Bonding and structure; Metallic bonds Flashcards
What do metals exist as?
Giant metallic lattice structures
Explain the formation of giant metallic lattice structures and provide an example.
Electrons on the outermost shells of metals form positive ions.
eg. magnesium has 2 electrons on outermost shellβ> in group 2β> has a 2+ charge
What type of force is in metals and what is it with?
Electrostatic forces between positive ions and the sea of delocalised electrons
What does it mean in metals if there are more electrons per atom?
stronger metallic bonding with the positive ions+sea of delocalised electronsβ> higher mp
What is an example of an element that has more electrons per atom than group 1 metals?
E.g. magnesium is in group 2 β> has a higher melting pointβ> magnesium donates 2 delocalised electrons per atom to delocalised system RATHER THAN sodiumβ> in group 1β> donates 1 electron per atom
What factors affect the melting point of metals?
size of the metal ion + lattice structure
state the physical properties of metals.
-good thermal conducters
-high mp
-insoluble
-malleable and ductile
-good electrical conductors
why are metals good thermal conductors?
the delocalised electrons transfer kinetic energy to each other .
why do metals have high mp?
strong metallic bondingβ>due to the strong electrostatic forces
$$why are metals good electrical conductors?
the delocalised electrons are mobile and carry current
why are metals insolouble and what state is an exception ?
metallic bond too strong to break
-exception is the state liquid metals
why are metals mallebale and ductile?
there are no bonds holding specific ions together β>metal ions can slip over each other when hit with a hammer β> still retain attraction between ions and delocalised electrons.
