Worksheets4.2 Molecular Geometry and Polarity
Total questions: 15
Worksheet time: 26mins
State VSEPR Theory.
The electron pairs in the valence shell surrounding a terminal atom repel one another and arrange themselves as far apart as possible to minimize the repulsion.
The electron pairs in the valence shell surrounding a central atom repel one another and arrange themselves as far apart as possible to minimize the repulsion.
The electron pairs in the valence shell surrounding a central atom repel one another and arrange themselves as close as possible to minimize the repulsion.
Any molecule with only two atoms must be linear. Three-atom molecules such as BeCl2 can also be linear. For linear molecules, the bond angle is
90°
180°
108°
120°
Which molecule would have this molecular geometry?
BF3
CH4
PCl5
CO2
What molecular geometry would PH3 have?
Trigonal Pyramidal
Trigonal Bipyramidal
Linear
Bent
A molecular geometry with 2 lone pairs and 4 bonding pairs is
Tetrahedral
Trigonal Bipyramidal
Square Planar
Square Pyramidal
To determine the molecular geometry of a compound by using VSEPR theory, double bond and triple bonds are considered as
two or three bonding pairs
two bonding pairs
five bonding pairs
one bonding pair
Classify the above molecule.
Polar
Non polar
Why is the molecule polar?
There is a non bonding pair electrons on the central atom.
There are different types of elements bonded to the central atom.
There are no non bonding pairs on the central atom and all of the atoms bonded to the central atom are the same.
Which of the following pairs has the same molecular geometry?
BF3 and PCl3
PCl3 and NBr3
NBr3 and AlCl3
BeCl2 and O3
For CS2, determine its shape and polarity
Linear, Polar molecule
Linear, Non polar molecule
V-shaped, Polar molecule
V-shaped, Non polar molecule
Predict the shape and bond angle for IF4+
Tetrahedral
109.5
Square planar
90
See Saw
<120, < 90
Trigonal bipyramidal,
120, 90
The PCl3 molecule is trigonal pyramidal while the BCl3 molecule is trigonal planar. This is because
the atomic size of phosphorus is bigger than boron
the presence of a lone pair electrons in the PCl3 molecule
the boron atom has d orbitals in its valence shell
the boron-chlorine bond is stronger than the phosphorus-chlorine bond
Which of the following compounds has zero dipole moment (μ=0)?
CHCl3
ICl2+
PCl3
CO32-
