1. Metallic Bonding A metallic bond is the attraction
of a ________ _______for ____________electrons
Metallic cation
delocalized

2. Electron Sea Model proposes that the nuclei of the metallic cations hold onto their correct ________ of _________, but they may be any valence e- of a neighboring nucleus. They are NOT ______ or _____; they are floating in a sea above the _______ and can move freely from one atom to the next.

3. Electron Sea Model proposes that the nuclei of the metallic cations hold onto their correct number of electrons, but they may be any valence e- of a neighboring nucleus. They are NOT _______ or _____; they are floating in a sea above the ______and can move freely from one atom to the next.

4. Electron Sea Model proposes that the nuclei of the metallic cations hold onto their correct number of electrons, but they may be any valence e- of a neighboring nucleus. They are NOT shared or lost; they are floating in a sea above the nuclei and can move freely from one atom to the next.

5. delocalized electron =
Attractions between positive cations and the negative “sea of e-“ hold the metal atoms together in a lattice.
The valence e- of a metal that is free to move easily from one cation to another

6. Properties of metals med. high melting points high boiling points
malleable and ductile
heat conductors
electrical conductors

7. Brittleness is typical of ionic substances
Brittleness is typical of ionic substances. Imagine what happens to the crystal if a stress is applied which shifts the ion layers slightly.
Ions of the same charge are brought side-by-side and so the crystal repels itself to pieces!

8. Malleability of metals
Whereas ionic cmpds shatter when hit with
a mallet (hammer), metallic cmpds can be
flattened and shaped. Why?

9. As the number of
increases, increase.
In the transition metals, mobile electrons consist of both the
electrons (highest s) and the inner electrons.
delocalized electrons
hardness & strength
valence d

10. Alloy = mixture of metals; not a cmpd 18 carat Gold Au 75% Ag/Cu 25%
Sterling silver Ag 92.5% Cu 7.5%
Coinage silver Ag 90% Cu 10%
Plumber’s solder Pb 67% Sn 33%
Pewter Sn 85% Cu 7.3% Bi 6% Sb 1.7%
Brass Cu 60% Zn 39% Sn 1%
Steel Fe 99% C 1%
Cast Iron Fe 96% C 4%
Stainless Steel Fe 80.6% Cr 18%
C 0.4% Ni 1%

11. Types of alloys When two metals with similar size ions are mixed, a
alloy is formed
examples:
substitutional
Brass, pewter, 10 carat gold

12. When one of the metals’ ions is considerably smaller than the other metal, the smaller ions fill in the small spaces (___________) between the larger ones. This is
an __________ _____
example:
interstices
Interstitial alloy
Carbon steel

13. Summary “Sea of electrons” are reason for a metal’s properties
Alloys are mixtures of metals
Substitutional alloys have similar sized elements
Interstitial alloys have different sized elements
Metals are malleable (can be flattened) and ductile (can be drawn into wires), and have luster (are shiny)