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WorksheetsMetals: Structure & Properties
Total questions: 20
Worksheet time: 10mins
How does metallic bonding occur in metals?
Metallic bonding occurs due to the sharing of protons between metal atoms
Metal atoms form covalent bonds with each other
Metal atoms repel each other due to the positive charges they carry
Delocalization of electrons from the outer energy levels of metal atoms creates a 'sea of electrons' that hold the metal atoms together.
Explain the conductivity of metals.
Metals have high electrical conductivity due to the presence of free electrons.
Metals have high electrical conductivity due to the presence of positive ions.
Metals have high electrical conductivity due to the presence of fixed protons.
Metals have low electrical conductivity due to the presence of free electrons.
What are the mechanical properties of metals?
Weight, color, texture
Strength, hardness, ductility, malleability, toughness, elasticity, and conductivity
Viscosity, acidity, luminosity
Transparency, flexibility, porosity
What is the role of electrons in the atomic structure of metals?
Electrons in metals contribute to their color
Electrons in metals have no impact on their properties
Electrons in metals are responsible for their hardness
Electrons in metals contribute to their unique properties such as electrical conductivity, thermal conductivity, malleability, and ductility.
Why are metals good conductors of electricity?
Metals contain insulating properties.
Metals have a sea of delocalized electrons.
Metals have a surplus of protons.
Metals repel electricity.
How does the arrangement of atoms affect the mechanical properties of metals?
The arrangement of atoms in metals affects their mechanical properties by influencing factors such as strength, ductility, hardness, and toughness.
The mechanical properties of metals are solely determined by their color, not their atomic arrangement.
Metals with atoms arranged in a specific pattern are always weaker than those with random arrangements.
The arrangement of atoms in metals has no impact on their mechanical properties.
What is the significance of the valence electrons in metals?
Valence electrons in metals determine their color.
Valence electrons in metals are responsible for their conductivity.
Valence electrons in metals affect their boiling point.
Valence electrons in metals are responsible for their magnetic properties.
Discuss the relationship between metallic bonding and malleability.
Metals with strong metallic bonding are typically brittle and not malleable.
Malleability is a result of covalent bonding in metals, not metallic bonding.
Metallic bonding causes rigidity in metals, leading to decreased malleability.
The relationship between metallic bonding and malleability is that metallic bonding enables malleability in metals due to the delocalization of electrons allowing layers of atoms to slide over each other easily.
Why do metals have high thermal conductivity?
High density of atoms
Presence of free electrons
Presence of protons
Low melting point
Explain the concept of ductility in relation to metallic properties.
Ductility in metals refers to their ability to deform under tensile stress without breaking, enabling them to be stretched into wires or other shapes.
Ductility is the measure of how easily metals can be magnetized.
Ductility is the ability of metals to conduct electricity efficiently.
Ductility refers to the hardness of metals under pressure.
How do impurities affect the conductivity of metals?
Impurities decrease resistance and increase conductivity in metals.
Impurities cause metals to become superconductors.
Impurities have no effect on conductivity in metals.
Impurities increase resistance and decrease conductivity in metals.
Discuss the relationship between crystal structure and mechanical properties of metals.
Crystal structure only impacts the color of metals, not their mechanical properties.
Metals with different crystal structures have identical mechanical properties.
The crystal structure of metals significantly impacts their mechanical properties.
The mechanical properties of metals are not affected by their crystal structure.
Which properties of metal makes it a good choice to make a cooking pot out of? Choose TWO
it has luster - it is shiny
it is a good conductor of heat
it is ductile - able to be made into a wire
it has a high melting point
1 and 2
1 and 7
3 and 5
5 and 6
Which phrase best describes the arrangement of the heavier particles in a metal?
lattice of positive ions
lattice of atoms
lattice of negative ions
lattice of positive and negative ions
Which of the following best describes the arrangement of electrons in a metal?
All of the electrons are delocalised
None of the electrons are delocalised
Only the valency electrons are delocalised
A maximum of 2 electrons are delocalised for each atom
Metals are senorus, meaning you can do this
make a sound
make metal soft
make metal hard
none of the above
These two metals are soft
sodium and mercury
lead and potassium
lead and steel
sodium and potassium
metals are this at room temperature?
liquid
solid
gas
plasma
