1. METALS
Bonds and
Properties
Alloys
Pure Elements

2. Some Properties of Metals
Low (lowest: Fr)
ELECTRONEGATIVITY
IONIZATION ENERGY
Lose e- to form (+) ions
Ion FORMATION
Solid (except Hg)
PHASE at STP
Good to Excellent
CONDUCTIVITY :
HEAT AND ELECTRICITY
Malleable & Ductile
DEFORMABILITY
HIGH
LUSTER

3. Many metals have high luster
Hmmm….
How much is this
shiney Gold worth !?
400 ounces (27.5lbs)
$ / ounce
$483, per bar
12 bars =
$5,806,848.00

4. Many Metals have high melting points

5. Metal bonding Metallic bonding: different from ionic bond
Both bond types involve electrostatic attraction
Ionic bond: transfer electrons from one atom to another
Metal bonds:
valence electrons ROAM FREELY between metal atoms
this sea of mobile electrons accounts for
properties of metals

6. Why can electrons in metals roam freely about?

7. Metal bonding
Metals: form organized lattice structures similar to ionic cmpds
adjacent atoms in metal lattice are all same
close proximity of atoms allows outer electron energy levels to overlap
So…

8. electrons in outer valence shell can move freely through these overlapping energy levels
results in “sea of mobile electrons”

9. Na 3s Na 3s1
overlapping valence electron orbitals

10. Metal bonding Freely moving electrons: called “delocalized” electrons
allows (+) metal cation to form
Delocalized electrons move freely
throughout metal from one cation to next
creates “sea of mobile electrons”

11. sea of electrons: binds each metal cation to neighboring cation
this creates the metal bond

12. Metal Properties How do electrons do this?
sea of mobile electrons gives metals some unique properties
since electrons move freely from place to place they:
conduct electricity (flow of electrons)
conduct heat
account for metals being:
malleable
ductile
shiney (luster)
How do electrons do this?

13. - + Electrical Conductivity
Flow of electrons
free flow of electrons through the metal
e- flow from metal through metal wire towards
(+) terminal; then flow from (-) terminal back into
metal

14. Malleability
Metals & non-metals behave very differently when hit with a force such as hammer: Metals DEFORM & Non-metals SHATTER
Why?
metals have free
flowing electrons
& non-metals do not!

15. If apply force to metal:
metal atoms shift away from force & free electrons bond newly
overlapping metal ions together
metal’s shape is deformed
but shift doesn't change
metal atoms
If apply force to non-metal:
like charges align (+) to (+)
(-) to (-) which results in
shattering due to repulsion
forces
Metal
Non-Metal

16. Deformation of Metals
Deformation of Metals

17. As # of electrons that can be delocalized ↑ so does:
Hardness and Strength
Na has one valence electron that can be delocalized so:
- is relatively soft ( can be cut with a butter knife)
Mg has two valence electrons that can be delocalized so:
- still can be cut but is much harder than Na
Transition metals have varied # of e-'s that can be delocalized
- Chromium (Cr+6) is very hard and has high strength

18. Alloys mixture of elements that have metallic properties
mixture can be adjusted to get desired properties
two types:
substitutional and interstitial alloy
(depends on size of elements – same or different size)

19. Common alloys Brass: Cu & Zn Bronze: Cu, Sn & Al Pewter: Sn, Pb & Cu
Solder: Pb & Sn
Rose gold: Cu & Al
White gold: Au & Ni, Pd or Pt
Sterling silver: Ag & Cu
Steel: C & Fe
Stainless steel: Cr & Ni