Question
Discuss the hybridisation of Be in gaseous state and solid state.
✓
Answer
In gaseous state at high temperature, $\mathrm{BeCl}_2$ exists as linear molecule, $\text{Cl}-\text{Be}-\text{Cl},$ thus the hybridisation of the central atoms is sp.$\ \ \ \ \ \text{Cl}-\text{Be}-\text{Cl} \\\ \ \ \ \ \ \text{Structure of}\\\ \text{BeCl in gaseous state}$
In solid state, it has a polymeric structure with chlorine bridges as follows.
Two Cl-atoms are listed to be atom by two coordination bonns and two by covalent bonds. For these bonds to be formed, Be in the excited state with the configuration $\text{1s}^2\ \text{2s}^1\ 2\text{p}_\text{x}^1\ 2\text{p}^0_\text{y}\ 2\text{p}_\text{z}^0$ undergoes $\mathrm{sp}^3$ hybridisation. Two half-filled hybrid orbitals will form normal covalent bonds with two Cl-atom. The other two Cl-atoms are coordinated to Be-atom by donating electron pairs into the empty hybrid orbtitals.
In solid state, it has a polymeric structure with chlorine bridges as follows.
Two Cl-atoms are listed to be atom by two coordination bonns and two by covalent bonds. For these bonds to be formed, Be in the excited state with the configuration $\text{1s}^2\ \text{2s}^1\ 2\text{p}_\text{x}^1\ 2\text{p}^0_\text{y}\ 2\text{p}_\text{z}^0$ undergoes $\mathrm{sp}^3$ hybridisation. Two half-filled hybrid orbitals will form normal covalent bonds with two Cl-atom. The other two Cl-atoms are coordinated to Be-atom by donating electron pairs into the empty hybrid orbtitals.
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