Question

a central atom has two lone pairs on opposite sides and four single bonds. what is the molecule geometry of the result? (1 point) square planar octahedral tetrahedral linear

Explanation:

To determine the molecular geometry, we analyze the central atom's electron - pair arrangement. The central atom has 2 lone pairs and 4 single bonds. The total number of electron - dense regions (lone pairs + bonding pairs) is \(2 + 4=6\), so the electron - pair geometry is octahedral. When there are 2 lone pairs on opposite sides and 4 bonding pairs, the molecular geometry (the arrangement of the bonded atoms) is square planar. Let's analyze the other options:

• Linear geometry typically occurs with 2 bonding regions (e.g., \(CO_2\)) or a specific electron - pair arrangement that doesn't match here.
• Tetrahedral geometry is associated with 4 bonding regions and 0 lone pairs (e.g., \(CH_4\)) or 1 lone pair and 3 bonding pairs (e.g., \(NH_3\) has a trigonal pyramidal molecular geometry, but the electron - pair geometry is tetrahedral), which is not the case here.
• Octahedral is the electron - pair geometry, not the molecular geometry when there are lone pairs affecting the bonded - atom arrangement.

Answer:

A. square planar