Periodic Table Group 2 Flashcards

Group 2: Alkaline-Earth Metals

• Elements have 2 valence electrons, indicating reactivity.
• Examples include Beryllium, Magnesium, Calcium, Strontium, Barium, and Radium.
• Less reactive than alkali metals (Group 1).

Group 13

• Elements possess 3 valence electrons, deducing the "1" in double-digit group numbers.
• Aluminum is a key example.
• 3rd ionization energy represents energy required to remove a third electron from a cation, with a value of 6913 kJ/mol for Na2+.

Group 1: Alkali Metals

• Characterized by having 1 valence electron, resulting in high reactivity.
• Includes Lithium, Sodium, and Potassium.

Group 3-12: Transition Metals

• Properties of these metals vary widely but retain metallic characteristics.
• Common examples are Iron, Gold, Zinc, Silver, and Copper.

Lanthanides and Actinides Series

• Located in two rows at the bottom of the periodic table, comprising transition metals from periods 6 and 7.
• The top row, the Lanthanide series, includes elements from Lanthanum (atomic number 57) to Lutetium (atomic number 71).
• Examples include Neodymium, Thorium, and Europium.

Group 17: Halogens

• Composed of nonmetals with 7 valence electrons.
• Notable elements include Fluorine, Chlorine, Bromine, Iodine, and Astatine.

Group 18: Noble Gases

• Unreactive nonmetals with a complete outer electron shell containing 8 electrons.
• Examples include Helium, Neon, Argon, Krypton, Xenon, and Radon.
• Helium is notable for its small size, and is commonly used to fill balloons for floating.

Hydrogen

• Though associated with alkali metals due to having 1 valence electron, Hydrogen is nonmetallic and very reactive.
• Has only one electron level, making it unique compared to alkali metals.