section 4 – pg 198 bonding in metals
Post on 18-Jan-2018
220 Views
Preview:
DESCRIPTION
TRANSCRIPT
Chapter 5
Section 4 – pg 198Bonding in Metals
Metals and Alloys• Alloy: a mixture made of two or more elements, at
least one of which is a metal• Alloys are generally stronger and less reactive than
the pure metals from which they are made Zinc + Copper = Brass Carbon + Iron = Steel
Copper + Silver = Sterling Silver
Pg 199
Physical Properties of Alloys• The properties of an alloy can differ greatly from those
of its individual elements– May also retain many physical properties of the metals
depending on how they are mixed
Pg 199
Chemical Properties of Alloys• The chemical properties of an alloy are different than
what it is made of– IE: Iron is strong and a good material to make tools out of
but it rusts so we add carbon to get steel, which is hard and does not rust
Pg 199
Iron rusts
Steel does not
Metallic Bonding• The properties of solid metals and their alloys can
be explained by the structure of metal atoms and the bonding between those atoms– Most metals have 1-3 valence electrons– These are held loosely and are easily lost causing the
metal atom to become positively charged
Pg 200
Metallic Bonding Continued• Metal atoms combine in regular patterns in which the
valence electrons are free to move from atom to atom– Crystalline Solids– Positively charged ions are closely packed together– Metallic Bond: an attraction between a positive metal
ion and the many electrons surrounding it
Pg 200
Metallic Properties• The “sea of electrons” model of metallic bonding
helps explain the malleability, ductility, luster. High electrical conductivity, and high thermal conductivity of solid metals
Pg 201
Malleability and Ductility• Metals are malleable (can be rolled into sheets or
beaten into shapes) and ductile (easily bent and pulled into thin strand or wire) because the positive ions are attracted to the loose electrons all around them rather than to the other metal ions– This is also why metals bend before breaking
Pg 201
Luster• A metals luster (shininess) is due to its valence
electrons– When light strikes these electrons, they absorb the light
and then give it off again
Pg 202
Electrical Conductivity• Metals conduct current easily b/c the electrons in a
metal can move freely among the atoms
Pg 202
Thermal Conductivity• Metals conduct heat easily because of the valence
electrons’ freedom of motion within a metal or metal alloy
Pg 202
Chapter 5 Section 4Homework – pg 203
1A. What is an alloy?
1B. From what pure metals is stainless steel made?
1C. Compare and contrast the general properties of alloys and
pure metals
2A. What is a metallic bond?
2B. Explain how metal atoms form metallic bonds. What role do the
valence electrons play?
2C. Review what you learned earlier about ionic bonds. How
does a metallic bond differ from an ionic bond?
3A. Name 4 properties of metals. What accounts for these
properties?
3B. In a light bulb, a thin tungsten wire filament that is wound in a coil
conducts electric current. Describe two properties of the metal tungsten that make it good material for the filament
3C. Why is it safer to use a nonmetal mixing spoon when cooking something
on a stove?
top related