The question asks about the geometry adopted by a molecule like BeCl₂ when sp hybrid orbitals are formed. Let's examine this step-by-step.

Step 1: Understand Hybridization

Hybridization is the mixing of atomic orbitals to form new hybrid orbitals. These are used in chemical bonding to explain molecular geometry.

In BeCl₂, the central atom is Beryllium (Be), which in its ground state has the electronic configuration: 1s² 2s². The valence electrons are in the 2s orbital. To form bonds, beryllium promotes one electron from the 2s orbital to the 2p orbital, allowing for hybridization as follows:

• 1 x 2s orbital
• 1 x 2p orbital

This results in the formation of two equivalent sp hybrid orbitals.

Step 2: Determine Geometry

Each hybrid orbital forms a sigma bond with a chlorine atom. Because there are only two pairs of electrons around the beryllium atom (one pair in each of the sp hybrid orbitals), the geometry is aimed at minimizing repulsion between these two bonding pairs.

According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the shape that minimizes electron pair repulsion for two electron pairs is linear. Therefore, the molecule BeCl₂ adopts a linear geometry.

Step 3: Conclusion

The correct geometry for the molecule BeCl₂ with sp hybridization is linear. This corresponds to the description where bond angles are approximately 180 degrees between bonded pairs.

Rule Out Other Options:

• Tetrahedral: Requires sp³ hybridization, which involves four electron pairs.
• Trigonal planar: Requires sp² hybridization, suitable for three electron pairs, not two.
• Octahedral: Involves six electron pairs, typically sp³d² hybridization.

Hence, the correct answer is Linear.