Explain whether C2H3Cl is polar or non-polar and why? Explain how electronegativity is applied to the answer.

If we think of this molecule as a chain, the CH3 is on one end, Cl is on the other, with CH2 between. Cl has an EN (electronegativity) of 3.5, but C on the other end is 2.5 and H is 2.1 so there is a difference and that produces a polar molecule. There isn't that much difference so it may not be highly polar but that's the principle behind it.

To determine whether C2H3Cl (also known as vinyl chloride) is polar or non-polar, we need to consider the molecular geometry and the electronegativities of its constituent atoms.

First, let's determine the molecular geometry of C2H3Cl. In C2H3Cl, the central carbon atom is bonded to two hydrogen atoms (H2C) and one chlorine atom (Cl). The carbon atom and the hydrogen atoms lie in the same plane, forming a flat structure. This molecular geometry is known as trigonal planar.

Next, we need to look at the electronegativity values of the atoms involved. Electronegativity is the tendency of an atom to attract the shared electrons in a covalent bond. The higher the electronegativity value of an atom, the more strongly it attracts electrons.

The electronegativity values (on the Pauling scale) of carbon, hydrogen, and chlorine are approximately 2.5, 2.1, and 3.0, respectively. Chlorine is more electronegative than both carbon and hydrogen.

Now, let's apply electronegativity to determine the polarity of C2H3Cl. In a polar molecule, there is an uneven distribution of electron density, resulting in a positive and negative end (poles). This occurs when there is a difference in electronegativity between bonded atoms.

In C2H3Cl, the chlorine atom is more electronegative than carbon and hydrogen. As a result, it pulls the shared electrons towards itself, creating a partial negative charge (δ-) on the chlorine atom and partial positive charges (δ+) on the carbon and hydrogen atoms. This uneven distribution of charges leads to a polar molecule.

Therefore, C2H3Cl is a polar molecule due to the difference in electronegativity between its constituent atoms.

To determine whether C2H3Cl is polar or non-polar, we need to consider the polarity of each individual bond within the molecule and the overall molecular geometry.

First, let's look at the Lewis structure of C2H3Cl. Carbon (C) is in the center, with two hydrogens (H) bonded to one carbon and one hydrogen and one chlorine (Cl) bonded to the other carbon.

H
|
H - C - C - Cl
|
H

Now, let's examine the electronegativity of the atoms in the molecule. Electronegativity is the measure of an atom's ability to attract electrons towards itself in a chemical bond. The higher an atom's electronegativity, the more it pulls the shared electrons towards itself.

In this case, carbon (C) has an electronegativity value of approximately 2.5, hydrogen (H) has a value of 2.1, and chlorine (Cl) has a value of 3.0.

To determine the polarity of the individual bonds, we compare the electronegativities of the atoms involved. In C-H bonds, the electronegativity difference between carbon (C) and hydrogen (H) is 0.4 (2.5 - 2.1), resulting in a non-polar bond.

In C-Cl bonds, the electronegativity difference is 0.5 (3.0 - 2.5), also resulting in a non-polar bond.

Now, let's examine the overall molecular geometry. Since carbon (C) has two hydrogen atoms attached to it and one chlorine atom attached to it, the molecule has a trigonal planar shape. In a trigonal planar molecule, the bond dipoles (polarity of individual bonds) can cancel out, resulting in a non-polar molecule.

In summary, although C2H3Cl contains polar bonds (C-H and C-Cl), the molecule as a whole is non-polar due to its trigonal planar geometry, which results in the cancellation of the bond dipoles.

It's important to note that understanding electronegativity and molecular geometry is crucial in determining the polarity of a molecule. By applying these concepts, we can determine whether a molecule is polar or non-polar.