1. Elements and Their Properties
Chapter 20
Elements and Their Properties

2. Chapter 20
Section 1: Metals

3. You will learn how to…….. Describe the properties of a typical metal
Identify the alkali metals and alkaline earth metals
Differentiate among three groups of transition elements
This is important because metals are a part of your everyday life--- from electric cords to the cars you ride in.

4. Metals on the Periodic Table
On the periodic table, the metals are found on the LEFT side of the zig-zag line.

5. Properties of Metals Conduct heat and electricity Luster (shiny)
Malleable (bendable or able to shape)
Ductile (Drawn into wires)
Solid at room temperature (EXCEPT Mercury (Hg)= liquid)

6. Metals
Valence electron
Metals generally have 1-3 electrons on their outer energy level (valence electrons).
In chemical reactions, metals tend to GIVE UP electrons easily because they are close to having an empty outer energy level.
3 P 4N
Lithium

7. Metals
When a metal GIVES UP an electron, the atom then has MORE protons than electrons and the atom is no longer neutral. The atom is MORE POSITIVE.
When a metal gives up an electron it becomes a positively charged ion.
Na gave up an electron to Cl. The Na atom becomes a positively charged ion because it has more protons than electrons.

8. Bonding in Metals
When metals give electrons to nonmetals, an ionic bond is formed.
Metal (Na) + Nonmetal (Cl) = Ionic Bond (NaCl)

9. Types of Metals Alkali Metals Alkaline Earth Metals
Transition Elements
Inner Transition Elements

10. Alkali Metals Located in GROUP 1 of the periodic table
MOST HIGHLY REACTIVE because they only have 1 valence electron, so these elements are NOT found free in nature
Gives away the 1 valence electron because it is easier to LOSE 1 versus gaining 7 electrons to complete the octet (8 electrons)
+1 ion

11. Alkali Metals Some uses of Alkali Metals
Living things need potassium and sodium compounds to stay healthy.
Doctors use lithium compounds to treat bipolar depression

12. Alkaline Earth Metals Located in GROUP 2 of the periodic table
2nd MOST HIGHLY REACTIVE because they only have 2 valence electron, so these elements are NOT found free in nature
Gives away the 2 valence electrons because it is easier to LOSE 2 versus gaining 6 electrons to complete the octet (8electrons)
+2 ion

13. Alkaline Earth Metals Some uses of Alkaline Earth Metals
Magnesium and strontium are used in are used in fireworks to produce the brilliant white color and the bright red flashes.
Calcium compounds are needed for life. Calcium compounds in your bones helps make them strong.

14. Transition Metals Located in GROUP 3-12 of the periodic table
Iron Triad = iron, cobalt, nickel (used to make steel and other metal mixtures)
Coinage metals = copper, silver, gold (used to make coins)

15. Inner Transition Metals
Located at the bottom of the periodic table
Lanthanides
Actinides- ALL are unstable and radioactive- nucleus breaks down and gives off particles and energy

16. Chapter 20
Section 2: Nonmetals

17. You will learn how to…….. Recognize hydrogen as a nonmetal
Compare and contrast properties of the halogens
Describe properties and uses of the noble gases
This is important because nonmetals are not only all around you, the are an essential part of your body!

18. Nonmetals on the Periodic Table
On the periodic table, the nonmetals are found on the RIGHT side of the zig-zag line.
REMEMBER: HYDROGEN IS A NONMETAL!

19. Properties of Nonmetals
Poor conductors of heat and electricity
No luster (not shiny)
Not malleable (bendable)
Not ductile (CAN NOT be drawn into wires)
Usually gases OR brittle solids (EXCEPTION: Bromine (Br) = liquid)
Sulfur
Oxygen

20. Did you know….. Most of your body mass is made up of nonmetals!
oxygen, carbon, hydrogen, and nitrogen

21. NONMETAL + NOMETAL = COVALENT BONDING
Bonding in Nonmetals
Nonmetals tend to GAIN electrons to become stable.
When a nonmetal gains an electron it becomes a NEGATIVELY charged ION.
NONMETAL + NOMETAL = COVALENT BONDING
(SHARE electrons)

22. Hydrogen
Highly reactive
Is a nonmetal that acts like a metal

23. Diatomic Molecules
Diatomic molecule – consists of two atoms of the same element in a covalent bond.
Hi Bronclf ( HI BrONClF)
H2, I2, Br2, O2, N2, Cl2, F2) H
SHARE electrons

24. Nonmetals
Halogens
Noble Gases

25. The Halogens Located in group 7A (17) of the periodic table
Forms a SALT when reacts with a metal (Example: NaCl)
MOST HIGHLY reactive nonmetals because they have 7 valence electrons
Gains 1 electron to become stable
- 1 ions

26. Sublimation Sublimation- SOLID GAS without forming a LIQUID
Example. Dry ice

27. Noble Gases on the Periodic Table
Located in group 8A (18) of the periodic table
Inert gases (Do not react)
Outermost energy levels are full
STABLE

28. Chapter 20
Section 3: Mixed Groups

29. You will learn how to….
Distinguish among metals, nonmetals, and metalloids
Describe the nature of allotropes
Recognize the significance of differences in crystal structure in carbon
Understand the importance of synthetic elements
This is important because the elements in mixed groups affect your life every day, because they are in everything from the computer you use to the air you breathe.

30. Metalloids
Elements ABOVE and BELOW the zig-zag line (EXCEPTION: Aluminum (Al)
Has properties of both METALS and NONMETALS

31. Boron Group

32. Carbon Group

33. Allotrope
Allotrope- SAME element with a DIFFERNET molecular structure

34. Allotropes
This figure shows three allotropes of carbon.

35. Nitrogen Group

36. Oxygen Group