Question:
Which of the following is not a similarity of beryllium with aluminium ?
Which of the following is not a similarity of beryllium with aluminium ?
Updated On: Jul 7, 2022
- It becomes passive when treated with conc. $HNO_3$
- It forms polymeric covalent hydrides
- Carbonate of $Be$ is extremely stable
- Salts of $Be$ do not impart colour to the flame
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The Correct Option is C
Solution and Explanation
Beryllium shows resemblance with its diagonally opposite element aluminium. Points of similarity are-
Both metals have a tendency to form covalent bonds. Eg; Chlorides of both are being covalent are being soluble in organic solvents.
Both $BeCl _{2}$ and $AlCl _{3}$ act as Lewis acids and are used as Friedal Kraft's catalyst.
These two elements have the same electronegativity and polarizing power i.e. charge per radius ration of their ions are very similar.
They form polymeric covalent hydrides.
They become passive when treated with conc. $HNO _{3}$
Salts of Be do not impart colour to the flame.
But, the stability of Carbonate of Be is not similar to carbonate of Al.
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Concepts Used:
Group 1 Elements
Group one of alkali metals is s-block elements with just one electron in their s-orbital. They are are alkali metals. They are named so because of the alkaline nature of the hydroxides and oxides.
Alkali metals are characterized by one s-electron in the valence shell of their atoms.
Alkali metals have a corresponding [Noble gas] ns1 electronic configuration. They occupy the first column of the periodic table. Alkali elements are:
- Lithium(Li)
- Sodium(Na)
- Potassium (K)
- Rubidium (Ru)
- Cesium (Cs)
- Francium (Fr)
They have occupied successive periods from first to seven. Francium is a radioactive element with very low half-life.
Electronic Configuration:
- Alkali metals have one electron in their valence shell.
- The electronic configuration is given by ns1. For example, the electronic configuration of lithium is given by 1ns1 2ns1.
- They tend to lose the outer shell electron to form cations with charge +1 (monovalent ions).
This makes them the most electropositive elements and due to the same reason, they are not found in the pure state.