The dipole moment of methanol is m = 1.70 D. Use arrows to indicate the direction in which electrons are displaced.

Verified step by step guidance

1. Identify the atoms in the methanol molecule: carbon (C), hydrogen (H), and oxygen (O).
2. Recognize that the dipole moment is a vector quantity that points from the positive to the negative charge.
3. Determine the electronegativity of each atom: Oxygen (O) is more electronegative than Carbon (C) and Hydrogen (H).
4. Draw arrows indicating the direction of electron displacement: from the less electronegative atoms (C and H) towards the more electronegative atom (O).
5. Ensure the arrows point towards the oxygen atom, indicating the direction of the dipole moment.

Key Concepts

Dipole Moment

The dipole moment is a vector quantity that measures the separation of positive and negative charges in a molecule. It is represented in Debye units (D) and indicates the direction of electron displacement due to differences in electronegativity between atoms. A higher dipole moment signifies a greater polarity, influencing the molecule's physical properties and interactions.

Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. It varies across the periodic table, with elements like fluorine being highly electronegative. In methanol, the oxygen atom is more electronegative than the hydrogen and carbon atoms, leading to an uneven distribution of electron density and the formation of a dipole moment.

Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. In methanol (CH3OH), the geometry is influenced by the tetrahedral arrangement around the carbon atom and the bent shape around the oxygen atom due to lone pairs. Understanding molecular geometry is crucial for predicting the dipole moment direction and the overall polarity of the molecule.