What is the Difference Between Group 1 and Group 2 Elements?
🆚 Go to Comparative Table 🆚The key difference between Group 1 and Group 2 elements lies in the number of unpaired electrons in their outermost orbitals. Group 1 elements have unpaired electrons in their outermost orbital, whereas Group 2 elements have paired electrons in their outermost orbital. Both Group 1 and Group 2 elements are found in the S block of the periodic table and have their outermost electrons in the s orbital.
Here are some further differences between Group 1 and Group 2 elements:
- Electronic Configuration: Group 1 elements have unpaired electrons in their outermost orbital, while Group 2 elements have paired electrons in their outermost orbital.
- Reactivity: Group 1 elements are more reactive than Group 2 elements.
- Cation Formation: Group 1 elements tend to form +1 cations, while Group 2 elements tend to form +2 cations.
- Melting Points: Group 2 elements have higher melting points compared to Group 1 elements.
- Basicity of Hydroxides: The hydroxides of Group 2 elements are less basic compared to those of Group 1 elements.
In summary, Group 1 elements have unpaired electrons in their outermost orbitals and are more reactive, while Group 2 elements have paired electrons and form +2 cations. Group 2 elements also have higher melting points and less basic hydroxides compared to Group 1 elements.
Comparative Table: Group 1 vs Group 2 Elements
The main difference between Group 1 and Group 2 elements lies in the number of electrons in their outermost orbitals. Group 1 elements have unpaired electrons in their outermost orbitals, while Group 2 elements have paired electrons in their outermost orbitals. Here is a comparison table highlighting the differences between Group 1 and Group 2 elements:
| Property | Group 1 Elements | Group 2 Elements |
|---|---|---|
| Number of electrons in outermost orbital | Unpaired electrons | Paired electrons |
| Reactivity | Highly reactive | Less reactive compared to Group 1 elements |
| Ionization energy | Lower ionization energy | Higher ionization energy |
| Electronic configuration | Tend to lose one electron to achieve stability in their electron configuration | Tend to lose two electrons to achieve stability in their electron configuration |
| Cation formation | Form +1 cations | Form +2 cations |
| Melting points | Lower melting points | Higher melting points |
| Basicity of hydroxides | More basic hydroxides | Less basic hydroxides |
Group 1 elements are also called alkali metals, while Group 2 elements are called alkaline earth metals. The alkali metals are highly reactive due to their unpaired electrons in the outermost orbital, while the alkaline earth metals are less reactive because their electrons in the outermost orbital are paired.
- Group 1 Metals vs Transition Metals
- Atoms vs Elements
- Atomic vs Molecular Elements
- Group I vs Group II Introns
- Isotopes vs Elements
- Periods vs Groups
- Elements vs Compounds
- D Block Elements vs Transition Elements
- Alkali Metals vs Alkaline Earth Metals
- Element vs Compound
- Phosphoryl Group vs Phosphate Group
- Transition Metals vs Metals
- Group vs Team
- Representative vs Transition Elements
- Chalcophile vs Siderophile Elements
- Halogens vs Halides
- Copper 1 vs Copper 2
- Point Group vs Space Group
- Mineral vs Element