of metallic substances?
Lattice structure and delocalized electrons
Metals are malleable because layers of metal atoms can slide over each other due to the delocalized electron sea.
What two key features of metals contribute to their exceptional conductive and mechanical properties?
Sea of delocalized electrons and lattice structure
What are the two main factors contributing to the high thermal conductivity of metals?
Delocalized electrons and lattice vibrations
What type of bonding is present in metallic substances?