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# Why does CH3Clchloromethane have a larger dipole moment than CHCl3chloroform?

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# Why does $CH_3Cl$CH3Cl have morea larger dipole moment than $CHCl_3$CHCl3?

Why does $$CH_3Cl$$$$\ce{CH3Cl}$$, methyl chloride, have morea larger dipole moment than $$CHCl_3$$$$\ce{CHCl3}$$, chloroform?

Let us consider $$C-Cl$$$$\ce{C-Cl}$$ bond moment to be $$x$$ and that of $$C-H$$$$\ce{C-H}$$ bond to be $$y$$.

In $$CCl_4$$$$\ce{CCl4}$$, the dipole moment of any three C-Cl$$\ce{C-Cl}$$ atoms is balanced by the dipole moment of the fourth $$C-Cl$$$$\ce{C-Cl}$$ bond dipole moment. This means the resultant of dipole moment of three $$3\ C-Cl$$$$\ce{C-Cl}$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$C-Cl$$$$\ce{C-Cl}$$ bond.
Now

Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$CH_3Cl$$$$\ce{CH3Cl}$$ it can be proved that its dipole moment is also $$x+y$$.

Where have I gone wrong?

# Why does $CH_3Cl$ have more dipole moment than $CHCl_3$

Why does $$CH_3Cl$$ have more dipole moment than $$CHCl_3$$?

Let us consider $$C-Cl$$ bond moment to be $$x$$ and that of $$C-H$$ bond to be $$y$$.

In $$CCl_4$$, the dipole moment of any three C-Cl atoms is balanced by the dipole moment of the fourth $$C-Cl$$ bond dipole moment. This means the resultant of dipole moment of $$3\ C-Cl$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$C-Cl$$ bond.
Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$CH_3Cl$$ it can be proved that its dipole moment is also $$x+y$$.

Where have I gone wrong?

# Why does CH3Cl have a larger dipole moment than CHCl3?

Why does $$\ce{CH3Cl}$$, methyl chloride, have a larger dipole moment than $$\ce{CHCl3}$$, chloroform?

Let us consider $$\ce{C-Cl}$$ bond moment to be $$x$$ and that of $$\ce{C-H}$$ bond to be $$y$$.

In $$\ce{CCl4}$$, the dipole moment of any three $$\ce{C-Cl}$$ atoms is balanced by the dipole moment of the fourth $$\ce{C-Cl}$$ bond dipole moment. This means the resultant of dipole moment of three $$\ce{C-Cl}$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$\ce{C-Cl}$$ bond.

Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$\ce{CH3Cl}$$ it can be proved that its dipole moment is also $$x+y$$.

Where have I gone wrong?

3 added 122 characters in body

Why does $$CH_3Cl$$ have more dipole moment than $$CHCl_3$$?

Let us consider $$C-Cl$$ bond moment to be $$x$$ and that of $$C-H$$ bond to be $$y$$.

In $$CCl_4$$, the dipole moment of any three C-Cl atoms is balanced by the dipole moment of the fourth $$C-Cl$$ bond dipole moment. This means the resultant of dipole moment of $$3\ C-Cl$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$C-Cl$$ bond.
Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$CH_3Cl$$ it can be proved that its dipole moment is also $$x+y$$.

Where
Where have I gone wrong?

Why does $$CH_3Cl$$ have more dipole moment than $$CHCl_3$$?

Let us consider $$C-Cl$$ bond moment to be $$x$$ and that of $$C-H$$ bond to be $$y$$.

In $$CCl_4$$, the dipole moment of any three C-Cl atoms is balanced by the dipole moment of the fourth $$C-Cl$$ bond dipole moment. This means the resultant of dipole moment of $$3\ C-Cl$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$C-Cl$$ bond.
Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$CH_3Cl$$ it can be proved that its dipole moment is also $$x+y$$.

Where have I gone wrong?

Why does $$CH_3Cl$$ have more dipole moment than $$CHCl_3$$?

Let us consider $$C-Cl$$ bond moment to be $$x$$ and that of $$C-H$$ bond to be $$y$$.

In $$CCl_4$$, the dipole moment of any three C-Cl atoms is balanced by the dipole moment of the fourth $$C-Cl$$ bond dipole moment. This means the resultant of dipole moment of $$3\ C-Cl$$ bonds in tetrahedral structure is equal to $$x$$, which is equal and opposite to the dipole moment $$x$$ of the fourth $$C-Cl$$ bond.
Now, when we replace one of the chlorines with a hydrogen, the net dipole moment equals $$x+y$$, (as they are in the same directions). Similarly if we carry out the same procedure for $$CH_3Cl$$ it can be proved that its dipole moment is also $$x+y$$.

Where have I gone wrong?

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