Carbon reacts with chlorine and hydrogen to form the compound CH3Cl.

(a) Construct the structure of CH3Cl.
What is the dominant form of secondary bonding for CH3Cl?
Dipole-dipole interactions, London dispersion forces, Covalent bonding, Ionic bonding

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This is a dipole.

To construct the structure of CH3Cl, we need to determine the arrangement of the atoms and the types of bonds between them.

First, we have one carbon atom (C), one chlorine atom (Cl), and three hydrogen atoms (H).

The carbon atom is in the center, and it forms four chemical bonds. One bond is formed with the chlorine atom, and the other three bonds are formed with the hydrogen atoms.

The chlorine atom forms one bond with the carbon atom, and it has three lone pairs of electrons, denoted as "dots" around the atom.

The hydrogen atoms each form one bond with the carbon atom.

To represent the structure, we can use a Lewis structure or a molecular formula.

Lewis structure:
H
|
H - C - Cl

Molecular formula:
CH3Cl

Now, moving on to the dominant form of secondary bonding for CH3Cl, we need to consider the types of intermolecular forces present.

Dipole-dipole interactions occur between the positive end of one polar molecule and the negative end of another polar molecule. In CH3Cl, the carbon-chlorine bond is polar due to the difference in electronegativity between carbon and chlorine. This polarity allows for dipole-dipole interactions to occur between CH3Cl molecules.

London dispersion forces, also known as van der Waals forces, occur between all molecules, whether they are polar or nonpolar. These forces arise due to temporary fluctuations in electron distribution, leading to temporary dipoles. While all molecules have London dispersion forces, they are typically weaker than dipole-dipole interactions.

Covalent bonding refers to the sharing of electrons between atoms within a molecule. It does not apply to intermolecular forces.

Ionic bonding involves the transfer of electrons from one atom to another, resulting in the formation of oppositely charged ions. In the case of CH3Cl, it does not involve ionic bonding.

Therefore, for CH3Cl, the dominant form of secondary bonding is dipole-dipole interactions.