Structure 2.3 Metallic Bonds

lattice of cations surrounded by delocalized electrons

electrostatic attraction between lattice of cations and delocalized electrons

low ionization energy

(when looking at elements within a period)
metal atoms relatively have less protons and electrons ∴less nuclear charge ∴less attraction between the nucleus and electrons ∴easier to remove electrons

→ metal atoms are bigger in size (less nuclear charge ∴ electrons are further away from the nucleus)

losing valence electrons and forming positive ions (cations)

loss of control over valence electrons + sea of delocalized electrons

valence electrons of metal atoms that are not associated with one specific electron nucleus but move freely among a lattice of cations

delocalized electrons

• good electrical conductivity

• good thermal conductivity

• malleability

• ductility

• high melting points

• high boiling points

• shiny, lustrous appearance

• delocalized electrons are highly mobile

  • electrons are considered electricity

    • when voltage is applied (negative and positive terminals are added to metals), electrons freely move in one direction from the negative terminal toward the positive terminal

• when heat is applied, particles vibrate

• delocalized electrons easily influence other particles to vibrate since they are mobile

• heat energy from the vibration is delivered all throughout the metal

physical property of elements that can be shaped under pressure

• delocalized electrons are non-directional therefore movement is random

• when under pressure, metallic bond still remains since electrons can move freely and prevent repulsion between cations

Physical property of elements to be drawn our into threads.

• delocalized electrons are easily evenly distributed among cations ∴stronger bonds

  • more energy is needed to overcome the electrostatic forces in the metallic bond

• delocalized electrons in the metal crystal structure reflect light

Non-directional

• mixture of metal with other metals or non-metal elements (in a molten state) (homogenous)

• enhances the properties of metallic elements

Charge and radius of metal ions

respectively,

• # of delocalized electrons (valence electrons)

• charge of cations (metal ions)

• radius of cations (metal ions)

• more delocalized electron density (more valence electrons)

• smaller cation (high nuclear charge, more protons)

melting point

• ↑# electrons

  • ↑ delocalized electron density

• ↑# protons

  • ↑nuclear charge

  • ↓ size of atom

  • ↑ electrostatic attraction between delocalized electrons and cations

    • ↑ ionization energy

    • ↓ reactivity

• ↑ melting point

• ↑STRENGTH

• ↑ shielding

  • ↑ radius of metal atom

• ↓ ionization energy

  • ↑ reactivity

• ↓melting point

• ↓STRENGTH

• Elements with an incomplete d sublevel

• Elements that can lead to cations with an incomplete d sublevel )d sublevel elections are delocalized)

• ↑of electrons in d sublevel

  • ↑of delocalized electrons

• ↑ of protons

  • ↑nuclear charge (positive charge)

  • ↓size

  • ↑electrostatic attraction

• All of them:

  • can lose ↑# of electrons (have ↑ # of delocalized electrons)

  • have ↑ positive charge (nuclear charge)

    • ↓size

• ↑# of delocalized electrons (mobile)