The Structure of Metals Brittany Braeutigan Ch. 6.4 Dustin Whitehead

Vocab Metallic Bonds The attraction between a metal cation and the shared electron around it.

Vocab Alloy A mixture of two or more elements, at least one is a metal.

Metals are made up of metallic bonds. In a metallic bond, the cations form a lattice that is held in place by the strong metallic bonds between the cations and the surrounding valence electrons. Metal atoms achieve stable configuration by losing electrons.

The more valence elections in an atom makes the metallic bond stronger. Therefore, an atom with less valence electrons would be weak metallic bonds. Examples of weak metals are alkali metals; they only have one valence electron.

Properties of metals affect a metals structure greatly. The mobility of electrons within a metal lattice explains some of the properties of metals.

The two most important properties of a metal are the ability to conduct electric currency and malleability. If a metal can conduct an electric current, it will allow the electricity to be carried through the atom. If a metal is malleable, it will be able to be hit with a hammer and not shatter. The ions change positions in the atom but they are so closely packed together due to the metallic bond.

 Some types of alloys Copper o Bronze – the first most important alloy. In its simplest form, bronze contains only copper and tin o Brass – contains copper and zinc. Shinier than bronze and to shape.

 Other types of alloys: Lightweight metals. Aluminum – bends and dents easily and is a very light weight metal. Magnesium – a lightweight metal and is used to make aircraft.

Gold – expressed in karats and is made up of silver, copper, nickel, or zinc. Can be dented and worn down.

Steel – 1900’s Age of Steel o Alloy of iron that contains carbon o Age of Steel because skyscrapers, automobiles, and ships were being built o Stainless steel contains more the 10% of chromium by mass, but almost no carbon.

Tungsten is the metal that has the highest melting point at 3410 degrees Tungsten is the metal that is in light bulbs Valence electrons are able to move freely among the atoms

The lattice in a metal is flexible compared to the rigid lattice in an ionic compound Metallic bonds explain why metals can be made into thin wires without breaking A flow of charged particles is called an electronic current

1.Metal atoms achieve stable electron configurations by losing what? a. protons b. neutrons c. electrons 2. A ________ is the attraction between a metal cation and the shared electrons that surround it. a. nuclear bond b. metallic bond c. ionic bond 3. What was the first important alloy? a. silver b. bronze c. gold 4. The purity of gold is expressed in what? a. steel b. powder c. karats 5. The 1900’s could be called the Age of Steel because of what? a. automobiles b. skyscrapers c. both a and b 6. Stainless steel contains more that __% chromium by mass, but almost no carbon. a. 40 b. 10 c The body of a plane is large and needs to be made from a ___ material. a. Light weight b. medium weight c. heavy weight 8. A mixture of two or more elements, at least on of which is a metal, that has the characteristics preparative of a metal is the definition of what? a. metal b. steel c. alloy 9. The lattice in a metal is flexible compared to the rigid lattice in a what? a. Cohh2o b. ionic compound c. angle compound 10. What is the melting point of tungsten? a. 34 degrees C b. 310 degrees C c degrees C

1.C 2.B 3.B 4.C 5.C 6.B 7.A 8.C 9.B 10.C