The II group elements in the periodic table is known as
Alkaline earth metals
Understanding II Group Elements in the Periodic Table
The periodic table organizes elements based on their properties. Elements are arranged in groups (vertical columns) and periods (horizontal rows). Each group contains elements that have similar chemical properties, mainly due to having the same number of valence electrons.
What are II Group Elements?
The elements found in Group II of the periodic table are commonly known by a specific name. These elements include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
Let's look at the options provided and determine the correct name for these II group elements.
Analyzing the Options
- Alkali metals: This group refers to the elements in Group I of the periodic table (Lithium, Sodium, Potassium, Rubidium, Cesium, Francium). They are very reactive metals.
- Alkaline earth metals: This name is given to the elements in Group II of the periodic table. They are also reactive metals, but generally less so than alkali metals. Their oxides form alkaline solutions in water, and many are found in the Earth's crust. This is why they are called "alkaline earth" metals.
- Lanthanides: These are a series of 15 metallic elements from lanthanum (atomic number 57) to lutetium (atomic number 71) on the periodic table, typically placed in a separate row below the main body. They are part of the f-block elements.
- Transition metals: These are elements found in Groups 3 to 12 of the periodic table. They are known for having variable oxidation states and forming colored compounds.
Based on the definitions, the II group elements are specifically known as Alkaline earth metals.
Properties of II Group Elements (Alkaline Earth Metals)
The II group elements share several common properties:
- They are reactive metals, though less reactive than Group I alkali metals.
- They have two valence electrons, which they tend to lose to form ions with a $+2$ charge (e.g., $\text{Mg}^{2+}$).
- They are good conductors of heat and electricity.
- They have relatively high melting and boiling points compared to alkali metals.
- Their oxides react with water to form alkaline hydroxides.
The name "Alkaline earth metals" accurately describes the nature and occurrence of these II group elements.
| Group Name | Periodic Table Group | Key Characteristics |
|---|---|---|
| Alkali metals | Group 1 | Highly reactive metals, 1 valence electron, form +1 ions |
| Alkaline earth metals | Group 2 (II Group Elements) | Reactive metals, 2 valence electrons, form +2 ions, found in Earth's crust |
| Lanthanides | Atomic numbers 57-71 (f-block) | Rare earth elements, similar properties, often placed separately |
| Transition metals | Groups 3-12 (d-block) | Variable oxidation states, form colored compounds |
Therefore, the correct classification for the II group elements is Alkaline earth metals.
Important Questions from Periodic Table
The electronic configuration of an element is 2, 8, 8. It belongs to group
The correct order of decreasing electron gain enthalpy with negative sign for chalcogens is - Identify
Inert gases are?
In computers, chip is made up of:
Modern periodic table has:
