Anomalous bohoniour of
period eleste
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Explanation:
The reasons for differences in periodic properties and hence in chemical behaviour are:
- Small size of these atom
- High electronegativity
- Large charge/radius ratio
- These elements also have only 4 valence orbitals available (2s and 2p) for bonding as compared to the 9 available (3s, 3p, and 3d) to the other members of the respective groups, so their maximum covalency is 4. (This is why Boron can only form [BF4]– whereas Aluminium can form [AlF6]3-).
- It has been observed that Lithium, Beryllium, Boron, Carbon, Nitrogen, Oxygen, and Fluorine have slightly different periodic properties than the rest of the elements belonging to Group 1, 2, 13-17 respectively.
- For example, Lithium and Beryllium form covalent compounds, whereas the rest of the members of Groups 1 and 2 form ionic compounds.
- Also, the oxide that is formed by Beryllium when it reacts with Oxygen is amphoteric in nature, unlike other Group 2 elements that form basic oxides.
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