Following vanderwaal forces are present in ethyl acetate liquid

Options

A. Dipole-dipole and hydrogen bonding
B. London dispersion and dipole-dipole
C. London dispersion, dipole-dipole and hydrogen bonding
D. hydrogen bonding and London dispersion

Answer

To determine the types of Van der Waals forces present in ethyl acetate (C4H8O2), we will analyze the molecular structure and the types of intermolecular interactions that can occur.

### Step 1: Identify the Molecular Structure
- Ethyl acetate has the molecular formula C4H8O2.
- Its structural formula can be represented as CH3COOCH2CH3.

### Step 2: Analyze Dipole-Dipole Interactions
- Dipole-dipole interactions occur between polar molecules.
- In ethyl acetate, the carbonyl group (C=O) creates a dipole due to the electronegativity difference between carbon and oxygen.
- The presence of the polar C=O bond indicates that ethyl acetate can engage in dipole-dipole interactions.

### Step 3: Analyze Hydrogen Bonding
- Hydrogen bonding occurs when hydrogen is bonded to highly electronegative atoms like nitrogen (N), oxygen (O), or fluorine (F).
- In ethyl acetate, while there are hydrogen atoms, they are not bonded to highly electronegative atoms (like O, N, or F) in a way that would facilitate hydrogen bonding.
- Therefore, ethyl acetate does not exhibit hydrogen bonding.

### Step 4: Analyze London Dispersion Forces
- London dispersion forces are present in all molecules, regardless of polarity, and are the result of temporary dipoles that occur due to fluctuations in electron distribution.
- Ethyl acetate, being a molecular compound, will also exhibit London dispersion forces.

### Conclusion
- Ethyl acetate exhibits dipole-dipole interactions due to its polar carbonyl group and London dispersion forces due to the presence of electrons in the molecule.
- Therefore, the correct answer is that ethyl acetate has dipole-dipole interactions and London dispersion forces.

### Final Answer
The types of Van der Waals forces present in ethyl acetate liquid are dipole-dipole interactions and London dispersion forces.