Quiz review
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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

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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!!

Go back


Trigonal planar very good2

Trigonal planar…Very good!

What is the polarity?

Polar

Nonpolar


Try again28

Try again!!

Go back


Polar very good3

Polar…Very good!

What is its principal IMF?

London Dispersion

Dipole - Dipole

Hydrogen Bonding


Try again29

Try again!!

Go back


Hydrogen bonding very good

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


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