Multiple Choice
In the Lewis dot structure of BrF_3, how many lone pairs are present on the central bromine atom?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Exceptions
Multiple Choice
After drawing the Lewis structure of BeF_2, what is the ideal bond angle around the central beryllium atom?
A
90^ext{o}
B
109.5^ext{o}
C
120^ext{o}
D
180^ext{o}
Verified step by step guidance1
Identify the central atom in BeF_2, which is beryllium (Be), and note that it is bonded to two fluorine (F) atoms.
Draw the Lewis structure by placing Be in the center and connecting it with single bonds to each F atom. Since Be has only two valence electrons, it forms two single bonds and has no lone pairs.
Determine the electron domain geometry around the central atom by counting the regions of electron density. In this case, there are two bonding pairs and zero lone pairs around Be.
Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular shape. Two bonding pairs with no lone pairs arrange themselves to minimize repulsion, which results in a linear shape.
Recall that a linear molecular geometry corresponds to an ideal bond angle of \(180^\circ\) around the central atom.
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