What is the Difference Between Ionic Covalent and Metallic Hydrides?
🆚 Go to Comparative Table 🆚The main difference between ionic, covalent, and metallic hydrides lies in the type of chemical bond involved and the elements they are formed with. Here is a summary of the three types of hydrides:
- Ionic Hydrides:
- Formed when hydrogen reacts with highly electropositive s-block elements (alkali metals and alkaline earth metals).
- Generally binary compounds, insoluble in solutions.
- In the solid state, they are crystalline, non-conducting, and non-volatile, but in the liquid state, they conduct electricity.
- Examples: NaH, CaH2.
- Covalent Hydrides:
- Formed when hydrogen reacts with non-metals, sharing a covalent bond.
- Can be volatile or non-volatile compounds, either liquids or gases.
- Examples: SiH4 (silane).
- Metallic Hydrides:
- Formed when hydrogen reacts with transition metals or their alloys.
- Also known as interstitial hydrides.
- The bond is mostly covalent, but sometimes hydrides are formed with ionic bonds.
- They conduct heat and electricity, but not to the extent of their parent metals.
- Examples: TiH, aluminium, cadmium, magnesium.
In summary, ionic hydrides are formed with highly electropositive elements, covalent hydrides are formed with non-metals, and metallic hydrides are formed with transition metals. The physical properties and chemical bonding of these hydrides depend on the type of hydride and the elements involved.
Comparative Table: Ionic Covalent vs Metallic Hydrides
Here is a table comparing the differences between ionic, covalent, and metallic hydrides:
Property | Ionic Hydrides | Covalent Hydrides | Metallic Hydrides |
---|---|---|---|
Formation | Formed when hydrogen reacts with highly electropositive s-block elements (e.g., alkali and alkaline earth metals). | Formed when hydrogen reacts with non-metals, sharing a covalent bond. | Formed when hydrogen reacts with transition metals, mostly through covalent bonds, but sometimes through ionic bonds. |
Bond Type | Ionic bonds. | Covalent bonds. | Covalent or ionic bonds, depending on the specific hydride. |
State in Solid Form | Crystalline, non-conducting, and non-volatile. | Volatile or non-volatile compounds, either liquids or gases. | Interstitial hydrides, conducting heat and electricity but not to the extent of their parent metals. |
Conductivity | In solid state: Non-conducting. In liquid state: Conducts electricity. | Non-conducting. | Conducting, but not as much as their parent metals. |
Examples | Lithium hydride (LiH), sodium hydride (NaH), and calcium hydride (CaH2). | Silicon hydride (SiH4), boron hydride (BH3), and phosphine (PH3). | Titanium hydride (TiH), aluminum hydride (AlH), and magnesium hydride (MgH2). |
Ionic hydrides are formed when hydrogen reacts with highly electropositive s-block elements, resulting in ionic bonds. In contrast, covalent hydrides form when hydrogen reacts with non-metals, sharing covalent bonds. Metallic hydrides, on the other hand, are formed when hydrogen reacts with transition metals, mostly through covalent bonds, but sometimes through ionic bonds.
- Ionic Bonding vs Metallic Bonding
- Molecular vs Metallic Hydrogen
- Ionic vs Covalent Bonds
- Ionic vs Metallic Solids
- Ionic vs Covalent Compounds
- Hydrogen Bond vs Ionic Bond
- Hydrogen Bond vs Covalent Bond
- Ionic vs Molecular Compounds
- Ionic vs Molecular Solids
- Electrovalent vs Covalent Bond
- Electrovalency vs Covalency
- Metal Carbonate vs Metal Hydrogen Carbonate
- Covalent Radius vs Metallic Radius
- Ionic vs Binary Compounds
- Covalent vs Noncovalent Bonds
- Covalent vs Polar Covalent
- Ionic vs Electrostatic Interactions
- Molecular Equation vs Ionic Equation
- Coordinate Covalent Bond vs Covalent Bond