Periodic Table Group 2 Flashcards

Study Notes

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.

Description

Test your knowledge with these flashcards focusing on Group 2 of the Periodic Table. Each card includes a definition and examples of elements with two valence electrons. Perfect for chemistry students looking to reinforce their understanding of this element group.