Section 14: Covalent Compounds
[POLARITY OF COMPOUNDS LAB]
Purpose
The purpose of this lab is to examine the polarities of different substances and observe the “like dissolves like”
phenomenon.
Introduction
Electrons are not always shared equally between two bonding atoms; one atom might exert more of a
force on the electron cloud than the other. This "pull" is termed electronegativity and measures the
attraction for electrons a particular atom has. The unequal sharing of electrons within a bond leads
to the formation of an electric dipole: a separation of positive and negative electric charge. Partial
charges are denoted as δ+ (delta plus) and δ− (delta minus).
Atoms with high electronegativities — such as fluorine, oxygen, and nitrogen — exert a greater pull on electrons
than atoms with lower electronegativities. In a bond, this can lead to unequal sharing of electrons between atoms, as
electrons will be drawn closer to the atom with the higher electronegativity. Bonds can fall between one of two
extremes — being completely non-polar or completely polar. A completely non-polar bond occurs when the
electronegativities are identical and therefore possess a difference of zero. A completely polar bond is more correctly
termed ionic bonding and occurs when the difference between electronegativities is large enough that one atom
takes an electron from the other. The terms "polar" and "non-polar" bonds usually refer to covalent bonds. To
determine the polarity of a covalent bond using numerical means, the difference between the electronegativity of the
atoms is taken. If the result is between 0.4 and 1.7 then, generally, the bond is polar covalent.
Molecular polarity is dependent on the difference in electronegativity between atoms in a compound and the
asymmetry of the compound's structure. For example, a molecule of water is polar because of the unequal sharing of
its electrons between oxygen and hydrogen in which the former has larger electronegativity than the latter,
resulting in a "bent" structure, whereas methane is considered non-polar because the carbon shares the electrons
with the hydrogen atoms almost uniformly. Polarity underlies a number of physical properties including surface
tension, solubility, and melting- and boiling-points.
Procedure
 Create a data table like the one below on a sheet of white paper: (Make the boxes somewhat large.)
Solute
Water
Alcohol
Paint Thinner
(very polar)
(somewhat polar)
(non-polar)
Crayon
“Washable”Marker
Permanent Marker
Post-Lab Questions
1. What does it mean for a substance to be polar? List 3 examples of non-chemistry things that can be labeled as
polar.
2. Draw VSEPR structures of NH3 and CH4 and use the delta plus and minus to indicate partial charge.
3. Is NH3 polar or non-polar? How do you know?
4. Is CH4 polar or non-polar? How do you know?
5. Which one of the following will dissolve more easily in water: NH 3 or CH4?
6. What does the phrase “like dissolves like” mean? How does it apply to this experiment?
7. Discuss any compounds that were difficult to determine their polarity. What could you do to make the results
less “gray” and more “black-and-white?”
8. Capsaicin is the spice that is in jalapenos to give them their kick. Using some Flamin’ Hot Cheetos and some
water (which is polar) determine if capsaicin is a polar molecule or a nonpolar molecule. If you are trying to
soothe your mouth after eating spicy food, which should you drink: water, alcohol, or 2% milk (fat is non-polar).
Justify your answer.