1. Chapter 3: Elements and the Periodic Table
Section 3: Metals

2. Metal
A class of elements characterized by physical properties that include shininess, malleability, ductility, and conductivity.

3. Physical Properties of Metals
Shininess
Malleability – ability to be hammered or rolled into flat sheets and other shapes
Ductility – ability to be pulled out, or drawn, into a long wire
Conductivity – ability to transfer heat or electricity
*some metals are magnetic (iron, cobalt, nickel)
*most are solids at room temperature (except for mercury)

4. Malleability

5. Ductility

6. Conductivity

7. Checkpoint 1
What property of metals allows them to be drawn into wires?

8. Checkpoint 1
What property of metals allows them to be drawn into wires?
Ductility

9. Chemical Properties of Metals
Metals have a range of reactivities (ease and speed with which an element combines, or reacts with other elements); react by losing electrons to other atoms
Sodium (Na) reacts very strongly when exposed to air or water
Gold (Au) and platinum (Pt) have a lack of reactivity
Iron (Fe) falls in the middle; corrodes to form rust when it comes into contact with oxygen (O)
Corrosion – gradual wearing away of a metal element due to a chemical reaction
The reactivity of metals tends to decrease as you move from left to right across the periodic table.

10. Checkpoint 2
What is reactivity?

11. Checkpoint 2 What is reactivity?
The ease and speed with which an element combines, or reacts with other elements.

12. Metals in the Periodic Table
Alkali metals
Alkaline earth metals
Transition metals
(Metals in mixed groups)
Lanthanides
Actinides

13. Alkali Metals Metals in Group 1, from lithium to francium.
React with other elements by losing one electron.
So reactive that they are never found as uncombined elements in nature.
Some are shiny and so soft that you can cut them with a plastic knife.
Examples
Sodium (Na): found in large amounts in seawater and salt beds, important in body
Potassium (K): important in body
Lithium (Li): used in batteries and some medicines

15. Alkaline Earth Metals Group 2 of the periodic table.
Fairly hard, gray-white, and good conductor of electricity.
React by losing two electrons.
Not as reactive as alkali metals, but still very reactive; not found uncombined in nature
Examples
Magnesium (Mg): can be mixed with aluminum to make a strong but light-weight material
Calcium (Ca): essential part of teeth and bones; helps muscles work properly

17. Transition metals Elements in Groups 3 through 12 Hard and shiny
Good conductors of electricity
Many form colorful compounds
Less reactive; may take many years to react (rust/corrode)
Examples
Iron (Fe): important in blood
Copper (Cu)
Nickel (Ni)
Silver (Ag)
Gold (Au)

18. Metals in mixed groups
Some elements in Groups 13 through 15 are metals (don’t fit into any other category)
Not very reactive
Examples
Aluminum (Al): lightweight metal
Tin (Sn): protects steel from corrosion in some cans of food
Lead (Pb): once used in paints and water pipes; poisonous; now used in car batteries and weights for balancing tires

20. Lanthanides Top row of elements placed beneath the periodic table
Soft, malleable, shiny, high conductivity
Mixed with more common metals to make alloys (mixtures of a metal with at least one other element, usually another metal)
Usually found together in nature; difficult to separate from one another because they all share very similar properties

21. Actinides Bottom row of elements placed beneath the periodic table.
Only thorium (Th) and uranium (U) occur naturally on Earth
Uranium used to produce energy in nuclear power plants
All others created artificially in laboratories
Nuclei of these elements are very unstable, meaning that they break apart very quickly into smaller nuclei
Some only exist for fraction of a second

22. Extended Periodic Table

23. Checkpoint 3
What happens to reactivity as you move from left to right across the periodic table?

24. Checkpoint 3
What happens to reactivity as you move from left to right across the periodic table?
It decreases.

25. Synthetic elements
Elements with atomic numbers higher than 92 (after uranium) do not occur naturally on Earth; they are made – or synthesized – when nuclear particles are forced to crash into one another.
Examples
Plutonium is made by bombarding nuclei of uranium-238 with neutrons in a nuclear reactor.
Americium-241 is made by bombarding plutonium nuclei with neutrons
Particle accelerator: powerful machines that move atomic nuclei faster and faster until they crash into one another, sometimes forming heavier elements
Gets more difficult as atomic number increases
New elements given temporary three-letter names

27. Checkpoint 4
What is a synthetic element?

28. Checkpoint 4 What is a synthetic element?
An element that does not occur in nature. They are made in laboratories, sometimes using particle accelerators. They are heavier than uranium.

29. Post-lesson Quiz Which is not a property of metals? a. shininess
b. ductility
c. malleability
d. poor conductivity

30. Post-lesson Quiz
2. Which metals are the most reactive? a. alkaline earth metals b. alkali metals c. transition metals d. lanthanides

31. Post-lesson Quiz
3. What tells us the ease and speed with which an element combines with other elements? a. reactivity b. ductility c. conductivity d. malleability

32. Post-lesson Quiz
4. Which category of metals is found in Group 2? a. alkali metals b. transition metals c. alkaline earth metals d. actinides

33. Post-lesson Quiz
5. What does it mean for an element to be “synthesized”? a. it is on the left side of the periodic table b. it is lightweight c. it is made in laboratories d. it is found in nature