Chapter 7 - Metallic Bonding Flashcards
Describe the structure and bonding in metals.
Metals are described as having a giant metallic lattice structure of positive ions surrounded by a “sea of mobile electrons”. There is a strong electrostatic force of attraction between the positive metal ions and the “sea of mobile electrons”.
Explain, in terms of bonding and structure, why metals have high boiling and melting point?
They have a giant metallic lattice structures. Since they have a strong electrostatic force of attraction between the cations and “sea of mobile electrons”, a large amount of heat energy is required to overcome it.
why do metals have high density?
The ions are very closely packed together.
Why are metals malleable?
In metallic bonding, the valence electrons do not belong to any particular metal atom. If sufficient force is applied, one layer of atoms can slide over one another without disrupting the metallic bonding. Thus, metallic bonds and strong but flexible.
Why are metals good conductors of heat?
Since the ions are closely packed, the proximity (closeness) of ions allows them to transfer heat energy by vibration quickly from one ion to another. The movement of mobile electrons further speed up the rate of transfer. Hence, metals are good conductors of heat.
when would metals conduct electricity?
In solid and molten state.
Why would metals conduct electricity?
Presence of “sea of mobile electrons”.
How are metal atoms arranged?
Metal atoms are packed very closely in an orderly arrangement.
