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Quiz review. Lewis Structures, VSEPR shape, polarity, and IMFs. Get started!. Draw the Lewis Structure for…. SBr 6. HNO 3. Once you have drawn a Lewis Structure, click on the molecule to check your answer and complete the rest of the questions. H 2 S. OF 4. CO 3 2-. KrF 4. SiCl 4.

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Quiz review

Quiz review

Lewis Structures, VSEPR shape, polarity, and IMFs

Get started!


Draw the lewis structure for
Draw the Lewis Structure for….

SBr6

HNO3

Once you have drawn a Lewis Structure, click on the molecule to check your answer and complete the rest of the questions

H2S

OF4

CO32-

KrF4

SiCl4

BCl3

I3-

TeO2


Quiz review

What is its shape?

tetrahedral

angular

linear


Try again
Try again!!

Go back


Angular very good
Angular…Very good!

What is the polarity?

Polar

Nonpolar


Try again1
Try again!!

Go back


Polar very good
Polar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again2
Try again!!

Go back


Dipole dipole very good
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


Quiz review

What is its shape?

Trigonal planar

Pyramidal

Tetrahedral


Try again3
Try again!!

Go back


Trigonal planar very good
Trigonal Planar…Very good!

What is the polarity?

Polar

Nonpolar


Try again4
Try again!!

Go back


Nonpolar very good
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again5
Try again!!

Go back


London dispersion very good
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.

Back to Lewis Structures


Quiz review

What is its shape?

tetrahedral

octahedral

pyramidal


Try again6
Try again!!

Go back


Octahedral very good
Octahedral…Very good!

What is the polarity?

Polar

Nonpolar


Try again7
Try again!!

Go back


Nonpolar very good1
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again8
Try again!!

Go back


London dispersion very good1
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


Quiz review

What is its shape?

tetrahedral

angular

square planar


Try again9
Try again!!

Go back


Tetrahedral very good
Tetrahedral…Very good!

What is the polarity?

Polar

Nonpolar


Try again10
Try again!!

Go back


Nonpolar very good2
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again11
Try again!!

Go back


London dispersion very good2
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


Quiz review

What is its shape?

tetrahedral

pyramidal

see saw


Try again12
Try again!!

Go back


See saw very good
See Saw…Very good!

What is the polarity?

Polar

Nonpolar


Try again13
Try again!!

Go back


Polar very good1
Polar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again14
Try again!!

Go back


Dipole dipole very good1
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


Quiz review

What is its shape?

tetrahedral

trigonal planar

pyramidal


Try again15
Try again!!

Go back


Trigonal planar very good1
Trigonal planar…Very good!

What is the polarity?

Polar

Nonpolar


Try again16
Try again!!

Go back


Nonpolar very good3
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again17
Try again!!

Go back


London dispersion very good3
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


Quiz review

What is its shape?

Square planar

Pyramidal

Octahedral


Try again18
Try again!!

Go back


Square planar very good
Square Planar…Very good!

What is the polarity?

Polar

Nonpolar


Try again19
Try again!!

Go back


Nonpolar very good4
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again20
Try again!!

Go back


London dispersion very good4
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


Quiz review

What is its shape?

see saw

angular

linear


Try again21
Try again!!

Go back


Linear very good
Linear…Very good!

What is the polarity?

Polar

Nonpolar


Try again22
Try again!!

Go back


Nonpolar very good5
Nonpolar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again23
Try again!!

Go back


London dispersion very good5
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


Quiz review

What is its shape?

angular

trigonal planar

linear


Try again24
Try again!!

Go back


Angular very good1
Angular…Very good!

What is the polarity?

Polar

Nonpolar


Try again25
Try again!!

Go back


Polar very good2
Polar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again26
Try again!!

Go back


Dipole dipole very good2
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


Quiz review
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 again27
Try again!! an O), the hydrogen is bonded to one of the oxygen atoms

Go back


Trigonal planar very good2
Trigonal an O), the hydrogen is bonded to one of the oxygen atoms planar…Very good!

What is the polarity?

Polar

Nonpolar


Try again28
Try again!! an O), the hydrogen is bonded to one of the oxygen atoms

Go back


Polar very good3
Polar…Very good! an O), the hydrogen is bonded to one of the oxygen atoms

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again29
Try again!! an O), the hydrogen is bonded to one of the oxygen atoms

Go back


Hydrogen bonding very good
Hydrogen bonding…Very good! an O), the hydrogen is bonded to one of the oxygen atoms

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