1. Chapter 7
The Elements

2. Properties of S-Block Elements
Diagonal Relationships: In addition to horizontal and vertical trends, there is a diagonal relationship between elements such as Li and Mg, Be and Al, B and Si, that have an adjacent upper left/lower right relative location in the periodic table.
The elements within these diagonal relationships have closer properties to the period-3 element in the next group than their own group.

3. Properties of S-Block Elements
Hydrogen:
Officially in group 1A as it has 1 valence electron
Does not have the same properties of the Alkali Metals
Discovered in 1766 by Henry Cavendish
Called “Flammable Air”
Universe contains more than 90% Hydrogen by mass.
Single valence electron is the reason for its unusual set of both metallic and non-metallic properties.

4. Properties of S-Block Elements
Group 1A
Alkali Metals
React with water to form Alkaline Solutions
Alkali comes from the Arabic word al-qili meaning “Ashes of the Saltwort Plant”.
Easily lose valence electrons
ALWAYS form a cation with a +1 Charge
Easily cut with a knife
Found combined with other elements in nature
Good conductors of heat and electricity

5. Properties of S-Block Elements
Group 2A
Alkaline Earth Metals
Medieval Alchemists couldn’t burn them in their fires and therefore classified them as “Earths”
Form compounds with oxygen called Oxides
Except for Beryllium Oxide, when these react with water from a alkaline solution
Alkaline Earth – reflective of the following two properties:
Alkaline: Forms alkaline solutions with water
Earth: Reacts with oxygen to form an oxide

6. Properties of S-Block Elements
Group 2A
Less reactive that Group 1A
Usually found combined with oxygen and other non-metals in the Earth’s crust
ALWAYS lose 2 valence electrons when bonding
When exposed to oxygen, alkaline earth metals form a thin oxide coating
Do not dissolve easily in water

7. Properties of P-Block Elements
Group 3A
The Boron Group
Always found combined with other elements in nature
Boron is a metalloid
Always form an ion with a 3+ charge
Thallium is the most metallic member of this group.
Exceptions:
Thallium, Gallium and Indium only lose 1 electron for form a +1 Cation.

8. Properties of P-Block Elements
Group 4A
The Carbon Group
Carbon is non-metal
Silicon and germanium are metalloids
Tin and lead are metals
Only group that few rules apply to
Only trend that applies is that Carbon is not representative of the other elements within the Carbon group.

9. Properties of P-Block Elements
Group 4A
Mineral: An element or inorganic compound found in nature as solid crystals
Ore: A material in which a mineral can be removed at a reasonable cost
Allotropes; Forms of an element in the same physical state (solid, liquid, gas) but that have different structures and properties.
Think diamonds, carbon and graphite.

10. Properties of P-Block Elements
Group 5A
The Nitrogen Group
Have 5 Valence Electrons
Gain 3 electrons to form -3 Anions
As there are nonmetals, metals and metalloids within this group there are a wide variety of properties
Nitrogen and Phosphorus – Nonmetals
Bismuth – Metal
Arsenic and Antimony - Metalloid
Bismuth is an exception, which can LOSE 3 electrons to form cations with +3 charge

11. Properties of P-Block Elements
Group 6A
The Oxygen Group
Have 6 Valence Electrons
Nonmetal Members: Oxygen and Sulfer
Metalloids: Selenium and Tellurium
Metal: Polonium
Elements act mainly as non-metals
Take to electrons to form a -2 anion
Can share to electrons form a stable electron configurations

12. Properties of P-Block Elements
Group 7A
The Halogen Group
Named for their ability to form compound with almost all metals (Called SALTS)
Halogen = “Salt Former”
Differ in Physical Properties
Iodine a solid that changes into a vapor directly
Chlorine is a gas at room temperature
Bromine is a liquid, but it evaporates easily
Chemical behavior of halogens is similar
Reactive non-metals that are found combined with other elements in nature
Astatine is the exception, as it is radioactive with no known uses
7 Valence Electros
Anion with -1 Charge

13. Properties of P-Block Elements
Group 8A
The Noble Gases
Last naturally occurring elements to be discovered
Non-reactive and colorless
Very stable, but can form compounds in the right environment
No known compounds of helium, neon or argon.
8 valence electrons
Unable/Unwilling to form ions

14. Properties of D-Block Elements
Transition Metals
Rows 3-12
Starts at Period 4 (Row 4)
Contain Filled and/or Partially Filled D Orbitals
Labeled “B” on the periodic table columns
Share properties including:
Conductivity
Luster
Malleability with other metals
Unable/Unwilling to form ions

15. Properties of D-Block Elements
Transition Metals
Little variation across the periods (rows):
Atomic Size
Electronegativity
Ionization Energy
Variation in Physical Properties
Most are hard solids with high melting and boiling points
Determined by their electron configuration
Ability of the unpaired “D” electron to move into the valence level.
Hardness, melting and boiling points increase with more unpaired electrons

16. Properties of F-Block Elements
Inner-Transition Metals
Lanthanide Series
Silvery metals
High melting points
Extremely little variation in nature
Mixed together in nature
Very hard to separate
Fun Fact: Neodymium and Praseodymium are added to the glass used to make welder’s goggles to help shield their eyes from the radiation
Actinide Series

17. Properties of F-Block Elements
Inner-Transition Metals
Actinide Series
Radioactive Elements
Only 3 exist in nature
The rest are synthetic elements AKA Transuranium Element
Transuranium Element = Element with a number grater than 92
92 = Atomic Number of Uranium
Decay quickly
Exception: Plutonium-239 with a half-life of 24,000 years