Quiz review
Lewis Structures, VSEPR shape,
polarity, and IMFs
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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
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
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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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Structures
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.
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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.
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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
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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 dipoledipole IMF
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Structures
What is its shape?
tetrahedral
trigonal planar
pyramidal
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Trigonal planar…Very good!
What is the polarity?
Polar
Nonpolar
Try again!!
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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
**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
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Structures
What is its shape?
Square planar
Pyramidal
Octahedral
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Square Planar…Very good!
What is the polarity?
Polar
Nonpolar
Try again!!
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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 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.
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Structures
What is its shape?
see saw
angular
linear
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Linear…Very good!
What is the polarity?
Polar
Nonpolar
Try again!!
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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 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.
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Structures
What is its shape?
angular
trigonal planar
linear
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Angular…Very good!
What is the polarity?
Polar
Nonpolar
Try again!!
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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 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
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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
Try again!!
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Trigonal planar…Very good!
What is the polarity?
Polar
Nonpolar
Try again!!
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Polar…Very good!
What is its principal IMF?
London
Dispersion
Dipole Dipole
Hydrogen
Bonding
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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
**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
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Structures