QuestionDichlorobenzene ( $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$ ) exists in three forms, called ortho, meta, and para: ortho meta para
Which of the structures has/have a nonzero dipole moment? Select all that apply. ortho meta para

Studdy Solution

STEP 1

What is this asking? Which versions of dichlorobenzene have a dipole moment, meaning they have an uneven distribution of electrical charge? Watch out! Symmetry can be tricky!
Even if individual bonds have polarity, the overall molecule might not have a dipole if the polarities cancel each other out.

STEP 2

1. Analyze Ortho-dichlorobenzene
2. Analyze Meta-dichlorobenzene
3. Analyze Para-dichlorobenzene

STEP 3

Let's look at ortho-dichlorobenzene!
The two chlorine atoms are right next to each other on the benzene ring.
Imagine those chlorines pulling on electrons.
They're both pretty electronegative, so they're both tugging on the electrons in the C-Cl bonds.

STEP 4

These two "tugs" don't cancel out!
They combine to give a net dipole moment pointing somewhere between the two C-Cl bonds.
Think of it like adding two vectors pointing in slightly different directions.
The resulting vector isn't zero!

STEP 5

Now for meta-dichlorobenzene!
Here, the chlorines are one carbon apart.
Again, each chlorine is pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 6

These pulls don't completely cancel out either!
They're at a $120^\circ$ angle from each other on the benzene ring.
If you add those two "tug" vectors, you get a net dipole moment pointing downwards from the center of the ring.

STEP 7

Finally, para-dichlorobenzene!
The chlorines are directly across from each other.
Each one is still pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 8

But here's the catch!
Because they're directly opposite each other, the pulls are perfectly balanced!
It's like a tug-of-war with equally strong teams.
The net dipole moment is zero!
The individual bond dipoles cancel each other out perfectly due to the symmetry.

STEP 9

Ortho-dichlorobenzene and meta-dichlorobenzene have nonzero dipole moments. Para-dichlorobenzene has a net dipole moment of zero.

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QuestionDichlorobenzene ( $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$ ) exists in three forms, called ortho, meta, and para: ortho meta para
Which of the structures has/have a nonzero dipole moment? Select all that apply. ortho meta para

Studdy Solution

STEP 1

What is this asking? Which versions of dichlorobenzene have a dipole moment, meaning they have an uneven distribution of electrical charge? Watch out! Symmetry can be tricky!
Even if individual bonds have polarity, the overall molecule might not have a dipole if the polarities cancel each other out.

STEP 2

1. Analyze Ortho-dichlorobenzene
2. Analyze Meta-dichlorobenzene
3. Analyze Para-dichlorobenzene

STEP 3

Let's look at ortho-dichlorobenzene!
The two chlorine atoms are right next to each other on the benzene ring.
Imagine those chlorines pulling on electrons.
They're both pretty electronegative, so they're both tugging on the electrons in the C-Cl bonds.

STEP 4

These two "tugs" don't cancel out!
They combine to give a net dipole moment pointing somewhere between the two C-Cl bonds.
Think of it like adding two vectors pointing in slightly different directions.
The resulting vector isn't zero!

STEP 5

Now for meta-dichlorobenzene!
Here, the chlorines are one carbon apart.
Again, each chlorine is pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 6

These pulls don't completely cancel out either!
They're at a $120^\circ$ angle from each other on the benzene ring.
If you add those two "tug" vectors, you get a net dipole moment pointing downwards from the center of the ring.

STEP 7

Finally, para-dichlorobenzene!
The chlorines are directly across from each other.
Each one is still pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 8

But here's the catch!
Because they're directly opposite each other, the pulls are perfectly balanced!
It's like a tug-of-war with equally strong teams.
The net dipole moment is zero!
The individual bond dipoles cancel each other out perfectly due to the symmetry.

STEP 9

Ortho-dichlorobenzene and meta-dichlorobenzene have nonzero dipole moments. Para-dichlorobenzene has a net dipole moment of zero.

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QuestionDichlorobenzene ( C6H4Cl2\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}C6​H4​Cl2​ ) exists in three forms, called ortho, meta, and para: ortho meta paraWhich of the structures has/have a nonzero dipole moment? Select all that apply. ortho meta para

Studdy Solution

STEP 1

What is this asking? Which versions of dichlorobenzene have a dipole moment, meaning they have an uneven distribution of electrical charge? Watch out! Symmetry can be tricky!Even if individual bonds have polarity, the overall molecule might not have a dipole if the polarities cancel each other out.

STEP 2

1. Analyze Ortho-dichlorobenzene2. Analyze Meta-dichlorobenzene3. Analyze Para-dichlorobenzene

STEP 3

Let's look at *ortho*-dichlorobenzene!The two chlorine atoms are right next to each other on the benzene ring.Imagine those chlorines pulling on electrons.They're both pretty electronegative, so they're both tugging on the electrons in the C-Cl bonds.

STEP 4

These two "tugs" don't cancel out!They combine to give a net dipole moment pointing somewhere between the two C-Cl bonds.Think of it like adding two vectors pointing in slightly different directions.The resulting vector isn't zero!

STEP 5

Now for *meta*-dichlorobenzene!Here, the chlorines are one carbon apart.Again, each chlorine is pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 6

These pulls don't *completely* cancel out either!They're at a 120∘120^\circ120∘ angle from each other on the benzene ring.If you add those two "tug" vectors, you get a net dipole moment pointing downwards from the center of the ring.

STEP 7

Finally, *para*-dichlorobenzene!The chlorines are directly across from each other.Each one is still pulling on those electrons, creating a dipole along each C-Cl bond.

STEP 8

But here's the catch!Because they're directly opposite each other, the pulls are perfectly balanced!It's like a tug-of-war with equally strong teams.The net dipole moment is **zero**!The individual bond dipoles cancel each other out perfectly due to the symmetry.

STEP 9

*Ortho*-dichlorobenzene and *meta*-dichlorobenzene have nonzero dipole moments. *Para*-dichlorobenzene has a net dipole moment of zero.

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Studdy solves anything!

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

QuestionDichlorobenzene ( $\mathrm{C}_{6} \mathrm{H}_{4} \mathrm{Cl}_{2}$ ) exists in three forms, called ortho, meta, and para: ortho meta para
Which of the structures has/have a nonzero dipole moment? Select all that apply. ortho meta para

1. Analyze Ortho-dichlorobenzene
2. Analyze Meta-dichlorobenzene
3. Analyze Para-dichlorobenzene

Let's look at ortho-dichlorobenzene!
The two chlorine atoms are right next to each other on the benzene ring.
Imagine those chlorines pulling on electrons.
They're both pretty electronegative, so they're both tugging on the electrons in the C-Cl bonds.

These two "tugs" don't cancel out!
They combine to give a net dipole moment pointing somewhere between the two C-Cl bonds.
Think of it like adding two vectors pointing in slightly different directions.
The resulting vector isn't zero!

Now for meta-dichlorobenzene!
Here, the chlorines are one carbon apart.
Again, each chlorine is pulling on those electrons, creating a dipole along each C-Cl bond.

These pulls don't completely cancel out either!
They're at a $120^\circ$ angle from each other on the benzene ring.
If you add those two "tug" vectors, you get a net dipole moment pointing downwards from the center of the ring.

Finally, para-dichlorobenzene!
The chlorines are directly across from each other.
Each one is still pulling on those electrons, creating a dipole along each C-Cl bond.

But here's the catch!
Because they're directly opposite each other, the pulls are perfectly balanced!
It's like a tug-of-war with equally strong teams.
The net dipole moment is zero!
The individual bond dipoles cancel each other out perfectly due to the symmetry.

Ortho-dichlorobenzene and meta-dichlorobenzene have nonzero dipole moments. Para-dichlorobenzene has a net dipole moment of zero.