Questions: Lab Quiz Review
UNIVERSITY
- Practice Question
- Find the correct information for XeF2: # of electron groups, electron geometry, bond angle, # of bonded atoms, molecular geometry,
- A) 5, trigonal bipyramidal, 120 90, 2, linear
- B) 3, trigonal planar, 120, 2, bent
- C) 4, tetrahedral, 109.5, 2, bent
- D) 2, linear, 180, 2, linear
Transcript text: Lab Quiz Review
UNIVERSITY
- Practice Question
- Find the correct information for XeF2: # of electron groups, electron geometry, bond angle, # of bonded atoms, molecular geometry,
- A) 5 , trigonal bipyramidal, $120 \& 90,2$, linear
- B) 3 , trigonal planar, 120,2 , bent
- C) 4 , tetrahedral, $109.5,2$, bent
- D) 2 , linear, 180,2 , linear
Solution
Solution Steps
Step 1: Determine the Number of Electron Groups
To find the number of electron groups around the central atom in xenon difluoride (XeF2), we need to consider both the bonded atoms and lone pairs on the central atom, xenon (Xe). Xenon has 8 valence electrons. In XeF2, two electrons are used to form bonds with the two fluorine atoms, leaving 6 electrons, which form 3 lone pairs. Therefore, the total number of electron groups is 5 (2 bonded atoms + 3 lone pairs).
Step 2: Determine the Electron Geometry
With 5 electron groups, the electron geometry is trigonal bipyramidal. This geometry accounts for the arrangement of all electron groups around the central atom.
Step 3: Determine the Bond Angle
In a trigonal bipyramidal electron geometry, the bond angles are typically 90° and 120°. However, for the linear molecular geometry of XeF2, the bond angle between the bonded atoms is 180°.
Step 4: Determine the Number of Bonded Atoms
XeF2 has 2 bonded atoms, which are the two fluorine atoms.
Step 5: Determine the Molecular Geometry
The molecular geometry of XeF2 is linear. This is because the three lone pairs occupy equatorial positions in the trigonal bipyramidal arrangement, forcing the two fluorine atoms to be opposite each other, resulting in a linear shape.