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Quiz reviewLewis Structures, VSEPR shape,
polarity, and IMFs
Get started!
Draw the Lewis Structure for….
Once you have drawn a Lewis Structure, click on the molecule to check your answer and complete the rest of the questions
H2S
KrF4CO32-
BCl3
HNO3
I3-
SiCl4
OF4
TeO2
SBr6
What is its shape?
tetrahedral angular linear
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Angular…Very good!
What is the polarity?
Polar Nonpolar
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Polar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
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Dipole-Dipole…Very good!
This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 2 lone pairs. It is polar because it is
angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF
Back to Lewis Structures
What is its shape?
Trigonal planar
Pyramidal Tetrahedral
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Trigonal Planar…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
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London Dispersion…Very good!
This molecule is trigonal planar because it has 3 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is nonpolar
and therefore will experience london dispersion intermolecular forces.
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What is its shape?
tetrahedral octahedral pyramidal
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Octahedral…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
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London Dispersion…Very good!
This molecule is octahedral because it has 6 e- pairs around the central atom, 6 atoms bonded to it, and 0 lone pairs. It is nonpolar
so it will experience london dispersion intermolecular forces.
Back to Lewis Structures
What is its shape?
tetrahedral angular square planar
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Tetrahedral…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Try again!!Go back
London Dispersion…Very good!
This molecule is angular because it has 4 e- pairs around the central atom, 4 atoms bonded to it, and 0 lone pairs. Since it is nonpolar
it will experience london dispersion intermolecular forces.
Back to Lewis Structures
What is its shape?
tetrahedral pyramidal see saw
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See Saw…Very good!
What is the polarity?
Polar Nonpolar
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Polar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Try again!!Go back
Dipole-Dipole…Very good!
This molecule is see saw shape because it has 5 e- pairs around the central atom, 4 atoms bonded to it, and 1 lone pairs. It is polar because it has one lone pair which will distort the
shape. Since it is polar, it will have a dipole-dipole IMF
Back to Lewis Structures
What is its shape?
tetrahedral trigonal planar pyramidal
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Trigonal planar…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Try again!!Go back
London Dispersion…Very good!
This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar
because it is angular with two lone pairs. Since it is polar, it will have a dipole-dipole IMF
Back to Lewis Structures
**It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You
get the same answer
What is its shape?
Square planar Pyramidal Octahedral
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Square Planar…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
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London Dispersion…Very good!
This molecule is square planar because it has 6 e- pairs around the central atom, 4 atoms bonded to it, and 2 lone pairs. Although it has lone pairs, it is nonpolar because it is
one of the exceptions. The fluorines cancel each other out, as do the lone pair in this specific shape. Since it is nonpolar it experiences london dispersion intermolecular
forces.
Back to Lewis Structures
What is its shape?
see saw angular linear
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Linear…Very good!
What is the polarity?
Polar Nonpolar
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Nonpolar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
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London Dispersion…Very good!
This molecule is linear because it has 5 e- pairs around the central atom, 2 atoms bonded to it, and 3 lone pairs. Although it has lone pairs, this is one of the exceptions and is
nonpolar since the lone pairs are on the same plane and cancel each other out. Since is it nonpolar, it will experience london dispersion intermolecular forces.
Back to Lewis Structures
What is its shape?
angular trigonal planar linear
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Angular…Very good!
What is the polarity?
Polar Nonpolar
Try again!!Go back
Polar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Try again!!Go back
Dipole-Dipole…Very good!
This molecule is angular because it has 4 e- pairs around the central atom, 2 atoms bonded to it, and 1 lone pair. It is polar because it is angular with a lone pair. Since it is polar, it will have a dipole-dipole
IMF
Back to Lewis Structures
Remember for any acid with an oxygen (starts with H and has an O), the hydrogen is bonded to one of the oxygen atoms
What is its shape?
tetrahedral angular trigonal planar
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Trigonal planar…Very good!
What is the polarity?
Polar Nonpolar
Try again!!Go back
Polar…Very good!
What is its principal IMF?
London Dispersion
Dipole - Dipole
Hydrogen Bonding
Try again!!Go back
Hydrogen bonding…Very good!
This molecule is trigonal planar because it has 4 e- pairs around the central atom, 3 atoms bonded to it, and 0 lone pairs. It is polar because all of the
electrons around the central atom are not pulled equally because of the -OH group. Since it is polar and there is an oxygen atom covalently bonded
to a hydrogen atom, this molecule will experience hydrogen bonding
Back to Lewis Structures
**It is also ok to determine shape by saying 3 electron regions, 3 atoms bonded to it, and 0 lone pairs. You
get the same answer