Metals: Structure & Properties

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.