Ch3OH intermolecular forces has hydrogen bonding, dipole dipole attraction and London dispersion forces.

Hello, reders welcome to another fresh article. today we will discuss about ch3oh intermolecular forces.

We will provide a best information about this topic,

So, hold your seat and be with the end of guide.

You could get valuable information out of it.

Read More – What is the Intermolecular forces strongest to weakest?


What is methanol?

Methanol is also an organic chemical compound with the formula CH3OH.

It is also known as methyl alcohol. it is light, colourless, flammable liquid.

Methanol Structure – CH3OH

methanol structure - ch3oh

Properties of Methanol

Properties of methanol

CH3OH Lewis structure

Here, we will discuss about how to created ch3oh Lewis structure.

We can create a Lewis structure of ch3oh with the help of some simple steps.

first we will draw the structure of ch3oh.

ch3oh lewis structure

Here, according to ch3oh lewis structure, there are five bonds are form in ch3oh (methanol).

There are some important point are required to make/ draw ch3oh lewis structure.

Here we will discuss about all the important steps for makeing ch3oh lewis structure.

first of all we will find out valence electron of all the atoms such as, hydrogen, carbon, and oxygen.

The valence electron of hydrogen in ch3oh(methanol)?

The valence electron of hydrogen is 1.

The valence electron of carbon in ch3oh(methanol)?

The valence electron of carbon is

What are CH3OH intermolecular forces

There are three main or important different type of intermolecular forces occur in between two methanol molecules. such as,

  1. Hydrogen bonding
  2. dipole-dipole interaction
  3. London dispersion forces

Lets know in details,

Hydrogen bonding

Yes, hydrogen bonding is present between two methanol molecules. because oxygen is directly attached to hydrogen and due to this hydrogen bonding form. this forces is called strong intermolecular forces and it occur between oxygen and hydrogen. You know that oxygen is highly electronegativity atoms compare with hydrogen.due to this, oxygen has partial negative charge whereas hydrogen has partial positive charge. According to this, both atoms are attracted each other. As a results hydrogen bonding occur between this two methanol molecule. and in case of ethanol molecules there same types of intermolecular occur between two ethanol molecules. The intermolecular forces of ethanol are, hydrogen bonding, dipole dipole forces. and i meant to say that the ethanol intermolecular forces are hydrogen bonding, dipole dipole interaction. this mean, the same intermolecular forces occur between, two methanol or ethanol molecules.

Now, You can understand properly with the help of methanol chemical structure.

ch3oh intermolecular forces

Dipole-dipole interaction

Yes, dipole-dipole interaction occur in methanol because it creat dipole moment between molecules due to the presence of the electronegative oxygen atom.

The electronegative atom which is oxygen that create a permanent positive charge on the molecules and rest of the molecules are create partial negative charge that are easily create parmanent dipole within each of the methanol molecules with opposing charge. this type of interaction is called dipole-dipole interaction.

London dispersion forces:

Yes, it is absolutely true, methanol are also generate london dispersion forces between two non polar molecules. the basic concepts is this that, the interaction between two non polar methanol molecules. it mean, one hydrogen atom of first methanol interacted with second hydrogen of second methanol molecules. But It generated very weak intermolecular forces. In other words, there is not any poles to interact each other. this is one type of interaction between two methanol molecules in which very weak intermolecular forces are generated. this weak interaction is know as London dispersion forces. this is shown in figure.

London dispersion forces

this type of interaction created between non polar molecules. this type of force is called london dispersion forces. So, we can say that, ch3oh intermolecular forces has also London dispersion forces.

Read MoreWhat is the intermolecular forces of HCl?

Example of intermolecular Forces

There is various examples for intermolecular forces. such as,

Intermolecular forces of i2, co2, h2O, ch3br, and ch4.

lets know in details,

1. i2 intermolecular forces

In case of i2 molecules, the i2 intermolecular forces are van der waals dispersion forces due to the nature of molecules. It has also temporary dipole. So we can say that, I2 intermolecular forces are only London dispersion forces.

2. Co2 intermolecular forces

CO2 has polar dipole, and it create bonds such as, and C-O bonds. But in this case, the dipole point is in opposite directions. It is properly cancel each other. because the nature of molecules. So, we can say that it is non polar molecules. Mainly, Weak forces (london dispersion forces) occur non polar molecules.

Therefore, CO2 has only intermolecular forces are london dispersion forces.

3. H2O intermolecular forces

H2O has strongest intermolecular forces because this molecules make hydrogen bonding.

Hydrogen bonding are created if hydrogen are bound with oxygen, nitrogen, and fluorine.

If any molecules held together by hydrogen bonding. then it make strongest type of intermolecular forces. Such as, dipole dipole hydrogen bond.

So, h2O has strongest type intermolecular forces such as, dipole dipole hydrogen bond.

Read More – What type of intermolecular forces persent in CO?

4. Ch3br intermolecular forces

ch3br is a polar molecules. because this molecules have different Electronegativity. and forces of attraction occur due to different Electronegativity. Ch3br has not permanent dipole but it has strong overall force of attraction between ch3br molecules.

If i m talking about boiling point. If any one ask me, how to determine the higher/lower boiling point. My answer is,

if molecules have temporary dipole then molecules has higher boiling point. but if molecules have permanent dipole then molecules have lower boiling point. finely. ch3br has dipole dipole force and dispersion forces.

5. Ch4 intermolecular forces

Yes, it is true that ch4 has not parmanent dipole dipole because in this molecules hydrogen is not bound with Electronegative atoms.

For example, H-N, H-O, H-F

So, ch4 has temporary dipole, not parmanent dipole. and resion is already explained. but ch4 is a non polar molecules because this molecules are bound or attached four carbon-hydrogen with single covalent bonds. So, this molecules is called non polar. So, finely I can say that ch4 intermolecular forces are only London dispersion forces (weak force).

Frequentily Asked Question

1. What type of intermolecular forces persent in ch3och3?

If you see carefully on the structure of dimethyl ether. it is clear that, oxygen atoms is directly attached with two methyl group. and this methyl group connect to oxygen. Due to this hydrogen bonding are generated between this molecules.

for example, – CH3 – O – CH3

O – oxygen

CH3 – Methyl group

In case of CH3OCH3, oxygen is highly electronegativity atoms hydrogen atoms is directly attached to oxygen. So, it mean that, if hydrogen atoms are not attached to oxygen then hydrogen bond are not created between the molecules. because that electronegative of oxygen have permanent charge. carbon has less electronegative then oxygen and hydrogen has less electronegativity then carbon.

You know that, permanent dipole attraction between partial positive end of one molecules to partial negative end of another molecules. this type of attraction is called dipole-dipole intraction. London dispersion forces is also persent in this molecules.

therefore, we can say that ch3och3 has three type of intermolecular. such as,

  1. Hydrogen bonding
  2. Dipole dipole
  3. Dispersion forces

2. is CCl4 dipole moment?

Yes, CCl4 has dipole moment. Dipole moment is generated between CCl4 molecule because chlorine atom has high electronegativity compare with carbon. so, we can say that, according to this, chlorine has partial negative charge and carbon has partial positive charge. due to this, both are attracted each other and it generate dipole moment between carbon and chlorine atoms. As shown in figure.

ccl4 intermolecular forces

but if you add all vectorial then it all cancel out because the dipole arrow point at opposite direction so, due to this, it all cancel out and it make zero dipole. therefore, ccl4 has no net dipole moment. CCl4 is a non polar molecules. So, there is dipole moment present in CCl4.

3. Which type of intermolecular forces exist in cl2 and ccl4?

The proper answer of this question is, both molecules exist weakest intermolecular forces (only london dispersion forces) because both are non polar molecules.

You know that, non polar molecules has no any dipole to attract each other. this mean, there is a no any negative pole Or no any positive pole. this mean, there is no chance to attract each other because attraction is possible between two pole. so, no pole it mean no attraction, so it create weakest intermolecular forces (London dispersion forces).

So, we can say that the correct answer is London dispersion forces.

4. Hydrogen bond is stronger then dipole-dipole forces?

yes, hydrogen bond is 10 time stronger then all dipole -dipole forces. therefore, hydrogen bond is more stronger then dipole-dipole forces.

5. Hydrogen bond is stronger then covalent bond?

No, hydrogen bond is 20 time weaker then covalent bond. therefore, we can say that, hydrogen bond is not more stronger then ionic or covalent bond.


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