What is the dominant intermolecular forces for C2H5OC2H5 (diethyl ether)?
Is it dispersion and polar?
I would go along with that.
To determine the dominant intermolecular forces in diethyl ether (C2H5OC2H5), we need to analyze the molecular structure.
Diethyl ether consists of two ethyl groups (-C2H5) attached to an oxygen atom (-O-). The oxygen atom has two lone pairs of electrons, making it a polar molecule. The electronegativity difference between carbon and oxygen in diethyl ether is significant, resulting in a polar bond between the carbon and oxygen atoms.
The dominant intermolecular forces in diethyl ether are dispersion forces and dipole-dipole interactions. Dispersion forces, also known as London forces, are present in all molecules and arise from temporary fluctuations in electron distribution, leading to temporary dipoles. In diethyl ether, these dispersion forces exist between both the carbon atoms and the oxygen atom.
Additionally, diethyl ether exhibits dipole-dipole interactions due to the polar nature of the molecule. The oxygen atom is more electronegative than the carbon atoms, resulting in a partial negative charge on the oxygen and partial positive charges on the carbon atoms. This polarity allows for attractive forces between the positive end of one molecule and the negative end of another.
Therefore, the dominant intermolecular forces in diethyl ether are dispersion forces and dipole-dipole interactions.